Chem 1 Pearson ch. 3

ionic bonding

metal + nonmetal, cation gives electron to anion

covalent bonding

nonmetal + nonmetal or more, make molecules, share electrons

empirical formula

smallest whole number ration of atoms (ex. CH2)

molecular formula

number of each atoms a compound has (ex. C6H12)

structural formula

physical diagram, can tell bond multiplicity and molecular geometry

ionic formula charges

swap the charges for the subscripts

ex. Na^+1 and P^-3 = Na3P

group 1 charge

1+

group 2 charge

2+

group 13 charge

3+

group 15 charge

3-

group 16 charge

2-

group 17 charge

1-

type I metals

main group (groups 1, 2, 13), have fixed charges

type ii metals

transition metals, variable charges, indicate with roman numeral

ex. Cu^2+ = copper (II)

type ii metal exceptions

Ag^1+, Zn^3+, Sc^3+

monoatomic ions

single atom with + or - charge

monoatomic ion naming

anion base + ide

ex. Cl^1- = chlorida

polyatomic ions

covalently bonded interior, interacts ionically

type I binary naming

cation + anion base + ide

ex. NaCl = sodium chlorida

type II binary naming

cation (roman numeral) + anion base + ide

ex. NiCl2 → Ni^2+ and Cl^1- = nickel (II) chlorida

polyatomic

cation + anion (usually polyatomic)

ex. Na^+ + ClO^- = sodium chlorite

polyatomic ion naming

most = per + polyatomic ion + ate (ex. ChO4^1- = perchlorate)

more = polyatomic ion + ate (ex. ChO3^1- = chlorate)

less = polyatomic ion + ite (ex. ChO2^1- = chlorite)

least = hypo + polyatomic ion + ite (ex. ChO^1- = hyporchlorite)

binary molecular compounds

2 nonmetals

prefix + atom + ide

(ex. CO2 = carbon dioxide)

binary acid

H^+ + one nonmetal

binary acid naming

hydro + nonmetal + ic acid

(ex. HCl^1- = hydrochloric acid)

oxyacid

include oxygen

oxyacid naming

anion root + ic acid

(ex. HNO3 = nitric acid)

total molar mass

(atoms)(molar mass) + (atoms)(molar mass) + (atoms)(molar mass) + …

mass percent

(((atoms)(molar mass)) / (total molar mass of compound))(100)

elements that are diatomic in nature

Br I N Cl H O F (brinclhof)

found in pairs, usually doubled (N2, I2, etc)