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physical chem > atomic structure > Flashcards

atomic structure Flashcards

1
Q

atomic number

A

amount of protons

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2
Q

what expression gives mass number

A

proton number plus neutron number

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3
Q

expression for proton number

A

mass number- neutron number

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4
Q

expression for neutron number

A

mass number - proton number

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5
Q

whats mass number

A

neutron number plus proton number

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6
Q

atomic mass unit

A

measures weight of atoms 1/12 of carbon 12

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7
Q

how to calculate relative mass

A

take isotope and times relative abundance by atomic mass
add together and divide by 100

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8
Q

symbol for relative atomic mass

A

Ar

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9
Q

whats the relative atomic mass definition

A

the average mass of one atom of an element relative to one twelfth of the mass of carbon 12

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10
Q

kinetic energy equation

A

0.5 times mass times velocity squared

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11
Q

unit for kinetic energy

A

Joules

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12
Q

unit for mass in kinetic energy

A

kg

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13
Q

rearranged kinetic energy equation for mass

A

m= 2ke/v squared

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14
Q

rearranged equation of kinetic energy for speed

A

v= square root 2ke/m

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15
Q

time of flight

A

distance travelled by atom to calculate its mass

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16
Q

equation for atoms mass from time of flight

A

m=2ke times t squared/distance aquared

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17
Q

rearranging time of flight formula for time subject

A

t= root distance root m/2ke

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18
Q

time of flight mass equation for distance subject

A

d= root t times root 2ke/m

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19
Q

why do we turn atoms into ions in time of flight

A

because atoms nuetral they need charge to be attracted to charged metal plate

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20
Q

what do we need to do so charged plate can give atoms kinetic energy

A

ionise them

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21
Q

whats a time of flight mass spectrometer

A

measures time of flight of atom to work our mass of atom

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22
Q

4 steps of mass spectrometry

A

-ionisation
-acceleration
-ion drift
-detection

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23
Q

electron gun ionisation

A

hot wire that emits electric current which emits fast moving electrons and knocks electron of atom and makes positive charged atom

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24
Q

vaporisation

A

to get atoms ready for electron gun they are heated to get ready for electron gun

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25
Q

accelaration step

A

negative charged plate moves positive atom towards it
-atom gains kinetic energy and speed

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26
Q

what determines how much energy ion receives

A

the charge of the atom so big or small all ions have the same kinetic energy as all equal in charge

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27
Q

ion drift stage

A
  • hole in negative plate allows ion to move distance down tube
    -distance known
    -flight tube
    -
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28
Q

drifting ion

A

when ion moves through flight tube with known charge and kinetic energy and mass

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29
Q

how to get ion to drift

A

suck all air out of flight tube to allow ion to drift

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30
Q

detection stage

A

when electrons hit negative final plate electric current given off measured by computer
-bigger the current the large the movement
gain an electron

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31
Q

how to determine mass of atom in spectrometry

A

measure time taken to reach detector

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32
Q

how to determine number of atoms of particular mass in spectrometry

A

size of electrical current at detector

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33
Q

what happens after detection

A

computer produces mass spectrum

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34
Q

x and y axis of mass spectra

A

mass/charge ratio and relative abundance

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35
Q

how to calculate RAM from mass spectra

A

identify ions -mass number
-express relative intensity in percentage
-total ions divide by how many of ions your working out times 100 as percentage
-percentage of each times mass number adding individuals up dividing all by 100

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36
Q

formula for comparing two ions to predict flight of mass

A

m1/t2 = m2/t2

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37
Q

rearranged equation for comparing two ions flight of mass

A

t2 = root m2/m1 times t1

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38
Q

bohr model of the atom

A

orbits electron in 3D
at specific distances from nucleus

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39
Q

how are electrons quantised

A

because of fixed distance from nucleus they are restricted to energy levels

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40
Q

how to go up energy level or down

A

lose or gain energy

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41
Q

1 way of electron gaining energy

A

absorbing light

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42
Q

why do electrons only absorb specific colours

A

energy quantised so cant have any energy it likes
-not all colours absorbed

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43
Q

good things with bohr rutherford model of atom

A
  • no evidence electrons spiral into nucleus
    -uses data to made predictions
    -elegant and clear
    -good at explaining chemistry
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44
Q

schrodingers model of atom

A

-electrons energy quantised
-energy levels would be exactly values earlier experiment shown

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45
Q

how to find electrons energy levels

A

free electron and find out gaps between jumping from energy level to level
-relative to free electron

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46
Q

orbital

A

space where electrons can be
probability
-where electrons can be most of the time

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47
Q

orbitals in first energy level

A

1

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48
Q

orbitals for second energy level

A

4

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49
Q

orbitals for third energy level

A

9

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50
Q

orbitals for fourth energy level

A

16

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51
Q

s sub level orbitals

A

1

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52
Q

p sub level orbitals

A

3

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53
Q

d sub level orbitals

A

five orbitals

54
Q

f sublevel orbitals

A

7 orbitals

55
Q

naming sub levels

A

1s
2s
3s
4s
1p
2p
3p
4p
and so fucking on

56
Q

difference between 2s and 3s sub level

A

-energy of sub level
-radius of the orbital in the sub level

57
Q

ground state

A

lowest energy level of atom

58
Q

energy levels with more protons

A

stronger gaps between levels so stronger attraction

59
Q

energy of atoms when adding more electrons

A

more gaps and energy levels break down into sub levels
repulsion of electrons

60
Q

order of sub levels

A

s
p
d
f

61
Q

lowest to highest energy levels order

A

1s
2s
2p
3s
3p
4s
3d
4p
5s
4d
5p
6s

62
Q

aufbau principle

A

build up on electron configuration from lowest energy sub levels

63
Q

pauli exclusion principle

A

an orbital can contain a max of two electrons

64
Q

max electrons for s sub level

A

2

65
Q

mas electrons for p sub level

A

6

66
Q

max electrons for d sublevel

A

10

67
Q

d block of table

A

group 1 and 2 and hydrogen

68
Q

p block

A

group 3 4 5 6 7 0

69
Q

d block

A

all transition elements

70
Q

shorthand electron configurration

A

element before with added configuration with elements own notation

71
Q

spin

A

spin up and spin down

72
Q

problem with spin

A

not electrons spinning but quantam effect

73
Q

rules of spin

A

pauli says cant have sub level with 2 or more electrons with same spin

74
Q

pauli exclusion principle

A

no orbital cant have same spin electron

75
Q

hunds rule

A

-within a sub level every orbital is singly occupied before any doubly occupied

-all electrons in singly occupied orbitals have the same spin

76
Q

why do orbitals in the same level have single spin before they become doubled

A

-electrons in same orbital repel each other more than electrons in different orbitals
-electrons occupy different orbitals to reduce repulsion

77
Q

find out electron conc of ions

A
78
Q

electron conc of cations

A

remove electrons with highest energy from origional conc

79
Q

electron config of anions

A

add electrons to original config

80
Q

nuclear charge

A

how many protons are in nucleus

81
Q

how does nucleus charge effect electrons

A

larger charge is more
= more protons so more force electrons have on them

82
Q

as you across period how does nuclear charge change

A

increases by 1

83
Q

nuclear charge change as going down group

A

increases by more than 1

84
Q

distance from nucleus

A

-further away less electrostatic force
-weaker force of attraction
-lower energy levels have electrons closer to nucleus

85
Q

protons and distance

A

higher nuclaeu charge closer each shell is to nucleus

86
Q

what effects the distance between nucleus and outer electrons

A

nuclear charge and which shell the outer electrons are in

87
Q

distance down group

A

increases as electrons in different shell so further away fromn nucleus

88
Q

electron electron repulsion effect on electrostatic force on electron

A

because electrons repel each other that decreases some of force felt by electrons because of protons

89
Q

rules of shielding

A

-electron closer to nucleus shields charge of one proton
-electron in same shell shields small amount of one proton
-electron further in shell doesnt shield at all

90
Q

moving across period for shielding

A

number of outer electrons increases so shielding increases

91
Q

down group shielding

A

increases because new shell made

92
Q

factors that effect forces on electrons

A

-nuclear charge
-distance from nucleus
-shielding

93
Q

group 1 elements and water

A

-electrons removed
-higher energy level equals less energy to move
-moves from highest energy sublevel

94
Q

first ionisation energy

A

the energy required to remove one mole of electrons from one mole of gaseous atoms of element

95
Q

unit for ionisation energy

A

KJ/ mole

96
Q

first ionisation energy equation

A

element(g) + element ion (g) + e-

97
Q

first ionisation energy down a group

A

decrease down group
-attraction to nucleus decreases

98
Q

first ionisation energy across period

A

–increases
-nuclear charge increases
-harder to remove electrons
-generally increases

99
Q

why do ionisation energies decrease down group

A

-weaker attraction to nucleus
-outer electrons more shielded and further away from nucleus
-

100
Q

why first ionisation energy across period generally increases

A

-nuclear charge increases
-shielding of outer electrons stays roughly the same
-strong attraction to nucleus

101
Q

why does potassium have lower ionisation energy than sodium

A

potassiums outer electron more shielded and further away from nucleus
weaker attraction to nucleus

102
Q

why does magnesium have higher ionisation energy than sodium

A

-magneisum gas higher nuclear charge than sodium and both atoms have same shielding since in same shell
-masgnesiums outer shell electrons have stronger force of attraction to nucleus than sodium

103
Q

magnesium and aluminium first ionisation energies

A

-Al has lower first ionisation energy than magnesium
-Al electron removed from 3p but Mg from 3s
-3p sublevel further away from nucleus and also shielded by aluminiums 3s electrons
-less energy to remove electron from AL
-

104
Q

phosphorus and sulfur ionisation energies

A

-sulfur has paired electron in 3p sublevel
-electron repulsion between pairs
-less energy needed

105
Q

second and so forth ionisation energy

A

removing second and whatnot electrons from ions

106
Q

successive ionisation energies

A

-always increasing
-in certian points bigger jumps

107
Q

second ionisation energy deifnition

A

the energy required of an element to remove one mole of electrons from one mole of gaseous 2+ ions of that element

108
Q

why do successive ionisation energies always increase

A

because electrons are removed from a increasingly positive ion which requires more energy

109
Q

how do graphs of successive ionisation energies give evidence for shells

A

-big jumps give evidence for shells
-we can explain jumps by saying electron is being removed from an inner shell

110
Q

how does graph of first ionisation energy across period give evidence for subshells

A

-drop between al and mg on graph give us evidence
-Al has greater nuclear charge than mg so first ionisation would be greater
Al lower than mg so Al outer electorn in different sublevel

111
Q

how does graph of first ionisation energy across period give evidence that electrons in same orbital repel more than electrons in different orbital

A

-drop between P and S
-sulfur has greater nuclear charge than P
-sulfur isnt higher than P so idea that electrons in same orbital repel each toher more

112
Q

rutherford and current model difference

A

-current model has neutrons and protons but rutherfords doesnt
-current model shows electrons in different energy levels- rutherfords doesnt

113
Q

missing percentage abundance

A

add al known percentages and take away from one hundred

114
Q

equation for electrospray ionisation

A

X(g) + H+ → XH+(g)

115
Q

define mass number of an atom

A

number of protons and neutrons in nucleus of atom

116
Q

finding number of neutrons

A

take away top number from proton number

117
Q

number of protons same as

A

number of electrons

118
Q

define relative atomic mass

A

average mass of an atom of an element compared to 1/12 the mass of carbon 12 atom

119
Q

working out RAM when given relative intensities

A

add all intensities up and divide by total number

120
Q

why you need to ionise atoms before doing time of flight

A

-ions will interact with and be accelerated by electrical current
-ions create current when hitting detector

121
Q

describe how molecules are ionised using electrospray

A

-sample dissolved in volatile substance
-injected through needle at high positive charge
-each molecule gains a proton

122
Q

explain first ionisation energies pattern from lithium to neon

A

general trend li to ne
-first ie increases
-more protons
-electrons in same shell
-no extra shielding
-stronger attraction between nucleus and outer electrons

deviation be - B
-B lower than Be
-outer electron in 2p
-higher in energy than 2s

deciation N to O
-O lower than N
-2 electrons needed in 2p to pair
-pairing electrons cause repulsion

123
Q

role of water with calcium reaction

A

oxidising agent

124
Q

trend in group 2 first ionisation energies

A

-decrease
-ions get bigger
-weaker attraction of ion to lost electron

125
Q

electron impact ionisation

A

sample bombarded with high energy electrons
-sample of molecules lose electron forming positive ion

126
Q

how TOF separates two species to give peaks

A

-positive ions accelerated by electric field
-to constant kinetic energy
-all have same kinetic energy
-so lower mass ratio move faster

127
Q

how to predict m/z ratios on graph

A

add all possibilities of all isotopes added up
2 combinations

128
Q

how to work out relative intensity of peaks

A

work out probability of each isotope in each combination and put into fraction and times fractions

129
Q

small peaks on mass spectra

A

caused by fragmenting of molecules with electron gun

130
Q
A

physical chem (7 decks)

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