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Separate Chemistry > T1: Atomic Structure > Flashcards

T1: Atomic Structure Flashcards

1
Q

The Bohr Model

A
  • p and n found in the centre of the atom -> nucleus.
  • p and n also called nucleons.
  • e- are held in shells / energy levels.
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2
Q

Subatomic Particles Relative Charge

A

p = +1, n = 0, e- = -1

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3
Q

Subatomic Particles Relative Mass

A

p = 1, n = 1, e- = 1/1840

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4
Q

Atomic number

A

Z, equal to the number of protons.

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5
Q

Mass number

A

A, equal to the number of protons and neutrons combined.

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6
Q

X

A

the symbol of the element

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7
Q

Cations

A

+ Atom lost electrons so there are more protons than electrons p > e-

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8
Q

Anions

A
  • Atoms gained electrons so there are more electrons than protons p < e-
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9
Q

Ions definition

A

An atom equal of neutral charge (no charge) where the number of protons (Z) is equal to the number of electrons

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10
Q

Isotopes definition

A

Atoms with the same number of protons but a different number of neutrons.

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11
Q

Chemical properties of Isotopes

A

isotopes of the same element have the same chemical properties because they have the same electron configuration.

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12
Q

ER: He 2+ ions went through foil and arrived at point P

A

He concluded that most of the atom has empty space

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13
Q

ER: very small number of He 2+ ions detected at point Q

A

He concluded that the atom must have a small positive nucleus.

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14
Q

ionisation energy meaning

A

the amount of energy needed to remove a mole of electrons from a mole of atoms, in the gaseous state. units = kJmol-1

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15
Q

EXAMPLE 1st IE of K

A

K(g) -> K+(g) + e-

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16
Q

3 things that will influence IE

A

Nuclear Charge (No of protons in the nucleus), Distance from the nucleus, Shielding

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17
Q

Nuclear Charge (No of protons from the nucleus)

A

More protons = stronger attraction

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18
Q

Distance from the nucleus

A

Closer = stronger attraction

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19
Q

Shielding

A

e- in inner shell give outer e- slight repulsion

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20
Q

IE Boron graph outer shell

A

IE 1-3 increase -> each electron removed from a more positive ion each time

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21
Q

IE boron graph p and e- attraction

A

Attraction of p and e- increases -> less electrons being attracted by same number of protons

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22
Q

IE boron graph inner shell

A

4th e- removed from shell closer to the nucleus = more stronger attraction to nucleus

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23
Q

why 2nd IE is higher than the 1st

A

The 2nd e- is removed from an ion that already has a positive charge.

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24
Q

MA: successive IE for element identification

A
  • The largest increase is between 4th and 5th IE
  • the 5th e- is on the shell closer to the nucleus
  • element must have 4 electrons on its outer shell
  • in period 3 this must be silicon
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25
Q

Bigger radius

A

Lower ie

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26
Q

why Li is a bigger atom than Be

A
  • Both atoms have the same number of shells
  • they have the same shielding
  • but Be has more protons
  • so it attracts the outer most electrons more strongly so its smaller
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27
Q

why He has the highest 1st IE

A

it has more p than H and only 1 shell so the same shielding as H

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28
Q

why Li is a bigger atom than He

A
  • Li has an extra e- shell and is further away from the nucleus
  • the outer e- is more shielded
  • the outer e- is less strongly attracted to the nucleus
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29
Q

Why is Li a bigger atom than F

A

Both atoms have the same number of shells
They have the same shielding
But F has more protons
So it attracts the outer most electrons more strongly

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30
Q

Why is Li+ a smaller ion than F-

A

Li+ ion has only 1 shell
The electrons are closer to the nucleus so there is less shielding
So outer electrons are more strongly attracted

31
Q

Predicting trends in 1st IE across a period

A

The 1st IE will increase
There are more protons in the nucleus
The shielding remains the same
So the attraction between the nucleus and the outer electrons increases

32
Q

No of e- in shell 1

A

2

33
Q

No of e- in shell 2

A

8

34
Q

No of e- in shell 3

A

2, 10, 8 = 18

35
Q

No of e- in shell 4

A

2, 10, 8, 14 = 32

36
Q

S orbital shape

A

Spherical shape

37
Q

P orbital shape

A

Dumbbell shape

38
Q

S subshell

A

1 s orbital

39
Q

P subshell

A

3 p orbitals

40
Q

D subshell

A

5 d orbitals

41
Q

F subshell

A

7 f orbitals

42
Q

Chromium electron configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

43
Q

Copper electron configuration

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

44
Q

1st IE trend across a period

A

general trend increases
no. of protons increase (nuclear charge)
same amount of shielding
greater attraction between the nucleus and outer electron

45
Q

1st dip in 1st IE (s2 and p1)

A
  • 1st e- removed from Be is from 2s sb lv
  • 1st e- removed from B is from 2p sb lv
  • 2s sb lv is lower in energy than 2p
  • therefore less energy is needed to remove the electron from B
46
Q

2nd dip in 1st IE (p3 and p4)

A
  • 1st e- removed from N is from 2p sb lv + unpaired
  • 1st e- removed from O is from 2p sb lv + a paired orbital
  • O has a lower IE due to electron pair repulsion
  • therefore less energy is needed to remove the electron from O
47
Q

how does IE change down the group

A
  • atoms get bigger
  • more shielding
  • weaker attraction from nucleus to e- in the outer shell
  • IE decreases down the group
48
Q

trend in atomic radius down the group

A

atomic radius increases
no. of shells and amount of shielding increases
weaker attraction between nucleus and outer e-

49
Q

trend in atomic radius across the period

A

atomic radius decreases
no. of protons increases but amount of shielding stays the same
greater attraction between e- and nucleus

50
Q

what 2 factors does the mass spectrometer measure

A

relative abundance
mass/charge ratio (m/z)

51
Q

mass spectrometer vacuum

A

entire machine in vacuum to prevent any particles being tested colliding with molecules from the air

52
Q

mass spectrometer ionisation

A

2 methods
electrospray ionisation
electron impact ionisation
sample particles gain a positive charge in both

53
Q

mass spectrometer acceleration

A

the positive ions are attracted to the negatively charged plate and accelerate towards it. amount of acceleration depends on m/z ration of the ion. high m/z ratio ions accelerate to lower speeds than low m/z ration ions once accelerated all ions will have the same kinetic energy

54
Q

mass spectrometer ion drift

A

some ions will pass through a hole in the negatively charged plate. they form a beam of particles to travel along tube towards detector. particles travel at different speeds so drift apart as slow particles cant keep up with faster ones

55
Q

mass spectrometer detection

A

different m/z ratio ions arrive at the detector at different times due to different velocities. TOF recorded as each ion hits detector it gains an electron. generates current the size of which is proportional to the number of each type of atom (abundance)

56
Q

mass spectrometer data analysis

A

the signal from the detector is passed to a computer which generates a mass spectrum.

57
Q

electron impact ionisation

A
  • sample is vaporised
  • high energy electrons are fired at it from an electron gun
  • knocks off 1 electron from each particle forming 1+ ion
58
Q

electron impact ionisation equation

A

X(g) -> X+(g) + e-

59
Q

for electron impact ionisation the molecular ion…

A

breaks down into smaller fragments

60
Q

electrospray ionisation

A
  • sample dissolved in a volatile solvent
  • injected through a fine hypodermic needle
  • the needle is attached to the positive terminal of high voltage
  • particles are ionised by gaining a proton H+ ion
61
Q

electrospray ionisation equation

A

X + H+ -> XH+

62
Q

for electrospray ionisation fragmentation…

A

rarely takes place

63
Q

Ar =

A

(Mass1 x Abundance1) + (Mass2 x Abundance2) + (Mass n x Abundance n) / ∑ Abundances

64
Q

KE =

A

(m x v^2) / 2

65
Q

m =

A

2KE / v^2

66
Q

v^2 =

A

2KE / m

67
Q

v =

A

√v^2

68
Q

t =

A

d / v

69
Q

t is

A

time of flight (s)

70
Q

d is

A

length of flight tube (m)

71
Q

v is

A

velocity of the particle (m s^-1)

72
Q

m is

A

mass of the particle (kg)

73
Q

KE is

A

kinetic energy o particle (J)

74
Q

mass of an atom

A

(mass number of element / 6.022 x 10^23) / 1000

Separate Chemistry (6 decks)

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