Chemistry Unit 2 Study Guide

Ions, ionic bonds, covalent bonds, lewis structures

Zinc

Zn⁺²

Silver

Ag⁺

Cadmium

Cd⁺²

Nitrate

NO₃⁻

Carbonate

CO₃⁻²

Sulfate

SO₄⁻²

Phosphate

PO₄⁻³

Ammonium

NH₄⁺

Cyanide

CN⁻

Hydroxide

OH⁻

Chlorate

ClO₃⁻

Hypochlorite

ClO⁻

Perchlorate

ClO₄⁻

Chlorite

ClO₂⁻

Phosphite

PO₃⁻³

Sulfite

SO₃⁻²

Carbonite

CO₂⁻²

Nitrite

NO₂⁻

Group 1A

Alkali metals

Group 2A

Alkaline earth metals

Group 7A

Halogens

Group 8A

Noble gases

valence electrons

outermost electrons that participate in chemical reactions

ion

atom with a charge

cation

positive ion

anion

negative ion

ionic compounds

transfer of electrons from metal to non-metal

covalent compounds

sharing of electrons between non-metals

-ous

"smaller"

-ic

"larger"

acids

formula starts with H no charge

binary

two elements

ternary

three elements

binary acids

begin with hydro-

ternary acids/oxyacids

no hydro-, 'ate - 'ous, 'ite - 'ic must be an O-H bond

mono

1

di

2

tri

3

tetra

4

penta

5

hexa

6

hepta

7

octa

8

nona

9

deca

10

VSB table

valence (add negative charge, subtract positive), shared (subtract negative charge, add positive), bonds (shared/2)

electronegativity

ability of an atom to attract electrons

electronegativity increases

as you go right and up

most electronegative atoms:

1. Fluorine

2. Oxygen

3. nitrogen/chlorine

pure ionic

ionic bond, electronegativity difference ≥ 2.0

polar covalent

most covalent bonds, partial charges indicated by δ symbol

pure covalent

identical electronegativities