chem:1070 exam 2

oxidation

loss of electrons

reduction

gain of electrons

synthesis

when 2+ elements or single compounds combine to form 1 product

decomposition

when 1 substance splits into 2+ simpler substances

single replacement

when 1 element takes the place of a different element in another reacting compound

double replacement

when both ions in reactant compounds switch places

combustion

when energy is released as a product in the form of heat

nonpolar molecules

when a molecule contains all nonpolar bonds & no lone pairs on central atom

when a molecule contains polar bonds but dipoles cancel in symmetrical arrangement

polar molecules

when electrons are shared unequally in a polar covalent bond

when polar bonds in a molecule don’t cancel out

when lone pairs are present on central atom

180 degrees

bond angle for 2 electron groups

120 degrees

bond angle for 3 electron groups

109 degrees

bond angle for 4 electron groups

linear

molecular shape for 2 bonded atoms & 0 lone pairs

trigonal planar

molecular shape for 3 bonded atoms & 0 lone pairs

bent

molecular shape for 3 electron groups of 2 bonded atoms & 0 lone pairs or 4 electron groups of 2 bonded atoms & 2 lone pairs

tetrahedral

molecular shape for 4 bonded atoms & 0 lone pairs

trigonal pyramid

molecular shape for 3 bonded atoms & 1 lone pair

periodic trends of electronegativity

increasing across a period

increasing from bottom to top

high for nonmetals, low for metals

nonpolar covalent bonds

occur between nonmetals by equal/almost-equal sharing of electrons by 2 bonded atoms

polar covalent bonds

usually occur between nonmetal atoms by unequal sharing of electrons

ionic bonds

occur between metal & nonmetal ions by electron transfer

diatomic molecules

H2 (hydrogen)

N2 (nitrogen)

O2 (oxygen)

F2 (fluorine)

Cl2 (chlorine)

Br2 (bromine)

I2 (iodine)

mono-

1

di-

2

tri-

3

tetra-

4

penta-

5

hexa-

6

hepta-

7

octa-

8

nona-

9

deca-

10

OH^–

hydroxide

NH₄⁺

ammonium

NO₃^–

nitrate

NO₂^–

nitrite

ClO₄^–

perchlorate

ClO₃^–

chlorate

ClO₂^–

chlorite

ClO^–

hypochlorite

CO₃^2–

carbonate

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–

phosphite

periodic elements that become cations

metals, group 1A, group 2A, group 3A

periodic elements that become anions

nonmetals, group 5A, group 6A, group 7A

peta- (P)

1×10^15

tera- (T)

1×10^12

giga- (G)

1×10^9

mega- (M)

1×10^6

kilo- (k)

1×10³

deci- (d)

1×10^-1

centi- (c)

1×10^-2

micro- (μ)

1×10^-6

nano- (n)

1×10^-9

pico- (p)

1×10^-12

femto- (f)

1×10^-15

heat of vaporization for water

2260 J/g

540 cal/g

heat of fusion for water

334 J/g

80. cal/g

heat equation

(mass) x (temp change) x (specific heat)

specific heat equation

specific heat = (amount of heat) / (mass x temp change)

calories (cal)

amount of energy needed to raise temp of 1g of water by 1 degree C

absolute zero (0 K)

-273.15 degrees

Celsius to Kelvin conversion

T(K) = T(C) + 273.15

Celsius to Fahrenheit conversion

T(F) = 1.8(T(C)) + 32

Fahrenheit to Celsius conversion

T(C) = (T(F) - 32) / 1.8

periodic trends of ionization energy

low for metals, high for nonmetals

decreases down a group, increases across a period

s sublevel block

group 1A

d sublevel block

group 3B through group 2B

p sublevel block

group 3A through group 8A

number of electrons in sublevel s

1 orbital, 2 electrons

number of electrons in sublevel p

3 orbitals, 6 electrons

number of electrons in sublevel d

5 orbitals, 10 electrons

number of electrons in sublevel f

7 orbitals, 14 electrons

how to name a molecular compound

1st nonmetal gets element name

2nd nonmetal named using 1st syllable of element name with suffix -ide

numeric prefix added when subscript indicates 2+ atoms of the same element

how to name a compound containing polyatomic ions

ends in -ite when related ion has 1 less oxygen

adds +1 to charge when related ion has 1 more hydrogen

name of positive ion followed by name of polyatomic ion

how to name polyatomic ions

ends in -ite when related ion has 1 less oxygen

adds +1 to charge when related ion has 1 more hydrogen

most halogens form 4 polyatomic ions with oxygen

how to name ionic compounds with fixed charge

name of metal comes 1st

1st syllable of nonmetal with -ide ending

how to name ionic compounds with variable charge

roman numeral equal to ion charge placed in parentheses immediately after metal name