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10th grade > chem final > Flashcards

chem final Flashcards

1
Q

to convert from one resonance structure to another, _

A

only electrons can be moved

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2
Q

elements _ exhibit similar physical and chemical properties

A

in the same group on the periodic table

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3
Q

group periodic table

A

vertical and down (same physical and chemical properties)

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4
Q

periods periodic table

A

across and horizontal and left to right

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5
Q

the gold foil experiment performed in Rutherford’s lab _

A

led to the discovery of the atomic nucleus

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6
Q

valence electron

A

the number of electrons on the outermost shell of an atom

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7
Q

how do u find valence electrons?

A

the number at the top row

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8
Q

alkali metals

A

group 1 metals
1 valence electron
highly reactive
soft (like butter)
low melting points
shiny

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9
Q

alkaline earth metals

A

group 2 metals
2 valence electrons
very reactive but less than alkali metals
harder than alkali metals
higher melting point than alkali metals
metal luster shiny

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10
Q

halogens

A

group 17
7 valence electrons
highly reactive
very colorful

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11
Q

transition metals

A

group 3-12
vary in everything
valence electrons based on orbitals

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12
Q

noble gasses

A

group 18
complete valence shell
highly stable
very unreactive
colorless, odorless, tasteless
low boiling and melting point
nonflammable

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13
Q

metalloids

A

on the line thing
between metals and non metals
metallic luster but brittle
moderate electrical conductivity
low thermal conductivity

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14
Q

nonmetals

A

right of metalloid line

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15
Q

metals

A

left of metalloid line

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16
Q

metalloid line

A

dividing line between metals and nonmetals

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17
Q

electron configuration

A

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 5f14 6s2 6p6 6d10 7s2 7p6

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18
Q

ionic

A

metal + non metal

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19
Q

covalent

A

nonmetal + nonmetal

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20
Q

anion

A

negative charge (right)

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21
Q

cation

A

positive charge (left)

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22
Q

how do u find number of electrons

A

atomic number (bottom left)

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23
Q

how do u find mass number

A

protons + neutrons (top left)

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24
Q

how do u find number of protons

A

atomic number (bottom left)

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25
Q

how do u find number of neutrons

A

mass number - atomic number
top left - bottom left

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26
Q

which is NOT one of the postulates of Dalton’s atomic theory

A

atoms are composed of protons, neutrons, and electrons

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27
Q

which ARE some of the postulates of Dalton’s atomic theory

A

-each element is composed of extremely small particles called atoms
-atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions
-compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms
-all atoms of a given element are identical; the atoms of different elements are different and have different properties

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28
Q

each s-subshell can accommodate a maximum of _ electrons

A

2

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29
Q

if a mixture is uniform throughout and can be separated into other substances by physical means, it is _

A

a homogeneous mixture

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30
Q

homogeneous

A

same thru the whole mixture

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31
Q

heterogeneous

A

different thru the whole mixture

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32
Q

what type of change: tarnishing of silver

A

chemical

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33
Q

what type of change: dissolving sugar in water

A

physical

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34
Q

what type of change: crushing of stone

A

physical

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35
Q

what type of change: melting of lead

A

physical

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36
Q

what type of change: dropping a penny in a glass of water

A

physical

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37
Q

element

A

substance made up of one type of atom

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38
Q

compound

A

a substance that is made up of more than one type of atom bonded together

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39
Q

mixture

A

a combination of two or more elements or compounds which have not reacted to bond together

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40
Q

what type of change: chopping a log into sawdust

A

physical

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41
Q

what type of change: charging a cell phone

A

chemical

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42
Q

what type of change: burning a plastic water bottle

A

chemical

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43
Q

what type of change: the tarnishing of a copper penny

A

chemical

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44
Q

what type of change: the production of hydrogen gas from water

A

chemical

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45
Q

cathode rays are deflected away from a negatively charged plate, leading to the discovery of _

A

negatively charged particles

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46
Q

all atoms of a given element have the same _

A

number of protons

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47
Q

all atoms of a given element can have different _

A

density, mass, number of neutrons, and number of electrons

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48
Q

octet rule

A

atoms try to make their outer shell full

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49
Q

element-mass number

A

element
(top left - mass)
(bottom left - atomic number/number of protons)
(top right - charge)

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50
Q

sig fig rules

A

-All non-zero numbers ARE significant
-Zeros between two non-zero digits ARE significant
-Leading zeros are NOT significant
-Trailing zeros to the right of the decimal ARE significant
-Trailing zeros in a whole number with the decimal shown ARE significant

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51
Q

moles to grams

A

multiply by molar mass

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52
Q

grams to moles

A

divide by molar mass

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53
Q

going TO mole island

A

divide

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54
Q

leaving mole island

A

multiply

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55
Q

atom/molecule to mole

A

divide by 6.022 × 10²³

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56
Q

mole to atom/molecule

A

multiply by 6.022 × 10²³

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57
Q

liter/volume to mole

A

divide by 22.4L

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58
Q

mole to liter/volume

A

multiply by 22.4L

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59
Q

precision

A

how close a measured number is to other measured numbers

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60
Q

accuracy

A

how close a measure number is to the ACTUAL value

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61
Q

an empirical formula always indicates _

A

the simplest whole number ratio of different atoms in a compound

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62
Q

molecular formula

A

how many atoms of each element are in a compound

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63
Q

when a hydrocarbon burns in air, a compound produced is _

A

carbon dioxide and water

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64
Q

synthesis (types of reactions)

A

2 to 1
H + Cl –> HCl

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65
Q

decomposition (types of reactions)

A

1 to 2
HCl –> H + Cl

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66
Q

single replacement (types of reactions)

A

1 is changed around
AlCl + Br –> AlBr + Cl

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67
Q

double replacement (types of reactions)

A

2 are changed around
NaCl + KBr –> KCl + NaBr

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68
Q

combustion (types of reactions)

A

ANYTHING reacts with oxygen

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69
Q

King Henry Died By Drinking Chocolate Milk (0.001 –> 1000)
small to big
(remember to cancel out the units)

A

divide
243 / 100 cm = 2.43m

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70
Q

King Henry Died By Drinking Chocolate Milk (0.001 –> 1000)
big to small
(remember to cancel out the units)

A

multiply
243m x 100 cm = 24300cm

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71
Q

m/s –> km/hr

A

convert m to km
convert s to hr

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72
Q

how do u find the empirical formula?

A
  1. divide each percent by the molar mass
  2. divide the ending molar masses by the smallest molar mass
  3. the number you get goes in the formula
    EX: 3C, 6H, and 2O –> C3H6O2
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73
Q

how do u find the molecular formula?

A
  1. take empirical formula
  2. multiply by molar mass
  3. add the molar masses together
  4. use the given mass and divide it by the molar masses total
  5. multiply the empirical formula by the answer in step 4
    EX: (given-290g/mol)/(calculated thru steps 1-3(58.09g.mol)) = 5
    5 x (C3H6O2) = C15 H30 O10
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74
Q

PV =

A

nRT

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75
Q

pressure x volume =

A

moles of gas x ideal gas constant (0.08206) x temperature in K (C + 273)

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76
Q

crystalline solids _

A

have highly ordered structures

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77
Q

sublimation

A

solid to gas

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78
Q

polar

A

lewis dot is not even, and its strong ish, dipole-dipole

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79
Q

if a lewis dot is even, and there are dots on the outside but not the inside, it is _

A

not polar

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80
Q

if a lewis dot is even, and there are dots in the middle but not the outside, it is _

A

polar

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81
Q

non polar

A

lewis dot is even, and its weak, london dispersion

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82
Q

strong to weak intermolecular forces

A

ionic, hydrogen, dipole-dipole, london dispersion

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83
Q

weak to strong intermolecular forces

A

london dispersion, dipole-dipole, hydrogen, ionic

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84
Q

ionic intermolecular force

A

metal and non metal, or + <–> -

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85
Q

hydrogen intermolecular force

A

Hydrogen + F, N, or O

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86
Q

dipole-dipole intermolecular force

A

polar = non even
<– <–
–> –>
different charge everywhere

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87
Q

london dispersion intermolecular force

A

non polar = even
–> <–
<– –>
same charge everywhere

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88
Q

how does atomic radius increase

A

left and down

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89
Q

how does electronegativity increase

A

up and right

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90
Q

how does ionizing energy increase

A

up and right

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91
Q

bent/angular

A

2 surrounding atoms
1 or 2 lone pairs
<120* if 1 lone pair
<109.5* if 2 lone pairs

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92
Q

trigonal pyramidal

A

3 surrounding atoms
1 lone pair
<109.5*

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93
Q

trigonal planar

A

3 surrounding atoms
0 lone pairs
120*

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94
Q

tetrahedral

A

4 surrounding atoms
0 lone pairs
109.5 degrees

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95
Q

linear

A

2 atoms
180*
2 surrounding atoms w/ 0 lone pairs

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96
Q

non polar covalent number

A

<0.3

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97
Q

polar covalent number

A

0.3 < x < 1.7

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98
Q

ionic number

A

1.7<

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99
Q

deposition

A

gas to solid

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100
Q

changing phases formula (straight line on graph)

A

q = n(ΔH)
q=heat
n=moles of substance
ΔH=mole enthalpy (energy per moles) KJ/mol

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101
Q

ΔH fusion number

A

6.02

102
Q

fusion

A

melting / solid to liquid

103
Q

ΔH freezing number

A

-6.02

104
Q

ΔH vaporization number

A

40.6

105
Q

ΔH condensation number

A

-40.6

106
Q

changing temp formula (diagonal line on graph)

A

q = mCΔT
q=heat
m=mass in grams
C=heat capacity
ΔT=change in temp (final-initial)

107
Q

water specific heat capacity number

A

4.184 J/gxC

108
Q

one significant difference between gases and liquids is that _

A

a gas expands to fill its container

109
Q

1 atm = _ torr

A

760

110
Q

1 atm = _ mmHg

A

760

111
Q

1 atm = _ psi

A

14.7

112
Q

1 atm = _ kPa

A

101.325

113
Q

pressure conversions formula

A

given x (transforming value / given value) = given transformed value

114
Q

in liquids, the attractive molecular forces are _

A

strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other

115
Q

the weakest interparticle attractions occur between particles of a _ and the strongest interparticle attractions exist between particles of a _

A

gas, solid

116
Q

Avogadro’s law

A

volume and number of moles in a gas are directly related

117
Q

inversly related

A

one increase, other decrease

118
Q

directly related

A

one increase, other increase

119
Q

boyle’s law

A

pressure and volume are inversely related

120
Q

charles’ law

A

volume and temp are directly related

121
Q

Gay-Lussac’s Law

A

pressure and temp are directly related

122
Q

gas laws formula

A

PV/T = PV/T

123
Q

gas laws formula: if it’s multiplied, it is _ related

A

inversely

124
Q

gas laws formula: if it’s divided, it is _ related

A

directly

125
Q

STP (standard temp & pressure)

A

273 K
1 atm

126
Q

how do u do gas stoichiometry at STP?

A

g –> mol –> other element mole/current element mole –> volume (22.4L/1mol)

127
Q

how do u do gas stoichiometry not at STP? (ideal gas law formula)

A
  1. convert moles
  2. V = nRT / P
    V = volume
    n = moles
    R = 0.08206
    T = temp in K
    P = pressure
128
Q

mole fraction / partial pressure formula

A

Xi = ni / ntotal
Xi = mole fraction
ni = # of mole component
ntotal = total # of moles

129
Q

partial pressure formula

A

pressure A = ((volume B x pressure B) - (volume C x pressure C)) / volume A

130
Q

beta particle

A

0 / -1 e

131
Q

positron

A

0 / 1 e

132
Q

emission

A

1 / 0 B

133
Q

alpha

A

4 / 2 e

134
Q

triple point

A

solid, liquid, and gas at the same time

135
Q

supercritical fluid

A

liquid and gas at same time

136
Q

molecules with stronger intermolecular forces have higher _ _

A

melting points

137
Q

in general, as activation energy increases, reaction rate_

A

goes down regardless of whether the reaction is exothermic or endothermic

138
Q

exothermic

A

releases heat

139
Q

endothermic

A

absorbs heat

140
Q

the reaction rate depends on _

A

all of the above

141
Q

at equilibrium, _

A

the rates of the forward and reverse reactions are equal

142
Q

first order reaction

A

k[element]^1

143
Q

second order reaction

A

k[element]^2

144
Q

the magnitudes of Kf and Kb depend on the identity of the _

A

solvent

145
Q

the _ is the material that usually decides the solution’s physical state (solid, liquid or gas)

A

solvent
A solution of salt and water, for example, has water as the solvent and salt as the solute.

146
Q

the _ is the product that the solvent dissolves

A

solute
A solution of salt and water, for example, has water as the solvent and salt as the solute.

147
Q

how do u write the equilibrium constant

A

products / reactants

148
Q

specific heat capacity formula

A

q=mcAT
q=energy
m=mass in grams
c=specific heat capacity
AT=temp change

149
Q

the phrase “like dissolves like” refers to the fact that _

A

polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes

150
Q

∆S is _

A

entropy

151
Q

∆H is _

A

enthalpy

152
Q

in general, as temp goes down, reaction rate _

A

goes down regardless of whether the reaction is exothermic or endothermic

153
Q

in general, as temp goes up, reaction rate _

A

goes up regardless of whether the reaction is exothermic or endothermic

154
Q

If the volume of the container is increased (at constant T), the system will shift in the direction that _ the number of moles of gas in the container

A

increases

155
Q

If the volume of the container is decreased (at constant T), the system will shift in the direction that _ the number of moles of gas in the container

A

decreases

156
Q

catalyst

A

reactant –> product

157
Q

intermediates

A

product –> reactant

158
Q

how do u write rate law?

A

rate=k[A]^m[B]^n
k=rate constant
A and B=reactants
m and n=orders (how much they affect the reaction)

159
Q

in general, as temperature goes up, reaction rate _

A

goes up regardless whether the reaction is exothermic or endothermic

160
Q

in general, as temperature goes down, reaction rate _

A

goes down regardless whether the reaction is exothermic or endothermic

161
Q

solution

A

everything is even
homogenous

162
Q

solute + solvent =

A

solution

163
Q

what affects dissolving rate?

A

surface area - substance pulls apart more
stirring - clears dissolved particles out of way and allows water to pull apart rest of substance
temp - high temp means molecules move faster and can pull apart faster

164
Q

concentration

A

how strong a solution is, and how much has been dissolved

165
Q

dilute solution

A

not much has been dissolved

166
Q

concentrated solution

A

a lot has been dissolved

167
Q

molarity definition

A

amount of moles that have been dissolved in a specific volume of a solution

168
Q

molarity formula

A

moles of solute / liters of solution
mol / L

169
Q

dilution formula

A

M1V1 = M2V2
M = molarity
V = volume

170
Q

a solid is formed

A

known as precipiate

171
Q

When two solutions are mixed, there are a few signs that a reaction has actually occurred:

A

a solid, gas, or liquid is formed

172
Q

soluble

A

dissolves in water
aka dissociation

173
Q

insoluble

A

doesn’t dissolve in water
stays as a solid

174
Q

Colligative properties

A

properties that depend on the concentration of the solute dissolved in solvent and that will change the normal properties of the solvent

175
Q

Freezing Point Depression

A

By adding a solute to water, the water will now have a lower freezing point

176
Q

Boiling Point Elevation

A

By adding a solute to water, the water will now have a higher boiling point

177
Q

Electrolytes

A

substance that dissolve into their separate ions and allow water to conduct electricity (ionic)

178
Q

Non-electrolytes

A

substances that dissolve, but do not break into different ions (covalent) (i=1 always)

179
Q

freezing point depression formula

A

∆t = Kf x m x i
∆t = change in freezing point
Kf = -1.86 (freezing point constant for water)
i = van hoff’s factor (number of particles)
m = molality

180
Q

boiling point elevation formula

A

∆t = Kb x m x i
∆t = change in temp
Kb = boiling point constant for water (0.51)
i = number of particles

181
Q

reversible reactions

A

can go in both directions

182
Q

if Keq < 1 and Q > K, _ is favored

A

reverse reaction
more reactants than products

183
Q

if Keq > 1 and Q < K, _ is favored

A

forward reaction
more products than reactants

184
Q

if Q = K, the reaction _

A

is at equilibrium

185
Q

Le Chatelier’s Principle states

A

a system will always try to be at equilibrium

186
Q

what are the 3 ways to stress a system?

A

change pressure, concentration, or temp

187
Q

changing the pressure only affects the system if there is a _

A

gas

188
Q

if the pressure increase, the volume will _

A

decrease
With less volume, the system will move to the side of the reaction that has fewer moles of gas

189
Q

if the pressure decrease, the volume will _

A

increase
With a larger volume, the system will move to the side that has more moles of gas

190
Q

if we increase concentration, there is _ of a substance. the reaction moves in the direction that uses up the _

A

extra

191
Q

if we decrease concentration, there is no longer _ of that substance. the reaction moves in the direction to replace the ) substance

A

enough, missing

192
Q

temperature: exothermic
energy is a _

A

product

193
Q

temperature: endothermic
energy is a _

A

reactant

194
Q

decrease temp changes how much _ there is. we do the same thing as with _

A

energy
concentration

195
Q

aq solutions are when ions get _

A

separated

196
Q

In order for a reaction to occur, the molecules must _ in the correct orientation and with enough energy to break the bonds. Once the bonds are broken, new bonds can be formed and a new molecule is made
The energy required to do this is called _ _

A

collide
activation energy

197
Q

what are the several factors that determine how quickly a reaction will take place?

A

nature of reactants
surface area
temp
concentration

198
Q

rate laws are used to determine how _ a reaction can take place

A

quickly

199
Q

Energy flows in or out of a reaction because

A

molecules require energy to keep the atoms bonded together

200
Q

negative ΔH means energy is lost by the system, or is _

A

exothermic

201
Q

positive ΔH means energy is gained by the system, or is _

A

endothermic

202
Q

activation energy (Ea)

A

Minimum energy required for particles to collide and react

203
Q

catalyst

A

speeds up reaction

204
Q

Many reactions do not happen in one single step, but instead require multiple reactions to get the desired results is who’s law?

A

hess’s law

205
Q

rate determining step

A

slowest step in reaction

206
Q

slowest step in diagram has highest

A

activation energy

207
Q

the entropy of a pure crystalline substance at absolute zero is _

A

0

208
Q

entrophy meaning

A

the measure of randomness in a system

209
Q

standard entropies increase with _

A

molar mass and number of atoms

210
Q

For a reaction to be spontaneous, it means that the reaction can happen without any _

A

outside influence

211
Q

In order for a reaction to be spontaneous, ∆Suniverse must be

A

positive

212
Q

∆G means _

A

Gibb’s free energy

213
Q
A
214
Q

∆G formula

A

∆G = ∆H - T∆S
free energy = enthalpy - temp in K x entropy

215
Q

whats an acid?

A

a substance that has an H+ ion

216
Q

whats a base?

A

produces OH- and accepts H+

217
Q

what are Conjugate pairs?

A

shows us how a reactant changes to become a product (follow the anion)

218
Q

conjugate base

A

the substance created after H+ has been donated (removed)
anion of acid
paired with acid

219
Q

conjugate acid

A

the substance created after H+ has been accepted (added)
made from base
paired with base

220
Q

_ has a pH of 7

A

pure water

221
Q

< 7pH

A

acidic
more hydrogen

222
Q

> 7pH

A

basic
more hydroxide

223
Q

A strong acid produces a _ conjugate base
We say the _ reaction is favored

A

weak
forward

224
Q

A weak acid produces a _ conjugate base
We say the _ reaction is favored

A

strong
reverse

225
Q

Titration

A

is a controlled addition and measurement of a solution with a known concentration to react with a solution of unknown concentration

226
Q

Standard solution

A

a solution in which we know the concentration

227
Q

Equivalence point

A

point at which there are equal amounts of moles of each solution

228
Q

Endpoint

A

the point in the titration where the indicator has changed color

229
Q

Indicator

A

a substance used to show when the is a change in pH (going from basic to acidic or from acidic to basic)
Most common is phenolphthalein
Turns pink when solution becomes basic

230
Q

Electrochemistry

A

the study of the relationships between electricity and chemical reactions

231
Q

chemical cell

A

a battery, where two different metals are used.
One metal will oxidized and the other metal will be reduced.
A battery “dies” when this process can no longer be continued.

232
Q

redox reaction

A

one substance undergoes reduction and the second substance is oxidized, both of which happen because of a change in number of electrons

233
Q

If the oxidation number decreases for an element, that element is _

A

reduced

234
Q

If the oxidation number increases for an element, that element is _

A

oxidized

235
Q

oxidation numbers: elements, not ion form

A

0

236
Q

oxidation numbers: monatomic ion (ion of one type of atom

A

charge

237
Q

oxidation numbers: F (when in a compound)

A

-1

238
Q

oxidation numbers: O

A

–2 (unless peroxide = –1) (when in a compound)
you know it’s peroxide based on the cation it is bonded with

239
Q

oxidation numbers: H

A

+1 (unless a metal hydride = –1) (when in a compound)

240
Q

The sum of the oxidation numbers equals the overall charge:

A

(0 in a compound)

241
Q

a species is _ when it loses electrons

A

oxidized

242
Q

a species is _ when it gains electrons

A

reduced

243
Q

how do u balance redox equations

A
  1. make 2 half reactions (oxidation and reduction)
  2. balance the atoms other than O and H first
  3. balance O using H2O and H using H+
  4. add electrons to balance charges
  5. Multiply by common factor
    to make electrons in half-
    reactions equal.
  6. Add the half-reactions.
  7. Simplify by dividing by common factor if necessary.
  8. Double-check atoms and charges balance!
244
Q

voltaic cell other name

A

galvanic cell

245
Q

voltaic cell oxidation occurs at the _

A

anode

246
Q

voltaic cell reduction occurs at the _

A

cathode

247
Q

voltaic cell meaning

A

a device that generates electrical energy thru a chemical reaction

248
Q

_ are formed in the anode compartment as the metal dissolves

A

cations

249
Q

As the electrons reach the cathode, cations in solution are attracted to
the now negative _

A

cathode

250
Q

The potential difference between the anode and cathode in a cell is called the _.
It is also called the cell potential and is designated Ecell.
For a spontaneous cell, the cell potential must be positive

A

electromotive force
EMF
measured in volts (V)

251
Q

The more positive the value, the more likely the reaction is to occur as written
So to decide which substance is more likely to reduce, look for the one with the larger _

A

E°

252
Q

The cell potential at standard conditions can be found through this equation:

A

Ecell = Ered (cathode) – Ered (anode)

10th grade (23 decks)

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