Unit 7b: Chemical Formulas
|
|
- Clarissa Rose
- 7 years ago
- Views:
Transcription
1 Unit 7b: Chemical Formulas Student Name: Key Class Period: Website upload 2014 Page 1 of 55
2 Page intentionally blank Website upload 2014 Page 2 of 55
3 Unit 7b Vocabulary: 1. Binary compound: A compound that consists of only two elements. 2. Dipole attractions: The attraction of the partially negative (δ - ) end of one polar molecule to the partially positive (δ + ) end of another polar molecule. 3. Dipole moment: An arrow along the line of symmetry in a polar molecule that shows the net direction that electrons are being pulled towards the partially negative (δ - ) end of the molecule. 4. Electronegativity difference: The difference in electronegativity between two elements in a bond. 5. Electrical conductivity (of metals): The ability of a substance to allow electrons to pass from atom to atom through a substance from a source of electricity to an electrical ground. 6. Electrolyte: A solution containing dissolved ions that can conduct electricity within the solution. 7. Empirical formula: The simplest whole-number mole ratio of elements in a compound; used to write the formulas of ionic compounds. 8. Formula mass: The sum of the atomic masses of an element or compound, measured in grams per mole (g/mole). Reported to the nearest tenth (0.1) of a g/mole. 9. Hydrogen bonds: The strong attraction of the H (δ + ) end of one polar molecule to the N, O, or F (δ - ) ends of another molecule. The two molecular ends form temporary covalent bonds. 10. InterMolecular Attractive Force (IMAF): The forces that hold molecules together in the solid and liquid phases. These are the forces that must be overcome to melt or boil a substance. IMAF forces are also called van der Waal s forces. 11. Ionic compound: Compounds consisting of a metal and a nonmetal ionic bonded in a whole-number ratio. 12. London Dispersion Force: The weak attractive forced caused by temporary dipoles in nonpolar molecules. Website upload 2014 Page 3 of 55
4 13. Metallic bond: A bond formed between metal atoms as they collectively share their conducting electrons evenly between metal kernals. 14. Molecular formula: The actual number of nonmetal atoms in a molecule; a whole-number multiple of the empirical formula. 15. Molecule: A group of nonmetal atoms covalently bonded together to form a distinct particle. 16. Network solid: A crystal lattice formed from covalently bonded nonmetal atoms with no distinct molecules. 17. Nonpolar molecule: A molecule with symmetrical electron distribution resulting in any polar bonds cancelling each other out to yield no partially charged ends. 18. Percent composition: The formula mass of an element divided by the formula mass of the compound containing the element and the divisor then multiplied by Polar molecule: A molecule with asymmetric electron distribution resulting in partially charged ends. 20. Polyatomic ion: An ion formed by atoms bonding together in way that a net charge (positive or negative) is formed. 21. Ternary compound: A compound that consists of three (or more) elements, usually containing a polyatomic ion. Website upload 2014 Page 4 of 55
5 Notes page: Website upload 2014 Page 5 of 55
6 Unit 7b Homework Assignments: Assignment: Date: Due: Website upload 2014 Page 6 of 55
7 Notes page: Website upload 2014 Page 7 of 55
8 Topic: Writing Binary Formulas Objective: How do you write formulas for TWO element compounds? Binary Ionic Compounds: Binary Compounds are compounds that are made of only TWO elements combined in a simple, whole-number ratio. The ratio of the elements in the compounds is dependent on the oxidation numbers (or charges) of the elements that are combining to form the compound. Atoms combine in ratios so that the oxidation numbers add up to ZERO (numbers cancel out). In a chemical formula, the CATION is written first and the ANION is written second. A subscript (#) that represents the number of atoms in the compound is placed after the atom. The number 1 is not written as a subscript for single atoms. Examples would include: NaCl has one sodium atom and one chlorine atom; Li 2 O has two lithium atoms and one oxygen atom. Website upload 2014 Page 8 of 55
9 Writing Binary Ionic Formulas: *NOTE: X designates a metal ion; Y designates a nonmetal ion Ions to be Bonded How to determine the formula (How to make the + and - charges each cancel out) Formula Example X +1 and Y and -1 cancel each other XY K +1 and F -1 KF X +2 and Y and -2 cancel each other XY Zn +2 and S -2 ZnS X +3 and Y and -3 cancel each other XY Al +3 and N -3 AlN X +2 and Y -1 X +3 and Y -1 Need two -1 ions to cancel out +2 ion Need three -1 ions to cancel out +3 ion XY 2 Ca +2 and 2 x Cl -1 CaCl 2 XY 3 Fe +3 and 3 x Br -1 FeBr 3 X +1 and Y -2 Need two +1 ions to cancel out -2 ion X 2 Y 2 x Li +1 and O -2 Li 2 O X +1 and Y -3 X +2 and Y -3 X +3 and Y -2 X +4 and Y -2 Need three +1 ions to cancel out -3 ion Find COMMON DENOMINATOR of 6: Need three +2 ions to cancel out two -3 ions Find COMMON DENOMINATOR of 6: Need two +3 ions to cancel out three -2 ions Need two -2 ions to cancel out +4 ion X 3 Y 3 x Na +1 and P -3 Na 3 P X 3 Y 2 3 x Cu +2 and 2 x N -3 Cu 3 N 2 X 2 Y 3 2 x Cr +3 and 3 x S -2 Cr 2 S 3 XY 2 Pb +4 and 2 x O -2 PbO 2 Website upload 2014 Page 9 of 55
10 Notes page: Website upload 2014 Page 10 of 55
11 Topic: Naming Binary Compounds Objective: How do we name compounds containing TWO elements? Naming Binary Ionic compounds: 1. When naming Binary Compounds we place the name of the metal ion first. 2. If the metal ion has more than one listed charge on the Periodic Table, use the Stock system to place a roman numeral in parenthesis after the metal s name representing the charge of the metal ion. 3. Use the first syllable of the nonmetal s name and add the suffix ide to the nonmetal. Roman numeral system: Watch Bozeman Science Naming Compounds video Website upload 2014 Page 11 of 55
12 Naming Binary Ionic Compounds: Use the ion charges as shown here when looking at the samples below. Formula How to determine the name Compound Name KCl ZnO FeBr 2 FeBr 3 K has only one charge listed, so K +1 is named potassium. Chlorine -1 is changed to chloride. Zn has only one charge listed, so Zn +2 is named zinc. Oxygen -2 is changed to oxide. Fe has two charges listed, so use the Br to determine the charge of the Fe. Br has the first listed charge as -1, so two Br -1 ions would be (-1) + (-1) = -2. To make the -2 charge from the two Br -1 ions cancel to zero, the Fe ion MUST have a charge of +2. The Fe +2 cation would be named iron (II), and bromine -1 is changed to bromide. Fe has two charges listed, so use the Br to determine the charge of the Fe. Br has the first listed charge as -1, so three Br -1 ions would be (-1) + (-1) + (-1) = -3. To make the - 3 charge from the three Br -1 ions cancel to zero, the Fe ion MUST have a charge of +3. The Fe +3 cation would be named iron (III), and bromine -1 is changed to bromide. Potassium chloride Zinc oxide Iron(II) bromide Iron(III) bromide Website upload 2014 Page 12 of 55
13 Formula How to determine the name Ag 2 S Cr 2 O 3 CrO 3 Ca 3 P 2 CuS Cu 2 S Ag has only one charge listed, so Ag +1 is named silver. Two Ag +1 ions are needed to cancel the S -2 ion. Sulfur -2 is changed to sulfide. Cr has three charges listed, so use the O to determine the charge of the Cr. Three oxygen ions each have a -2 charge totaling a -6 charge. The Cr therefore MUST have a +6 charge, so each of the two Cr ions has a +3 charge. The Cr +3 cation would be chromium (III) and the oxygen -2 is changed to oxide. Cr has three charges listed, so use the O to determine the charge of the Cr. Three oxygen ions each have a -2 charge totaling a -6 charge. The Cr therefore MUST have a +6 charge, so the single Cr ion has a +6 charge. The Cr +6 cation would be chromium (VI) and the oxygen -2 is changed to oxide. Ca has only one charge listed, so Ca +2 is named calcium. P has the first listed charge as -3, and two P -3 ions have a charge of -6, so three Ca +2 ions are needed. The Ca +2 cation would be calcium and the phosphorous -3 is changed to phosphide. Cu has two charges listed, so use the S to determine the charge of Cu. S has a -2 charge, so the Cu MUST have a +2 charge. The Cu +2 cation is copper (II) and the sulfur -2 is changed to sulfide. Cu has two charges listed, so use the S to determine the charge of Cu. S has a -2 charge, so the two Cu ions MUST equal a +2 charge. The Cu +1 cation is copper (I) and the sulfur -2 is changed to sulfide. Compound Name Silver sulfide Chromium(III) oxide Chromium(VI) oxide Calcium phosphide Copper(II) sulfide Copper(I) sulfide Website upload 2014 Page 13 of 55
14 Topic: Writing Formulas Objective: How do we write a formula given the compound name? Writing the formulas when given an Ionic Compound name: If you are given the name of a compound, use the Period Table to confirm the ion charge (oxidation number) of the element to ensure you have the correct number of ions in each compound. If given a metal with a Stock number, use that to determine the number of ions in the compound. Compound Name How to write the formula (using Periodic Table) Potassium sulfide Potassium is always K +1 ; sulfide is S -2 K 2 S Derived Formula Cobalt(II) oxide Oxide is always O -2 ; cobalt is Co +2 CoO Cobalt(III) oxide Oxide is always O -2 ; cobalt is Co +3 Co 2 O 3 Tin(II) sulfide Sulfide is S -2 ; tin is Sn +2 SnS Tin(IV) sulfide Sulfide is S -2 ; tin is Sn +4 SnS 2 Calcium phosphide Calcium is always Ca +2 ; phosphorous is P -3 Ca 3 P 2 Aluminum bromide Aluminum is always Al +3 ; bromide is Br -1 AlBr 3 Silver nitride Silver is always Ag +1 ; nitride is usually N -3 Ag 3 N Watch Bozeman Science Writing Formulas video Website upload 2014 Page 14 of 55
15 Topic: Ternary Compounds Objective: What compounds do polyatomic ions form? Ternary Compound: A Ternary Compound is an ionic compound containing at least one polyatomic ion. Polyatomic ion: A Polyatomic Ion is an ion made from two or more atoms that is treated as one charged ion in chemistry, and not as the individual atoms it is composed of. Polyatomic atoms are listed in Reference Table E. Note these four things about polyatomic ions. Table E: Selected Polyatomic Ions 1. They are made of more than one atom; 2. All but three have a negative charge; 3. Most of them contain oxygen; 4. The polyatomic cations end in -ium ; the polyatomic anions end in -ide, -ite, or -ate. If the ion contains two atoms it ends in -ide ; (CN -, OH -, O 2-2 ) If the ion has few oxygen atoms, it ends in -ite ; (NO 2 - = nitrite) If the ion has many oxygen atoms, it ends in -ate ; (NO 3 - = nitrate) Website upload 2014 Page 15 of 55
16 Website upload 2014 Page 16 of 55
17 Notes page: Website upload 2014 Page 17 of 55
18 Topic: Writing Ternary Compounds Objective: How do we write a formula with polyatomic ions in it? Writing Ternary Compound Names: When writing names for Ternary Compounds the rules are the same as those for binary compounds, with following exceptions: 1. Parentheses surround the polyatomic ion and a subscript will be used when more than polyatomic ion is in the formula; 2. The metal cation name remains and still uses the Stock system, if needed; Only the ammonium (NH + 4 ) cation retains its name as is. 3. The anion will most likely be the polyatomic ion, and it will keep its given name. Website upload 2014 Page 18 of 55
19 Writing Ternary Formulas from a given Ternary Compound Name: Compound Name How to write the formula (using Periodic Table E Selected Polyatomic Ions) Derived Formula Ammonium sulfide Ammonium is NH 4 +1 ; sulfide is S -2 (NH 4 ) 2 S Cobalt(II) cyanide Cobalt(II) is Co +2 ; cyanide is CN -1 Co(CN) 2 Cobalt(III) sulfate Cobalt(III) is Co +3 ; sulfate is SO 4-2 Co 2 (SO 4 ) 3 Tin(II) nitrate Tin(II) is Sn +2 ; nitrate is NO 3-1 Sn(NO 3 ) 2 Tin(IV) nitrate Tin(IV) is Sn +4 ; nitrate is NO 3-1 Sn(NO 3 ) 4 Calcium phosphate Calcium is Ca +2 ; phosphate is PO 4-3 Ca 3 (PO 4 ) 2 Aluminum dichromate Aluminum is Al +3 ; dichromate is Cr 2 O 7-2 Al 2 (Cr 2 O 7 ) 3 Silver nitrite Silver is Ag +1 ; nitrate is NO 2-1 AgNO 2 Website upload 2014 Page 19 of 55
20 Topic: Naming Ternary Compounds Objective: How do we name a formula with polyatomic ions in it? *Note: Use the listed ionic charges on the Periodic Table. Formula How to determine the name Derived Name KNO 3 ZnSO 4 Fe(NO 2 ) 2 Fe(NO 2 ) 3 K is always +1, so K +1 is potassium; NO 3-1 is nitrate. Zn is always +2, so Zn +2 is zinc; SO 4-2 is sulfate. Fe has two listed charges, so use the polyatomic NO 2-1 ion to determine the charge of the Fe cation. There are two NO 2-1 anions, so together they have a total -2 charge. The Fe cation MUST be +2 to cancel the charges. Fe +2 is then iron (II), and NO 2-1 is nitrite. Fe has two listed charges, so use the polyatomic NO 2-1 ion to determine the charge of the Fe cation. There are three NO 2-1 anions, so together they have a total -3 charge. The Fe cation MUST be +3 to cancel the charges. Fe +3 is then iron (III), and NO 2-1 is nitrite. Potassium nitrate Zinc sulfate Iron(II) nitrite Iron(III) nitrite Ag 2 CO 3 Ag is always +1, so Ag +1 is silver; CO 3-2 is carbonate. There needs to be two Ag +1 ions to cancel the charge of the single polyatomic CO 3-2 ion. Silver carbonate Website upload 2014 Page 20 of 55
21 Formula How to determine the name Derived Name Cr 2 (SO 3 ) 3 Cr(SO 3 ) 3 Ca 3 (PO 4 ) 2 CuCrO 4 Cu 2 CrO 4 Cr has three listed charges, so use the polyatomic SO 3-2 ion to determine the charge of the Cr cation. There are three SO 3-2 ions, totaling -6 charge, so the total charge of cations MUST be +6. There are two Cr ions, so each Cr cation would be a Cr +3 ion. Cr +3 is then chromium (III), and SO 3-2 is sulfite. Cr has three listed charges, so use the polyatomic SO 3-2 ion to determine the charge of the Cr cation. There are three SO 3-2 ions, totaling -6 charge, so the total charge of the cation MUST be +6. There is only one Cr ion, so the Cr cation would be a Cr +6 ion. Cr +6 is then chromium (VI), and SO 3-2 is sulfite. Ca is always +2, so Ca +2 is calcium; PO 4-3 is phosphate. The three Ca +2 cations have a total +6 charge, and the two PO 4-3 polyatomic ions have a total -6 charge. Cu has two listed charges, so use the charge of the polyatomic CrO 4-2 chromate ion. There is only one CrO 4-2 ion, so the single Cu ion MUST be a Cu +2 cation. Cu +2 is then copper (II), and CrO 4-2 is chromate. Cu has two listed charges, so use the charge of the polyatomic CrO 4-2 chromate ion. There is only one CrO 4-2 ion, but the two Cu ions MUST be Cu +1 cations. Cu +1 is then copper (I), and CrO 4-2 is chromate. Chromium(III) sulfite Chromium (VI) sulfite. Calcium phosphate Copper(II) chromate Copper(I) chromate Website upload 2014 Page 21 of 55
22 Topic: Molecular Compounds Names Objective: How do we name a molecular compound? Molecular compounds may be written two ways: using the Stock System, or using the Prefix System. 1. The Stock System for Molecular Compounds: The Stock System works the same for molecular compounds as with ionic compounds. A Roman numeral is used to show the charge of the first atom written in the formula (which has the LOWER electronegativity). Molecular Formula Name (Stock System) Molecular Formula Name (Stock System) CO 2 Carbon(IV) oxide SO Sulfur(II) oxide CO Carbon(II) oxide SO 2 Sulfur(IV) oxide NO 2 Nitrogen(IV) oxide CCl 4 Carbon(IV) chloride NO 3 Nitrogen(VI) oxide NCl 3 Nitrogen(III) chloride N 2 O 5 Nitrogen(V) oxide P 2 O 3 Phosphorous(III) oxide *Note: NO metals in molecules here! Website upload 2014 Page 22 of 55
23 2. The Prefix System for Molecular Compounds: The Prefix System uses specific prefixes to describe how many atoms of each element are found in the molecule. 1 atom 2 atoms 3 atoms 4 atoms 5 atoms 6 atoms Mono- (or none) Di- Tri- Tetra- Penta- Hexa- Molecular Formula Name (Prefix System) Molecular Formula Name (Prefix System) CO 2 Carbon dioxide SO Sulfur monoxide CO Carbon monoxide SO 2 Sulfur dioxide NO 2 Nitrogen dioxide CCl 4 Carbon tetrachloride NO 3 Nitrogen trioxide NCl 3 Nitrogen trichloride N 2 O 5 Dinitrogen pentoxide P 2 O 3 Diphosphorous trioxide *NOTE: The Prefix System MAY NOT be used for naming ionic compounds. The Prefix System may ONLY be used to name molecular compounds. *Note: NO metals in molecules here! Website upload 2014 Page 23 of 55
24 Notes page: Website upload 2014 Page 24 of 55
25 Student name: Key Class Period: _3, 5, & 10_ Please carefully remove this page from your packet to hand in. Naming and Writing Binary and Ternary Formulas Homework: Binary Compounds: Write the formulas for the following binary compounds (4 pts): Name Formula Lead (II) nitride Pb 3 N 2 Potassium oxide K 2 O Iron (III) chloride FeCl 3 Lead (IV) oxide PbO 2 Write the name of the following binary compounds (4 pts): Formula AuCl Cu 2 S CuS FeO Name Gold(I) chloride Copper(I) sulfide Copper(II) sulfide Iron(II) oxide Ternary Compounds: Write the formulas of the following ternary ionic compounds (4 pts): Name Formula Potassium oxalate K 2 C 2 O 4 Lead (II) nitrite Pb(NO 2 ) 2 Lead (IV) hypochlorite Pb(ClO) 4 Ammonium nitrate NH 4 NO 3 Cont d next page Website upload 2014 Page 25 of 55
26 Name the following ternary compounds (4 pts): Formula Cu 3 PO 4 Cu 3 (PO 4 ) 2 (NH 4 ) 2 O Zn(CH 3 COO) 2 Name Copper(I) phosphate Copper(II) phosphate Ammonium oxide Zinc acetate Both Binary and Ternary Compounds (1 pt ea): Indicate if the formula is binary or ternary, and then write the compound name. Formula Type (Binary or Ternary) Name Na 2 O B Sodium oxide Fe 3 (PO 4 ) 2 T Iron(II) phosphate (NH 4 ) 2 SO 4 T Ammonium sulfate Fe 2 S 3 B Iron(III) sulfide Indicate if the formula is binary or ternary, and then write the compound formula. Name Type (Binary or Ternary) Formula Potassium oxide B K 2 O Sodium phosphate T Na 3 PO 4 Aluminum iodide B AlI 3 Sodium cyanide T NaCN Website upload 2014 Page 26 of 55
27 Topic: The Mole Concept Objective: How do we know what a chemical formula means in use? The Mole Concept: A Mole is to chemistry as the term dozen applies to doughnuts or eggs. You buy packages of doughnuts or eggs by the dozen, and we use chemical formulas and calculate reactions by the mole. A mole equals x of ANYTHING. One mole is the number of atoms that have a combined mass of their given atomic mass measured in grams. According to the Periodic Table, hydrogen has an atomic mass number of , so one mole of hydrogen gas would have a mass of grams. o Just how big is this number? o One mole of marbles spread over the earth would result in a layer three miles thick. Website upload 2014 Page 27 of 55
28 Topic: Empirical Formulas Objective: How do we know what a chemical formula means in use? Empirical Formulas: An Empirical Formula is the simplest, whole-number mole ratio of the elements in an ionic compound. If no subscript is shown, then the number of moles of that ion is given as one. When interpreting chemical formulas, if there are parentheses around the written elements then any subscript outside the parentheses multiplies ALL the elements within the parentheses by that subscript. As an example, Ca(NO 3 ) 2 has a 2 as the subscript outside the parentheses, so multiply the number of each element INSIDE the parentheses to find the total number of atoms for that element: (2 x one N = 2 N; 2 x three O = 6 O). As Ca is NOT within the parentheses, it is not affected. There remains only the single Ca in the formula. Website upload 2014 Page 28 of 55
29 Empirical Formula Examples: Empirical Formula # of ions of each element in the compound # of moles of each element in one mole of the compound Total # of moles of ions in one mole of the compound NaCl 1 x Na, 1 x Cl 1 x Na, 1 x Cl = 2 CaCl 2 1 x Ca, 2 x Cl 1 x Ca, 2 x Cl = 3 Al 2 O 3 2 x Al, 3 x O 2 x Al, 3 x O = 5 KNO 3 1 x K, 1x N, 3 x O 1 x K, 1 x N, 3 x O = 5 K 2 SO 4 2 x K, 1 x S, 4 x O 2 x K, 1 x S, 4 x O = 7 Al(NO 3 ) 3 1 x Al, 3 x N, 9 x O 1 x Al, 3 x N, 9 x O = 13 Al 2 (SO 4 ) 3 2 x Al, 3 x S, 12 x O 2 x Al, 3 x S, 12 x O = 17 Website upload 2014 Page 29 of 55
30 Topic: Interpreting Formulas Objective: How do we know what a chemical formula means in use? Coefficients: A coefficient is a number in FRONT of given formula that tells you how many moles of the compound you are working with. To find the total of moles of atoms you have, multiply the number of a particular element by the coefficient given. If no coefficient is given, then it is assumed as 1. Coefficient Examples: Empirical Formula # of moles of each atom in one mole the compound Formula with coefficient Total # of moles each of atom in given number of moles of the compound KBr 1 K, 1 Br 2 KBr 2 x (1 K, 1 Br) = 2 K, 2 Br MgF 2 1 Mg, 2 F 3 MgF 2 3 x (1 Mg, 2 F) = 3 Mg, 6 F CaSO 4 1 Ca, 1 S, 4 O 4 CaSO 4 4 x (1 Ca, 1 S, 4 O) = 4 Ca, 4 S, 16 O Au(NO 2 ) 3 1 Au, 3 N, 6 O 5 Au(NO 2 ) 3 5 x (1 Au, 3 N, 6 O) = 5 Au, 15 N, 30 O Co(OH) 3 1 Co, 3 O, 3 H 4 Co(OH) 3 4 x (1 Co, 3 O, 3 H) = 4 Co, 12 O, 12 H Mg 3 (PO 4 ) 2 3 Mg, 2 P, 8 O 3 Mg 3 (PO 4 ) 2 3 x (3 Mg, 2 P, 8 O) = 9 Mg, 6 P, 24 O Website upload 2014 Page 30 of 55
31 Topic: Molecular Formulas Objective: How do we know what a molecular formula means in use? Molecular Formulas: A Molecular Formula gives the total number of atoms of each element needed to form the molecule. Molecules are particles formed from the covalent bonding of two or more types of nonmetal atoms. Molecular Formula examples: i. A molecule of methane has one carbon atom and four hydrogen atoms, giving methane the molecular formula of CH 4. ii. A molecule of benzene has six carbon atoms and six hydrogen atoms, giving benzene a molecular formula of C 6 H 6. Website upload 2014 Page 31 of 55
32 Topic: Empirical Formulas Objective: How do we know what an empirical formula means? Empirical Formulas: Empirical Formulas show the simplest whole-number ratio in which atoms may combine to form a compound. Empirical formulas are used to represent ionic compounds which form crystals of alternating + and - charges rather than separate molecules. Calcium chloride is ionic, and the empirical formula CaCl 2 represents a ratio of one Ca +2 cation to every two Cl -1 anions. i. If a sample of calcium chloride contains 3000 Ca +2 ions, then it must contain 6000 Cl -1 ions. ii. If a sample of calcium chloride contains 1.5 moles of Ca +2 ions, then it must contain 3.0 moles of Cl -1 ions. ALL ionic compound formulas are empirical formulas. o KCl has a 1:1 ratio, CaCl 2 has a 1:2 ratio, and Al 2 (SO 4 ) 3 has a 2:3:12 ratio. None of these may be further simplified. Molecular Compound Empirical formulas: o Certain molecular compounds such as CH 4 (1:4), NO 2 (1:2), and H 2 O (2:1) cannot be simplified further. For these molecular compounds, the molecular formula is also the empirical formula. o Other molecular compounds may have their molecular formula simplified to a new empirical formula. Website upload 2014 Page 32 of 55
33 Benzene, C 6 H 6 (6:6), may be simplified to a 1:1 ratio, giving CH as the empirical formula for benzene. Hydrogen peroxide, H 2 O 2 (2:2), may be simplified to a 1:1 ratio, giving HO as the empirical formula for hydrogen peroxide. Isobutene, C 4 H 8 (4:8), may be simplified to a 1:2 ratio, giving isobutene the empirical formula of CH 2. Website upload 2014 Page 33 of 55
34 Topic: Stoichiometry Objective: Define the process of stoichiometry in chemistry. Stoichiometry: The study of quantitative relationships as derived from chemical formulas and equations is known as stoichiometry. When working with chemical formulas, stoichiometry involves the relationships of the ratios between the numbers of moles of atoms of different compounds that comprise the various compounds. i. The mass of one mole of atoms of an element is equal to that element s atomic mass in grams. This is known as the gram atomic mass of the element. The gram atomic mass is written above left of the atomic symbol on the Periodic Table, and may be rounded to the nearest tenth of a gram for the purposes of this course. ii. The mass of one mole of molecules or formula units is equal to the sum of the gram atomic masses of the atoms that make up a mole of a particular molecule or formula unit. This number represents the gram formula mass, and is also known as just the formula mass. Website upload 2014 Page 34 of 55
35 Topic: Gram Formula Mass Objective: How do we calculate the Molar Mass of a compound? Determining the Gram Formula Mass of a Compound: You will find below some atomic symbols and information as found on the Periodic Table. Before working on the gram formula mass calculations for the examples given, we will round each gram atomic mass as given to the nearest tenth (written below each atomic symbol). KCl: (1 mole of 39.1 g/mol = 39.1 g of K) + (1 mole of 35.5 g/mol = 35.5 g of Cl) = 74.6 g/mol each mole of KCl Ca(NO 3 ) 2 : (1 mole of 40.1 g/mol = 40.1 g of Ca) + (2 moles of 14.0 g/mol each = 28.0 g of N) + (6 moles of 16.0 g/mol each = 96.0 g of O) = g/mol each mole of Ca(NO 3 ) 2 Al 2 (SO 4 ) 3 : (2 moles of 27.0 g/mol each = 54.0 g of Al) + (3 moles of 32.1 g/mol each = 96.3 g of S) + (12 moles of 16.0 g/mol each = g of O) = g/mol each mole of Al 2 (SO 4 ) 3 Website upload 2014 Page 35 of 55
36 Topic: Chemistry recipes Objective: What does chemistry and cooking have in common? Think about using a recipe to create some new food. You need to buy certain ingredients, measure them, follow directions, apply energy, and hopefully you will end up with what was in the picture! Chemistry is the same idea; we measure, follow directions, apply energy, and hopefully you will end up with what you originally planned to make. The recipe to be followed in chemistry is called a CHEMICAL REACTION. To make a triple batch of chicken wings for a party, triple the recipe ingredients. In chemistry, we can triple a reaction by tripling the reactants (ingredients). For chemistry, our recipes call for measurements in moles, but we can t measure moles. We need to measure the amount of ingredients (reactants) in grams; therefore we have a need to convert moles to grams, and also grams to moles. Website upload 2014 Page 36 of 55
37 Topic: Converting Grams to Moles Objective: How do we convert grams to moles? Determining the number of moles in a measured mass of a substance: To convert grams to moles, divide the given mass of your substance by the formula mass of that substance: given mass (g) formula mass ( g mole ) = # of moles Examples: 1. How many moles of KCl are in grams of KCl? Step #1: Find the formula mass for KCl: (1 mole of 39.1 g/mole = 39.1 g of KCl) + (1 mole of 35.5 g/mole = 35.5 g of Cl) = 74.6 g/mole of KCl Step #2: given mass (g) formula mass ( g mole ) = # of moles g of KCl / 74.6 g/mole of KCl = 2.45 moles of KCl Website upload 2014 Page 37 of 55
38 2. How many mole of Ca(NO 3 ) 2 are in 45.5 grams of Ca(NO 3 ) 2? Step #1: Find the formula mass for Ca(NO 3 ) 2 : (1 mole of 40.1 g/mole = 40.1 g of Ca) + (2 moles of 14.0 g/mole each = 28.0 g of N) + ( 6 moles of 16.0 g/mole each = 96.0 g of O) = g/mole of Ca(NO 3 ) 2 Step #2: given mass (g) formula mass ( g mole ) = # of moles 45.5 g of Ca(NO 3 ) 2 / g/mole of Ca(NO 3 ) 2 = moles of Ca(NO 3 ) 2 Website upload 2014 Page 38 of 55
39 Topic: Converting Moles to Grams Objective: How do we convert moles to grams? Determining the mass (in g) of a given number of moles of substance: To convert moles to grams, multiply the given number of moles of your substance by the formula mass for that substance: [given # of moles x formula mass (g/mole)] = mass in grams Examples: 3. What will be the mass of a 2.45 mole sample of KCl? Step #1: Find the formula mass of KCl: (1 mole of 39.1 g/mole = 39.1 g of KCl) + (1 mole of 35.5 g/mole = 35.5 g of Cl) = 74.6 g/mole of KCl Step #2: [given # of moles x formula mass (g/mole)] = mass in grams 2.45 moles of KCl x 74.6 g/mole of KCl = 183 g of KCl Website upload 2014 Page 39 of 55
40 4. What will be the mass of a mole sample of Ca(NO 3 ) 2? Step #1: Find the formula mass of Ca(NO 3 ) 2 : (1 mole of 40.1 g/mole = 40.1 g of Ca) + (2 moles of 14.0 g/mole each = 28.0 g of N) + ( 6 moles of 16.0 g/mole each = 96.0 g of O) = g/mole of Ca(NO 3 ) 2 Step #2: [given # of moles x formula mass (g/mole)] = mass in grams moles of Ca(NO 3 ) 2 x g/mole of Ca(NO 3 ) 2 = 91.0 g of Ca(NO 3 ) 2 Watch Bozeman Science Mole conversions video Website upload 2014 Page 40 of 55
41 Student name: Key Class Period: _3, 5, & 10_ Please carefully remove this page from your packet to hand in. Formula Mass homework (1 pt ea.) Determine the number of moles of an element in one mole of these compounds: Formula Number of moles: Number of moles: Number of moles (if any): CaBr 2 Ca: 1 Br: 2 XXXXXXXXXXXXXXXXX K 2 SO 4 K: 2 S: 1 O: 4 SO 3 S: 1 O: 3 XXXXXXXXXXXXXXXXX CH 3 COOH C: 2 H: 4 O: 2 Determine the total number of moles of atoms in the following formulas: Formula Total # of moles of atoms Formula Total # of moles of atoms Formula Total # of moles of atoms NaCl 2 2 NaNO K 2 Cr 2 O 7 33 Calculate the formula masses in g/mole for the compounds listed below. Determine the gram atomic masses to the nearest tenth. Formula Work space (Show ALL work!) Gram Formula Mass Na 2 SO 4 (2 x 23.0)+(1 x 32.1)+(4 x 16.0) = g/mol NaOH (1 x 23.0)+(1 x 16.0)+(1 x 1.0) = 40. g/mol H 2 O (2 x 1.0)+(1 x 16.0) = 18. g/mol C 6 H 12 O 6 (6 x 12.0)+(12 x 1.0)+(6 x 16.0) = 180. g/mol N 2 O 4 (2 x 14.0)+(4 x 16.0) = 92.0 g/mol Ba(NO 3 ) 2 (1 x 137.3)+(2 x 14.0)+(6 x 16.0) = g/mol C 2 H 6 (2 x 12.0)+(6 x 1.0) = 30. g/mol Website upload 2014 Page 41 of 55
42 Identify each of the following formulas as either empirical or molecular. If it is a molecular formula, write the simplified empirical formula. Formula Empirical or Molecular? Simplified Empirical Formula Empirical or Molecular? Simplified Empirical C 2 H 6 M CH 3 N 2 O 4 M NO 2 Ba(NO 3 ) 2 E C 6 H 12 O 6 M CH 2 O Determine how many moles of each substance is represented by the given mass. Mass and formula Work space (Show ALL work!) Moles 36. g of H 2 O 36 g H 2 O x 1mol H 2 O / 18.0 g/mol of H 2 O = g of NaOH 60. g NaOH x 1 mol NaOH / 40.0 g/mol of NaOH = g of Na 2 SO 4 71 g Na 2 SO 4 x 1 mol Na 2 SO 4 / g mol of Na 2 SO 4 = Website upload 2014 Page 42 of 55
43 Topic: Percent Composition Objective: How do we find the percentage of each element? Percent Composition: The Percent Composition of a compound is the proportion by mass of all the elements that are in a compound. Determination of Percent Composition: Qualitative analysis tells us WHAT elements are in a compound, but we need quantitative analysis to determine how much of each element is in a compound. One of the ways this is accomplished is to weigh a sample of the compound, then take the compound and decompose it into its individual elements. After decomposition, weigh each element alone and then calculate what percent by mass each element was of the whole compound. Watch Percent Mass, Composition, Empirical Formulas & Molecular Formulas video Website upload 2014 Page 43 of 55
44 Experimental Determination of Percent Composition: given mass of an element in a sample given mass of the total sample x 100 Example: A sample of compound containing only nitrogen and oxygen has a mass of 80.0 grams. Experiments show that the sample is made up of 56.0 grams of oxygen and 24.0 grams of nitrogen. What is the percent composition by mass of each element in the compound? o Percent of oxygen: (56.0 g of O/80.0 g of sample) x 100 = 70.0% O o Percent of nitrogen: (24.0g of N/80.0 g of sample) x 100 = 30.0% N Determination by given formula (need periodic table): given mass of an element in a sample given mass of the total sample x 100 Examples: 1. What is the percent composition by mass of the elements in SiO 2? Formula mass of SiO 2 : ( g/mole) + ( g/mole) = 60.1 g/mole of SiO 2 o Percent of Si: (28.1/60.1) x 100 = 46.8% Si in SiO 2 o Percent of O: (32.0/60.1) x 100 = 53.2% O in SiO 2 Website upload 2014 Page 44 of 55
45 2. What is the percent composition by mass of the elements in H 2 O? Formula mass of H 2 O: (2 1.0 g/mole) + ( g/mole) = 18.0 g/mole of H 2 O o Percent of H: (2.0/18.0) x 100 = 11% H in H 2 O o Percent of O: (16.0/18.0) x 100 = 88.9% O in H 2 O 3. What is the percent composition by mass of each element in H 2 SO 4? Formula mass of H 2 SO 4 : (2 1.0 g/mole) + ( g/mole) + ( g/mole) = 98.1 g/mole of H 2 SO 4 o Percent of H: (2.0/98.1) x 100 = 2.0% H in H 2 SO 4 o Percent of S: (32.1/98.1) x 100 = 32.7% S in H 2 SO 4 o Percent of O: (64.0/98.1) x 100 = 65.2% O in H 2 SO 4 Website upload 2014 Page 45 of 55
46 Topic: Hydrated Compounds Objective: What is a hydrate, and how does it affect chemistry? Hydrates: i. A hydrate is an ionic solid crystal that has water trapped within the crystalline structure. Different hydrates may have differing amounts of water within the crystal structure. ii. A hydrate is represented by n H 2 0, where the n is the number of water molecules within each hydrate crystal. iii. The water molecules are not a part of the compound; the water molecule(s) are trapped between the crystals ions. iv. The water molecules within the hydrate may be removed by heating, leaving the anhydrous salt behind. Hydrate examples: 5 water molecules locked in 10 water molecules locked in 7 water molecules locked in 2 water molecules locked in 2 water molecules locked in Watch Hydrates video Website upload 2014 Page 46 of 55
47 Topic: Hydrate Percentage Objective: How may we determine the ratio of water in a hydrate? Determining the Percentage of Water in a Hydrate Experimentally: given mass of the water in a hydrate compound given mass of the hydrate compound x 100 i. To determine the mass of water that was removed from the hydrate: a. Subtract the mass of the (dried) anhydride from the original hydrate sample mass. ii. To determine the percent of water in the original hydrate sample: a. Take the mass of removed water (found above) and divide it by the Example: original hydrate sample mass and multiply by 100. A gram sample of hydrate crystal is heated to an anhydride with a final mass of 8.72 grams. (Assumption is that ALL water has been lost) 1. Calculate the mass of water removed from the original hydrate sample. (mass of sample - mass of anhydride) = g g = 1.68 g H 2 O lost 2. Calculate the percent by mass of the water in the hydrate sample. (mass of H 2 O lost / mass of hydrate) x 100 = (1.68 g/10.40 g) x 100 = 16.2% water by mass Website upload 2014 Page 47 of 55
48 Determining the Percentage of Water in a Hydrate using the formula: formula mass of the water in a hydrate compound formula mass of the hydrate compound x 100 Formula mass of H 2 O: (2 1.0 g/mole) + ( g/mole) = 18.0 g/mole of H 2 O o If the hydrate coefficient (n) is 2, then (2 x 18.0 g/mole) = 36.0 g/mole H 2 O in the hydrate o If the hydrate coefficient (n) is 4, then (4 x 18.0 g/mole) = 72.0 g/mole H 2 O in the hydrate To determine the formula mass of the hydrate: 1. Find the formula mass of the crystal; 2. Find the formula mass of the number of moles (n) in the hydrate; 3. Add the two numbers together. 4. To determine the percentage of water in the hydrate: 5. Divide the formula mass of the water in the hydrate by the total formula mass and multiply by 100. Website upload 2014 Page 48 of 55
49 Examples: 1. What is the percent composition by mass of each element in CuCO 3 2 H 2 O? Note that the 2 H 2 O means this is a hydrate, in this case containing 2 molecules of water. i. Find the formula mass for CuCO 3 2 H 2 O: ( g/mole) + ( g/mole) + ( g/mole) + (4 1.0 g/mole) = g/mole CuCO 3 2 H 2 O Note the three O in the crystal, and a total of two O in the hydrate. Note also the hydrate has a total of four H (2 x 2). % Cu: (63.5 g/mole Cu / g/mole CuCO 3 2 H 2 O) x 100 = 39.8% Cu % O: (80.0 g/mole O / g/mole CuCO 3 2 H 2 O) x 100 = 50.2% O % C: (12.0 / g/mole CuCO 3 2 H 2 O) x 100 = 7.52% C % H: (4.0 / g/mole CuCO 3 2 H 2 O) x 100 = 2.5% H 2. What is the percent composition by mass of only the water in CuCO 3 2 H 2 O? i. Formula mass of H 2 O: (2 1.0 g/mole) + ( g/mole) = 18.0 g/mole of H 2 O ii. Find the formula mass for CuCO 3 2 H 2 O: ( g/mole) + ( g/mole) + ( g/mole) + (4 1.0 g/mole) = g/mole CuCO 3 2 H 2 O % H2O: (18.0 g/mole H 2 O / g/mole CuCO 3 2 H 2 O) x 100 = 22.6% H 2 O in CuCO 3 2 H 2 O Website upload 2014 Page 49 of 55
50 Topic: Molecular Formulas Objective: How do we calculate a molecular formula? A molecular formula shows the true number of atoms of each element in a chemical formula. An empirical formula only states the ratio of the different types of elements in a chemical formula. If we have the empirical formula and a molecular mass we can calculate the molecular formula. To determine the molecular formula of a compound given the molecular mass and empirical formula: i. Determine the formula mass of the empirical formula; ii. Divide the molecular mass by the empirical mass to give a wholenumber multiple; iii. Multiply the whole number above by the empirical formula. Website upload 2014 Page 50 of 55
51 Example: 1. What is the molecular formula of a compound with an empirical formula of C 2 H 3 and a molecular mass of 54.0 g/mole? i. Determine the formula mass of the empirical formula: C 2 H 3 : ( g/mole) + (3 g/mole) = 27.0 g/mole C 2 H 3 ii. Divide the molecular mass by the empirical mass, giving the wholenumber multiple: (54.0 g/mole) / (27.0 g/mole) = 2 The 2 means the molecular formula is TWICE the empirical formula iii. Multiply the calculated whole-number multiple by the empirical formula: 2 x C 2 H 3 = C 4 H 6 The molecular formula for the compound in this problem is C 4 H 6 Website upload 2014 Page 51 of 55
52 Notes page: Website upload 2014 Page 52 of 55
53 Student name: Key Class Period: _3, 5, & 10_ Please carefully remove this page from your packet to hand in. Percent Composition and Formulas homework Determine the percentage by mass of each element in the following compounds. Show ALL work, and make sure that your answers are properly rounded. (3 pts each) CO: % C = _42.9%_ % O = _57.1%_ 42.9% % = 100% C = 12.0 g/mol O = 16.0 g/mol % C = (12.0 g/mol of C) / (28.0 g/mol of CO) x 100 = 42.9% C in CO % O = (16.0 g/mol of O) / (28.0 g/mol of CO) x 100 = 57.1% O in CO CO = (12.0 g/mol of C) + (16.0 g/mol of O) = 28.0 g/mol of CO (NH 4 ) 2 SO 3 : % N = 24.1% % O = 41.3% % S = 27.6% % H = 6.9% N = 14.0 g/mol % N = (28.0 g of N) / {116.1 g/mol of (NH 4 ) 2 SO 3 } x 100 = 24.1% N in (NH 4 ) 2 SO 3 O = 16.0 g/mol % O = (48.0 g of O) / {116.1 g/mol of (NH 4 ) 2 SO 3 } x 100 = 41.3% O in (NH 4 ) 2 SO 3 H = 1.0 g/mol % H = (8.0 g of H) / {116.1 g/mol of (NH 4 ) 2 SO 3 } x 100 = 6.9% H in (NH 4 ) 2 SO 3 S = 32.1 g/mol % S = (32.1 g of S) / {116.1 g/mol of (NH 4 ) 2 SO 3 } x 100 = 27.6% S in (NH 4 ) 2 SO 3 (NH 4 ) 2 SO 3 = 2 x { (4 x 1.0)} (3 x 16.0) = g/mol of (NH 4 ) 2 SO 3 CuSO 4 5 H 2 O : % Cu = 25.4% % O = 57.7% % S = 12.9% % H = 4.0% O = 16.0 g/mol H = 1.0 g/mol S = 32.1 g/mol Cu = 63.5 g/mol % O = (144.0 g of O) / (249.6 g/mol of CuSO 4 5 H 2O) x 100 = 57.7% O in CuSO 4 5 H 2O % H = (10.0 g of H) / (249.6 g/mol of CuSO 4 5 H 2O) x 100 = 4.0 % H in CuSO 4 5 H 2O % S = (32.1 g/mol of S) / (249.6 g/mol of CuSO 4 5 H 2O) x 100 = 12.9 % S in CuSO 4 5 H 2O % Cu = (63.5 g/mol of Cu) / (249.6 g/mol of CuSO4 5 H2O) x 100 = 25.4 % Cu in CuSO4 5 H2O CuSO 4 5 H 2O = (63.5) + (32.1) + (9 x 16.0) + (10 x 1.0) = g/mol of CuSO 4 5 H 2O Cont d next page Website upload 2014 Page 53 of 55
54 Determine the percent by mass of water in the hydrate below. Show ALL work, and correct labels. (3 pts) Formula mass of H 2 O: (2 x 1.0 g/mol of H) g/mol of O = 18.0 g/mol for H 2 O Formula mass of CuSO 4 5 H 2 O: g/mol of CuSO 4 5 H 2 O Formula mass of _5_ H 2 O: (5 x 18.0 g/mol H 2 0) = 90.0 g of H 2 O / mol of CuSO 4 5 H 2 O Calculate the % of water in CuSO 4 5 H 2 O: (90.0 g/mol of H 2 O in CuSO 4 5 H 2 O) / (249.6 g/mol of CuSO 4 5 H 2 O) x 100 = 36.1% H 2 O in CuSO 4 5 H 2 O Determine the molecular formulas for each question below. Show ALL work. (3 pts ea.) 1. The empirical formula of a compound is found to be CH, and the molecular mass is determined to be 78.0 g/mole. Write the molecular formula for this compound. CH = (12.0 g/mole of C) + (1.0 g/mol of H) = 13.0 g/mol for CH (78.0 g/mol molecular mass) / (13.0 g/mol for CH) = 6 (6 x 1 C) + (6 x 1 H) = C 6 H 6 molecular formula 2. The empirical formula of a compound is found to be CH 2 O, and the molecular mass is determined to be g/mole. Write the molecular formula for this compound. CH 2 O = (12.0 g/mole of C) + (2 x 1.0 g/mol of H) + (16.0 g/mol of O) = 30. g/mol for CH 2 O (180.0 g/mol molecular mass) / (30. g/mol for CH 2 O) = 6 (6 x 1 C) + (6 x 2 C) + (6 x 1 O) = C 6 H 12 O 6 Website upload 2014 Page 54 of 55
55 Notes page: Website upload 2014 Page 55 of 55
Compounds. A molecule with asymmetrical electron distribution resulting in partially
Compounds Word Binary compound Dipole attractions Dipole moment Electronegativity difference Electrical conductivity (metals) Electrolyte Empirical formula mass Hydrogen bonds Intermolecular Attractive
More informationMonatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on
More informationCHAPTER 5: MOLECULES AND COMPOUNDS
CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting
More informationStudy Guide For Chapter 7
Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance
More informationChapter 4 Compounds and Their Bonds
Chapter 4 Compounds and Their Bonds 4.1 Octet Rule and Ions Octet Rule An octet is 8 valence electrons. is associated with the stability of the noble gases. He is stable with 2 valence electrons (duet).
More informationTopic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
More informationMoles, Molecules, and Grams Worksheet Answer Key
Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3
More informationNomenclature of Ionic Compounds
Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.
More informationElements and Compounds. Chemical Bonds compounds are made of atoms held together by chemical bonds bonds are forces of attraction between atoms
Elements and Compounds elements combine together to make an almost limitless number of compounds the properties of the compound are totally different from the constituent elements Tro, Chemistry: A Molecular
More informationCHEMICAL NAMES AND FORMULAS
9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages 253 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the
More informationBalancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
More information19.2 Chemical Formulas
In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula
More informationChapter 5. Chapter 5. Naming Ionic Compounds. Objectives. Chapter 5. Chapter 5
Objectives Name cations, anions, and ionic compounds. Write chemical formulas for ionic compounds such that an overall neutral charge is maintained. Explain how polyatomic ions and their salts are named
More informationName: Block: Date: Test Review: Chapter 8 Ionic Bonding
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fill-in-the-blank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity
More informationWRITING CHEMICAL FORMULA
WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.
More informationPolyatomic ions can form ionic compounds just as monatomic ions.
1 POLYATOMIC IONS We have seen that atoms can lose or gain electrons to become ions. Groups of atoms can also become ions. These groups of atoms are called polyatomic ions. Examples: O hydroxide ion NO
More informationExam 2 Chemistry 65 Summer 2015. Score:
Name: Exam 2 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of
More informationPART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
More informationChapter 8 How to Do Chemical Calculations
Chapter 8 How to Do Chemical Calculations Chemistry is both a qualitative and a quantitative science. In the laboratory, it is important to be able to measure quantities of chemical substances and, as
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationChapter 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
More informationChapter 1: Moles and equations. Learning outcomes. you should be able to:
Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including
More informationNAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide
NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationTutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE
T-6 Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE FORMULAS: A chemical formula shows the elemental composition of a substance: the chemical symbols show what elements are present and the numerical
More informationProblem Solving. Percentage Composition
Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine
More information(b) Formation of calcium chloride:
Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. An ionic compound combines a metal and a non-metal joined together by an ionic bond. 2. An electrostatic force holds
More informationChapter 3. Molecules, Compounds and Chemical Equations
3. Molecules, Compounds and Chemical Equations Stoichiometry Mole concept and Avogadro s Number Determining Chemical Formulas Name Compound Balancing Chemical Reactions Yields Solutions and Stoichiometry
More informationStoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
More informationCHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals
CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying
More informationW1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
More informationChapter 3 Stoichiometry
Chapter 3 Stoichiometry 3-1 Chapter 3 Stoichiometry In This Chapter As you have learned in previous chapters, much of chemistry involves using macroscopic measurements to deduce what happens between atoms
More informationCHEMICAL NAMES AND FORMULAS
6 CEMICAL NAMES AND FORMULAS SECTION 6.1 INTRODUCTION TO CEMICAL BONDING (pages 133 137) This section explains how to distinguish between ionic and molecular compounds. It also defines cation and anion
More informationStoichiometry. What is the atomic mass for carbon? For zinc?
Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon-12
More informationFormulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
More informationMolar Mass Worksheet Answer Key
Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol
More informationMOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
More informationSample Exercise 2.1 Illustrating the Size of an Atom
Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationPERIODIC TABLE OF THE ELEMENTS
PERIODIC TABLE OF THE ELEMENTS Periodic Table: an arrangement of elements in horizontal rows (Periods) and vertical columns (Groups) exhibits periodic repetition of properties First Periodic Table: discovered
More informationNaming and Writing Formulas for Ionic Compounds Using IUPAC Rules
Naming and Writing Formulas for Ionic Compounds Using IUPAC Rules There are three categories of ionic compounds that we will deal with. 1.Binary ionic o simple ions (only single charges) o multivalent
More informationNaming Ionic Compounds
Naming Ionic Compounds I. Naming Ions A. Cations (+ions) 1. Element name followed by "ion" (when in Group IA, IIA, Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag +, Ni 2+ ). Na + sodium ion, K + potassium ion, Al 3+ aluminum
More informationNomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula
Purpose: Theory: Nomenclature and Formulas of Ionic Compounds 1. To become familiar with the rules of chemical nomenclature, based on the classification of compounds. 2. To write the proper name of the
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
More informationChapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
More informationUnit 9 Stoichiometry Notes (The Mole Continues)
Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationCalculating Atoms, Ions, or Molecules Using Moles
TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary
More informationUnit 4 Conservation of Mass and Stoichiometry
9.1 Naming Ions I. Monatomic Ions A. Monatomic ions 1. Ions formed from a single atom Unit 4 Conservation of Mass and Stoichiometry B. Naming Monatomic Ions 1. Monatomic cations are a. Identified by the
More informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More informationExercise 3.5 - Naming Binary Covalent Compounds:
Chapter Exercise Key 1 Chapter Exercise Key Exercise.1 Classifying Compounds: Classify each of the following substances as either a molecular compound or an ionic compound. a. formaldehyde, CH 2 O (used
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationMOLECULAR MASS AND FORMULA MASS
1 MOLECULAR MASS AND FORMULA MASS Molecular mass = sum of the atomic weights of all atoms in the molecule. Formula mass = sum of the atomic weights of all atoms in the formula unit. 2 MOLECULAR MASS AND
More informationH 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.
CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,
More informationMolecules, Compounds, and Chemical Equations (Chapter 3)
Molecules, Compounds, and Chemical Equations (Chapter 3) Chemical Compounds 1. Classification of Elements and Compounds Types of Pure Substances (Figure 3.4) Elements -- made up of only one type of atom
More informationUnit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?
More informationb. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.
CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationChemistry Final Study Guide
Name: Class: Date: Chemistry Final Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The electrons involved in the formation of a covalent bond
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
More informationChemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
More informationNaming Compounds Handout Key
Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion
More informationChapter 6 Notes Science 10 Name:
6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and
More informationChapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c.
More informationHOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
More informationChapter 9 Practice Test - Naming and Writing Chemical Formulas
Chapter 9 Practice Test - Naming and Writing Chemical Formulas Matching Match each itme with the correct statement below. Match each item with the correct statement below. a. monatomic ion f. cation b.
More informationStoichiometry. Unit Outline
3 Stoichiometry Unit Outline 3.1 The Mole and Molar Mass 3.2 Stoichiometry and Compound Formulas 3.3 Stoichiometry and Chemical Reactions 3.4 Stoichiometry and Limiting Reactants 3.5 Chemical Analysis
More informationTOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.
TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually
More informationstoichiometry = the numerical relationships between chemical amounts in a reaction.
1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse
More informationOther Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :
Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
More informationChapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
More informationDavid A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationMole Calculations Multiple Choice Review PSI Chemistry
Mole Calculations Multiple Choice Review PSI Chemistry Name The Mole and Avogadro's Number 1)What is the SI unit for measurement of number of particles in a substance? A) kilogram B) ampere C) candela
More informationNomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride
Nomenclature Packet Worksheet I: Binary Ionic Compounds (representative metals) metals from groups 1A, 2A, and 3A (1, 2, and 13) have constant charges as ions and do NOT get Roman Numerals in their names
More informationChemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.
1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.
More informationCHAPTER 3 Calculations with Chemical Formulas and Equations. atoms in a FORMULA UNIT
CHAPTER 3 Calculations with Chemical Formulas and Equations MOLECULAR WEIGHT (M. W.) Sum of the Atomic Weights of all atoms in a MOLECULE of a substance. FORMULA WEIGHT (F. W.) Sum of the atomic Weights
More informationDescription of the Mole Concept:
Description of the Mole Concept: Suppose you were sent into the store to buy 36 eggs. When you picked them up you would get 3 boxes, each containing 12 eggs. You just used a mathematical device, called
More informationRules for Naming and Writing Compounds
Rules for Naming and Writing Compounds I. Ionic Bonds bonding between a metal and nonmetal or the bond between a positive ion and a negative ion forming a binary compound. end in the suffix "ide" Or bonding
More informationExperiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
More informationEnglish already has many collective nouns for fixed, given numbers of objects. Some of the more common collective nouns are shown in Table 7.1.
96 Chapter 7: Calculations with Chemical Formulas and Chemical Reactions Chemical reactions are written showing a few individual atoms or molecules reacting to form a few atoms or molecules of products.
More informationThe Mole Concept and Atoms
Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 4 24 September 2013 Calculations and the Chemical Equation The Mole Concept and Atoms Atoms are exceedingly
More informationCHEMICAL NOMENCLATURE
CHEMICAL NOMENCLATURE Chemical nomenclature The process of giving unambiguous chemical formulas or chemical names to elements and compounds Introduction Chemistry is the study of matter (elements and compounds)
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More informationMole Notes.notebook. October 29, 2014
1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the
More informationCHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS
CHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS 1. THE MEANING OF A CHEMICAL FORMULA A chemical formula is a shorthand method of representing the elements in a compound. The formula shows the formulas
More informationNomenclature and the Periodic Table To name compounds and to determine molecular formulae from names a knowledge of the periodic table is helpful.
Nomenclature and the Periodic Table To name compounds and to determine molecular formulae from names a knowledge of the periodic table is helpful. Atomic Number = number of protons Mass Number = number
More informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationChemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
More informationNumber of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V
44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts
More informationChapter 12: Oxidation and Reduction.
207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following
More informationIn the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
More informationQuestion Bank Electrolysis
Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationChemical Proportions in Compounds
Chapter 6 Chemical Proportions in Compounds Solutions for Practice Problems Student Textbook page 201 1. Problem A sample of a compound is analyzed and found to contain 0.90 g of calcium and 1.60 g of
More informationNET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:
NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More informationConcept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.
Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of
More information