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midterm Flashcards

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1
Q

extensive property

A

property that depends on the AMOUNT of matter in a sample

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2
Q

intensive property

A

a property that depends on the TYPE of matter in a sample, not the amount

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3
Q

intensive property example

A

magnetism, thermal conductivity, electrical conductivity, color, melleability, ductility, condensation, luster, state at room temp., density

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4
Q

physical property

A

quality or condition of a substance that can be observed or measured without changing the substances composition

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5
Q

gas to liquid

A

condensation

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6
Q

liquid to solid

A

freezing

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7
Q

gas to solid

A

deposition

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8
Q

liquid to gas

A

boiling

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9
Q

solid to liquid

A

melting

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10
Q

solid to gas

A

sublimation

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11
Q

solid

A

a form of matter that has a definite shame and volume. the shape of a solid doesnt depend on the shape of its container

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12
Q

particles of a solid

A

packed tightly together often in an orderly arrangement

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13
Q

liquid

A

form of matter that has indefinite shape, flows, yet has a fixed volume. liquids volume doesnt change but it takes shape of the container it is in

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14
Q

particles of a liquid

A

close together but are free to flow past one another

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15
Q

gas

A

a form of matter that takes both shape and volume of its container

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16
Q

particles of a gas

A

relatively far apart and can move freely

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17
Q

vapor

A

the gaseous state of a substance that is generally a liquid or solid at room temperature

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18
Q

endothermic processes include:

A

Fusion, vaporization, and sublimation

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19
Q

exothermic processes include:

A

freezing, condensation, and deposition

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20
Q

endothermic

A

a process that requires the absorption of heat

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21
Q

exothermic

A

a process that requires the releasing of heat

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22
Q

increasing the pressure on gas changes the state to a …

A

liquid

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23
Q

increasing the pressure on a liquid changes the state to a….

A

solid

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24
Q

mixture

A

a physical blend of two or more components

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25
Q

heterogenous mixture

A

a mixture in which the composition is not uniform throughout

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26
Q

homogenous mixture

A

a mixture in which the composition if uniform throughout

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27
Q

solution

A

another name for a homogenous mixture

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28
Q

phase

A

any part of a sample with uniform composition and properties

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29
Q

filtration

A

the process that separates a solid from a liquid in a heterogenous mixture

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30
Q

distillation

A

a process that separates water from other components in tap water

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31
Q

element

A

simplest form of matter that has a unique set of properties ( only one type of atom)

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32
Q

compound

A

a substance that contains two or more elements chemically combined in a fixed proportion

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33
Q

can compounds be broken down into simpler substances by chemical means?

A

yes

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34
Q

can elements be broken down into simpler substances by chemical means?

A

no

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35
Q

chemical change

A

a change that produces matter with a different composition than the original matter

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36
Q

chemical property

A

the ability of a substance to undergo a specific chemical change

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37
Q

chemical reaction

A

when the composition of matter changes

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38
Q

possible clues to chemical change include:

A

transfer in energy, color change, gas production, precipitate

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39
Q

precipitate

A

a solid that forms and settles out of a liquid mixture

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40
Q

law of conservation of mass

A

in any physical change or chemical reaction, mass is conserved. mass is neither created nor destroyed

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41
Q

alloy

A

homogeneous mixture of metals

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42
Q

kilo (k)

A

10^3

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43
Q

centi (c)

A

10^-2

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44
Q

milli (m)

A

10^-3

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45
Q

micro (u)

A

10^-6

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46
Q

nano (n)

A

10^-9

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47
Q

1kg =

A

2.2 lbs

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48
Q

1 inch =

A
  1. 54 cm
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49
Q

1 ML =

A

1 cm^3

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50
Q

for multiplying and diving sig figs:

A

round answer to match value with the lowest number of sig figs

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51
Q

for adding and subtracting sig figs:

A

round answer to match value with lowest number of decimal places

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52
Q

accepted value

A

what I SHOULD get for my result

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53
Q

experimental value

A

what I ACTUALLY get

54
Q

error =

A

what you got - what you should get

55
Q

% error formula

A

|error| / accepted value x 100%

56
Q

accuracy

A

how close you are to hitting the target value

57
Q

precision

A

how repeatable your results are

58
Q

0 degrees C =

A

273 Kelvins

59
Q

daltons atomic theory

A

all elements are composed of tiny indivisible particles called atoms, atoms of the same element are identical and the atoms of any one elements are different from those of any other element, atoms of different elements can physically mix together or can chemically combine in simple whole number ratios to form compounds, chemical reactions occur when atoms are separated from each other, joined, or rearranged in a different combination and atoms of one element are never changed into atoms of another element as a result of a chemical reaction

60
Q

JJ thomson

A

discovered the electron using an electric current through gases at a low pressure which resulted in a cathode ray

61
Q

cathode ray

A

a glowing beam that showed how elections exist

62
Q

plum pudding model

A

an atomic model discovered by JJ Thomson, where electrons were stuck into a lump of positive charges and the model was proven wrong by Thomas Rutherford

63
Q

Thomas Rutherford

A

he tested the plum pudding model by using a gold foil alpha particle experiment and his experimented resulted in the founding of the nucleus in an atom

64
Q

atomic number

A

number of protons in an atom

65
Q

mass number

A

number of protons and the number of neutrons in an atom

66
Q

electron symbol, charge, relative mass

A

e- , 1-, 1/1840

67
Q

proton symbol, charge, relative mass

A

p+, 1+, 1

68
Q

neutron symbol, charge, relative mass

A

n0, 0, 1

69
Q

where are protons and neutrons located in an atom?

A

nucleus

70
Q

where are electrons located in an atom?

A

outside the nucleus

71
Q

average atomic mass

A

weighted average of the masses of the different isotopes for an element according to their proportions in nature

72
Q

isotopes

A

atoms of the same element (with the same amount of protons) with different numbers of neutrons or different masses

73
Q

anion

A

negatively charged atom, caused when an atom GAINS electrons

74
Q

cation

A

positively charged atom, caused when an atom LOSES electrons

75
Q

radioisotopes

A

isotopes of an atom with unstable (radioactive) nuclei

76
Q

stable isotopes

A

atoms that DO NOT release protons, neutrons, particles, or energy from the nucleus and ARE NOT radio active

77
Q

unstable isotopes

A

atoms that spontaneously release protons, neutrons, particles or energy from the nucleus

78
Q

alpha radiation

A

least dangerous radiation, least penetrating (paper can block)

79
Q

beta radiation

A

middle dangerous (dense wood can block)

80
Q

gamma radiation

A

most dangerous and most penetrating (walls of lead/concrete can block)

81
Q

alpha radiation symbol, charge, mass #, and identity

A

4He2, +2, 4, helium nucleus

82
Q

beta radiation symbol, charge, mass #, and identity

A

0e-1, -1, 0, electron

83
Q

gamma radiation symbol, charge, mass #, and identity

A

0Y0, 0, 0, photon of light

84
Q

half life

A

the time it takes for 1/2 of a sample to decompose. it Is a constant value of time for that specific isotope, and it is NOT affected by any environmental conditions life temperature, pressure, or humidity

85
Q

fission

A

the splitting of a nucleus into smaller fragments, accompanied by the release of neutrons and a large amount of energy

86
Q

fusion

A

the process of combining nuclei to produce a nucleus of greater mass

87
Q

frequency

A

the number of wave cycles that pass a point in a unit of time (unit: hz)

88
Q

wavelength

A

the distance from a point on one wave to the equivalent point on the next wave (unit: m)

89
Q

energy is ___ proportional to frequency

A

directly

90
Q

wavelength and frequency are ____ proportional

A

inversely

91
Q

energy is ____ proportional to wavelength

A

inversely

92
Q

e- can go from a lower to a higher level by _____ energy

A

absorbing

93
Q

e- can go from a higher to a lower level by ____ energy

A

releasing

94
Q

quantum

A

specific amount of energy between energy levels

95
Q

quantum leap/electron transition

A

electronic transition (e- moving between energy levels)

96
Q

ground state

A

the lowest possible energy level an electron can be at

97
Q

excited state

A

an energy level higher than the ground state

98
Q

orbitals

A

defined regions around the nucleus where e- are likely to be found

99
Q

Aufbau principle

A

e- fill into orbitals from lowest to highest energy

100
Q

Hunds Rule

A

e- will fill equal energy orbitals individually before they will pair up

101
Q

Pauli exclusion

A

2e- in the same orbital must spin opposite of each other and no 2e- can have the same main level, sub level, orbital, and spin

102
Q

column =

A

group and tells you the number of valence electrons

103
Q

row =

A

period and tells you the outermost principle energy level containing electrons

104
Q

metals are:

A

good conductors of heat and electriccurent, have high luster/sheen, solids at room temp, and most are malleable

105
Q

nonmetals are;

A

not good conductors of heat or electricity (except fro carbon) and generally have properties opposite of metals

106
Q

group 1:

A

alkali metals

107
Q

group 2:

A

alkaline earth metals

108
Q

group 17:

A

hallogens

109
Q

group 18:

A

noble gases

110
Q

entire d block:

A

transition metals

111
Q

entire f block:

A

inner transition metals

112
Q

representative elements:

A

form many different chemical compounds and are the entire s & p block elements

113
Q

Mendeleevs original table was organized by:

A

atomic mass and chemical properties

114
Q

elements in same groups have:

A

similar chemical properties

115
Q

metals are located at

A

the bottom left of the PT

116
Q

nonmetals are located at

A

upper right corner of the PT

117
Q

metalloids are located at

A

border the heavy “stair step” line diving metals from nonmetals

118
Q

atomic radius

A

half the distance between the nuclei of two atoms of the same element bonded together

119
Q

atomic radius ___ going down a group

A

increases, because a principle energy level is added with each step

120
Q

atomic radius ____ going across a period

A

decreases, because the combination of more protons in a nucleus and more electrons in valence level cinches atom in

121
Q

cations are ____ in radius than their neutral atom

A

smaller

122
Q

anions are ____ in radius than their neutral atom

A

bigger

123
Q

ionization energy

A

the amount of energy required to remove the first outermost electron from an energy

124
Q

ionization energy ____ going down a group

A

decreases, because the outermost electrons are further away from the nucleus

125
Q

ionization energy ____ going across a period

A

increases because the greater attractive pull on valence electrons because more protons are added to the nucleus

126
Q

Coulombs law

A

attractive force is directly proportional to an amount of a charge and inversely proportional to the distance between charge

127
Q

force is ___ proportional to magnitude of charge

A

directly

128
Q

force is ____ proportional to the distance between charges

A

inversely

129
Q

electronegativity

A

attraction that an atom has for ANOTHER atoms electrons (same direction of trend as IE)

130
Q

____ is the most electronegative atom

A

fluorine

131
Q

noble gases ____ have a defined electronegativity

A

DONT because they aren’t reactive so they don’t form bonds so they don’t need electrons

132
Q

the higher the IE the ____ the electronegativity

A

higher

chemistry (9 decks)

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