Chem 2 Exam: chapters 2, 6, 7

nonsignificant digits

zeros at the end of a large number (without a decimal point) OR zeros at the beginning of a decimal number

multiplication and division sig figs

final answer has the same as the measurement with the least number of sig figs

addition and subtraction sig figs

final answer has the same number of decimal places as the measurement with the fewest number of decimal places

giga (G)

10^9 (1,000,000,000)

mega (M)

10^6 (1,000,000)

kilo (k)

10^3 (1,000)

centi (c)

10^-2 (0.01)

milli (m)

10^-3 (0.001)

micro (mc)

10^-6 (0.000001)

nano (n)

10^-9 (0.000000001)

cubic centimeter volume

same as 1 mL

ionic bond

electrons are transferred from the atom of a metal to the atom of a nonmetal

covalent bond

valence electrons of nonmetal atoms are shared

cation

positively charged ion

anion

negatively charged ion

naming ionic compounds (fixed charge)

name of the metal followed by the first syllable of the nonmetal + ide

naming ionic compounds (variable charge)

same has fixed charge, but a roman numeral indicating the cation charge is placed immediately after the metal name

charges of: Cr, Mn, Fe, Co, Ni

2+ or 3+

charges of: Zn, Cd, Hg2, Hg

2+

charges of: Sn, Pb

2+ or 4+

charge of Cu

+ or 2+

charge of Ag

+

charge of Au

+ or 3+

charge of Al

3+

charge of Bi

3+ or 5+

polyatomic ions

group of atoms with an overall charge

OH^-

hydroxide

NH4^+

ammonium

NO3^-

nitrate

NO2^-

nitrite

ClO4^-

perchlorate

ClO3^-

chlorate

ClO2^-

chlorite

ClO^-

hypochlorite

CO3^2-

HCO3^-

hydrogen carbonate (bicarbonate)

CN-

cyanide

C2H3O2^-

acetate

SO4^2-

sulfate

HSO4^-

hydrogen sulfate (bisulfate)

SO3^2-

sulfite

HSO3^-

hydrogen sulfite (bisulfite)

PO4^3-

phosphate

HPO4^2-

hydrogen phosphate

H2PO4^-

dihydrogen phosphate

PO3^3-

phoshpite

diatomic molecules

H, N, O, F, Cl, Br, I

exceptions to the octet rule

Hydrogen (1 bond), Beryllium (2 bonds), Boron (3 bonds)

nonpolar covalent electronegativety

0.0-0.4

polar covalent electronegativety

0.5-1.8

ionic electronegativety

1.9+

2 bonded atoms, 0 lone pairs

linear electron group geometry, linear molecular shape

3 bonded atoms, 0 lone pairs

trigonal planar electron group geometry, trigonal planar molecular shape

2 bonded atoms, 1 lone pair

trigonal planar electron group geometry, bent molecular shape

4 bonded atoms, 0 lone pairs

tetrahedral electron group geometry, tetrahedral molecular shape

3 bonded atoms, 1 lone pair

tetrahedral electron group geometry, trigonal pyramidal molecular shape

2 bonded atoms, 2 lone pairs

tetrahedral electron group geometry, bent shape

nonpolar molecules

a molecule contains all nonpolar bonds OR the dipoles of polar bonds are symmetrical and cancel our

ion-dipole interaction

between ions and polar molecules

dipole-dipole interaction

between polar molecules

hydrogen bonds

hydrogen bonded to F, O, or N

dispersion forces

weak attraction force that occurs between all molecules, but allows nonpolar molecules to form liquids and solids

weakest to strongest intermolecular forces

dispersion, dipole-dipole, hydrogen bonding, ion-dipole

mole

6.02 x 10^23 particles

molar mass

the mass of one mole of an element, found through the average atomic mass expressed in grams (ex. 1 mol C = 12.01g C

law of conservation of mass

matter cannot be created or destroyed, the mass of the products equals the mass of the reactants

synthesis reaction

two or more elements form one product, simple compounds combine to form one product

decomposition reaction

one substance splits into two or more simpler substances

single replacement reaction

one element takes the place of a different element in another reacting compound

double replacement reaction (metathesis)

both ions in the reactant compounds switch places

combustion reaction

a carbon-hydrogen containing compound burns in oxygen gas to form carbon dioxide and water + energy

oxidation

loss of an electron

reduction

gain of an electron