chapter 1: periodic table, rules, nomenclature & common ion names

Group 1a: Li, Na, K, Kb, Cs, Fr

Alkali metals, form 1+ charge with nonmetals

Group 2a: Be, Mg, Ca, Sr, Ba, Ra

alkaline earth metals, form 2+ charge with nonmetals

Group 7a: F, Cl, Br, I

halogens, form salts with 1- charge

group 8a: He, Ne, Ar, Kr, Xe, Rn

noble gases, stable dont form ions

binary ionic compounds

1) Cation, Anion (fixed charges)

2) Monatomic cation is just name of element 3) Monatomic ions are just element name + ide

ex. H+ Cl- Hydrogen Chloride

binary covalent

2 nonmetals, 1) first element named first 2) second name as anion 3) prefixes denote number 4) mono is never used for first element

binary type 2

multiple ratios possible because charges can change (usually transition metals)

Fe+2 vs Fe +3 → FeCl2 vs FeCl3

nomenclature: lower charge called “ous” higher called “ic”

iron (III) ferric and iron (II) ferrous

Cu 2+ vs Cu+

Copper (II) Cupric

Copper (I) Cuprous

Co 3+ vs Co 2+

Cobalt (III) Cobaltic

Cobalt (II) Cobaltous

Sn4+ vs Sn2+

Tin (IV) Stannic

Tin (II) Stannous

Pb 4+ vs Pb 2+

Lead (IV) Plumbic

Lead (II) Plumbous

Hg 2+ vs Hg2²+

Mercurcy (II) Mercuric

Mercury (I) Mercurous *mercurcy I ions always occur bound together to form Hg _{2. ^{2 +}}

NH4+

Ammonium

NO₂^-

Nitrite

NO_3^-

Nitrate, soluble

SO_3^2-

Sulfite

SO_4^2-

Sulfate

HSO_4^-

hydrogen sulfate or bisulfate

OH-

hydroxide

CN-

cyanide

PO_4^3-

phosphate

HPO_4^2-

hydrogen phosphate

H₂ PO ₄ -

dihydrogen phosphate

CO _{3 ²-}

carbonate

HCO₃-

hydrogen carbonate, bicarbonate

C₂ H ₃ O₂ -

acetate

MnO ₄ -

permanganate

Cr ₂ O ₇ 2-

dichromate

Cr O_{4 ^2-}

chromate

O ₂ ^2-

peroxide

ClO -

hypochlorite

Cl O₂ -

chlorite

ClO₃ -

chlorate

Cl O₄ -

perchlorate

group 1: Li+, Na+, K+, Cs+, Rb+

always soluble

Cl-, Br-, I-

generally soluble unless with Ag+, Pb+2, (Hg2)2+

AgNO3 and Ag(C2 H3 O2)

soluble silver salts, all others are insoluble

sulfate salts

insoluble, all others are soluble

hydroxide (OH)+ group 1 element

soluble

hydroxide + group 2 (Ca, Sr, Ba)

slightly soluble

hydroxide + transition metals or Al3+

insoluble

sulfide of transition metals

highly insoluble (CdS, FeS, ZnS, Ag2S), Arsenic, antimony, bismuth, and lead sulfides are also insoluble.

carbonates (CO3), chromates (CrO4), phosphates (PO4), Fluorides (F2)

insoluble

oxidation state for atom in element ex. Na, O2, O3, Hg

0

oxidation state for monatomic ion ex. Na+, O2-, Fe 3+

same as its charge, ex +1, -2, +3

oxidation state for hydrogen covalent compounds with nonmetals ex. HCl, NH3, H2O, CH4

hydrogen assigned +1

oxidation state of oxygen in covalent compounds (CO, CO2, SO2, SO3)

always -2, unless peroxide O2 ²-, in this case it would be -1

binary compounds oxidation state example NH3, H2S, F

n=-3, s=-2, f=-1

rule for overall oxidation

if neutral must equal 0 (ex. water), otherwise equal overall charge

plumbous

lead 2

plumbic

lead 4