Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

A level Chemistry > Unit 1.2 - Basic ideas about atoms > Flashcards

Unit 1.2 - Basic ideas about atoms Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What is radioactivity?

A

When an unstable atomic nucleus decays, it spontaneously forms a new element by emitting ionising radiation, like alpha, beta or gamma

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

What is an alpha particle?

A

Helium nucleus

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

Alpha particle charge?

A

2+

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

Alpha particle relative mass

A

4

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

Alpha symbol

A

4
a
2

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

What is a beta particle?

A

An electron

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

Beta particle relative charge

A

-1

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

Beta particle relative mass

A

(about) 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Beta symbol

A

0
B
-1

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

What is a gamma wave?

A

Electromagnetic wave

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

What is a gamma waves relative charge?

A

0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a gamma waves relative mass?

A

0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Gamma symbol

A

0
Y
0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Alpha penetrating power

A

Stopped by paper

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

Beta penetrating power

A

A few mm’s of aluminium

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

Gamma penetrating power

A

Decreased by a few cm’s of lead of concrete

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

Which type of radioactive particle is the most ionising and which is the least?

A

Most - alpha
Least - gamma

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

What is nuclear decay?

A

When a radioisotope decays, forming a new element, meaning its properties can be deduced

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

What decays for radioactivity?

A

Unstable atomic nucleus

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

What decays for nuclear decay?

A

Radioisotopes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What happens during gamma radiation? Why?

A

No new element is formed as it’s only emitted when an atom loses energy

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

When is gamma radiation emitted?

A

When an atom loses energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What happens when alpha particles undergo nuclear decay?

A

Emits a helium nucleus (2 protons and 2 neutrons)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What happens to the mass and atomic number of the nucleus when undergoing the decay of alpha particles?

A

Mass number - loses four units of mass number
Atomic number - loses 2 units

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

How do you figure out which one is the new element after one has undergone nuclear decay of alpha particles?

A

2 places to the left on the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

When is a high energy beta electron formed?

A

When a neutron decays into a proton and an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What happens when beta particles undergo nuclear decay?

A

The nucleus decays and emits a high-energy electron, which is formed when a neutron decays into a proton and an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What type of electrons are beta particles?

A

High energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What happens to the mass and atomic number during the nuclear decay of beta particles?

A

Mass number - the same
Nuclear number - 1 more

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

How do you find out what the new element is once nuclear decay happens to beta particles?

A

One place to the right on the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Name 5 types of nuclear decay

A

-Gamma radiation
-Alpha particles
-Beta particles
-Electron capture
-Positron emission/beta plus decay

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What uses electron capture and why?

A

Unstable atoms use to become more stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

How does electron capture work?

A

-Electron from the atom’s inner shell is drawn to the nucleus
-Combines with a proton
-Becomes a neutron and a neutrino
-Neutrino is ejected from the atom’s nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Example of electron capture

A

Carbon 11 Boron 11
6 protons +electron ———> 5 protons + neutrino
5 neutrons 6 neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What type of radioactive decay can have two possible names? What are they?

A

Positron emission or beta plus decay

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What is the proton inside originally for positron emission/beta plus decay?

A

Radionuclide nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

How does position emission/beta plus decay work?

A

-Radioactive decay
-Proton inside a radionuclide nucleus is converted into a neutron while releasing a positron and an electron neutrino (Ve)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Electron neutrino symbol

A

Ve

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

What’s important to remember when writing equations involving nuclear decay?

A

The sum of the mass numbers on the reactants equals the sum of the mass numbers of the products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Why is radiation dangerous?

A

Can ionise and kill cells, and ionising molecules of living cells damages them, increasing cancer risks
Can also cause changes in the DNA, leading to mutations and cancer causing cells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What do changes in our DNA from radiation lead to?

A

Mutations and cancer causing cells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What does most of our annual radiation come from? How much?

A

80% - natural sources (radon especially)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

What’s the main radioactive natural source that we’re exposed to?

A

Radon gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

What type of particles ionise cells the most?

A

Larger ones

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

What type of particles ionise cells the most?

A

Larger ones

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Why are larger radioactive cells more dangerous?

A

They ionise more

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

Is alpha or beta the most dangerous? How come?

A

Alpha as the particles are larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

What, in terms of half life, makes a radioactive substance more dangerous? What factors does this effect?

A

Longer half life = more dangeous to environment
Shorter half life = more dangerous to living cells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

What’s important to remember when calculating the electrons in an ion?

A

That it’s lost/gained some and it’s no longer equal to the protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

Which radioactive particle has the smallest defective angle and why?

A

Alpha as its mass is higher = it’s heavier

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

How do you work out the new element from electron capture?

A

1 place to the left on the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

How do you work out the new element from positron emission / beta plus decay?

A

1 place to the left on the periodic table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

Positron symbol

A

0
e
+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

5 uses of radioactivity

A

-Radiotherapy
-Carbon dating (carbon 14)
-Smoke alarms
-Medical tracer
-Thickness monitoring

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

Do we copy mass numbers straight from the periodic table with radioactive decay equations?

A

No- copy the element, but make sure the mass numbers match for that question (might be a bit different from the one on the periodic table)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

Half life

A

The time taken for half the atoms in a particular amount of isotope to decay

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

4 characteristics of the half life of radioisotopes

A

-Own rate of decay
-Characteristic half-life
-Independent on the number of atoms present at the beginning
-Unaffected by changes in temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

How would you work out the fraction left of a radioactive substance?

A

Time
——— (halve how ever many times this is)
half life

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

How do you work out a radioactive substance’s half life?

A

How many half lives required to reach this?
time
——
this

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

What happens when an electron encounters a positron?

A

They annihilate eachother, creating gamma radiation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

What type of nucleus is the electron drawn to of for electron capture to happen?

A

proton-rich

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

What type of radiation does electron capture emit?

A

Gamma radiation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

What does gamma have a high?

A

-Frequency
-Energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

Why are alpha particles the most ionising?

A

High positive charge to strongly attract electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
64
Q

Why does gamma have the least ionising power?

A

Short wavelength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
65
Q

Which side of the equation do we show the electron loss during electron capture?

A

The left side, the rest on the right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
66
Q

Why are atoms ionised?

A

Due to an electron being removed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
67
Q

What does a cancerous cell do?

A

Divide uncontrollably

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
68
Q

What is the formation of tumours as a result of radiation an example of?

A

The late effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
69
Q

What is cell death as a result of radioactive exposure an example of?

A

Acute effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
70
Q

Acute effect

A

Happens rapidly after radioactive exposure (eg- cell death)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
71
Q

What type of radiation is the most dangerous INSIDE the body and why?

A

Alpha as it’s the most ionising

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
72
Q

What type of radiation is the most dangerous OUTSIDE the body and why?

A

Beta and Gamma as they penetrate dead cells on the surface and damage living cells underneath

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
73
Q

What does the radioactive source used for medical tracers require and why?

A
  • A short half life to avoid permanent damage
    -Emits enough radiation to be detected outside of the body
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
74
Q

What type of radiation is used for radiotherapy and thickness monitoring?

A

Beta radiation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
75
Q

Electronic configuration

A

The arrangement of electrons in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
76
Q

What type of energy do electrons have?

A

Fixed energies

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
77
Q

Where do electrons move around?

A

In their shells/energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
78
Q

What’s another word for the shells of electrons?

A

Energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
79
Q

What’s the name for the numbers of electron’s shells?

A

Principal quantum numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
80
Q

What do different shells have?

A

Different amounts of energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
81
Q

Which shell has the lowest amount of energy? Which electrons are these?

A

Level 1- electrons closest to the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
82
Q

What do electrons in different areas have?

A

Different orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
83
Q

Orbital

A

A region in the space of a cloud of negative charge where you’d likely find an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
84
Q

What can orbitals hold?

A

Up to 2 electrons with opposite spin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
85
Q

Why do the orbitals hold electrons with opposite spin?

A

In order to stop them totally repelling eachother

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
86
Q

What do orbitals have different?

A

Energies and shapes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
87
Q

What are the two orbitals whose shapes I need to be able to recognise?

A

S and P

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
88
Q

Shape of the S orbital

A

Spherical

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
89
Q

Shape of the P orbital

A

Dumb- bell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
90
Q

Draw the S orbital

A

lol go check your notes i’m not paying for premium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
91
Q

Draw the P orbital

A

(check notes)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
92
Q

What are shells divided into?

A

Sub shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
93
Q

Which shell isn’t divided into sub shells?

A

1st

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
94
Q

What do sub shells contain?

A

A specific number of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
95
Q

Number of orbitals and electrons in the S subshell (how do you know?)

A

1orbital, 2 electrons (count across the elements in their groups- this is the electrons, and the orbitals is half this as each one holds 2 electrons)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
96
Q

Number of electrons and orbitals in the P subshell

A

Orbitals- 3
Electrons -6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
97
Q

Number of orbitals and electrons in the d subshell

A

Orbitals- 5
Electrons - 10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
98
Q

How do we write out electronic configurations?

A

-Look at the periodic table - we have an an s, p and d block
-Write out in full, the big number is the number of that block followed by the letter and the amount of elements in indices until you reach it (eg- 1s2, 2s2, 2p6, 3s2, 3p4 etc

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
99
Q

How do we write shorthand electronic configurations?

A

The noble gas before and only the last bit- the electrons in the outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
100
Q

Where are the noble gases on the periodic table?

A

Group 0, downwards

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
101
Q

Why do we only write the electrons in the outer shell when writing electronic configurations short hand?

A

These are the only electrons that take part in chemical reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
102
Q

What do we write first, the 3 or 4 block? Which fills first?

A

The 4s block fills first, but you write however many 3s first

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
103
Q

With the 4s block and a non-full 3d block, what do you do when writing shorthand electronic configurations?

A

Show the electrons in the d subshell too as they can be involved in chemical reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
104
Q

What’s the first row of the d block?

A

3d

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
105
Q

Which block is helium part of?

A

The s block

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
106
Q

3 electron shell filling rules

A
  1. Electrons are placed in a shell with the lowest energy
  2. Only 2 electrons can occupy an orbital and they have opposite spins
  3. The electrons are placed in a subshell with parallel spins until the subshell is half full
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
107
Q

Which shell are electrons placed in?

A

The one with the lowest energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
108
Q

What are electrons placed in? Until when?

A

In a subshell with parallel spins until the subshell is half full

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
109
Q

How many electrons can occupy an orbital and what do they have?

A

2, opposite spins

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
110
Q

Which directions are the different p orbitals?

A

Px- sideways
Py - diagonal
Pz- upwards

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
111
Q

What do the arrows with the electron structures represent? Why is this?

A

Opposite spins that make it stable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
112
Q

Once we reach a certain orbital when writing out the electrons in their boxes, there’s a rule to remember. Which orbital is this and what’s the rule?

A

P orbital - half full them with just up arrows until full before filling with down arrows

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
113
Q

Which two elements have a specific exception when filling in the electron boxes? What is this exception?

A

Chromium and copper
Need a half filled 4s box before filling the 3d box to be stable
(Chromium- full of ups)
(Copper - full of ups and downs)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
114
Q

What sort of half life would machinery like a medical tracer need and why?

A

Longer so that it doesn’t constantly need replacing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
115
Q

Why do we have to half full the 4s box before filling the 3d box with chromium and copper?

A

The 3d orbital becomes lower in energy than the 4s orbital when filled (breaks rule no.1)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
116
Q

Why is 4s filled before 3d?

A

Because it is of lower energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
117
Q

How do you write the electronic configurations of ions?

A

-Write it as normal
-+ charge = take away that many electrons from the subshell with the highest energy (the last in the list)
(opposite for negative charge)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
118
Q

Where do we take away/add electrons for ions electronic configurations?

A

The subshell with the highest energy (the last in the list)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
119
Q

With ions in the d block, where are electrons lost first and why?

A

From the 4s subshell before the 3d as when the 4s subshell contains electrons, it has higher energy levels than the 3d subshell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
120
Q

Which one has the lowest energy - an empty 4s or an empty 3d level? What does this mean?

A

4s is lower so it’s filled first

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
121
Q

Ionisation energy (I.E.)

A

The energy required to remove one or more electrons from an atom
(There’s a value of the ionisation energy for every electron in the atom)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
122
Q

What is there a value of for every electron in the atom?

A

Ionisation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
123
Q

What does I.E. stand for?

A

Ionisation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
124
Q

Molar first ionisation energy

A

The energy required to remove one mole of electrons from one mole of its gaseous atoms to form one mole of gaseous ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
125
Q

What do you call the first ionisation energy?

A

Molar first ionisation energy

126
Q

Under what conditions is the ionisation energy of an electron at the standard molar first ionisation energy?

A

The standard conditions…
298K
1 atmosphere pressure

127
Q

What are the standard conditions and what do they cause?

A

298k and 1 atmosphere pressure cause the ionisation energy to be at the standard molar first ionisation energy

128
Q

What type of reaction is the first ionisation energy and why?

A

Requires energy = endothermic

129
Q

Is the first ionisation energy exothermic or endothermic?

A

Endothermic

130
Q

What are energy changes measured in?

A

kJ mol-1

131
Q

What causes variation in the standard molar first ionisation energy? What’s the phrase for this?

A

Outer electrons do not feel the full force of the positive charge of the nucleus, as the inner electrons screen them partially from its effects = screening

132
Q

Screening

A

Outer electrons do not feel the full force of positive charge from the nucleus as the inner electrons screen them partially from its effects

133
Q

What does screening cause variation in?

A

The values of standard molar first ionisation energy

134
Q

What do successive ionisation energies provide information about?

A

The arrangement of electrons around the nucleus

135
Q

Second ionisation energy

A

The energy required to remove one mole of electrons from 1 mole of 1+ ions to form 1 mole of gaseous 2+ ions
(same definition as you go up the ionisation energies, just it increases each ion charge by 1)

136
Q

What provides us with information about the arrangement of electrons around the nucleus?

A

Successive ionisation energies

137
Q

What does the value of the first ionisation energy depend upon?

A
  1. Nuclear charge (i.e -number of protons)
  2. Outer electron distance from the nucleus
  3. Screening produced by filled inner energy levels
138
Q

What tells us the nuclear charge of an element?

A

Number of protons

139
Q

As we move across the period, what happens to the ionisation energy?

A

Increases

140
Q

Why does ionisation energy increase as we move across the periods?

A
  • Nuclear charge increases
    -Electrons are added to the same shell, therefore there’s no effect on screening
    -More energy is required to remove them from the atom as the outer electrons are drawn closer to the nucleus across the period
141
Q

What happens to the electrons as we move across the period?

A

The outer electrons are drawn closer to the nucleus, making them more strongly attached

142
Q

For which elements would ionisation energy peaks appear on a graph?

A

Group 0 (noble gases)

143
Q

For which elements would troughs appear on an ionisation energy graph?

A

Group 1

144
Q

What are the two exceptions across the period for ionisation energies?

A
  1. Be to B and Mg to Al
  2. N to O and P to S
145
Q

Why are Be to B and Mg to Al exceptions to the rule that ionisation energy increases across the period?

A

Although Boron has an extra proton, there’s additional screening by a full 2s level and less energy needed to remove Boron’s 2p electron, therefore its a decrease in ionisation energy.
(same concept for Mg to Al but with 3s and 3p)

146
Q

What does a decrease in ionisation energy show on a graph?

A

Dips

147
Q

Why are N to O and P to S exceptions to the rule that ionisation energy increases across the period?

A

With oxygen, the new electron goes into an orbital which already has an electron, meaning that there’s increased repulsion between 2 electrons of the same orbital, making it easier to remove an electron
(same concept for P to S)
This outweighs the effect of the extra proton

148
Q

What happens when am electron goes into an orbital which already has an electron?

A

Increased repulsion between them

149
Q

What happens to the ionisation energy as you go down the group?

A

First ionisation energy decreases

150
Q

Why does the first ionisation energy decrease as you go down the groups?

A

Although there’s an increase in nuclear charge, there’s extra screening

151
Q

Describe hydrogens ionisation energy and give a reason why it’s like this

A

High, as it contains a single electron that’s close to the nucleus and strongly attached without screening

152
Q

Compare helium’s ionisation energy to hydrogen’s and give reasons for why you say this

A

It’s much higher, as similarly, the electron being removed is close to the nucleus and unscreened, however now the nucleus has 2 protons attaching the electrons instead of 1

153
Q

Describe the ionisation energy from helium to lithium and give reasons why you say this

A

In lithium, the outer electron is in the second energy level, further away from the nucleus, and the additional proton in the nucleus is outweighed by the screening given by the 1s electrons, therefore the ionisation energy decreases

154
Q

What is the nuclear charge?

A

The number of protons

155
Q

What do we have to make sure we write in ionisation energy formulas and why?

A

(g) as we can only ionise gas

156
Q

What’s screening caused by?

A

Full shells

157
Q

Which outweighs which - shielding or nuclear charge? What does this mean?

A

Shielding effect outweighs the increase in nuclear charge, which is why the first ionisation energy decreases going down the periodic table

158
Q

What is successive ionisation energy?

A

To successively remove all of the electrons until they’ve all been removed

159
Q

How many successive ionisation energies does an element have?

A

As many as it has electrons

160
Q

What’s a useful tip to remember when writing successive ionisation equations?

A

Whatever it’s labeled as is the target
e.g - third ionisation energy magnesium
Mg2+ (g) ——> Mg3+ (g) + e-

161
Q

What do successive ionisation energies do?

A

Always increase

162
Q

Why do successive ionisation energies always increase?

A

-Greater effective nuclear charge (same number of protons holding less electrons)
- Each one removed means less electron-electron repulsion so the shell is drawn closer to the nucleus
-The distance from the nucleus decreases so the nuclear attraction increases

163
Q

What number can we click on the calculator to make ionisation energies smaller?

A

log

164
Q

What is electromagnetic radiation?

A

Energy that can travel as waves + pass through a vacuum

165
Q

List the types of radiation on the electromagnetic spectrum

A

Radio
Micro
Infrared
Visible
Ultra violet
X-ray
Gamma

166
Q

What happens to energy, frequency and wavelength as you travel up the electromagnetic spectrum?

A

Increasing energy + frequency
Decreasing wavelength

167
Q

Equation linking wavelength and frequency

A

c= ŷ(upside down y)f

where
c - speed of light (constant)
upside down y - wavelength
f - freqency

168
Q

Equation for the energy of radiation

A

E = hf

where
E - energy
h - Planck’s constant
f - frequency

169
Q

Energy unit

A

J

170
Q

Wavelength unit

A

m

171
Q

Speed of light unit (why?)

A

ms-1

because…
c = wavelength x frequency
frequency unit - s-1
wavelength unit - m

172
Q

What’s the relationship between energy and frequency? Write this as a formula and give an example

A

Energy is directly proportional to frequency
E 🐟 f
(double frequency, double energy)

173
Q

What’s the relationship between wavelength and frequency? Write this an as equation and give an example

A

frequency is indirectly proper optional to wavelength
f 🐟 1
—
upside down y

double wavelength, halve frequency

174
Q

Wavelength + unit

A

Distance between one point on a wave to the same point in the next (usually the crest)
M

175
Q

What is wavelength usually measured on?

A

The crest

176
Q

Frequency + units

A

Number of waved produced by a source per second
Hz

177
Q

How do you deal with units/prefixes?

A

Multiply the number in THAT form with the prefix
e.g
1mj—> ? J
milli prefix is 10-3
1x10-3 = 0.001J

178
Q

what does the c symbol stand for?

A

centi

179
Q

What does the T symbol stand for?

A

Tetra

180
Q

Centi prefix

A

10^-2

181
Q

Tetra prefix

A

10^12

182
Q

What is light?

A

The visible region of the E-M spectrum

183
Q

What’s the wavelength range of visible light?

A

700nm-400nm

184
Q

What happens when you pass white light through a prism?

A

Split into a rainbow of colours known as the continuous spectrum

185
Q

Which has the highest energy - blue or red light? Why?

A

Blue as it has the highest frequency

186
Q

Emission line spectrum

A

elements are heated and give off light of certain wavelengths - seen as lines only on those specific wavelengths (the mostly black one)

187
Q

What type of gas would cause the emission line spectrum?

A

Hot

188
Q

What causes the emission line spectrum in terms of electrons?

A

Electron emits energy + drops down to ground level, releasing a photon of light

189
Q

Absorption line spectrum

A

All atoms and molecules absorb light of certain wavelengths - if white light is passed through the vapour of an element, it was absorb certain wavelengths= black lines corresponding (mostly rainbow one)

190
Q

What type of gasses are responsible for the absorption line spectrum?

A

Cold

191
Q

What does white light have to do to absorb certain wavelengths?

A

Pass through the vapour of an element

192
Q

What happens when white light passes through the vapour of an element?

A

Absorbs certain wavelengths of light

193
Q

What causes an absorption line spectrum in terms of electrons?

A

Electron absorbs energy + gets excited to a higher level

194
Q

What can both the emission and absorption line spectrums tell us?

A

Tell us about the arrangement of the electron shells in an atom by detecting the presence of particular elements, which all have a unique pattern due to different nuclear charges hence the arrangement of shells

195
Q

Why do different elements have different patterns?

A

Differing nuclear charges hence the arrangement of shells

196
Q

What do spectrometers and prisms do?

A

Separate light into its constituent frequencies

197
Q

What separates light into its constituent frequencies?

A

Spectrometers and prisms

198
Q

What do the excited states do as you move up them?

A

Converge (get closer)

199
Q

Which energy state has the lowest energy and why?

A

The ground state as it’s the one closest to the nucleus

200
Q

What do you call the numbers for all the excited states?

A

Quantum numbers

201
Q

What’s important to remember with quantum numbers?

A

There’s no zero

202
Q

What’s the word for an electron “jumping” to a higher energy level?

A

Being promoted

203
Q

Explain how an electron is promoted

A

Atom is heated/put in an electric field
Electrons absorb energy
Become “excited”
Can jump to a higher energy level

204
Q

What has to happen to an atom for electrons to absorb energy?

A

It has to be heated or put in an electric field

205
Q

What does it take to promote an electron to a higher energy level?

A

A specific amount of energy

206
Q

What is the energy absorbed by an electron equivalent to?

A

The amount needed for the jump = the line in the absorption spectrum

207
Q

What IS the line in the absorption spectrum?

A

The amount of energy absorbed as it’s needed for an electron to jump

208
Q

What does the frequency of the line on the absorption spectrum correspond to?

A

The specific energy needed
(E🐟f)

209
Q

What does each line on the absorption spectrum correspond to?

A

A different jump between levels

210
Q

What can you call the “jumps” of an electron?

A

Electronic transitions

211
Q

What causes the emission spectrum in terms of electrons?

A

Energy is removed
Electrons fall from their excited state
Release that specific amount of energy, known as a quantum of energy/a photon

212
Q

What is required for electrons to fall from their excited state?

A

Energy to be removed

213
Q

What do you call the specific amount of energy released by an electron as it falls from its excited state?

A

A quantum of energy/photon

214
Q

What’s the phrase for electrons being constrained to energy levels?

A

Quantised

215
Q

What does the fact that electrons are quantised mean?

A

They’re constrained to energy levels

216
Q

Because electrons are quantised, what do they do?

A

Emit specific photons of energy with discrete frequencies, causing sharp lines on the spectrums

217
Q

How do you calculate the energy taken in/given out by an electron?

A

The difference between energy levels

(can use the frequency formula after this if asked for frequency)

218
Q

What do you call 1s, 2s, 2p etc…?

A

Sub shells

219
Q

What does the visible atomic emission spectrum of hydrogen do?

A

Provides evidence for the theory that electrons are found in definite energy levels around the nucleus of an atom

220
Q

How do we obtain the visible atomic emission spectrum of hydrogen?

A

We use an electric discharge tube

221
Q

What does an electric discharge tube have in order for it to obtain the emission spectrum of hydrogen?

A

-Hydrogen gas of low pressure in the tube
-High potential difference across the electrodes
-High voltage supply

222
Q

Draw and label an electric discharge tube

A

check your notes lol

223
Q

What happens to hydrogen within an electric discharge tube?

A

Hydrogen molecules are split into atoms, and when the electrical discharge passes through the tube, electrons are promoted to higher energy levels, and when they fall back down to a lower level, energy is released as electromagnetic radiation

224
Q

Draw the visible atomic emission spectrum of hydrogen

A

check your notes

225
Q

What energy level does the violet stripe in hydrogens visible atomic emission spectrum fall from and down to?

A

n=6 to n=2

226
Q

What energy level does the dark blue stripe in hydrogens visible atomic emission spectrum fall from and down to?

A

n=5 to n=2

227
Q

What energy level does the blue stripe in hydrogens visible atomic emission spectrum fall from and down to?

A

n=4 to n=2

228
Q

What energy level does the red stripe in hydrogens visible atomic emission spectrum fall from and down to?

A

n=3 to n=2

229
Q

What do you call the visible atomic emission spectrum of hydrogen?

A

The Balmer series

230
Q

What energy level do all of the electrons in the Balmer series fall to?

A

n=2

231
Q

What’s the name of the limit point on the visible atomic emission spectrum of hydrogen?

A

Convergence limit

232
Q

Which colour is closest to the increasing frequency on the Balmer series?

A

Violet

233
Q

What does the Balmer series contain?

A

A number of coloured lines on a black background

234
Q

What do the lines on the Balmer series do?

A

Converge with increasing frequency

235
Q

Converge

A

To tend to meet in a point or line

236
Q

What happens to the energy levels and successive lines in the spectrum with increasing distance from the nucleus?

A

-Energy levels get closer
-Successive lines in the spectrum get closer

237
Q

What are electrons found in and what is forbidden?

A

Definite energy levels, energies between are forbidden

238
Q

What happens to an electron as it gains energy?

A

It’s promoted to higher levels

239
Q

What happens when electron falls to a lower energy level?

A

Energy is emitted as EMR - a photon of light

240
Q

Describe the difference in energy between any two levels in an atom

A

Fixed
Electron releases electromagnetic radiation unique to that transition, which is observed as a distinct line

241
Q

What is the EMR released by an electron observed as?

A

Distinct lines

242
Q

What makes the successive lines in the spectrum get closer?

A

With increasing distance from the nucleus, the energy levels get closer

243
Q

When has ionisation occurred?

A

When an electron is promoted from the first energy level to convergence

244
Q

When an electron is promoted from the first energy level to convergence, what has occurred?

A

Ionisation

245
Q

What is the ionisation energy of hydrogen?

A

The energy needed to transfer the electron from e=1 to e=♾️

246
Q

In which series does the the transition of hydrogen from e=1 to e=♾️ in order to ionise occur?

A

The Lyman series

247
Q

How do you calculate the ionisation energy of hydrogen?

A

E=hf
where f is the frequency of the convergence line in the Lyman series

248
Q

What is f in the E=hf formula for the ionisation energy of hydrogen?

A

the frequency of the convergence line in the Lyman series

249
Q

Which successive ionisation energy is the lowest and why?

A

The first as it’s the furthers from the nucleus

250
Q

Why is it unlikely that stable compounds containing Ba3+ ions exist?

A

-Barium is in group 2 and has 2 outer electrons
-Too much energy is needed to remove a third electron
-This necessitates removing an electron from a shell closer to the nucleus (to form a Ba3+ ion)

251
Q

Wave particle duality

A

Electrons can act like waves and particles

252
Q

What’s the phrase that expresses that electrons can act like waves and particles?

A

Wave particle duality

253
Q

What are the colours of the stripes on the Balmer series?

A

violet, dark blue, blue and red

254
Q

Which band has the highest amount of energy in the Balmer series?

A

Violet

255
Q

Which band has the highest wavelength in the Balmer series?

A

Red

256
Q

What’s it important to do when writing the arrows on a diagram showing how the spectrums arise?

A

Show their DIRECTION

257
Q

What do we know if an electron falls to n=1 on the hydrogen emission spectrum?

A

It’s part of the Lyman series

258
Q

What energy equations do we use when given frequency vs when given wavelength?

A

Frequency
E= hf

Wavelength
E= hc
—
upside down y

259
Q

Which series has the lowest wavelength?

A

Lyman series

260
Q

How do we calculate the first IE of an element in kJmol-1?

A

2 ways…
Either use E= hc
—
upside down y

Or
E=hf
(which you’d then have to use f=c
—
upside down y

for)

261
Q

What’s important to remember to do when calculating the first IE of an element in kJmol-1?

A

-change nm to metres
-change J to Jmol-1 (multiply by Avogadro constant)
-change Jmol-1 to kJmol-1 (divide by 1000)

262
Q

How do you get a unit in mol-1?

A

Multiply by Avogadro constant

263
Q

Why can atoms only emit certain definite frequencies of visible light?

A

-They energy levels are fixed/quantised
-Electron falls from higher energy levels

264
Q

What does the convergence limit of the Lyman series represent?

A

ionisation of the atom

265
Q

Why do the lines within each series of emission spectrums converge?

A

Energy difference between the shells decreases/energy levels get closer together

266
Q

How do you determine the group from successive ionisation energy?

A

-Look for a significant jump in IE - from an inner principal quantum shell
-Whichever one it’s jumped from = the group (e.g - 2nd = group 2)

267
Q

How do you identify an element from successive ionisation energies?

A

Electrons before the jump are valence electrons (the electrons in the outer shell)
= find the elements with that valence

268
Q

Valence

A

The electrons in the outer shell
Eg - Sodium valence = 1
(2,8 electrons used in first two shells, one left (atomic number of 11))

269
Q

Draw and label an electric discharge tube

A

(Check notes)

270
Q

What’s it important to remember with the penetrating power of gamma waves?

A

Concrete and lead only decreases it, not stop it

271
Q

What is an alpha particle?

A

A helium nucleus (key word - nucleus)

272
Q

What does having the greatest nuclear charge mean in terms of ionisation energy?

A

Has the largest last ionisation energy as the nucleus has the greatest charge to the last electron

273
Q

What does ionisation involve?

A

A transfer of energy from the radiation passing through that matter to the matter itself

274
Q

How do we calculate the maximum number of electrons we can fit in a shell?

A

2n squared, where n is the principal quantum number (the number of the shell)

275
Q

Principal quantum numbers

A

The numbers of the shells on an atom

276
Q

The distance of WHAT from the nucleus affects the first ionisation energy?

A

The outer electron

277
Q

What does an electron emit when falling down an energy level?

A

Electromagnetic radiation

278
Q

Describe the emission spectrum of hydrogen

A

-Coloured lines (violet, dark blue, blue, red) on a black background
-The lines converge with increasing frequency/energy

279
Q

Whats special about the Balmer series?

A

All lines can be seen in the visible part of the electromagnetic spectrum

280
Q

How can the atomic emission spectrum of hydrogen be used to determine a value for its ionisation energy?

A

E = hf
(Where f is the frequency of the convergence limit in the Lyman series)

281
Q

How do we convert from J to kJmol-1?

A
  1. X NA (Avogadro constant) - Jmol-1
  2. Divide by 1000 - kJmol-1
282
Q

What is radioactive decay?

A

The process that takes place when an unstable atomic nucleus loses energy by emitting radiation

283
Q

What is alpha decay?

A

A type of radioactive decay, during which an atomic nucleus loses two protons and two neutrons.
An alpha particle is equivalent to a helium nucleus.
Makes an element more stable by reducing the atomic number by 2 and the mass number by 4.

284
Q

Why is gamma radiations ionising power so low compared to alpha and beta?

A

Short wavelength

285
Q

Alpha particle range in air

A

Less than 5cm

286
Q

Beta particles range in air

A

Less than 1m

287
Q

Gamma wave range in air

A

Infinite

288
Q

Which type of electromagnetic radiation has an infinite range in air?

A

Gamma wave

289
Q

What’s a sub shell?

A

A division of electron shells separated by orbitals
(S, p d and f)

290
Q

What determines the chemical properties of an element?

A

Its electronic configuration

291
Q

Whats does electronic configuration determine for an element?

A

Its chemical properties

292
Q

Why does alpha radiation have the highest ionising power?

A

High positive charge

293
Q

How do beta particles ionise an atom?

A

Collides with the electron and knocks it out of the atom

294
Q

What type of radiation is often used in medical tracers? Why?

A

Gamma, as they can easily penetrate through the skin and aren’t very ionising + not as easily absorbed by cells as alpha radiation

295
Q

What actually are the 70, 72 and 74 numbers in the mass spectrum of chlorine? What does this mean?

A

Unified atomic mass units (u)

1u = the mass of 1/12 of the carbon-12 atom

296
Q

What does the fact that electrons are quantised mean for them?

A

-Sharp lines on the spectrum
-Emit discrete frequencies of light

297
Q

What do I need to ensure I’m doing enough of when answering ionisation energy questions?

A

Making references to specific subshells

298
Q

Why do the first row of d-block elements have a similar 1st ionisation energies?

A

-Electron removed comes from the 4s orbital
-As you add an extra proton to the nucleus, you add an extra electron to the 3d orbital, screening the affect of the extra proton

299
Q

Why is zinc’s first ionisation energy significantly higher than copper’s?

A

-Electron removed comes form the 4s orbital with a complete 3d level inside = equal screening
- Increase = attraction of the extra proton in the nucleus

300
Q

What is labelled as “y” on an orbital diagram?

A

The direction the orbital is facing

301
Q

Why do the mass numbers not change on isotopes undergoing radioactive decay by beta emission or electron capture?

A

Involves electrons with very little mass

302
Q

What do we do when showing the defective angle of a positron in an electrical field?

A

Attract it towards the negative side, similar to the beta one (only in the other direction) if it’s present

303
Q

What loses energy for gamma radiation to be emitted?

A

An atom

304
Q

Which way would the arrows face on the energy level diagram for an absorption spectrum?

A

Upwards

305
Q

Which way would the arrows face on an energy levels diagram for an emission spectrum?

A

Downwards

306
Q

What do we need to remember to do when writing equations for first ionisations?

A

-Include state symbols
-Put the electron on the right hand side of the equation
-Whatever labelled as = target

307
Q

Where do you remove the electron from first with the d block elements?

A

The 4s orbital

308
Q

What must we remember to include in the definition of molar first ionisation energy when its “STANDARD molar first ionisation energy”?

A

Under STANDARD conditions

309
Q

What is the whole system of a mass spectrometer under?

A

Vacuum

310
Q

Which region of the electromagnetic spectrum is the lyman series in?

A

UV

311
Q

Which orbital do we fill and empty first for transition metals?

A

4s

312
Q

Why are there several series on lines in the hydrogen emission spectrum?

A

Each series corresponds to electrons falling to different energy levels

313
Q

kJmol^-3 to J

A

X1000, divide by Na

A level Chemistry (39 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions