Atomic structure

The sample of chromium is analysed in a time of flight (TOF) mass spectrometer. Give two reasons why it is necessary to ionise the isotopes of chromium before they can be analysed in a TOF mass spectrometer. (2 marks)

The sample of chromium is analysed in a time of flight (TOF) mass spectrometer. Give two reasons why it is necessary to ionise the isotopes of chromium before they can be analysed in a TOF mass spectrometer. (2 marks)

• Ions will interact with and be accelerated by an electric field

• Ions create a current when hitting the detector

One of the methods of ionising samples in time of flight mass spectrometry is by electron impact. How is this ionisation done? (4 marks)

• high energy electrons

• from electron gun

• fired at sample

• knocks off one electron

A second method of ionising samples in time of flight mass spectrometry is by electrospray ionisation. How is this ionisation done? (4 marks)

• sample dissolved in volatile solvent

• injected through a fine hypodermic needle giving a fine mist / aerosol

• tip of needle has high voltage

• each gains a proton as it leaves the needle

A sample of germanium is analysed in a TOF mass spectrometer using electron impact ionisation. Give an equation, including state symbols, for the process that occurs during the ionisation of a germanium atom. (1 mark)

Ge_(g) + e^- → Ge⁺_(g) + 2 e^-
OR
Ge_(g) → Ge⁺_(g) + e^-

The first ionisation energies of the elements in Period 2 change as the atomic number increases. Explain the pattern in the first ionisation energies of the elements from lithium to neon (6 marks)

Stage 1: General Trend (Li → Ne)

1st IE increases
More protons/increased nuclear charge
Electrons in same energy level, no extra shielding

Stronger attraction between nucleus and outer e^- (ignore radius decreases)

 Stage 2: Deviation Be → B
B lower than Be
Outer electron in 2p
Higher in energy than 2s

Stage 3: Deviation N → O

O lower than N
2 electrons in 2p are paired in orbital
Pairing causes repulsion

The products of the reaction were separated and analysed in a time of flight (TOF) mass spectrometer. Two peaks were observed at m/z = 104 and 118.
Outline how the TOF mass spectrometer is able to separate these two species to give two peaks. (4 marks)

• Positive ions are accelerated by an electric field

• To a constant kinetic energy

• The positive ions with m/z of 104 have the same kinetic energy as those with m/z of 118 and move faster

• Therefore, ions with m/z of 104 arrive at the detector first

Explain why the atomic radius decreases across Period 3, from sodium to chlorine. (2 marks)

• The number of protons increases

• Shielding is similar/same OR electrons are added to the same shell

In a TOF mass spectrometer, explain how:

• ions are accelerated

• ions are detected

• the abundance of ions is determined

  (3 marks)

• Ions are accelerated by an electric field

• Detected by gaining electrons

• The current produced is proportional to ion abundance

What are the electron configurations of chromium and copper?

• Cr is [Ar] 3d⁵ 4s¹ (not [Ar] 3d⁴ 4s²⁾

• Cu is [Ar] 3d¹⁰ 4s¹ (not [Ar] 3d⁹ 4s²⁾

This is because these configurations are energetically stable.

State, in terms of fundamental particles, why the isotopes ¹⁰B and ¹¹B have similar chemical reactions. (1 mark)

• Same number of electrons

Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron. (1 mark)

• Electron being removed from a positive ion (therefore needs more energy)

Explain why the value of the first ionisation energy of neon is higher than that of sodium. (2 marks)

• In Ne the outer electron is lost from a 2p subshell, in Na it is lost from 3s

• Less shielding by inner electrons in Ne

Sketch a graph to show the successive ionisation energies of sodium. (2 marks)

Explain, in terms of structure and bonding, why the melting point of magnesium is higher than the melting point of sodium. (2 marks)

• Magnesium is a smaller ion compared to sodium

• Mg²⁺ has a higher charge than Na⁺

  (stronger electrostatic forces of attraction)