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Edexcel A Level Chemistry (9CH0)

Topic 1
Atomic Structure
& The Periodic Table

Topic 1 establishes the foundation of atomic theory: subatomic particles, isotopes, mass spectrometry, electron configuration, ionisation energies and periodic trends. These ideas underpin every other topic in the course and explain how experimental evidence supports the modern model of the atom.

Exam Paper
Paper 1
9CH0/01 – Advanced Inorganic and Physical Chemistry
Specification Points
1 – 26
26 points covered
Topic Parts
5 parts
Revision notes available
Exam Board
Edexcel
Pearson 9CH0

Revision Notes

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Atoms and isotopes
Atomic
Structure
protons, neutrons, electrons and isotopes
1
Available

Atomic Structure

Subatomic particles, relative mass and charge, atomic number, mass number, isotopes, relative isotopic mass and relative atomic mass.

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Spectra and abundance
Mass
Spectrometry
RAM, diatomic spectra and molecular ions
2
Available

Mass Spectrometry

Interpreting mass spectra, calculating relative atomic mass from isotope abundance, predicting diatomic spectra and determining relative molecular mass.

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Orbitals and subshells
Electron
Configuration
s, p, d subshells, orbital notation and blocks
3
Available

Electron Configuration

Quantum shells, s and p orbital shapes, sub-shells, electrons-in-boxes notation, electronic configurations up to Z = 36 and s, p, d block classification.

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Energy and shielding
Ionisation
Energy
first IE, successive IE, proton number and shielding
4
Available

Ionisation Energy

First and successive ionisation energies, influence of proton number, electron shielding and sub-shell, and evidence for electronic structure.

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Repeating patterns
Periodic
Trends
melting points, ionisation energy and periodicity
5
Available

Periodic Trends

Periodicity, trends in melting and boiling temperatures of periods 2 and 3, ionisation energy trends and using data to illustrate periodic properties.

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Specification Coverage

Topic 1 Atomic Structure and the Periodic Table – Edexcel A Level Chemistry (9CH0)

The following specification points outline the knowledge and skills students are expected to demonstrate for Topic 1. All points are assessed in Paper 1 (9CH0/01).

Atomic Structure

1
know the structure of an atom in terms of electrons, protons and neutrons
2
know the relative mass and relative charge of protons, neutrons and electrons
3
know what is meant by the terms atomic (proton) number and mass number
4
be able to determine the number of each type of sub-atomic particle in an atom, molecule or ion from the atomic (proton) number and mass number
5
understand the term isotopes
6
be able to define the terms relative isotopic mass and relative atomic mass, based on the ¹²C scale
7
understand the terms relative molecular mass and relative formula mass, including calculating these values from relative atomic masses. The term relative formula mass should be used for compounds with giant structures.

Mass Spectrometry

8
be able to analyse and interpret data from mass spectrometry to calculate relative atomic mass from relative abundance of isotopes and vice versa
9
be able to predict the mass spectra, including relative peak heights, for diatomic molecules, including chlorine
10
understand how mass spectrometry can be used to determine the relative molecular mass of a molecule. Limited to the m/z value for the molecular ion, M⁺, giving the relative molecular mass of the molecule.

Electron Configuration

15
understand how ideas about electronic configuration developed from:
i
the fact that atomic emission spectra provide evidence for the existence of quantum shells
ii
the fact that successive ionisation energies provide evidence for the existence of quantum shells and the group to which the element belongs
iii
the fact that the first ionisation energy of successive elements provides evidence for electron sub-shells
16
know the number of electrons that can fill the first four quantum shells
17
know that an orbital is a region within an atom that can hold up to two electrons with opposite spins
18
know the shape of an s-orbital and a p-orbital
19
know the number of electrons that occupy s, p and d sub-shells
20
know that electrons fill sub-shells singly, before pairing up, and that two electrons in the same orbital must have opposite spins
21
be able to predict the electronic configurations, using 1s notation and electrons-in-boxes notation, of:
i
atoms, given the atomic number Z, up to Z = 36
ii
ions, given the atomic number Z, and the ionic charge, for s and p block ions only, up to Z = 36
22
know that elements can be classified as s, p and d-block elements
23
understand that electronic configuration determines the chemical properties of an element

Ionisation Energy

11
be able to define the terms first ionisation energy and successive ionisation energies
12
understand how ionisation energies are influenced by the number of protons, the electron shielding and the electron sub-shell from which the electron is removed
13
understand reasons for the general increase in first ionisation energy across a period
14
understand reasons for the decrease in first ionisation energy down a group

Periodic Trends

24
understand periodicity in terms of a repeating pattern across different periods
25
understand reasons for the trends in the following properties of the elements from periods 2 and 3 of the Periodic Table:
i
the melting and boiling temperatures of the elements, based on given data, in terms of structure and bonding
ii
ionisation energy based on given data or recall of the plots of ionisation energy versus atomic number
26
be able to illustrate periodicity using data, including electronic configurations, atomic radii, melting and boiling temperatures and first ionisation energies