Brainscape's Knowledge GenomeTM

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


See full index

A-level chemistry my notes > Ph 1 Atomic Structure > Flashcards

Ph 1 Atomic Structure Flashcards

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

Democritus

A

Atoms are indivisible

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

John Dalton

A

1803
Atoms are indivisible.
Atoms of an element are identical
Different elements have atoms of different mass and size

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

Becquerel

A

1896
Radioactivity
Atoms can be split up

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

JJ Thompson

A

1897
Discovered the electron
Electrons are identical and negatively charged
Atoms are mainly positive with electrons scattered within the structure.
Plum pudding model

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

Rutherford

A

1911
Fired alpha particles at gold foil
Atoms are mainly empty space with a central positive nucleus surrounded by negatively charged electrons
Nuclear model

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

Bohr

A

1913
Electrons orbit the nucleus in fixed energy levels or shells.
Movement between shells emits energy

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

Chadwick

A

1932

Discovers the neutron

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

Arrangement of electrons

A

Electrons are arranged into main energy levels or shells.
These are split into sub-shells (s,p,d,f), each main shell has n number of sub-shells.
Each subshell consists of electron orbitals each holding a maximum of two electrons with opposite spins.
Orbitals should be thought of as a region of space where an electron in likely to be found.

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

Pauli’s Principle

A

No more than two electrons can occupy the same orbital

Electrons in the same orbital have opposite spins.

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

Aufbau Principle

A

Electrons fill lower energy atomic orbitals before filling higher energy ones

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

Hunds Rule of Maximum Multiplicity

A

Every orbital in a subshell is singly occupied with one electron before any one orbital in that subshell is doubly occupied.
All electrons in singly occupied orbitals have the same direction of spin.

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

order of electron fill up to 4p

A

1s 2s 2p 3s 3p 4s 3d 4p
The 4s and 3d orbital can overlap in energy level, the 4s orbital is actually a lower energy level so is filled with electrons first. 4s will also lose electrons before 3d.

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

s sub shell

A

found in all main shells

Contains one orbital = two electrons

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

p shell

A

Found from the second shell and upwards

contains three orbitals = six electrons

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

d shell

A

found from the third shell and upwards

contains five orbitals = ten electrons

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

Electronic configuration of copper

A

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

*Second numbers after subshell should be written in super script

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

Electronic configuration of Chromium

A

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

*Second numbers after subshell should be written in super script

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

Reason for chromium and copper anomalies in electronic configuration.

A

The 4s and 3d lie very close together in energy levels. The 4s sub-shell only contains one electron to allow the 3d sub-shell to be completely or half full as this is a more stable arrangement. Having a singly occupied 4s orbital decreases electron repulsion.

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

Proton overview

A

mass = 1.673x10^-27 (1)
charge= 1.602x10^-19 (+1)
Is a nucleon, found in the nucleus.

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

neutron overview

A

mass=1.675x10^-27 (1)
charge=0
Is a nucleon, found in the nucleus

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

electron overview

A

mass= 0.911x10^-30 (1/1840)
charge = -1.602x10^-19 (-1)
Found in shells orbiting the nucleus.

22
Q

What is an isotope?

A

Atoms of the same element, meaning they have the same number of protons, but with a different number of neutrons changing the mass number.
Isotopes of an element are chemically identical as they have the same electronic configuration

23
Q

Isotopes of Chlorine

A

35Cl 75% 37Cl 25%

24
Q

Chlorine molecule abundance

A 
35Cl+35Cl
35Cl+37Cl
37Cl+35Cl
37Cl+37CL multiply abundance of isotopes
72Cl = 6/16
74Cl = 1/16
70Cl=9/16
25
Q

Isotopes of carbon

A

12C 98.89
13C 1.11
14C traces

26
Q

Purpose of a mass spectrometer

A

To find the abundance and mass of each isotope in an element allowing us to calculate the Ar.
To find the relative molecular mass of a substance of molecules

27
Q

What are the four stages in a TOF mass spectrometer?

A

Ionisation
Acceleration
Flight tube
Detection

28
Q

Electron impact ionisation

A

Used for elements and substances with a low formula mass
Sample is vaporised so it is gaseous
An electron gun fires high energy electrons at the sample
This knock off one proton from each particle forming a +1 ion

29
Q

What is an electron gun?

A

A hot wire filament with a current running through it.

30
Q

Equation for electron impact ionisation

A

X(g) + e- -> X+1(g) + 2e-

31
Q

Electrospray ionisation

A

Used for substances with a higher molecular mass
Sample dissolved in a high volatile solvent
Injected through a fine hypodermic needle to give a fine mist
The needle is attached to the positive terminal of a high voltage power supply.
The particles gain a proton from the solvent forming a +1 ion. (Mr increases by one)
The solvent evaporates.

32
Q

Equation for electrospray ionisation

A

X(g) + H+ –> XH+(g)

33
Q

Why is the mass spectrometer kept under a vaccum?

A

To prevent the ions produced from colliding with molecules in the air.

34
Q

Why must ions be used in a mass spectrometer?

A

Only ions will interact with and be accelerated by the electric field to have the same kinetic energy
Only positive ions will gain an electron at the detector to generate a current and be detected.

35
Q

What can be manipulated to guide ions produced to the detector?

A

The electric field

36
Q

Acceleration in a mass spectrometer

A

Positive ions are accelerated using an electric field to have the same kinetic energy.
KE= 0.5mv^2
Lighter particles will have a faster velocity.

37
Q

Flight tube in a mass spectrometer

A

The accelerated positive ions pass through a hole in a negative plate into a tube. The time of flight of each ion through this tube depends on its velocity which, as each ion has the same kinetic energy, depends on each mass. The ions separate with lighter, faster ions reaching the detector first.

38
Q

Detection in a mass spectrometer

A

Positive ions hit a negatively charged plate.
Gain an electron as they hit the detector plate creating a movement of charge.
This generates a current that can be detected and is proportional to the amount of ions hitting the plate measuring their abundance.

39
Q

What is a mass spectrum?

A

A graph produced by a computer using the data from the mass spectrometer.
x axis - m/z ratio
y axis - abundance

40
Q

Element mass spectrum

A

can be used to calculate relative atomic mass

significantly lighter peaks are caused by 2+ ions of isotopes

41
Q

Molecule mass spectrum

A

The highest peak to the right is the molecular ion peak and the m/z gives the Mr, however in electrospray ionisation the Mr is the m/z minus one (weight gained by the proton)
Significantly lighter peaks are caused by fragmentation.

42
Q

Define relative atomic mass.

A

The average mass of one atom considering the existence of isotopes and their abundance divided by 1/12 the mass of one atom of carbon 12

43
Q

How do you calculate relative atomic mass?

A

(Sum of isotope abundance multiplied by mass) / sum of isotope abundance.

44
Q

Define first ionisation energy

A

The minimum energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous one plus ions.

45
Q

Define second ionisation energy

A

The minimum energy required to remove one mole of electrons from one mole of gaseous one plus ions to create one mole of gaseous two plus ions.

46
Q

What must we remember about ionisation equations?

A

The atom/ion must be gaseous.

47
Q

What is the trend of successive ionisation energies?

A

Electrons are removed one by one starting with the outer electron and moving inwards.
Successive ionisation energies increase slightly as the electron in being removed from a more positive species meaning their is a greater force of attraction between the nucleus and outer electron.
A large increase occurs when the electron is taken from a new shell as there is a large decrease in shielding.

48
Q

Successive ionisation energy trends is evidence for what.

A

The existence of principle energy shells.

A change of shell is shown by a large increase between successive ionisation energies.

49
Q

General trend of ionisation energy across a group

A 
Increases
more protons (greater nuclear charge)
smaller atomic radius
similar shielding
greater force of electrostatic attraction between the nucleus and outer electron.
50
Q

Group 2-3 trend in ionisation energy

A

Decreases
Group 2’s outer electron is taken from a s orbital
Group 3’s outer electron is taken from a p orbital.
Higher energy level, weaker force of attraction.
This is evidence for the existence of sub-shells.

51
Q

Group 5-6 trend in ionisation energy

A

Decreases
Group 5 the electron is removed from a singly occupied orbital
Group 6 the electron is removed from a doubly occupied/ paired orbital.
Greater electron- electron repulsion
Less energy required
This is evidence for Hund’s rule

52
Q

Trend in ionisation energy down a group

A

Decreases
Greater atomic radius
More shielding
Weaker force of attraction.

A-level chemistry my notes (7 decks)

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