Figure Some common monatomic ions of the elements. Can you see any patterns?

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1 Figure 2.16 Some common monatomic ions of the elements. Can you see any patterns?

2 Table 2.3 Common ions are in blue. Common Monoatomic Ions Cations Anions Charge Formula Name Charge Formula Name H + hydrogen hydride Li + lithium F - fluoride Na + K + Cs + Ag + Mg 2+ Ca 2+ Sr 2+ Ba 2+ Zn 2+ Cd 2+ Al 3+ sodium potassium cesium silver magnesium calcium strontium barium zinc cadmium aluminum H - Cl - Br - I - O 2- S 2- N 3- chloride bromide iodide oxide sulfide nitride

3 Naming binary ionic compounds The name of the cation is written first, followed by that of the anion. The name of the cation is the same as the name of the metal. Many metal names end in -ium. The name of the anion takes the root of the nonmetal name and adds the suffix -ide. Calcium and bromine form calcium bromide.

4 Sample Problem 2.5 Naming Binary Ionic Compounds PROBLEM: Name the ionic compound formed from the following pairs of elements: (a) magnesium and nitrogen (b) iodine and cadmium (c) strontium and fluorine (d) sulfur and cesium PLAN: SOLUTION: Use the periodic table to decide which element is the metal and which the nonmetal. The metal (cation) is named first and we use the -ide suffix on the nonmetal name root. (a) magnesium nitride (b) cadmium iodide (c) strontium fluoride (d) cesium sulfide

5 Sample Problem 2.6 Determining Formulas of Binary Ionic Compounds PROBLEM: PLAN: Write empirical formulas for the compounds named in Sample Problem 2.5. Compounds are neutral. We find the smallest number of each ion which will produce a neutral formula. Use subscripts to the right of the element symbol. SOLUTION: (a) Mg 2+ and N 3- ; three Mg 2+ (6+) and two N 3- (6-); Mg 3 N 2 (b) Cd 2+ and I - ; one Cd 2+ (2+) and two I - (2-); CdI 2 (c) Sr 2+ and F - ; one Sr 2+ (2+) and two F - (2-); SrF 2 (d) Cs + and S 2 - ; two Cs+ (2+) and one S 2 - (2-); Cs2 S

6 Table 2.4 (partial) Metals With Several Oxidation States Element Ion Formula Systematic Name Common Name Copper Cu +1 copper(i) cuprous Cobalt Iron Manganese Tin Cu +2 Co +2 Co +3 Fe +2 copper(ii) cupric cobalt(ii) cobalt (III) iron(ii) ferrous Fe +3 iron(iii) ferric Mn +2 Mn +3 Sn +2 Sn +4 manganese(ii) manganese(iii) tin(ii) stannous tin(iv) stannic

7 Sample Problem 2.7 PROBLEM: Determining Names and Formulas of Ionic Compounds of Elements That Form More Than One Ion Give the systematic names for the formulas or the formulas for the names of the following compounds: PLAN: SOLUTION: (a) tin(ii) fluoride (b) CrI 3 (c) ferric oxide (d) CoS Compounds are neutral. We find the smallest number of each ion which will produce a neutral formula. Use subscripts to the right of the element symbol. (a) Tin (II) is Sn 2+ ; fluoride is F - ; so the formula is SnF 2. (b) The anion I is iodide(i - ); 3I - means that Cr(chromium) is +3. CrI 3 is chromium(iii) iodide (c) Ferric is a common name for Fe 3+ ; oxide is O 2-, therefore the formula is Fe 2 O 3. (d) Co is cobalt; the anion S is sulfide(2-); the compound is cobalt (II) sulfide.

8 Table 2.5 (partial) Formula Name Some Common Polyatomic Ions Formula Name NH 4 + Cations ammonium H 3 O + hydronium Common Anions CH 3 COO - acetate CO 3-2 carbonate CN - OH - cyanide hydroxide CrO Cr 2 O chromate dichromate ClO 3 - chlorate O 2-2 oxide NO 2 - nitrite SO 4-2 sulfate NO 3 - nitrate PO 4-3 phosphate MnO 4 - permanganate

9 Figure 2.17 Naming oxoanions Prefixes Root Suffixes Examples No. of O atoms per root ate ClO - perchlorate 4 root ate ClO - chlorate 3 root ite ClO - chlorite 2 hypo root ite ClO - hypochlorite Table 2.6 Numerical Prefixes for Hydrates and Binary Covalent Compounds Number Prefix Number Prefix Number Prefix 1 mono 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9 nona 10 deca

10 Sample Problem 2.8 Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions PROBLEM: Give the systematic names or the formula or the formulas for the names of the following compounds: (a) Fe(ClO 4 ) 2 (b) sodium sulfite (c) Ba(OH) 2 8H 2 O PLAN: SOLUTION: Note that polyatomic ions have an overall charge so when writing a formula with more than one polyatomic unit, place the ion in a set of parentheses. (a) ClO - 4 is perchlorate; iron must have a 2+ charge. This is iron(ii) perchlorate. (b) The anion sulfite is SO 2-3 therefore you need 2 sodiums per sulfite. The formula is Na 2 SO 3. (c) Hydroxide is OH - and barium is a 2+ ion. When water is included in the formula, we use the term hydrate and a prefix which indicates the number of waters. So it is barium hydroxide octahydrate.

11 Sample Problem 2.9 Recognizing Incorrect Names and Formulas of Ionic Compounds PROBLEM: Something is wrong with the second part of each statement. Provide the correct name or formula. (a) Ba(C 2 H 3 O 2 ) 2 is called barium diacetate. (b) Sodium sulfide has the formula (Na) 2 SO 3. (c) Iron(II) sulfate has the formula Fe 2 (SO 4 ) 3. (d) Cesium carbonate has the formula Cs 2 (CO 3 ). SOLUTION: (a) Barium is always a +2 ion and acetate is -1. The di- is unnecessary. (b) An ion of a single element does not need parentheses. Sulfide is S 2-, not SO 2-3. The correct formula is Na 2 S. (c) Since sulfate has a 2- charge, only 1 Fe 2+ is needed. The formula should be FeSO 4. (d) The parentheses are unnecessary. The correct formula is Cs 2 CO 3.

12 Naming Acids 1) Binary acids solutions form when certain gaseous compounds dissolve in water. For example, when gaseous hydrogen chloride(hcl) dissolves in water, it forms a solution called hydrochloric acid. Prefix hydro- + anion nonmetal root + suffix -ic + the word acid - hydrochloric acid 2) Oxoacid names are similar to those of the oxoanions, except for two suffix changes: Anion -ate suffix becomes an -ic suffix in the acid. Anion -ite suffix becomes an -ous suffix in the acid. The oxoanion prefixes hypo- and per- are retained. Thus, BrO - 4 is perbromate, and HBrO 4 is perbromic acid; IO - 2 is iodite, and HIO 2 is iodous acid.

13 Sample Problem 2.10 Determining Names and Formulas of Anions and Acids PROBLEM: Name the following anions and give the names and formulas of the acids derived from them: (a) Br - (b) IO 3 - (c) CN - (d) SO 4 2- (e) NO 2 - SOLUTION: (a) The anion is bromide; the acid is hydrobromic acid, HBr. (b) The anion is iodate; the acid is iodic acid, HIO 3. (c) The anion is cyanide; the acid is hydrocyanic acid, HCN. (d) The anion is sulfate; the acid is sulfuric acid, H 2 SO 4. (e) The anion is nitrite; the acid is nitrous acid, HNO 2.

14 Sample Problem 2.11 Determining Names and Formulas of Binary Covalent Compounds PROBLEM: (a) What is the formula of carbon disulfide? (b) What is the name of PCl 5? (c) Give the name and formula of the compound whose molecules each consist of two N atoms and four O atoms. SOLUTION: (a) Carbon is C, sulfide is sulfur S and di-means 2 - CS 2. (b) P is phosphorous, Cl is chloride, the prefix for 5 is penta-. Phosphorous pentachloride. (c) N is nitrogen and is in a lower group number than O (oxygen). Therefore the formula is N 2 O 4 - dinitrogen tetraoxide.

15 Sample Problem 2.12 Recognizing Incorrect Names and Formulas of Binary Covalent Compounds PROBLEM: Explain what is wrong with the name of formula in the second part of each statement and correct it: (a) SF 4 is monosulfur pentafluoride. (b) Dichlorine heptaoxide is Cl 2 O 6. (c) N 2 O 3 is dinitrotrioxide. SOLUTION: (a) The prefix mono- is not needed for one atom; the prefix for four is tetra-. So the name is sulfur tetrafluoride. (b) Hepta- means 7; the formula should be Cl 2 O 7. (c) The first element is given its elemental name so this is dinitrogen trioxide.

16 Sample Problem 2.13 Calculating the Molecular Mass of a Compound PROBLEM: Using the data in the periodic table, calculate the molecular (or formula) mass of the following compounds: (a) tetraphosphorous trisulfide (b) ammonium nitrate PLAN: Write the formula and then multiply the number of atoms(in the subscript) by the respective atomic masses. Add the masses for the compound. SOLUTION: (a) P 4 S 3 molecular = (4xatomic mass of P) mass + (3xatomic mass of S) = (4x30.97amu) + (3x32.07amu) = amu molecular mass (b) NH 4 NO 3 = (2xatomic mass of N) + (4xatomic mass of H) + (3xatomic mass of O) = (2x14.01amu)+ (4x1.008amu) + (3x16.00amu) = 80.05amu

17 Sample Problem 2.14 Determining Formulas and Names from Molecular Depictions PROBLEM: Each box contains a representation of a binary compound. Determine its formula, name, and molecular (formula) mass. (a) (b) SOLUTION: (a) There is 1 sodium (brown) for every fluorine (green), so the formula is NaF. formula mass = (1x atomic mass of Na) + (1x atomic mass of F) = amu amu = amu (b) There are 3 fluorines (green) for every nitrogen (blue), so the formula is NF 3. molecular mass = (3x atomic mass of F) + (1x atomic mass of N) = (3x amu) amu = amu

18 Figure 2.19 The distinction between mixtures and compounds. S Fe Physically mixed therefore can be separated by physical means; in this case by a magnet. Allowed to react chemically therefore cannot be separated by physical means.

19 Organic chemistry is the branch of chemistry that deals with carbon compounds H Functional Groups H H O H C OH H C NH 2 H C C OH H methanol H methylamine H acetic acid 19

20 20

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