Chemistry 1 - Chapter 7: Study Guide

Ionic Bonding

Force of attraction between oppositely charged ions.

Iron(II)

Fe2+

Iron(III)

Fe3+

Zinc

Zn2+

Silver

Ag1+

Cadmium

Cd2+

Copper(I)

Cu+1

Chromium(II)

Cr+2

Copper(II)

Cu+2

Chromium(III)

Cr+3

Chromium(VI)

Cr+6

Manganese(II)

Mn+2

Mercury(I)

Hg2 ^+2

Manganese(III)

Mn+3

Mercury(II)

Hg+2

Manganese(VII)

Mn+7

Lead(II)

Pb+2

Cobalt(II)

Co+2

Lead(IV)

Pb+4

Cobalt(III)

Co+3

Tin(II)

Sn+2

Gold(I)

Au+1

Tin(IV)

Sn+4

Gold(III)

Au+3

Nickel(II)

Ni+2

Vanadium(II)

V+2

Nickel(III)

Ni+3

Vanadium(III)

V+3

Nickel(IV)

Ni+4

Vanadium(IV)

V+4

Acetate

C2H3O2-1 (CH3COO -1)

Hypochlorite

ClO-1

Ammonium

NH4+1

Chlorite

ClO2-1

Hydroxide

OH-1

Chlorate

ClO3-1

Hydronium

H3O+

Perchlorate

ClO4-1

Permanganate

MnO4-1

Cyanide

CN-1

Nitrate

NO3-1

Dichromate

Cr2O7-2

Nitrite

NO2-1

Chromate

CrO4-2

Sulfate

SO4-2

Hydrogen Sulfate

HSO4-1

Sulfite

SO3-2

Hydrogen Sulfite

HSO3-1

Phosphate

PO4-3

Hydrogen Phosphate

HPO4-2

Phosphite

PO3-3

Oxalate

C2O4-2

Carbonate

CO3-2

Hydrogen Carbonate

HCO3-1

Silicate

SiO4-4

Peroxide

O2-2

Bromate

BrO3-1

Arsenate

AsO4-3

Hydrate

when a water molecule (s) are chemically bonded to the ionic compound.

Hygroscopic

easily absorb water molecules from the air.

Deliquescent

very hygroscopic; takes out water from the air to dissolve completely to form a liquid solution.

Anhydrous

when all of the water has been removed.

Acids

Compounds that always begin with hydrogen.

Anion

A negatively charged ion.

Hydrochloric Acid

HCl

Hydrobromic Acid

HBr

Sulfuric Acid

H2SO4

Sulfurous Acid

H2SO3

Nitric Acid

HNO3

Hydrocyanic Acid

HCN

Phosphoric Acid

H3PO4

Cation

A positively charged ion.

Sodium Hydroxide

NaOH

Potassium Hydroxide

KOH

Ammonia

NH3

Hydrocarbons

Compounds composed solely of carbon and hydrogen.

Alkanes

Hydrocarbons with the generic formula: CnH2n+2.

Alkenes

Hydrocarbons with the generic formula: CnH2n.

Alkynes

Hydrocarbons with the generic formula: CnH2n-2.

Oxidation Number

Numbers assigned to atoms in a compound that indicate the distribution of electrons.

Molar Mass

The mass of 1 mole of a pure substance.

Formula Mass

The mass of the atomic mass units of one molecule or formula unit.

Empirical Formula

The lowest whole number ratio of atoms in a compound.

Molecular Formula

The true number of atoms of each element in the formula of a compound.

Mass Percent

The percentage by mass of each element in a compound.

Metals in general _ electrons

lose

Nonmetals in general _ electrons

gain

Transition metals are in groups ___

3-12

Transition metals can/cannot have multiple oxidaiton states

can

Exception to the transition metal oxidation state rule

Zinc (Zn), Silver (Ag), and Cadmium (Cd)

the roman numeral is equal to the oxidation state for atom of that element

one

In ionic bonds, there are no prefixes when naming - true or flase

true

"" always has more oxygen than ""

"ate", "ite"

prefix for 1 in hydrates and covalent bonding

mono

prefixes for 1 in organic compounds

meth

prefixes for 2 in hydrates and covalent bonding

di

prefix for 2 in organic compounds

eth

prefix for 3 in hydrates and covalent bonding

tri

prefixes for 3 in organic compounds

prop

prefixes for 4 in hydrates and covalent bonding

treta