Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Subatomic Particles Relative Charge

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Subatomic Particles Relative Mass

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Atomic number

A

Z, equal to the number of protons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Mass number

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

X

A

the symbol of the element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Cations

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Anions

A
  • Atoms gained electrons so there are more electrons than protons p < e-
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Isotopes definition

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Chemical properties of Isotopes

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

EXAMPLE 1st IE of K

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

3 things that will influence IE

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Nuclear Charge (No of protons from the nucleus)

A

More protons = stronger attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Distance from the nucleus

A

Closer = stronger attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Shielding

A

e- in inner shell give outer e- slight repulsion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

IE Boron graph outer shell

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

IE boron graph inner shell

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Bigger radius
Lower ie
26
why Li is a bigger atom than Be
- 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
27
why He has the highest 1st IE
it has more p than H and only 1 shell so the same shielding as H
28
why Li is a bigger atom than He
- 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
29
Why is Li a bigger atom than F
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
30
Why is Li+ a smaller ion than F-
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
Predicting trends in 1st IE across a period
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
No of e- in shell 1
2
33
No of e- in shell 2
8
34
No of e- in shell 3
2, 10, 8 = 18
35
No of e- in shell 4
2, 10, 8, 14 = 32
36
S orbital shape
Spherical shape
37
P orbital shape
Dumbbell shape
38
S subshell
1 s orbital
39
P subshell
3 p orbitals
40
D subshell
5 d orbitals
41
F subshell
7 f orbitals
42
Chromium electron configuration
1s2 2s2 2p6 3s2 3p6 4s1 3d5
43
Copper electron configuration
1s2 2s2 2p6 3s2 3p6 4s1 3d10
44
1st IE trend across a period
general trend increases no. of protons increase (nuclear charge) same amount of shielding greater attraction between the nucleus and outer electron
45
1st dip in 1st IE (s2 and p1)
- 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
2nd dip in 1st IE (p3 and p4)
- 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
how does IE change down the group
- atoms get bigger - more shielding - weaker attraction from nucleus to e- in the outer shell - IE decreases down the group
48
trend in atomic radius down the group
atomic radius increases no. of shells and amount of shielding increases weaker attraction between nucleus and outer e-
49
trend in atomic radius across the period
atomic radius decreases no. of protons increases but amount of shielding stays the same greater attraction between e- and nucleus
50
what 2 factors does the mass spectrometer measure
relative abundance mass/charge ratio (m/z)
51
mass spectrometer vacuum
entire machine in vacuum to prevent any particles being tested colliding with molecules from the air
52
mass spectrometer ionisation
2 methods electrospray ionisation electron impact ionisation sample particles gain a positive charge in both
53
mass spectrometer acceleration
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
mass spectrometer ion drift
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
mass spectrometer detection
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
mass spectrometer data analysis
the signal from the detector is passed to a computer which generates a mass spectrum.
57
electron impact ionisation
- 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
electron impact ionisation equation
X(g) -> X+(g) + e-
59
for electron impact ionisation the molecular ion...
breaks down into smaller fragments
60
electrospray ionisation
- 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
electrospray ionisation equation
X + H+ -> XH+
62
for electrospray ionisation fragmentation...
rarely takes place
63
Ar =
(Mass1 x Abundance1) + (Mass2 x Abundance2) + (Mass n x Abundance n) / ∑ Abundances
64
KE =
(m x v^2) / 2
65
m =
2KE / v^2
66
v^2 =
2KE / m
67
v =
√v^2
68
t =
d / v
69
t is
time of flight (s)
70
d is
length of flight tube (m)
71
v is
velocity of the particle (m s^-1)
72
m is
mass of the particle (kg)
73
KE is
kinetic energy o particle (J)
74
mass of an atom
(mass number of element / 6.022 x 10^23) / 1000

Separate Chemistry (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions