(a) Define first ionisation energy. (b) Successive ionisation energies for element A are shown in Table 1.1. Table 1.1 ionisation 1st 2nd 3rd 4th 5th 6th 7th 8th :--- :---: :---: :---: :---: :---: :---: :---: :---: ionisation energy / $\text{kJ mol}^{-1}$ 1310 3390 5320 7450 11000 13300 71000 84100 Use Table 1.1 to deduce the group of the Periodic Table that A belongs to. Explain your answer. Group ............... (c) Across Period 3 there is a general trend for first…

Chemistry 9701/23 — May/June 2022

Cambridge AS Level · AS Level Structured Questions · worked solutions for every part, with the mark scheme

questions

marks

minutes

Topics Hydroxy Compounds · Chemical Bonding · States of Matter · Group 17 · Hydrocarbons · Atomic Structure · +9 more

Q1Atomic StructureChemical BondingAtoms, Molecules and StoichiometryStates of MatterFree sample

(a)

Define first ionisation energy.

(b)

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

Table 1.1

ionisation	1st	2nd	3rd	4th	5th	6th	7th	8th
ionisation energy / $\text{kJ mol}^{-1}$	1310	3390	5320	7450	11000	13300	71000	84100

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

Group ...............

(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.

(d)

In an $\text{Al}^{2+}$ ion the nuclear attraction for the outer electron is stronger than in an atom of $\text{Na}$ .

Compare the electronic structures of $\text{Al}^{2+}$ and an atom of $\text{Na}$ and explain why the third ionisation energy of aluminium is greater than the first ionisation energy of sodium.

(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

	atomic number	nucleon number	number of neutrons	electronic arrangement
copper-65

(f)

(i)

The element copper has a relative atomic mass of 63.5.

Calculate how many atoms are present in $1.05\text{ g}$ of copper.

atoms of copper present = ..............................

(ii)

Copper has a melting point of $1085\text{ }^\circ\text{C}$ and a high electrical conductivity.

Explain these properties of copper by referring to its structure and bonding.

The rest of this paper

4 more questions

Q2Chemical Periodicity · Group 17 · States of Matter10M
Q3Chemical Bonding · Chemical Energetics · Equilibria · Reaction Kinetics · Introduction to Organic Chemistry · Hydroxy Compounds · Carbonyl Compounds16M
Q4Hydrocarbons · Halogen Compounds · Group 17 · Hydroxy Compounds12M
Q5Hydrocarbons · Hydroxy Compounds · Analytical Techniques9M

Loading the full paper…