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10th grade > chem test 4 > Flashcards

chem test 4 Flashcards

1
Q

nuclear reactions

A

reaction that affects the nucleus of an atom

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2
Q

nuclear fission

A

heavy nucleus splits into more stable nuclei, occurs in bombs/reactors, low mass combines to form more stable and heavier atom, happens in stars

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3
Q

chain reactions

A

starting material is made as product so reaction continues to happen

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4
Q

alpha

A

particle w/ 2 protons and 2 neutrons bound together and had positive charge. similar to helium. lowest penetrating abilities. 4/2He and 4/2a.

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5
Q

beta

A

an electron. more power than alpha. has negative charge. 0/-1B or 0/-1e.

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6
Q

positron (beta positive)

A

positivity charged beta particle. 0/+1e

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7
Q

neutron

A

has symbol 1/0n

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8
Q

gamma y

A

no mass and no charge. js energy. highest penetrating power. 0/0y

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9
Q

balancing nuclear reactions

A

mass number and atomic numbers on each side must be equal.

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10
Q

what radiation has the greatest penetrating power?

A

gamma

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11
Q

least penetrating power to the greatest penetrating power

A

alpha particle, gamma ray, beta particle

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12
Q

in order of increasing mass

A

electron → proton → alpha particle

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13
Q

What is the mass number of an alpha particle?

A

4

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14
Q

Which of the following particles has the least mass

A

beta

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15
Q

Which nuclear emission has no charge and no mass

A

gamma

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16
Q

Which nuclear emission has the greatest mass

A

alpha

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17
Q

Which type of radiation is identical in mass and charge to a helium nucleus

A

alpha

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18
Q

Which particle has the greatest mass?

A

alpha

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19
Q

Which nuclear decay emission consists of energy, only?

A

gamma

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20
Q

Artificial transmutation is brought about by using accelerated particles to bombard an atom’s

A

nucleus

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21
Q

A beta particle may be spontaneously emitted from

A

an unstable nucleus

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21
Q

A change in the nucleus of an atom that converts the atom from one element to another element is called

A

transmutation

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21
Q

Alpha particles and beta particles differ in

A

D) both mass and charge

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22
Q

What is the name of the process in which the
nucleus of an atom of one element is changed into
the nucleus of an atom of a different element?

A

transmutation

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23
Q

Which of these types of nuclear radiation has the
greatest penetrating power?

A

gamma

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24
Q

radioactive

A

nucleus will spontaneously decompose

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25
Q

alpha decay

A

alpha particle is created

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26
Q

beta decay/beta negative/electron emission

A

beta particle is created

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27
Q

positron decay/beta positive emission

A

positron is created

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28
Q

nuclear decay occurs bc the nucleus of the atom is

A

unstable in current form/radioactive

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29
Q

the nucleus will proceed to transmutate until it is

A

nonradioactive

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30
Q

decay can happen in _ steps. each step can be different type of decay, or take different amount of time bc each has its own half life

A

one or many

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31
Q

half life

A

time required for half of og sample of nuclei to decay

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32
Q

periodic

A

repeatable pattern

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33
Q

atomic radius

A

size of atom, or how far the electrons are from the nucleus

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34
Q

how does atomic radius change

A

down + left +

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35
Q

biggest atomic radius element

A

francium

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36
Q

smallest atomic radius element

A

fluorine

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37
Q

why does atomic radius size decrease as you move to the right and increase as u move down?

A

down = more electron shells and bigger radius
right = less protons so less electrons in nucleus

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38
Q

electronegativity

A

ability of the atom to attract electrons when in a bond with another atom

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39
Q

most electronegative element

A

fluorine

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40
Q

least electronegative element

A

francium

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41
Q

how does electronegativity change

A

up + right +

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42
Q

y is fluorine better at attracting the electrons than francium?

A

the smaller an atom, the closer its electrons are to the nucleus. they are more attracted the closer they are to the nucleus, and vis versa

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43
Q

ionization energy

A

energy needed to lose one electron (creating a cation)

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44
Q

how does ionizing energy increase

A

up + right +

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45
Q

highest ionizing energy element (hard to lose electron)

A

fluorine

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46
Q

lowest ionizing energy element (ez to lose electron)

A

francium

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47
Q

why is it so easy for Francium to lose an electron and so hard for Fluorine to lose an electron?

A

fluorine is the smallest, meaning the electrons are closer to the nucleus and harder to get away, and vis versa

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48
Q

VSEPR

A

valence shell electron pair repulsion

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49
Q

electron pairs around a central atom will…

A

get as far apart from each other as possible

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50
Q

tetrahedral

A

4 surrounding atoms. 0 lone pairs. bond angle 109.5*. AB4

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51
Q

linear

A

180* AB2. 2 atoms are bonded together, or 2 surrounding atoms and 0 lone pairs are bonded.

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52
Q

trigonal planar

A

3 surrounding atoms and 0 lone pairs. bond angle 120*. AB3

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53
Q

trigonal pyramidal

A

3 surrounding atoms and 1 lone pair. <109.5*. AB3E

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54
Q

bent or angular

A

2 surrounding atoms and 1 or 2 lone pairs. <120* if 1 lone pair or much less than 109.5* if 2 lone pairs. AB2E or AB2E2

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55
Q

polarity

A

2 poles

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56
Q

whats a pole

A

poles of a magnet or two sides of different charge

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57
Q

what does it mean if a molecule is polar

A

one region of the molecule has a positive charge, and another has a negative charge (separation of charge)

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58
Q

how do we create polartiy

A

when electrons are shared unequally in a covalent (2 non metals) bond. (electrons are attracted to one atom instead of another)

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59
Q

how do we know which atom the electrons are attracted to in polarity?

A

look at the electronegativity of the atoms

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60
Q

in order to find if a bond is polar, look at the difference between the _ of the two atoms

A

electronegativity

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61
Q

non-polar covalent

A

<0.3 and equal sharing

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62
Q

polar covalent

A

0.3<x<1.7, unequal sharing

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63
Q

ionic

A

<1.7 en

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64
Q

how do u know if a molecule is polar?

A

draw lewis dot and look at the shape. draw arrows facing more electronegative atoms.

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65
Q

dipole movement

A

a measure of how unequal the distribution of electric charge is in a molecule

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66
Q

if arrows point in same direction in dipole movement…

A

they are additive and all electrons move to that side, and we create different charged areas (polar!)

67
Q

if arrows point in opposite direction… (away or towards each other)

A

cancel each other out, the electrons are equally moved around and we have the same charge everywhere (nonpolar!)

68
Q

state of matter: solid

A

molecules are close, locked in place, vibrate, and crystalized in place

69
Q

types of crystalline structures

A

ionic solid, molecular solid, atomic solid

70
Q

ionic solid

A

crystal is made of separate ions and is a repeating pattern of positive and negative ions

71
Q

molecular soild

A

crystal is made of individual molecules that bond together

72
Q

atomic solid

A

crystal is made of individual atoms that bond together

73
Q

liquid

A

molecules are close but can move. they r not stuck together well, and can escape to gas phase (vapor pressure)

74
Q
A
75
Q

Solid

A

molecules are very close connected, and locked in place and can only vibrate to move. they usually form a very specific structure called crystalline solid. (crystalized in place)

76
Q

crystalline structures types

A

ionic solid, molecular solid, atomic solid

77
Q

ionic solid

A

the crystal is made of separate ions, and is a repeating pattern of positive and negative ions

78
Q

molecular solid

A

the crystal is made of individual molecules that bond together

79
Q

atomic solid

A

the crystal is made of individual atoms that bond together

80
Q

liquids

A

molecules are still close to each other but now have more freedom to move. they are not as stuck as solids, and can escape to gas phase (vapor pressure)

81
Q

gases

A

molecules are completely separate and have ultimate freedom to move around. they are independent of each other, and have many properties

82
Q

intermolecular forces

A

the forces that connect and separate molecule of a substance together

83
Q

the stronger intermolecular forces are, the harder it is to…

A

separate the molecules

84
Q

ionic intermolecular force

A

opposite charges on magnets pull on each other

85
Q

hydrogen bonding intermolecular force

A

hydrogen + F, N, or O

86
Q

dipole dipole bonding intermolecular force

A

polar / non even
(one molecule is positive and one is negative)

87
Q

london dispersion bonding intermolecular force

A

non polar / even
(not all molecules have dipole)

88
Q

polarity

A

lewis dot. draw arrows toward more electronegative element, to represent the direction the electrons are moving

89
Q

dipole

A

the arrangement of charges of a molecule. + -. the force between N and S

90
Q

if dipole arrows point in the same direction…

A

they are additive. all electrons move the the same side and different charges are created (polar)

91
Q

if dipole arrows point in different directions (towards or away from each other)…

A

they cancel each other out and the electrons are equally have the same charge everywhere (non polar)

92
Q

polarity

A

the property when there are two poles

93
Q

what is a pole

A

poles of a magnet or two sides of different charge

94
Q

for a molecule to be polar…

A

one side has to have a positive charge and the other negative (separation of charges)

95
Q

how do we create polarity?

A

when electrons are shared unequally in a covalent bond. the electrons are attracted to one atom more than the other

96
Q

how do we know which atom the electrons are more attracted to?

A

the more electronegative one

97
Q

non-polar covalent bond

A

equal sharing; en<0.3

98
Q

polar covalent

A

unequal sharing; 0.3<en<1.7

99
Q

ionic

A

1.7<en

100
Q

VSEPR

A

valence shell electron pair repulsion

101
Q

linear

A
  • 2 atoms 180* AB2
  • 2 surrounding atoms (3 total) 0 lone pairs 180*
102
Q

trigonal planar

A

3 surrounding atoms, 120*, AB3, 0 lone pairs

103
Q

tetrahedral

A

4 surrounding atoms, 0 lone pairs, 109.5*, AB4

104
Q

trigonal pyramidal

A

3 surrounding atoms, 1 lone pair, <109.5*, AB3E

105
Q

bent/angular

A

2 surrounding atoms, 1 or 2 lone pairs
- 1 LP = <120* and AB2E
- 2 LP = <109.5* and AB2E2

106
Q

what does phase diagram show

A

how pressure and temperature affect the 3 phases of matter

107
Q

triple point

A

a point where all 3 phases intersect, solid, liquid, and gas exist at same time

108
Q

critical point

A

liquid and gas coexist in new type of fluid called supercritical fluid

109
Q

melting

A

solid to liquid

110
Q

freezing

A

liquid to solid

111
Q

vaporizing

A

liquid to gas

112
Q

condensation

A

gas to liquid

113
Q

sublimation

A

solid to gas

114
Q

deposition

A

gas to solid

115
Q

joule

A

standard unit of measurement for energy

116
Q

caloire

A

amount of energy required to raise temp of 1 gram of water by 1*C

117
Q

how many cal is 1 J

A

1 cal = 4.184 J

118
Q

potential/stored energy

A

the energy that is bonding atoms and molecules togeether

119
Q

if energy is released…

A

there is less energy stored in the chemical bonds

120
Q

if energy is absorbed…

A

more energy is stored in the bonds

121
Q

evaporation

A

molecules at surface of liquid are able to break free of their forces and turn into gas molecules

122
Q

boiling

A

molecules inside liquid stare can separate and turn into gas molecules

123
Q

specific heat capacity

A

amount of energy required to change the temp of 1 gram of substance by 1*C, and is different for each substance and the state of matter

124
Q

heat curve

A

shows us how a substance is changing phase over time compared to the temperature change, shows what temp a phase change occurs

125
Q

temperature is related to kinetic energy… meaning

A

the faster a molecule moves, the higher the kinetic energy/temp

126
Q

pressure

A

force exerted over an area

127
Q

barometer

A

used to measure pressure from the atmosphere. its filled with mercury

128
Q

how does a gas apply force?

A

the force is when a molecule collides with the side of a container

129
Q

what are the gas laws

A

a way to relate pressure, volume, and temp of a gas. describes how if u change one variable, it will affect the other variables and allow u to see changes in them

130
Q

temperature definition

A

how fast particles move

131
Q

pressure definition

A

how often particles collide with container

132
Q

volume definition

A

how much space particles take up

133
Q

boyles law

A

there’s a connection between pressure and volume. they are inversely related, so if u increase one the other will decrease

134
Q

charles law

A

there is a connection btwn volume and temp. they are directly related, so if u increase one then the other will also increase

135
Q

directly related meaning

A

if u increase one factor, the other will also increase

136
Q

inversely related meaning

A

if u increase one part, the other will decrease

137
Q

gay lussac’s law

A

there is a connection btwn pressure and temp. pressure and temp are directly related. one increase the other increase

138
Q

combined gas law

A

pressure(1) x volume(1) / temp(1) = pressure(1) x volume(2) / temp(2)

139
Q

more pressure means ___ collisions

A

more collisions

140
Q

less volume means __ pressure

A

more pressure

141
Q

more temp means ___ particles

A

faster particles

142
Q

faster particles means __ volume and _ collisions

A

more volume/less collisions

143
Q

more movement means __ temp

A

higher temp

144
Q

what is temperature?

A

how fast particles are moving

145
Q

can temperature be negative?

A

no

146
Q

absolute scale

A

a scale in which numbers can only be positive

147
Q

what is the absolute scale for temperature?

A

kelvin scale

148
Q

whats the lowest temperature possible?

A

zero kelvin

149
Q

if temperature is zero, particles are…

A

no longer moving (hard to achieve, and no experiment has EVER done it)

150
Q

avogadro’s law:

A

there is a connection between volume and number of moles of a gas.

151
Q

more moles = __ space

A

more space

152
Q

if moles increase, volume _

A

increases

153
Q

number of moles and volume are ___ related

A

directly related (one increase the other increase)

154
Q

by looking at combined gas law and adding avogadro’s law, we learn that any gas can be described by its_, _, _, and _

A

pressure, volume, temp, number of moles

155
Q

P(pressure)V(volume) =

A

n(number of moles) R(0.08206) T(temp in K)

156
Q

what is the volume of a 1.00 mole of a gas at STP?

A

22.4L
- if we are not at STP we have to use the ideal gas law equation

157
Q

ideal gas law equation

A

PV = nRT

158
Q

when at STP, 1atm=_K, and 1mol gas = _ L

A

273, 22.4L

159
Q

when not at STP, use _ to find the number of moles

A

stoichemetry

160
Q

dalton gave us _ theory and law of _ _

A

atomic theory
law of partial pressure

161
Q

law of partial pressure

A

pressure a gas exerts is the same if it is in a mixture of gases or by itself

162
Q

partial pressure

A

the pressure of an individual gas when its in a mixture

163
Q

vapor pressure

A

pressure of a gas

164
Q

ideal gas law for law of partial pressure

A

ntotal = n1 + n2 + n3
n = PV/RT
Ptotal = p1 + p2 + p3
PtVt/RTt = P1V1/RT1 + 2 + 3 . . .

165
Q

mole fraction

A

mole of gas 1 / total moles of mixture
x1 = n1 / ntotal

166
Q

partial pressure formula

A

mole fraction x Ptotal

10th grade (23 decks)

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