Naming Compounds Aim: To understand why it is necessary to have a system for naming compounds
|
|
|
- Nelson Warren
- 7 years ago
- Views:
Transcription
1 Naming Compounds Aim: To understand why it is necessary to have a system for naming compounds Binary compounds- Compounds composed of two elements Two classes o Compounds that contain metals and nonmetals o Compounds that contain two metals Naming Compounds that Contain a Metal and Nonmetals Aim: To learn to name binary compounds of a metal and nonmetal Metals lose electrons to become cations Nonmetals gain electrons to become an anion Metal + Nonmetal = Binary Ionic Compound (+) (-) Type I compounds-metals that form ONLY one type of cation Type II compounds- Metals that can form two or more cations that have different charges Rules for naming Type I Compounds 1. The cation is always named first and the anion second 2. A simple cation (obtained from a single atom) takes its name from the name of the element. Ex. Na + is called sodium in the names of compounds containing this ion. 3. A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding ide. Thus Cl - ion is called chloride Noble gases are the least reactive; therefore they do not form compounds Octet rule-in most chemical reactions, atoms tend to match the s and p electron configuration of noble gases. The atoms want to have their p orbital filled. Type I Group 1 Group 2 Group 3 Charge Most reactive Most reactive When you form ionic compounds there is no net charge- Na + Cl - = NaCl Charge (+1) (-1) = 0 Sodium Chloride Al 3+ I - = AlI 3 Charge (+3) 3(-1) = 0 Aluminum iodide Remember to switch your charges and place as subscripts when you write your ionic compounds Nonmetals Group 15 Group 16 Group 17 Charge Common Simple Cations and Anions Cations Name Anion Name H +1 Hydrogen H -1 hydride Li +1 Lithium F -1 fluoride Na +1 Sodium Cl -1 chloride K +1 Potassium Br -1 bromide Cs +1 Cesium I -1 iodide Be 2+ Beryllium O 2- oxide Mg 2+ Magnesium S 2- sulfide Ca 2+ Calcium Ba 2+ Barium Al 3+ Aluminum Ag +1 Silver Zn 2+ zinc
2 Type II Ionic Compounds Type II Ions o Transition Metals and some other Metals o Typically they have several different ionic charges because electrons in d orbitals are very close in energy to the s and p valence electrons. As a result, these d electrons sometimes participate in ion formation. Some Common Type II Cations Ion Systematic Name Older Name Fe 3+ Iron (III) ferric Fe 2+ Iron (II) ferrous Cu 2+ Copper (II) cupric Cu +1 Copper (I) cuprous Co 3+ Cobalt (III) colbaltic Co 2+ Cobalt (II) cobaltous Sn 4+ Tin (IV) stannic Sn 2+ Tin (II) stannous Pb 4+ Lead (IV) plumbic Pb 2+ Lead (II) plumbous Hg 2+ Mercury (II) mercuric 2+ Hg 2 Mercury (I) mercurous 2+ Mercury (I) ions always occur bonded together in pairs to form Hg 2 Rules for Naming Type II Ionic Compounds 1. The cation is always named first and then the anion. 2. Because the cation can assume more than one charge, the charge is specified by a roman numeral in parentheses. What is the charge on the lead ion? Use the principle of charge balance to determine the cation charge. PbO 2 Remember Oxygen has a charge of -2. (?) 2(-2) = (-2) = 0 Naming Binary Compounds that contain only Nonmetals (Type III) Aim: To learn how to name binary compounds containing only nonmetals Rules for naming Type III binary compounds 1. The first element in the formula is named first, and the full element name is used. 2. The second element is named as though it were an anion. 3. Prefixes are used to denote the numbers of atoms present. 4. The prefix mono- is never used for naming the first element. Ex. CO is called carbon monoxide not monocarbon monoxide. Prefixes used to indicate numbers in chemical names Prefix mono- di- tri- tetra- penta- hexa- hepta octa- nona- deca- Number indicated NO nitrogen monoxide or N 2 O 5 dinitrogen pentoxide For easier pronunciation we often drop the o or a of the prefix when the second element is oxygen.
3 Chemistry: Binary Compounds List the oxidation numbers (charges) for each of the following elements. Ca 2+ N 3- Br 1- Be 2+ Ba 2+ Fr 1- K 1+ P 3- Al 3+ Group 1 1+ Group 2 2+ Group Group Group Group Zn 2+ Ag 1+ Fe (III) 3+ Write the formulas for the following binary compounds. calcium oxide beryllium chloride iron (II) oxide CaO BeCl 2 FeO sodium fluoride potassium iodide copper (I) chloride NaF KI CuCl copper (II) chloride aluminum chloride lead (IV) nitride CuCl 2 AlCl 3 Pb 3 N 4 iron (III) oxide strontium oxide lead (II) nitride Fe 2 O 3 SrO Pb 3 N 2 Write the names of the following binary compounds. Cr 2 O 3 chromium (III) oxide NaBr sodium bromide PbI 2 lead (II) iodide HCl hydrogen chloride Al 2 O 3 aluminum oxide BN boron nitride RbI rubidium iodide BaF 2 barium fluoride H 2 S hydrogen sulfide NaCl sodium chloride
4 Chemistry: Ionic Binary Compounds: Single-Charge Cations Write the name of each of the following compounds. 1. Na 2 S 1. sodium sulfide 2. Al 2 O 3 2. aluminum oxide 3. NaCl 3. sodium chloride 4. RbI 4. rubidium iodide 5. ZnBr 2 5. zinc bromide 6. AgCl 6. silver chloride 7. BN 7. boron nitride 8. BaF 2 8. barium fluoride 9. Sr 3 N 2 9. strontium nitride_ 10. MgCl magnesium chloride Write the chemical formula for each of the given names. 11. magnesium nitride 11. Mg 3 N calcium oxide 12. CaO 13. silver fluoride 13. AgF 14. beryllium chloride 14. BeCl potassium iodide 15. KI 16. aluminum chloride 16. AlCl zinc oxide 17. ZnO 18. barium bromide 18. BaBr lithium nitride 19. Li 3 N 20. potassium sulfide 20. K 2 S
5 Chemistry: Ionic Binary Compounds: Multiple-Charge Cations Write the name of each of the following compounds. 1. CuF 1. copper (I) fluoride 2. CuF 2 2. copper (II) fluoride 3. Cr 2 O 3 3. Chromium (III) oxide 4. PbI 2 4. lead (II) iodide 5. PbCl 4 5. lead (IV) chloride 6. CrO 3 6. chromium (VI) oxide_ 7. AuBr 7. gold (I) bromide 8. NiO 8. nickel (II) oxide 9. VI 3 9. vanadium (III) iodide 10. SnO _tin (IV) oxide Write the chemical formula for each of the given names. 11. manganese (VII) oxide 11. Mn 2 O niobium (V) chloride 12. NbCl titanium (III) phosphide 13. TiP 14. palladium (IV) sulfide 14. PdS platinum (II) fluoride 15. PtF osmium (III) oxide 16. Os 2 O iridium (IV) nitride 17. Ir 3 N cobalt (II) chloride 18. CoCl iron (III) sulfide 19. Fe 2 S gold (III) iodide 20. AuI 3
6 Chemistry: Oxidation Numbers and Ionic Compounds Write the correct formula for the compound formed by each of the following pairs of ions. 1. Na 1+ F 1-1. NaF 2. K 1+ S 2- EXAMPLE 2. K 2 S 3. Ni 2+ SO NiSO 4 4. Al 3+ O 2-4. Al 2 O 3 5. Ca 2+ ClO Ca(ClO 3 ) 2 6. NH 4 1+ P 3-6. (NH 4 ) 3 P 7. Cu 1+ NO Cu 2+ NO _CuNO 3 8. Cu(NO 3 ) 2 9. Pb 4+ O 2-9. PbO Li 1+ CO Li 2 CO 3 For each of the following compounds, write A) the symbols of the ions in the compound, B) the number of each ion in one molecule of that compound and C) the name of the compound. 11. CaI 2 Example 11. one Ca 2+ and two I 1- Calcium Iodide 12. Na 2 CO two Na + and one CO 3 2- sodium carbonate 13. Ga(ClO 3 ) one Ga 3+ and three ClO 3 1- gallium chlorate 14. CuF one Cu 2+ and two F - copper(ii) fluoride 15. (NH 4 ) 3 PO three NH 4 1+ and one PO 4 3- ammonium phosphate 16. FeSO one Fe 2+ and one SO 4 2- iron(ii) sulfate 17. Mg(NO 3 ) one Mg 2+ and two NO 3 1- magnesium nitrate 18. NH 4 NO one NH 4 1+ and one NO 2 1- ammonium nitrite 19. KC 2 H 3 O one K + and one C 2 H 3 O 2 1- potassium acetate 20. Na 2 Cr 2 O two Na + and one Cr 2 O 7 2- sodium dichromate
7 Chemistry: Covalent Binary Compounds: Nonmetal Nonmetal Combinations Write the name of each of the following compounds. 1. HF 1. hydrogen monofluoride 2. H 2 S 2. dihydrogen monosulfide 3. NO 3. nitrogen monoxide 4. N 2 O 4. dinitrogen monoxide 5. NO 2 5. nitrogen dioxide 6. N 2 O 5 6. dinitrogen pentoxide 7. SO 2 7. sulfur dioxide 8. CBr 4 8. carbon tetrabromide 9. C 2 H 6 9. dicarbon hexahydride (ethane) 10. C 4 H tetra carbon decahydride (butane) Write the chemical formula for each of the given names. 11. nitrogen triiodide 11. NI dinitrogen tetroxide 12. N 2 O sulfur trioxide 13. SO carbon monoxide 14. CO 15. dihydrogen monoxide 15. H 2 O 16. hydrogen monobromide 16. HBr 17. phosphorus trichloride 17. PCl tricarbon octahydride 18. C 3 H 8 (propane) 19. carbon tetrahydride 19. CH 4 (methane)_ 20. dicarbon tetrahydride 20. C 2 H 4 (ethane)_
8 Chemistry: Errors in Chemical Formulas and Nomenclature Each of the following formulas or chemical names contains an error. Correct each example. 1. aluminum (III) iodide 1. aluminum iodide AlI 3 2. Al 3 O 2 2. Al 2 O 3 aluminum oxide 3. (NH 4 ) 3 Cl 2 3. NH 4 Cl ammonium chloride 4. lead (III) oxide 4. lead (II) or (IV) oxide PbO or PbO 2 5. leadic oxide 5. lead (IV) oxide PbO 2 6. stannous (II) bromide 6. tin (II) bromide SnBr 2 7. monocalcium dioxide 7. calcium oxide CaO 8. K(ClO 2 ) 8. KClO 2 Potassium chlorite 9. (OH) 3 Al 9. Al(OH) 3 aluminum hydroxide 10. Cr 4 (CN) Cr(CN) 4 chromium (IV) cyanide 11. Pb(NO 3 ) Pb(NO 3 ) 4 Lead (IV) nitrate 12. copper (I) chloric 12. copper (I) chloride CuCl 13. ferric (III) oxide 13. iron (III)oxide Fe2O3 14. NiNO Ni(NO 3 ) 2 Nickel (II) nitrate 15. Mg 2 F 15. MgF 2 magnesium fluoride 16. ironic oxide 16. iron (III) oxide Fe 2 O ClK 17. KCl potassium chloride 18. Ca 2 O CaO calcium oxide 19. sodium (I) fluoride 19. sodium fluoride NaF 20. dititanium tetroxide 20. titanium (IV) oxide TiO dihydrogen oxide 21. dihydrogen monoxide H 2 O 22. magnesium dihydroxide 22. magnesium hydroxide Mg(OH) cuprous (I) sulfate 23. copper (I) sulfate Cu 2 SO strontium difluoride 24. strontium fluoride SrF NO 3 Na 25. NaNO 3 sodium nitrate
Monatomic 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
Name: 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
Nomenclature 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
Naming 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
Nomenclature 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.
CHAPTER 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
PERIODIC 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
Chapter 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).
CHAPTER 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
Polyatomic 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
Naming 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
Elements 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
CHEMICAL 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
Nomenclature 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
Naming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound.
Naming Compounds Naming compounds is an important part of chemistry. Most compounds fall in to one of three categories ionic compounds, molecular compounds, or acids. Part One: Naming Ionic Compounds Identifying
Moles, 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
19.2 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
NAMING 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
Decomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
Oxidation States of Nitrogen
Oxidation States of Nitrogen HNO 3 NH 3 HNO 2 NO N 2 O N 2 HN 3 N 2 H 5 + +3 +2 +1 0-1/3-2 Oxidation +5-3 Reduction Oxidation States of Chlorine HClO 4 HClO 3 ClO 2 HClO 2 HClO Cl 2 HCl +5 +4 +3 +1 0 Oxidation
Balancing 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.
Rules 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
David 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,
Naming Ionic Compounds Answer Key
Naming Ionic Compounds Answer Key Give the name of the following ionic compounds: Name 1) Na 2 CO 3 sodium carbonate 2) NaOH sodium hydroxide 3) MgBr 2 magnesium bromide 4) KCl potassium chloride 5) FeCl
Nomenclature 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
Periodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
Topic 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
Sample 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
Naming 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
FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31.
FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31. TYPES OF COMPOUNDS Ionic compounds are compounds composed of
Chapter 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
WRITING 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.
Chemistry 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
Chapter 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
= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
Chapter 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
SCH 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
Unit 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
Chapter 3 Chemical Compounds
Chapter 3 Chemical Compounds 3.1 (a) formula unit; (b) strong electrolyte; (c) molecular compound; (d) acid; (e) nonelectrolyte; (f) oxoanion 3.2 (a) molecular formula; (b) weak electrolyte; (c) ionic
Molar 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
Exercise 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
Polyatomic Ions Worksheet. 2. Name or write the formula for the following Type I polyatomic ionic compounds
Polyatomic Ions Worksheet Polyatomic Practice 1. Name or write the formula for the following polyatomic ions sulfate - CO nitrite MnO perphosphate - SO hypoiodite BrO chlorite - CO phosphite - PO percarbonate
CHEMICAL 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)
Solution. 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
7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8
HOMEWORK CHEM 107 Chapter 3 Compounds Putting Particles Together 3.1 Multiple-Choice 1) How many electrons are in the highest energy level of sulfur? A) 2 B) 4 C) 6 D) 8 2) An atom of phosphorous has how
CHEMICAL 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
Chapter 4: Nonionic Compounds and Their Nomenclature
50 Chapter 4: Nonionic Compounds and Their Nomenclature A nonionic compound is a substance composed of atoms held together by chemical bonding forces, called covalent bonds. Covalent bonds are formed by
Problem Solving. Mole Concept
Skills Worksheet Problem Solving Mole Concept Suppose you want to carry out a reaction that requires combining one atom of iron with one atom of sulfur. How much iron should you use? How much sulfur? When
Find a pair of elements in the periodic table with atomic numbers less than 20 that are an exception to the original periodic law.
Example Exercise 6.1 Periodic Law Find the two elements in the fifth row of the periodic table that violate the original periodic law proposed by Mendeleev. Mendeleev proposed that elements be arranged
EXPERIMENT 8: Activity Series (Single Displacement Reactions)
EPERIMENT 8: Activity Series (Single Displacement Reactions) PURPOSE a) Reactions of metals with acids and salt solutions b) Determine the activity of metals c) Write a balanced molecular equation, complete
Writing and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
(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
Calculating Molar Mass of a Compound
Instructions for Conversion Problems For every conversion problem Write the number in the problem down with unit and a multiplication sign Decide which conversion factor you should use, Avagadro s or molar
Chapter 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.
Unit 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
Success criteria You should be able to write the correct formula for any ionic compound
Chemical Formulas and Names of Ionic Compounds WHY? Going back to pre-historic times, humans have experimented with chemical processes that helped them to make better tools, pottery and weapons. In the
Tutorial 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
HOMEWORK 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
Stoichiometry 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
Name period Unit 3 worksheet
Name period Unit 3 worksheet Read chapter 8, 2.52.7 1. Explain the difference between metallic, ionic, and covalent bonding Metallic cations share a sea of electrons Ionic atoms give and take electrons
Periodic Table Questions
Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is
NET 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
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements
47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.
B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
INORGANIC NOMENCLATURE ~ NAMING INORGANIC COMPOUNDS
INORGANIC NOMENCLATURE ~ NAMING INORGANIC COMPOUNDS Every compound has its own CHEMICAL FORMULA and its own NAME. The nomenclature (naming systems) for IONIC and MOLECULAR compounds are different. IONIC
H 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,
Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
Chapter 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
Chemistry 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
Chapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
AP Chemistry Reaction Questions
AP Chemistry Reaction Questions Directions: Give the formulas to show the reactants and the products for the following chemical reactions. Each of the reactions occurs in aqueous solution unless otherwise
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3
CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3 Chapter 1 Chemistry: The Study of Change 1. Element, compound, homogeneous mixture (solution), or heterogeneous mixture: a) orange juice b)
Chapter 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
b. 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
PART 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
Chapter 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
100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals.
2.21 Ionic Bonding 100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals. Forming ions Metal atoms lose electrons to form +ve ions. Non-metal
TOPIC 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
Chapter 3 Chemical Compounds
19 Chapter 3 Chemical Compounds Review Skills 3.1 Classification of Matter 3.2 Compounds and Chemical Bonds Equal and Unequal Sharing of Electrons Transfer of Electrons Summary of Covalent and Ionic Bond
Chapter 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.
Ionic and Metallic Bonding
Ionic and Metallic Bonding BNDING AND INTERACTINS 71 Ions For students using the Foundation edition, assign problems 1, 3 5, 7 12, 14, 15, 18 20 Essential Understanding Ions form when atoms gain or lose
1. 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)
Chapter 2 Compounds and Chemical Reactions. 6. The number of atoms in one formula unit of the substance, CO(NH 2 ) 2, is
Chapter 2 Compounds and Chemical Reactions Multiple Choice 1. Which one of the following elements exists as a diatomic molecule when it is in the free state? a. H b. He c. Li d. Be e. B 6. The number of
Study 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
neutrons 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
Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
Exam 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
MOLES 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
Problem 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
6 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
A PREVIEW & SUMMMARY of the 3 main types of bond:
Chemical Bonding Part 1 Covalent Bonding Types of Chemical Bonds Covalent Bonds Single Polar Double NonPolar Triple Ionic Bonds Metallic Bonds Other Bonds InterMolecular orces first A PREVIEW & SUMMMARY
Answers and Solutions to Text Problems
Chapter 7 Answers and Solutions 7 Answers and Solutions to Text Problems 7.1 A mole is the amount of a substance that contains 6.02 x 10 23 items. For example, one mole of water contains 6.02 10 23 molecules
Experiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
Unit 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
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS
UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12
CHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas
Date In Class Homework 10/22 Thur Counting By Mass Lab 10/23 Fri (mole day!!!) THE MOLE! in room 137 10/26 Mon (LSM) More on the Mole Watch empirical and molecular formula video. 10/27 Tue % Composition
Formulae, 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
1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
Chapter 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