Chapter 7. Representative elements of the same groups usually have the same ionic charges. Group 1: H +, Li +, Na + Group 2: Be 2+, Mg 2+,

Ionic Compounds and Metals

Chapter 7

Ion Formation

The Octet Rule

Formation of Ionic Bonds

Representative elements of the same groups usually have the same ionic charges.

Group 1: H+, Li+, Na+

Group 2: Be2+, Mg2+, Ca2+

Group 15: N3-, P3-, As3-

Group 16: O2-, S2-, Se2-

Group 17: F-, Cl-, Br-

Transition elements can usually have more than one charge. Example Fe2+ and Fe3+

Common Ions and their charges

Most transition metals can have a few different charges.

Example: Fe2+, Fe3+

Fe2O3

FeO

Transition Metal Ions

Names and Formulas of Ionic Compounds

Polyatomic ions are ions that are made up of more than one atom.

Ammonium: NH4+

Nitrite: NO2-

Nitrate: NO3-

Hydroxide: OH-

Hypochlorite: ClO-

Polyatomic Ions

Chlorite: ClO2-

Chlorate: ClO3-

Perchlorate: ClO4-

Carbonate: CO32-

Sulfite: SO32-

Sulfate: SO42-

Peroxide: O22-

PO43-

NH4Cl

Fe(NO3)3

TiBr3

Pb(SO4)2

Chromium (VI) Phosphate

Tin (II) Nitrate

Cobalt (III) Oxide

Chromium (III) Hydroxide

Practice

Barium Carbonate

Aluminum Hydroxide

Copper (I) Sulfide

Lead (II) Phosphate

Zinc (II) Iodide

Chromium (III) Sulfite

NH4Br

NaClO3

Fe2S3

AgNO3

CuF2

Ni(ClO)3

Ru3(PO4)4

Covalent bondingChapter 8

What is a covalent bond?

Naming Molecules

Naming Practice CO2

SO2

NF3

CCl4

What is the formula of Diarsneic trioxide?

Fluorine Fluorine, and some other common

elements, usually exist as a molecule of F2.

Fluorine’s electron configuration is….

Fluorine’s structure is…

Lewis Structures

Draw the lewis structures for the following molecules.

PH3

HCl

PBr3

CCl4

SiH4

NH3

NF3

Lewis Structures of Polyatomic Ions To draw a lewis structure of a polyatomic

ion we first figure out how many valence electrons we have, then add or subtract electrons to account for the charge.

SO42-

Exceptions to the octet rule A small group of molecules have have an

odd number of valence electrons and be unable to form an octet around each atom.

NO2

An other group of molecules have expanded octets.

SF6