3.1.1 Atomic Structure Flashcards

1
Q

What is the mass of a proton?

A

1

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

What is the mass of a neutron?

A

1.001

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

What is the mass of an electron?

A

0.000005

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

What is J.J Thomson’s discovery?

A

Electrons were smaller than at atom.
Came up with the plum pudding model- electrons were embedded within a positively charged ball of atoms.

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

What did Rutherford discover?

A

Atoms are mostly empty space with a core that is positively charged.
He done this by firing alpha particle at a gold foil and observing that some of the alpha particles bounced back.

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

What did James Chadwick discover?

A

The nucleus is made up of both protons and neutrons.

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

What is an isotope?

A

Different versions of the same elements with a different number of nuetrons

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

Define the relative atomic mass

A

The relative atomic mass (Ar) is the average mass of atoms of an element relative to the mass of an atom of carbon-12

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

How does nuclear charge vary across a period?

A

It increases by 1 as proton number increases

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

What happens to nuclear charge as we go down a group?

A

It increase as the number of protons increases

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

What is nuclear charge?

A

The collective charge of all protons in a nucleus.

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

As the electrons distance from the nucleus increases____

A

The forces it experiences decreases

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

Across a period, the distance between the nucleus and the outer electrons_____

A

Decreases, this is because the nuclear charge increases so it pulls the shells towards the nucleus

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

As we move down a group, the distance between the nucleus and the outer electrons______

A

Increase as the outer electrons are in a different shell.

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

What is shielding?

A

Each electrons shields some of the nuclear charge from the other electrons. An electron closer to the nucleus would shield the charge of a proton

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

As we move across a period, shielding____

A

Is the same

17
Q

Down a group, the amount of shielding in the outer electrons…

A

Increases

18
Q

What is ionisation energy

A

The energy required to remove one mole electrons from one mole of gaseous atom of that element.

19
Q

As you go down a group, first ionisation energy…

A

Decreases. This is because the outer electrons become more shielded and further away from the nucleus so less energy is required to remove the electron

20
Q

Across a period, first ionisation energy…

A

Increases.

This is because nuclear charge increases whilst shielding stays the same, therefore the outer electrons experience stronger attraction to the nucleus.

21
Q

Why is there a dip in ionisation energy between magnesium and aluminium?

A
  • There outer electrons are in different sublevels.
    Magnesium: 3s
    Aluminium: 3p
    Therefore, as aluminium has a 3p orbital which is further from the nucleus and shielded from inner electrons it requires less energy.
22
Q

Explain why there is a dip in ionisation energy between phosphorus and sulfur.

A

Both phosphorus and sulphur have electrons in the 3p orbital. However sulfur has one paired electron which experiences extra repulsion. Therefore requiring less energy then phosphorus.

23
Q

what is stage 1 of mass spectrometry?

A

Ionisation:
the sample is first vapourised and an electron gun fires electrons knocking off one electron, making them 1+ ions.

24
Q

what is stage 2 of mass spectrometry?

A

acceleration:
the positive ions are accelerated by an electric plate with the same kinetic energy. this means that heavier particles will be slower and lighter ones will move faster.

25
Q

what is stage three of mass spectrometry?

A

Ion drift:
the ions are in a vacuum to stop them from slowing down, they carry on drifting toward the next stage.

26
Q

What did dalton discover?

A

Elements react together in different proportion but always in whole number ratios.- found the existence of atoms

27
Q

what is the last stage of mass spectrometry?

A

Detector:
The ions gain an electron from the plate. This movement of electrons creates a current which is detected by a computer which creating a mass spectra.

28
Q
A
29
Q

What experiment did Rutherford do?

A

He done this by firing alpha particle at a gold foil and observing that some of the alpha particles bounced back.

30
Q

What is nuclear force?

A

Protons and neutrons are held together by this

31
Q

What similar properties do isotopes have?

A

Same chemical properties

32
Q

What is the mass number?

A

The number of protons and neutrons.

33
Q

What is an ion?

A

At atom with a positive or negative overall charge

34
Q

What is the atomic number?

A

The number of protons

35
Q

Where does mass and atomic number go?

A

Mass number
Atomic number

36
Q

What is the period table ordered by?

A

Proton number