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chem test Flashcards

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1
Q

what is an element

A

pure substance that cannot be broken down

one type of atom

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2
Q

what is a compound

A

pure substance with 2+ different atoms

can be broken down chemically

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3
Q

physical vs chemical property

A

chemical is determined after undergoing a chemical reaction/ forming a new substance

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4
Q

physical vs chemical change

A

physical is state or form, chemical is rearrangement of atoms and new substance

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5
Q

some properties of metals

A 
lustrous or dull
good conductors 
solids at room temp
malleable and ductile
high melting and boiling
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6
Q

some properties of non metals

A 
low or no luster
suck at conducting 
solids or gases
brittle solids
low to moderate melting and boiling
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7
Q

properties of metalloids

A 
lustrous or dull
some are semiconductors 
solids
brittle sometimes
moderate melting and boiling
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8
Q

how do transition metals form ions

A

with multiple charges

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9
Q

smallest unit of an element

A

atom

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10
Q

lose two electrons, what is the charge

A

+2

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11
Q

an atom is electrically neutral if

A

of electrons = # of protons

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12
Q

metals lose electrons to form:

A

cations

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13
Q

non metals gain electrons to become:

A

anions

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14
Q

atomic number represents the number of:

A

protons (and electrons if neutral)

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15
Q

atomic mass:

A

protons and neutrons together

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16
Q

atomic symbol of chlorine:

A

Cl

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17
Q

iupac name for Au 3+

A

gold (iii)

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18
Q

iupac name for calcium ion

A

literally just calcium lol

suck it

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19
Q

prefix for seven

A

hepta

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20
Q

bohr model of the atom, planetary model. list ways it contributed.

A
  1. electron orbits around nucleus
  2. each orbit of electrons corresponds to energy levels
  3. the farther the electron is from the nucleus, the greater it’s energy
  4. electrons don’t lose energy travelling in energy levels
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21
Q

lewis symbols are convenient bc

A

they simply have the chemical symbol and a dot for each VALENCE electron

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22
Q

noble gases are fancy bc they’re:

A

stable. don’t need to lose or gain electrons

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23
Q

iso-electronic:

A

different atoms w the same number of electrons

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24
Q

bohr rutherford diagrams

A

Be 2e 2e

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25
Q

Isotope:

A

same element, different number of neutrons.

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26
Q

isotopes have the same number of protons but different masses bc:

A

atomic mass is determined by protons and neutrons, and isotopes have diff numbers of neutrons

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27
Q

atomic number vs atomic mass

A

number of protons vs number of protons and neutrons

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28
Q

ionic compound vs molecular compound

A

molecular shares electrons, ionic lends them

molecular: NON metals
ionic: metal + non metal

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29
Q

ionic bond:

A

electrostatic force from transferring electrons

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30
Q

some properties of ionic compounds

A 
hard brittle solids
crystal lattice structure 
DO NOT EXIST AS NEUTRAL MOLECULES
strong ionic bonds=high melting points
soluble in water
conduct electricity
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31
Q

electrolytes:

A

substances that conduct electricity when dissolved in water

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32
Q

molecular compounds are formed by the joining of

A

neutral atoms (to form a molecule)

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33
Q

bonding pair:

A

a pair of electrons holding two atoms together

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34
Q

lone pair:

A

electrons not involved in a bond

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35
Q

single, single, triple covalent bond

A

one, two, three shared pairs

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36
Q

steps for drawing lewis structures of molecular compounds

A
  1. count valence electrons for all atoms
  2. central atom will need most electrons
  3. place bond between central atom and each surrounding atoms to connect them
  4. lone pairs around all surrounding atoms (not H)
  5. (optional): if central atom doesn’t have full octet or electrons are remaining, add them as line pairs around central atom
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37
Q

electronegativity

A

tendency of an atom to attract a shared pair of electrons

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38
Q

electrons are shared equally (electronegativity):

A

non polar covalent bond

electronegativity difference is less than 0.4

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39
Q

electrons are shared unequally (electronegativity):

A

polar covalent bond

electronegativity difference is 0.4 or higher, less than 1.7

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40
Q

in ionic bonding, electrons are transferred. if the electronegativity diff between two atoms is ___ or higher, the bond is ___

A

1.7, ionic

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41
Q

some properties of molecular compounds

A 
solids liquids or gases
composed of neutral atoms 
melting and boiling low to moderate 
some are soluble in water
don’t conduct electricity 
NON electrolytes
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42
Q

prefix for 3

A

tri

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43
Q

when do you put prefixes?

A

molecular binary compounds only

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44
Q

prefix for nine

A

nono

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45
Q

prefix for 4

A

tetra

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46
Q

if compound has H before, it is an

A

acid

HCl = hydrochloride acid

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47
Q

tertiary acids: change ite to ___ and ___ to ic.

A

ous, ate

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48
Q

law of conservation of mass

A

matter is not created or destroyed

mass of reactants = mass of products

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49
Q

chemicals do NOT destroy or change ___ into other ___

A

atoms into other atoms

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50
Q

balanced version of

H2 (g) + O2 (g) = H2O

A

2H2 (g) + O2 (g) = 2H2O (l)

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51
Q

what state is a solution or acid

A

aq

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52
Q

synthesis reaction

A

two reactants, ONE new compound

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53
Q

decomposition reaction

A

compound breaks into two or more elements/compounds

54
Q

reaction with oxygen: complete combustion

A

hydrocarbons + crapload of oxygen = ONLY carbon dioxide and water.

55
Q

reaction with oxygen: incomplete combustion

A

hydrocarbons + smaller crapload of oxygen = 1+ of the following: CO2, CO, soot

56
Q

when reacting with oxygen, what is always a product (to account for hydrogen)

A

water

57
Q

reaction with oxygen: metals

A

form metal oxides or peroxides

58
Q

reaction with oxygen: nonmetal

A

nonmetal oxides

59
Q

reaction with oxygen: nonmetal oxides

A

produce other nonmetal oxides

60
Q

single displacement:

A

ELEMENT + COMPOUND = new element + new compound

61
Q

corrosion:

A

breakdown of metal resulting from reactions

62
Q

metals that don’t corrode

A

gold, platinum

63
Q

double displacement

A

two compounds = two new compounds

64
Q

double displacement: precipitation

A

two new compounds, one being precipitate.

precipitate= insoluble in solubility table

65
Q

double displacement: acid base neutralization

A

acid + base = water and a salt

if base is carbonate, CO2 is also produced

66
Q

mole:

A

unit of measurement

mole of one substance is atomic mass

67
Q

avodragos number

A

6.02 x 10 to the 23rd

68
Q

molar mass

A

mass of one mile of any substance in g/mol

69
Q

n = what

A

number of mol

70
Q

M =

A

molar mass

71
Q

m =

A

mass of sample

72
Q

N =

A

number of entities (u/molecules/atoms)

73
Q

NA =

A

6.02 x 10 to the 23rd entities/mol

74
Q

n = m/?

A

n = m/M

75
Q

n = ?/NA

A

n = N/NA

76
Q

m/? = N/NA

A

m/M = N/NA

77
Q

formula for stoich

A

given amount, convert to moles, molar mass, convert to desired units

78
Q

ALWAYS BALANCE THE

A

EQUATION

79
Q

AFTER ELEMENTS/COMPOUNDS, ADD

A

STATES

80
Q

the ostwald process:

A

used for making nitric acid

important for the time
fundamental change in agriculture

81
Q

properties of acids

A 
corrosive
sour tasting
release hydrogen ions when dissolved
pH is LESS THAN SEVEN
electrolytes
82
Q

properties of bases

A 
corrosive
bitter tasting 
release hydroxide ions when dissolved
pH GREATER THAN SEVEN
electrolytes
83
Q

ionization:

A

molecular compounds dissolve to produce ions

84
Q

dissociation:

A

ionic compounds dissolve to produce ions

85
Q

Arrhenius’s theory of acids and bases:

A

acids are substances that dissociate in water to yield ions

86
Q

pH:

A

measure of the concentratipn of hydrogen ions

87
Q

pH scale:

A

measures the level of acidity and basidity

88
Q

pH scale goes from 0-14. 14 is lowest ___ and highest ___

A

lowest acidity, highest basidity

89
Q

from pH level 7 to 6, it gets ___ more acidic.

A

10x

90
Q

pH level 0 (battery acid) formula

A

H > OH

91
Q

pH level 7 (fresh water) formula

A

H = OH

92
Q

pH level 14 (drain cleaner) formula

A

H < OH

93
Q

pH of 11 is

A

moderately basic

94
Q

pH of 2 is

A

very acidic

95
Q

strong ACIDS ___ completely

A

ionize

96
Q

weak ACIDS ___ partially

A

ionize

97
Q

strong BASES ___ completely

A

dissociate

98
Q

weak BASES partially react with

A

water

99
Q

strong and weak acids and bases of similar concentration have ___ properties

A

different

100
Q

acid base indicators (red cabbage) are chemicals that

A

change colour when reacting with bases or acids

101
Q

acid base indicators change ___ with different pH levels

A

colour

102
Q

nonmetal oxides react with water to form

A

acids

103
Q

metal oxides react with water to form

A

bases

104
Q

phosphoric acid is used in

A

soft drinks

105
Q

windex is

A

ammonium hydroxide

106
Q

how to determine the pH of a solution

A

acidic: H > 1 x 10 to the -7
basic: H < 1 x 10 to the -7

107
Q

if you are given the H+ in mol/L, what formula

A

pH = -log(1x10 to the -6)

108
Q

what is the pH of a solution with a H+ of 4.7 x 10 to the -11 mol/L

A

10.3

109
Q

how to convert pH to H+

A

inverse log of the - pH

H = 10 to the -9 = 1 x 10 to the -9 mol/ L

110
Q

what is the H+ of a solution with a pH of 2.8

A

1.6 x 10 to the -13 mol/L

111
Q

how can the pH of a solution be changed

A

adding acid, base, or water

112
Q

pH of normal rainwater, 0.0000026 mol/L

A

5.6

113
Q

hydrogen concentration of drain cleaner, pH of 14

A

1 x 10 to the -14 mol/L

114
Q

titration:

A

lab to find unknown concentration

115
Q

CA VA = CB VB

c = n/v

NA = NB

A

titration formula

116
Q

random example of acid base neutralization

A

baking: baking powder contains tartaric acid and sodium bicarbonate
bubbles of CO2 allow cake to rise as it bakes

117
Q

acid precipitation

A

any form of precipitation that becomes acidic from reaction the compounds in the atmosphere

118
Q

titration

A

process where a solution of known strength is added to a certain volume of a treated sample containing an indicator.

119
Q

can two atoms be isotopes if they have different atomic numbers but same atomic masses?

A

no. their masses can be different but their atomic numbers must be the same.

120
Q

if a lewis structure is of an ion, you must include the ion change of the

A

electrons

121
Q

determine the bond type for O-O

A

electronegativity difference: 3.5 - 3.5 = 0

non polar bond

122
Q

what is the bond type for S-Cl

A

electronegativity difference: 3-2.5=0.5

polar

123
Q

bond type of Na-O

A

electronegativity difference: 3.5 - 0.9 = 2.6

124
Q

differences between ionic and molecular compounds: PROPERTIES

A

ionic: high melting point, conduct electricity
molecular: low to moderate melting point, nonelectrical conductors

125
Q

differences between ionic and molecular compounds: ELECTRONS

A

ionic: TRANSFER of electrons (metals to non metals)
molecular: electrons SHARED between nonmetals

126
Q

what’s the difference between a strong and weak acid

A

strong acids ionize almost completely so there is a greater concentration of H+ ions, lower pH, and are more corrosive.

127
Q

neutral solutions have a pH of

A

7

128
Q

a solution with a pH of 4 has. a greater H+ than __

A

OH.

129
Q

the diatomic elements

A

HOFBrINCl

130
Q

what does HOFBrINCl stand for

A 
diatomic elements 
hydrogen
oxygen
fluoride
bromine
iodine
nitrogen
chlorine
131
Q

how many reactions in the ostwald process

A

three

132
Q

rate of reaction

A

time it takes for a given amount of product/reactants to react or form

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