Exam code: 9701
Which statement defines the first ionisation energy of an element?
The energy required to remove one electron from one atom in the gaseous state.
The energy required to remove one mole of electrons from one mole of atoms in the solid state.
The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions.
The energy required to remove one mole of electrons from one mole of gaseous 1+ ions.
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Which is the correct equation for the first ionisation energy for magnesium?
Mg → Mg+ + e-
Mg+ (g) → Mg2+ (g) + e-
Mg (g) → Mg+ (g) + e-
Mg+ → Mg2+ + e-
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Which statement explains why the second ionisation energy of magnesium is greater than the first ionisation energy?
There is less shielding after the first electron is removed.
The ionic radius of the magnesium ion increases after the first ionisation.
The nuclear charge increases after the first ionisation.
There is greater attraction between the nucleus and the remaining outer electrons.
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The first five ionisation energies of an element are shown below.
What element could this ionisation energy graph belong to?
Al
N
Na
P
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Which statement does not explain the increase in first ionisation energy across a period?
Nuclear charge increases.
Atomic radius decreases.
Shielding remains constant.
The number of electrons increases.
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The second ionisation energy of magnesium is 1451 kJ mol-1.
Which equation correctly represents this statement?
Mg (g) → Mg+ (g) + e- ΔH = +1451 kJ mol-1
Mg+ (g) → Mg2+ (g) + e- ΔH = +1451 kJ mol-1
Mg (g) → Mg2+ (g) + 2e- ΔH = +1451 kJ mol-1
Mg (g) → Mg+ (g) + e- ΔH = -1451 kJ mol-1
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The successive ionisation energies of element X are shown in the table below. In which group of the Periodic Table is element X found?
Ionisation number of X | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 |
|---|---|---|---|---|---|---|---|---|
Ionisation energy (kJ mol-1) | 1314 | 3388 | 5301 | 7469 | 10989 | 13327 | 71337 | 84080 |
13
14
15
16
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X, Y and Z are consecutive elements in Period 3 of the Periodic Table. Element Y has the highest first ionisation energy and also the lowest melting point of these three elements.
Which row could identify X, Y and Z?
silicon, phosphorus, sulfur
sodium, magnesium, aluminium
aluminium, silicon, phosphorus
magnesium, aluminium, silicon
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Successive ionisation energies for an element, Y, are shown in the table below.
Electrons removed | 1st | 2nd | 3rd | 4th | 5th |
|---|---|---|---|---|---|
Ionisation energy / kJ mol-1 | 736 | 1450 | 7740 | 10500 | 13600 |
What is the most stable ion formed by Y?
Y+
Y2+
Y3+
Y4+
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Values for the successive ionisation energies of an unknown element are given in the table below.
First ionisation energy / kJ mol-1 | Second ionisation energy / kJ mol-1 | Third ionisation energy / kJ mol-1 | Fourth ionisation energy / kJ mol-1 |
|---|---|---|---|
420 | 3600 | 4400 | 5900 |
In which group of the Periodic Table is this element found?
1
2
13
14
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The graph below shows the variation of a physical property for elements in Period 3 (Na to Ar).
Which physical property is shown?
atomic radius
electrical conductivity
melting point
first ionisation energy
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Element X is in period 2 and has the first seven ionisation energies in kJ mol-1 as shown.
1300 | 3380 | 5330 | 7460 | 11 010 | 13 320 | 71 200 |
What is the electronic configuration of element X?
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p6
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Between which two successive ionisation energies of oxygen is the largest increase?
First and second
Fifth and sixth
Sixth and seventh
Seventh and eighth
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The first ionisation energy of beryllium is greater than that of boron.
Which statement explains why?
Boron has a full outer shell.
Boron has a larger atomic radius than beryllium.
The outer electron in boron is in a 2p subshell, which is at a higher energy and further from the nucleus than the 2s subshell of beryllium.
The proton number of beryllium is greater than that of boron.
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The electronic configurations of four different atoms are shown.
Which atom has the highest first ionisation energy?
1s2 2s2 2p6 3s2
1s2 2s2 2p4
1s2 2s2 2p6
1s2 2s2
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The table gives the successive ionisation energies for an element R.
1st | 2nd | 3rd | 4th | 5th | 6th | |
|---|---|---|---|---|---|---|
Ionisation energy / kJ mol-1 | 950 | 1800 | 2700 | 4800 | 6000 | 12300 |
What could be the oxidation state of element R in its chloride?
+1
+2
+3
+4
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