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Chemistry H > FINALS! > Flashcards

FINALS! Flashcards

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1
Q

homogeneous

A

same properties throughout

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2
Q

heterogeneous

A

different properties in different parts of mixture

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3
Q

elements

A

cannot be broken down chemically into simpler substance

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4
Q

compounds

A

can be broken down chemically into elements

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5
Q

precision

A

degree of agreement among several measurements of the same quality

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6
Q

accuracy

A

the agreement of a particular value with the true value

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7
Q

sigfig zero rules

A
  • non-zero always count as sigfigs

a) leading 0s never count
2) captive 0s always count
3) trailing 0s only included if theres decimal points

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8
Q

density formula

A

mass/volume

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9
Q

atomic number

A

protons/electrons

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10
Q

atomic mass

A

protons + neutrons

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11
Q

ground state orbitals

A

lowest energy level/orbital

can be moved up by heat, electricity, light (excited)

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12
Q

quantum mechanics

A

how small particles behave

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13
Q

energy levels

A

measures fixed energy e-

since e- cannot exist between rungs, a quantum is the exact energy needed to move an e- up a rung

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14
Q

principal quantum number

A

denotes the energy level e- is located in
max in an energy level: 2n^2

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15
Q

aufbau

A

electrons enter the lowest energy level first

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16
Q

pauli exclusion

A

2 electrons max per orbital

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17
Q

hund’s rule

A

electrons don’t pair up unless they have to

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18
Q

alkali metals

A

group 1
most reactive
not found in nature
reacts with air and water

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19
Q

alkaline earth metals

A

group 2
reactive, but not as much as alkali

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20
Q

transition metals

A

group 3-12
all metals
least reactive on periodic table
found in nature

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21
Q

rare earth metals

A

bottom 2 rows

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22
Q

lanthanides

A

1st bottom row on periodic table
soft metals, not that rare

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23
Q

actinides

A

2nd bottom ro won periodic table
radioactive, synthetic

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24
Q

halogens

A

group 17
most reactive nonmetals

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25
Q

noble gases

A

group 18
rarely combine - low reactivity

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26
Q

group on periodic table

A

up & down, column

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27
Q

period on periodic table

A

left & right, row

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28
Q

atomic radius trend

A

1) increases down a group
2) decreases across a period

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29
Q

electronegativity trend

A

1) decreases down a group
2) increases across a period

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30
Q

ionization energy trend

A

1) decreases across a group
2) increases across a period

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31
Q

ion size trend

A

1) larger when anion (gain electron)
2) smaller when cation (lose electron)

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32
Q

metallic character trend

A

1) increases down a group
2) decreases down a period

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33
Q

ionic bond

A

attractions between oppositely charged ions

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34
Q

covalent bond

A

2 nonmetals bonding by sharing electrons

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35
Q

non-polar covalent

A

equal sharing of electrons

diatomic molecules

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36
Q

polar covalent

A

unequal sharing of electrons
electrons spend more time around the nonmetallic tom

charge seperation - dipole movement

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37
Q

metallic bonds

A

electrostatic attraction between cations (2 metals)

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38
Q

covalent network solids

A

combinations of nonmetals

hard and brittle
extreme melting and boiling points
interconnected, insoluble

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39
Q

1 central, 2 atoms

A

linear

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40
Q

1 central, 3 atoms

A

trigonal planar

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41
Q

1 central, 4 atoms

A

tetrahedral

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42
Q

1 central + 1 lone pair, 2 atoms

A

bent

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43
Q

1 central + 1 lone pair, 3 atoms

A

trigonal pyramidal

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44
Q

1 central + 2 lone pairs, 2 atoms

A

bent

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45
Q

polar bond vs polar molecule

A

polar bond: unequal sharing of e-

polar molecule: non symmetrical shape, lone pair on central atom

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46
Q

non polar bond vs non polar molecule

A

nonpolar bond: equal sharing of e-

nonpolar molecule: symmetrical molecular shape

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47
Q

hydrogen bonds

A

dipole-dipole
strong intermolecular froce
occurring between hydrogen atoms with fluorine, oxygen, nitrogen

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48
Q

type 1 binary compound

A

metal present forms 1 type of cation

1) cation first, anion 2nd
2) cation has same name elemtn
3) anion + root ide

49
Q

type 2 binary compound

A

metal present forms 2+ cations with diff charges

1) metal cation has more than 1 valence number
2) group 1&2 always type 2
3) transition metals almost always type 2
4) roman numeral placed to indicate valence

50
Q

mercury exception (type 2 binary compound)

A

roman numeral refers to subscript b/c mercury I and mercury II both have valence of 2+

51
Q

type 3 binary compound

A

2 nonmetals

1) named with full element
2) prefixes denote # of atoms present
3) mono never used for first element

mono:1
di:2
tri:3
tetra:4
penta:5
hexa:6
hepta:7
octa:8

52
Q

empirical formula

A

lowest whole number ratio of atoms in a compound

53
Q

molecular formula

A

the true number of atoms of each elements in the formula

54
Q

empirical & formula proccess

A

1) get the % of eachh part
2) divide by molar mass
3) divide by smallest
4) round

55
Q

A + X -> AX

A

synthesis/combination

56
Q

AX -> A + X

A

decomposition

57
Q

A + BX -> AX + B

A

single replacement reaction

58
Q

AX + BY -> AY + BX

A

double replacement

59
Q

CxHy + O2 -> CO2 + H2O

A

combustion
substance + oxygen –> energy (light, heat)

60
Q

evaporation

A

when liquid converts to gas when the liquid is NOT boiling (on the surface)

61
Q

boiling

A

a conversion of a liquid to a gas or vapor through the whole substance

62
Q

vaporization

A

conversion of ANY liquid molecule into a gas molecule

63
Q

q = m * cp * ∆T

A

q = thermal energy
m = mass (g)
cp = specific heat
∆T = change in temp

64
Q

cp of h2o

A

4.184 J/gºK

65
Q

heating curves, increasing sections

A

q = m * cp * ∆T
endothermic

66
Q

heating curves, plateaus

A

1) melting: q = mol * ∆Hfus
2) boiling q = mol * ∆Hvap

67
Q

kinetic theory of gases

A

1) gases are mostly empty space - no forces of attraction or repulsion
2) gases are in constant motion
3) collisions between gas particles are perfectly elastic

68
Q

boyles law

A

inverse
p1v1=p2v2

69
Q

charles law

A

proportional
v1/t1 = v2/t2

70
Q

gay-lussac law

A

proportional
p1/t1=p2/t2

71
Q

ideal gas law

A

PV=nRT

V = L
n = moles
R = gas constant
T = K = C+273

72
Q

stp

A

1 atm = 101.3 kPA = 760 mmHg

73
Q

dalton’s law of partial particles

A

p total = p1 + p2 + p3

74
Q

diffusion

A

effusion: passage of gas particles through a small opening
diffusion: the moment of particles for regions of high concentration to low concentration

75
Q

grahams law

A

rate1/rate2 = sqrt (m2/m1)

76
Q

ideal gas

A
  • no volume, no attraction/repulsion, all collisions are elastic

don’t exist
closest at low pressure and high temperature.

77
Q

properties of water

A
  • universal solvent
  • bent, v-shaped, 105
  • polar bonds (covalent between o-h)
  • oxygen slightly negative, hydrogen slightly positive
  • water molecules cant form h-bonds with air molecules, only attracted to h-bonds in the body of the liquid
78
Q

colloids

A

milky and cloudy

79
Q

surface tension

A

molecules @ top are only pulled to inside
molecules in middle are attracted in all directions
causes droplets to minimize surface area

80
Q

degree of solubility

A

1) nature of solute & solvent “like dissolves like”
2) temperature: increase temp increase solubility
3) pressure (FOR GASES) increase pressure, increase solubility

81
Q

rate of solution

A

1) increase TEMP, dissolve faster b/c kinetic energy
2) smaller PARTICLES dissolve faster
3) STIRRING dissolves faster bc concentration gradient
4) already dissolved solute dissolves slower bc less concentration gradient

82
Q

gas in liquid solubility

A

1) temperature: increase temp, less gas dissolved
2) pressure: increase pressure, more gas dissolved

(solids more soluble as temp increases / gas less soluble as temp increases)

83
Q

solubility curves

A

unsatured: more solute dissolves
saturated: no more solute dissolves
supersaturated: unstable, crystals form

84
Q

molarity

A

moles of solute/liters of solution

85
Q

molality

A

moles of solute/kg of solvent

86
Q

dilutions

A

made by adding more solvent to a solution
moles o/solute before dilution = moles o/solute after dilution

only concentration changes

m1v1=m2v2

87
Q

colligative properties

A

boiling point elevation
freezing point depression

88
Q

boiling point elevation

A

∆tb = i * kb * m

∆Tb = change in boiling point
I = # of subatomic particles
kb = molal boiling point constant (0.512 for water)
m = molality

89
Q

freezing point depression

A

∆Tf = i * kf * m

∆Tf = change in freezing pt
i = # of subatomic particles
Kf = molal freezing point constant (1.86 for water)
m - molality

90
Q

potential energy

A

stored energy

91
Q

kinetic energy

A

energy of motion

92
Q

temperature vs heat

A

temp: measure of the average kinetic energy of random motions of particles in substances

heat: measure of the total amount of energy

93
Q

specific heat capacity

A

amount of heat needed to increase temp of 1g of a substance by 1c

q = m * cp * ∆T

q = joules
m = mass
cp = specific heat
∆t = change in temp

94
Q

enthalpy

A

heat of fusion: energy needs to melt one mole
heat of vaporization: energy needed to boil one mole

95
Q

collision theory

A

1) frequency of collisions: high # of collisions needed for reactions to occur
2) effectiveness of collisions: particles collide at proper angles & enough energy

96
Q

rates of reaction

A

1) inc temp, inc rate
2) inc concentration, inc rates
3) inc pressure, inc rate
4) dec particle sizxe
5) cataylsts

97
Q

la chatelier’s pirnciple

A

if stress is applied to a system at equilibrium, the system changes to relieve the stress to establish a new equilibrium

98
Q

stress

A

1) change in concentration
2) change in temp
3) change in pressure

99
Q

stress
A + B <-> C + D

A

increase A or B shifts right (makes more products)
decrease A or B shifts left (makes more reactants)

100
Q

endo/exo stress
A+B <-> C+D

A

A+B <-> C+D + heat
exothermic, shifts right

A+B+heat <-> C+D
endothermic, shifts left

101
Q

Keq

A

equilibrium constant
[products]/[reactants]

([C]^c * [D]^d)/([A]^a * [B]^b)

exclude solids and pure liquids

102
Q

keq><=1

A

Keq>1, products favored
Keq=1, neither favored
Keq<1, reactants favored

103
Q

acid basic properties

A

changes litmus red
produces H+ when dissolved in water

104
Q

naming acids

A

1) -ide → starts with hydro, suffix ic, end acid
2) -ite → suffix ous, end acid
3) -ate → suffix ic, end acid

105
Q

base basic properties

A

changes litmus blue
produces OH- when dissolved in water

106
Q

bronsted-lowry acids

A

acid: H+ donor (proton donor)
base: H+ acceptor (proton acceptor)

HBr+H2O <-> H3O+ + Br-
acid. base.

107
Q

conjugate acid-base paris

A

2 substances that differ by 1 H+

acid -> conjugate base
H2O -> OH-

base -> conjugate acid
NH3 -> NH4+

108
Q

acid strenght

A

strong acids completely dissociate in water
HCl -> H+ + Cl-

weak acids only partially ionize in ater
H3COOH (aq) <-> CH3COO-(aq) + H+

109
Q

neutralizing reactions

A

all neutralization runs are double replacement
salt is an ionic compound formed form an acid (anion) and base (cation)

110
Q

normality

A

normality (N) is a unit of concentration in acid-base titrations
N1V1=N2V2

acids
monoprotic (N) = (M)
diprotic N=2M
triprotic N=3M

bases
1 OH- ion N=M
2 OH- ion N=2M
3 OH- ion N=3M

111
Q

buffers

A

solutions that resist changes in pH
the buffer cannot control the pH when too much acid/base is added

112
Q

titrations

A

a method to determined the concentration of a solution using neutralizing reactions

113
Q

titration indicators

A

indicators: added to signal when neutralization has occured
changes color @ end point
neutralization @ equivalence point

114
Q

titration curves

A

1) weak acids neutralized by strong bases produce basic salt solutions
2) strong acids neutralized by weak bases produce acidic salt solutions
3) strong acids neutralized by strong bases produce neutral salt solutions

115
Q

oxidation

A

loss of electrons (atoms becomes more positive)

116
Q

reduction

A

gain of electrons (atoms became more negative)

117
Q

oxidizing agent

A

causes oxidation of another element, gets reduced

118
Q

reducing agent

A

causes reduction of another element, gets oxidized

119
Q

redox

A

reactions with reduction and oxidation

synthesis, decomposition, single reaplcement
NOT double replacement, neutralization

Chemistry H (11 decks)

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