Naming Compounds Binary Compounds are composed of two

Naming Compounds

Binary Compounds are composed of two types of elements such as H 2 O or KBr, not necessarily just two atoms. Diatomic molecules consist of two atoms of the same type such as H 2 and O 2. 1. Binary Ionic Compounds Metal—nonmetal such as Na. Cl and Ca. Cl 2. Binary Covalent Compounds Nonmetal—nonmetal such as H 2 O and CO 2 2

• Binary ionic compounds contain positive cations and negative anions. § Type I compounds • § Metal present forms only one cation. Type II compounds • Metal present can form 2 or more cations with different charges. Copyright © Cengage Learning. All rights reserved 3

Type I Compounds Metals (Groups I, II, and III) and Non-Metals Metal _____ + Non-Metal _____ide Sodium Chlorine Sodium Chloride Na. Cl Calcium + Non-Metal _____ide Bromide Metal _____ Calcium Bromide Ca. Br 2 Aluminun + Non-Metal _____ide Oxide Metal _____ Aluminum Oxide Al 2 O 3

Common Simple Cations and Anions Copyright © Cengage Learning. All rights reserved 5

Rules for Naming Type I Ionic Compounds 1. The cation is always named first and the anion second. 2. A simple cation takes its name from the name of the element. 3. A simple anion is named by taking the first part of the element name (the root) and adding – ide. Copyright © Cengage Learning. All rights reserved 6

Binary Ionic Compounds (Type I) • Examples: KCl Potassium chloride Mg. Br 2 Magnesium

Exercise What is the name of the compound Sr. Br 2? a) b) c)

Binary Ionic Compounds (Type II) with Transition Metals • Metals in these • • • compounds can form more than one type of positive charge. Charge on the metal ion must be specified. Roman numeral indicates the charge of the metal cation. Transition metal cations usually require a Roman numeral. Copyright © Cengage Learning. All rights reserved 9

Type II Compounds Metals (Transition Metals) and Non-Metals Iron +Roman Numeral (__) III + Non-Metal ____ide Bromine Metal ______ Iron (III) Bromide Fe. Br 3 Compare with Iron (II) Bromide Fe. Br 2 Metals (Transition Metals) and Non-Metals Older System Ferrous + ous or ic + Non-Metal ____ide Bromine Metal (Latin) _______ Ferrous Bromide Fe. Br 2 Compare with Ferric Bromide Fe. Br 3 10

Common Type II Cations 11

Rules for Naming Type II Ionic Compounds 1. The cation is always named first and the anion second. 2. Because the cation can assume more than one charge, the charge is specified by a Roman numeral in parentheses. Copyright © Cengage Learning. All rights reserved 12

Binary Ionic Compounds (Type II) • Examples: Cu. Br Copper(I) bromide Fe. S Iron(II)

Exercise What is the name of the compound Cr. O 2? a) b) c)

Exercise What is the correct name of the compound that results from the most stable ion for sulfur and the metal ion that contains 24 electrons? a) b) c) d) iron(III) sulfide chromium(II) sulfide nickel(III) sulfate iron(II) sulfide Copyright © Cengage Learning. All rights reserved 15

Rules for Naming Type III Binary Compounds • Formed between two nonmetals. 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. Copyright © Cengage Learning. All rights reserved 16

Type III Compounds Non-Metals and Non-Metals Use Prefixes such as mono, di, tri, tetra, penta, hexa, hepta, etc. CO 2 Carbon dioxide CO Carbon monoxide PCl 3 Phosphorus trichloride CCl 4 Carbon tetrachloride N 2 O 5 Dinitrogen pentoxide CS 2 Carbon disulfide 17

Prefixes Used to Indicate Numbers in Chemical Names 18 Additional Prefixes 9 nona- 10 deca- 11 undeca- 12 dodeca- 13 trideca- 14 tetradeca- 15 pentadeca- 16 hexadeca- 17 heptadeca- 18 octadeca- 19 nonadeca- 20 icosa

Binary Covalent Compounds (Type III) • Examples: CO 2 Carbon dioxide SF 6 Sulfur

Exercise What is the name of the compound Se. O 2? a) b) c)

Flow Chart for Naming Binary Compounds Copyright © Cengage Learning. All rights reserved 21

Let’s Practice! Name the following. Ca. F 2 K 2 S Co. I 2 Sn. F 4 OF 2 Cu. I SO 2 Sr. S Li. Br Calcium Flouride Potassium Sulfide Cobalt (II) Iodide or Cobaltous Iodide Tin (II) Fluoride or Stannous Fluoride Tin (IV) Fluoride or Stannic Fluoride Oxygen diflouride Copper (II) Iodide or Cupric Iodide Copper (I) Iodide or Cuprous Iodide Sulfur dioxide Strontium Sulfide Lithium Bromide 22

• • Polyatomic ions are charged entities composed of several atoms bound together.

Names of Common Polyatomic Ions (page 101) 24

• Naming ionic compounds containing polyatomic ions follows rules similar to those for

Examples Na. OH Sodium hydroxide Mg(NO 3)2 Magnesium nitrate (NH 4)2 SO 4 Ammonium

Overall Strategy for Naming Chemical Compounds Copyright © Cengage Learning. All rights reserved 27

Exercise What is the name of the compound KCl. O 3? a) b) c)

Exercise Examine the following table of formulas and names. Which of the compounds are named correctly? a) b) c) d) I, III, IV I only Formula Name I P 2 O 5 Diphosphorus pentoxide II Cl. O 2 Chlorine oxide III Pb. I 4 Lead iodide IV Cu. SO 4 Copper(I) sulfate Copyright © Cengage Learning. All rights reserved 29

Acids • • Acids can be recognized by the hydrogen that appears first in

Rules for Naming Acids • • If the anion does not contain oxygen, the acid is named with the prefix hydro– and the suffix –ic attached to the root name for the element. Examples: HCl Hydrochloric acid HCN Hydrocyanic acid H 2 S Hydrosulfuric acid Copyright © Cengage Learning. All rights reserved 31

Acids That Do Not Contain Oxygen Copyright © Cengage Learning. All rights reserved 32

Rules for Naming Acids If the anion contains oxygen: § The suffix –ic is added to the root name if the anion name ends in –ate. • Examples: HNO 3 Nitric acid H 2 SO 4 Sulfuric acid HC 2 H 3 O 2 Acetic acid • Copyright © Cengage Learning. All rights reserved 33

Rules for Naming Acids If the anion contains oxygen: § The suffix –ous is added to the root name if the anion name ends in –ite. • Examples: HNO 2 Nitrous acid H 2 SO 3 Sulfurous acid HCl. O 2 Chlorous acid • Copyright © Cengage Learning. All rights reserved 34

Some Oxygen-Containing Acids Copyright © Cengage Learning. All rights reserved 35

Flowchart for Naming Acids Copyright © Cengage Learning. All rights reserved 36

Exercise Which of the following compounds is named incorrectly? a) KNO 3 b) Ti. O 2 c) Sn(OH)4 d) PBr 5 e) H 2 SO 3 Copyright © Cengage Learning. All rights reserved potassium nitrate titanium(II) oxide tin(IV) hydroxide phosphorus pentabromide sulfurous acid 37

Examples • Sodium hydroxide § • Potassium carbonate § • H 2 SO 4 Dinitrogen pentoxide § • K 2 CO 3 Sulfuric acid § • Na. OH N 2 O 5 Cobalt(III) nitrate § Co(NO 3)3 Copyright © Cengage Learning. All rights reserved 38

Exercise A compound has the formula XCl 3 where X could represent a metal or nonmetal. What could the name of this compound be? a) b) c) d) phosphorus trichloride carbon monochloride tin(IV) chloride magnesium chloride Copyright © Cengage Learning. All rights reserved 39

Lets Practice Some More! HF Na 2 CO 3 H 2 CO 3 KMn. O 4 HCl. O 4 H 2 S Na. OH Cu. SO 4 Pb. Cr. O 4 H 2 O NH 3 Hydroflouric acid Sodium carbonate Carbonic acid Potassium permanganate Perchloric acid Hyrdosulfuric acid Sodium hydroxide Copper (II) sulfate or Cupric sulfate Lead (II) chromate or Plubous chromate Hydrooxic acid (no……just water) Nitrogen trihydride (no. . just ammonia) 40