Chapter 5: Nomenclature Rules or

I Love It When a Plan

Comes Together

I. Types of Compounds

A. Molecular

B. Ionic

II. Naming Ionic Compounds

A. Binary Ionic Compounds

B. Compounds in Water

C. Ionic Compounds with

Polyatomic Anions and

Cations

III. Naming Molecular Compounds

IV. Naming Acids

A. Binary Acids

B. Acids from Oxyanions

V. Writing Formulas from Names

2

I. Types of Compounds

A) Molecular Compounds

Covalent Bonds - sharing of electrons

between elements

non-metal - non-metal

B) Ionic Compounds

Ionic Bonds - transfer of electrons

between elements

metal - non-metal

Chemistry is

the BOMB!

2,3,7,8-tetrachlorodibenzo-p-dioxin

potassium cyanide dihydrogen monoxide

Organic – mostly C, H, and a small amount of

other elements, generally with a C-

backbone

Inorganic – all others without the C-

backbone

H2O

3

II. Naming Ionic Compounds

A) Binary Ionic Compounds

Types of Binary Ionic Compounds Type 1 - contain metals that form only one ion of

specific charge

Type 2 - contain metals that can form ions with

different charges

Type 1

- most main group elements plus Ag, Zn, Cd, Ni

Type 2

- most transition metals and inner transition metals plus

Ga, In,Tl, Sn, Pb, Bi, Po*

4

Rules for Naming Binary Ionic Compounds

1. Cation Anion

2. Name of Cation =Type 1 - name of neutral metal

=Tpye 2 - name of neutral

metal (R.N.)

Cmpd Cation Anion Cation Name

3. Name of Anion = root name of neutral element with

-ide ending

Cmpd Cation Anion Anion Name

5

C.) Ionic Compounds with Polyatomic

Anions and Cations

Polyatomic Ion ion composed of

multiple atoms

Examples

Exception to Rule Rule Molecular Compd. – no metals

Ionic Cmpd. – metal and non-metal

6

Formulas for Ionic Compounds with Polyatomic Ions

Ions Formula

Fomula Ions

7

B.) Compounds in Water

Ionic and Molecular ???

www.newworldencyclopedia.org, igcsetuition.blogspot.com

H2O

8

I. WHAT IS AN AQUEOUS SOLUTION?

1. What is a solution?

Solution - a homogeneous mixture of two

or more substances (solute(s)

and solvent)

Solvent - chemical in the largest amount

Solute(s) - chemical dissolved in the

solvent

2. What does aqueous mean?

(aq) – aqueous

(s) – solid

9

II. Aqueous Compounds:

1. Electrolyte - Compound that dissolves in

water to produces ions

2. Non-Electrolyte - compound that dissolves

but does not produce ions

in water

1. Electrolytes

Strong Electrolyte - for every molecule or

formula unit that

dissolves we get at

least two ions

Weak Electrolyte - only a small fraction

of the compounds that

dissolve produce ions

H2O

10

Soluble Ionic Compounds 1. Are all strong electrolytes

2. Dissociate into constituent ions

11

Soluble Molecular Compounds (Acids)

- molecular compound with H listed first in

the formula or with an H after –COO in the

formula (this H or H’s can be transferred)

HI CH4 HC2H3O2 CH3COOH H3PO4

Properties of Acids

Strong Acids

12

Acids Continued

Weak Acid

- acid dissolves but only a small fraction of particles

ionize to produce H3O+

13

Bases - bases produce OH- when dissolved in water

Ionic

Molecular

Our Class (Chem. 130)

14

2. Non-Electrolytes

- dissolve but do not produce ions

- molecular compounds that are neither acids nor

bases

15

Examples

Compound

Formula Cation Anion Name

16

Naming Ionic Compounds With Polyatomic Ions

1. Name Cation (R.N. if needed)

2. Name Anion (memorize)

Help Distinguishing Between Oxyanions

Oxyanion - element bonded with

oxygen to form an anion

Increasing #’s of Oxygen

17

Examples

Oxyanion Non-metal # O’s Name

Original Ion Added H New Ion Name

18

Increasing #’s of Oxygen

Oxyanions with Halogens

Cl - ClO- or OCl

-, ClO2

-, ClO3

-, ClO4

-

Br - BrO- or OBr

-, BrO2

-, BrO3

-, BrO4

-

I - IO

- or OI

-, IO2

-, IO3

-, IO4

-

Ion Formula Name

19

Practice

Compound

Formula Cation Anion Name

20

III. Naming Molecular Compounds BINARY MOLECULAR COMPOUNDS

21

Rules for Names and Formulas of

Inorganic Binary Molecular Cmpds

1. Element furthest to the left and lowest on the

P.T. is usually written first in the name and

formula

2. In the name, numbers of atoms are given by

Greek prefixes (mono not used for first element)

and the second element has –ide added to the

root name of the element

3. If the element starts with an “a” or “o”,

the “a” or “o” is dropped from the end of

the greek prefix

22

Examples

23

IV. Naming Acids

http://jnuenvis.nic.in/subject/waterchem/acidrain.gif, http://trendsupdates.com/wp-content/uploads/2009/01/acid-rain.jpg

24

A. Naming Binary Acids

Rules

1. Name of the acid = the root name of the

second element with

hydro as a prefix and

–ic as a suffix

2. Add word acid

Non-Metal Acid Formula Name

25

Increasing #’s of Oxygen

Increasing #’s of Oxygen

B. Naming Acids from Oxyanions

- Add H to oxyanions

26

EXAMPLES

Oxyanion Acid Formula Name

27

V. Writing Formulas from Names

Name Cation Anion Compound

Formula Potassium

hydroxide

Lead(IV) oxide

Ammonium

perchlorate

Cobalt(III)

nitrate

Calcium

hypoiodite

Aluminum

sulfite

Sodium

phosphide

28

Hydrobromic Acid

Carbon tetrachloride

Iodous acid

Hypochlorous acid