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3.1 Physical Chemistry > 3.1.1 Atomic structure > Flashcards

3.1.1 Atomic structure Flashcards

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1
Q

Nucleons

A

Nucleons are protons and neutrons in the nucleus.

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2
Q

Position of protons

A

Nucleus

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3
Q

Relative mass of a proton

A

1

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4
Q

Relative charge of a proton

A

+1

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5
Q

Position of neutrons

A

Nucleus

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6
Q

Relative mass of a neutron

A

1

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7
Q

Relative charge of a neutron

A

0

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8
Q

Position of electrons

A

Orbitals

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9
Q

Relative mass of an electron

A

1/1800

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10
Q

Relative charge of an electron

A

-1

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11
Q

Mass number

A

Sum of protons and neutrons

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12
Q

Atomic number

A

The amount of protons in the nucleus

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13
Q

Number of neutrons is worked out by…

A

Subtracting the atomic number from the mass number

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14
Q

Isotopes

A

Atoms of the same element with the same number of protons but a different amount of neutrons

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15
Q

Isotopes have similar chemical properties because…

A

they have the same electron configuration

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16
Q

Isotopes have varying physical properties because…

A

they have different masses

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17
Q

Ions

A

A charged particle formed when an atom or molecule gains

or loses one or more electrons

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18
Q

Relative Isotopic Mass

A

The mass of an atom of a particular isotope compared to 1/12

the mass of an atom of carbon-12

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19
Q

Relative Atomic Mass (Ar)

A

The average mass of an atom compared to 1/12 the mass of

an atom of carbon-12

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20
Q

Relative Molecular Mass (Mr)

A

The average mass of a molecule compared to 1/12 the mass

of an atom of carbon-12

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21
Q

Mass Spectrometer: Why is it kept in vacuum conditions?

A

To prevents the ions produced colliding with molecules of air

22
Q

Mass Spectrometer: What happens during ionisation?

A

The sample is dissolved in a volatile solvent and forced
through a fine, hollow needle which is connected to a
positive terminal of a high voltage supply. The sample is shot
with an electron gun, which knocks off an electron,
producing positively charged ions.

23
Q

Mass Spectrometer: What happens during acceleration?

A

Positive ions are attracted to a negatively charged plate,
causing them to accelerate. Lighter ions with a higher charge
move faster

24
Q

Mass Spectrometer: What happens during ion drift?

A

The ions pass through a hole in the negatively charged plate,
forming a beam, which drift towards the detector

25
Q

Mass Spectrometer: What happens during detection?

A

The lighter ions which have the fastest velocities arrive at the
detector first. The positive ions pick up an electron, causing a
current to flow

26
Q

Mass Spectrometer: What happens during data analysis?

A

Signals from the detector are passed to a computer which

generates a mass spectrum

27
Q

Mass Spectrometer: What is the mass spectrometer

measuring?

A

M:Z ratio and abundance

28
Q

How do you calculate R.A.M from a mass spectrum?

A

You multiply the m:z ratio and abundance together for each
peak. You then add the totals together and divide by the total
relative abundance.

29
Q

What sub-level can principle level 1 hold?

A

1s

30
Q

What sub-levels can principle level 2 hold?

A

2s, 2p

31
Q

What sub-levels can principle level 3 hold?

A

3s, 3p, 3d

32
Q

What sub-levels can principle level 4 hold?

A

4s, 4p, 4d, 4f

33
Q

How many electrons can sub-level S hold?

A

2

34
Q

How many electrons can sub-level P hold?

A

6

35
Q

How many electrons can sub-level D hold?

A

10

36
Q

How many electrons can sub-level F hold?

A

14

37
Q

What shape are S sub-levels?

A

Spherical

38
Q

What shape are P sub-levels?

A

Dumbbells

39
Q

Why is the 3d sub-level filled after the 4s sub-level?

A

Because 3d is higher in energy, so 4s is filled first and then
when 3d is filled, the energy level drops to below 4s

40
Q

First Ionisation Energy

A

The enthalpy change when one mole of gaseous atoms forms
one mole of gaseous atoms with a singe positive charge by
losing one electron

41
Q

Second Ionisation Energy

A

The enthalpy change when one mole of gaseous ions with a
single positive charge forms one mole of gaseous ions with a
2+ charge by losing one electron

42
Q

Factors affect ionisation energy: Nuclear Charge

A

The higher the nuclear charge (the more protons there are)

the greater the attraction of the outer electrons to the nucleus

43
Q

Factors affect ionisation energy: The distance of the outer

electrons to the nucleus

A

The larger the atom, the further the outer electrons are away
from the nucleus, making the attraction weaker

44
Q

Factors affect ionisation energy: Shielding

A

Electrons in the outer shell are repelled by electrons in
complete inner shells, weakening the attraction of the
nucleus

45
Q

Factors affect ionisation energy: In-orbital Repulsion

A

Once the electrons are paired, they start repelling each other,
the degree of repulsion affects how easy it is to remove
electrons

46
Q

Why are the successive ionisation energies always higher?

A

Because a positive ion is formed from the first ionisation
energy, meaning the nuclear attraction increases, making it
harder for the second electron to be removed

47
Q

Why is He’s ionisation energy bigger than H’s?

A
  • Increased nuclear charge (gone from + to +2)
  • Same shielding
  • Same distance from nucleus to outer electron
48
Q

Why is there such a large drop of ionisation energy between

He and Li?

A
  • Increased shielding (Li enters 2s orbital, He still on 1s)
  • Increased nuclear charge
  • Outer electrons are further away from the nucleus
49
Q

Why is Be’s ionisation energy greater than Li?

A

-Increased nuclear charge
-Shielding same as Li
-Outer electrons are the same distance away from the nucleus
in both

50
Q

Why is Be’s ionisation energy higher than B?

A

-Increased nuclear charge
-Increased shielding (B enters 2p orbital) so is shielded by 1s
and 2s orbitals
-Outer electrons are further away in B

51
Q

Why is there a drop of ionisation energy between N and O?

A
  • Increased nuclear charge
  • Shielding same (still in 2p orbital)
  • Same amount of shielding

3.1 Physical Chemistry (5 decks)

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