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CAIE A-Level Chemistry 1 Atomic Structure

Practise subatomic particles, isotopes, electron arrangements, ionisation energy and atomic or ionic radius using CAIE-style evidence.

Syllabus
2028–2030
Course
Chemistry 9701
Level
AS

Covered syllabus points

1.1 Particles in the atom and atomic radius1.2 Isotopes1.3 Electrons, energy levels and atomic orbitals1.4 Ionisation energy

1. Atomic structure question 1

[Maximum number: 7]

The model of the nuclear atom was first proposed by Ernest Rutherford. He developed this model on the basis of results obtained from an experiment using gold metal foil.

Question (a)

(a)

Complete the table with information for two of the particles in an atom of 197Au{ }^{197} \mathrm{Au}.

Table for Question (a) — CAIE A-Level Chemistry AS
[ 4 ]

Question (b)

(b)

A sample of gold found in the earth consists of only one isotope.

[ 3 ]

Question (i)

(i)

Explain what is meant by the term isotopes.

[ 2 ]

Question (ii)

(ii)

A different sample of gold contains more than one isotope.

Suggest why this different sample of gold has the same chemical properties as the sample found in the earth.

[ 1 ]

1. Atomic structure question 2

[Maximum number: 1]

Neutrons are passed through an electric field. The mass of one neutron relative to 112\frac{1}{12} the mass of a 12C{ }^{12} \mathrm{C} atom and any deflection in the electric field is recorded.

Which row is correct?

mass of

neutron

behaviour of beam of

neutrons in an electric field

0

deflected

1

deflected

0

not deflected

1

not deflected

1. Atomic structure question 3

[Maximum number: 10]

Question (a)

(a)

Define first ionisation energy.

[ 2 ]

Question (b)

(b)

Successive ionisation energies for element A are shown in Table 1.1.

Table 1.1

Table 1.1

Use Table 1.1 to deduce the group of the Periodic Table that A belongs to. Explain your answer. Group

[ 1 ]

Question (c)

(c)

Across Period 3 there is a general trend for first ionisation energies to increase due to the increase in attraction between the nucleus and the outer electron.

Explain why the first ionisation energy of sulfur is less than the first ionisation energy of phosphorus.

[ 2 ]

Question (d)

(d)

In an Al2+\mathrm{A} l^{2+} ion the nuclear attraction for the outer electron is stronger than in an atom of Na .

Compare the electronic structures of Al2+\mathrm{A} l^{2+} and an atom of Na and explain why the third ionisation energy of aluminium is greater than the first ionisation energy of sodium.

[ 2 ]

Question (e)

(e)

An isotope of copper has a relative isotopic mass of 65 .

Complete Table 1.2 for an atom of copper-65.

Table 1.2

Table 1.2

[ 3 ]

1. Atomic structure question 4

[Maximum number: 5]

Vanadium, niobium and tantalum are metals in the same group of the Periodic Table.

Question (a)

(a)

The shorthand electronic configuration of vanadium in the ground state is [Ar]3 d34 s2[\mathrm{Ar}] 3 \mathrm{~d}^{3} 4 \mathrm{~s}^{2}.

[ 3 ]

Question (i)

(i)

State what is meant by the term ground state.

[ 1 ]

Question (ii)

(ii)

Show the electronic configuration of vanadium using electrons in boxes notation.

Figure for Question (ii) — CAIE A-Level Chemistry AS
[ 1 ]

Question (iii)

(iii)

Deduce the total number of electrons in the p sub-shells of a vanadium atom.

[ 1 ]

Question (b)

(b)

Pelopium was the suggested name for a new element discovered in a mineral.

Pelopium was later found to be a mixture of niobium, Nb , and tantalum, Ta .
Only one naturally occurring isotope exists for each of Nb and Ta .

[ 2 ]

Question (i)

(i)

Complete Table 1.1.

Table 1.1

Table 1.1

[ 2 ]
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