Welcome to the Quiz!
This quiz contains 18 questions from a mix of 1 subtopics.
What is the term for the reduction in attraction between outer electrons and the nucleus due to the presence of inner shells of electrons?
repulsion
shielding
attraction
repelling
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First ionisation energy is the energy required to remove mole of from one mole of atoms.
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Which equation correctly shows the first ionisation energy of sodium?
Na(s) ➔ Na+(s) + e-
Na(s) + e- ➔ Na+(s)
Na(g) ➔ Na+(g) + e-
Na(g) + e- ➔ Na+(g)
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Select ALL of the factors which affect ionisation energy.
atomic radius
nuclear charge
number of neutrons
shielding
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What happens to ionisation energy when atomic radius increases?
it stays the same
it increases
it decreases
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As nuclear charge increases, ionisation energy
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How does ionisation energy change as shielding increases?
it decreases
it increases
it stays the same
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The greater the electrostatic attraction between nucleus and outermost electron, the the ionisation energy
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First ionisation energy down a group, as the electrostatic attraction between the nucleus and outermost electron becomes .
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Which statement is incorrect?
as you go down a group, the nuclear charge increases
as you go down a group, the shielding decreases
as you go down a group, the atomic radius increases
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What is the general trend in first ionisiation energies going across a period on the periodic table?
first ionisation energy increases
first ionisation energy decreases
first ionisation energy remains the same
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Why is the ionisation energy of oxygen less than that of nitrogen?
the outer electron in oxygen is paired in a 2p orbital
the outer electron in oxygen is in a higher energy subshell
the outer electron in oxygen is unpaired in a 2p orbital
the outer electron in oxygen is in a lower energy subshell
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The distance between the nucleus and an electron in a 2s orbital is than the distance between the nucleus and an electron in a 2p orbital
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How do two electrons in the same orbital interact?
they don't interact
they repel
they attract
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What is the trend in successive ionisation energies of an element?
they increase
they don't change
they decrease
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The graph shows successive ionisation energies for an element. Which group of the periodic table is this element in?
3
4
1
7
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Which correctly shows the second ionisation energy of magnesium?
Mg+(g) ➔ Mg2+(g) + e-
Mg(g) ➔ Mg2+(g) + 2e-
Mg+(s) ➔ Mg2+(s) + e-
Mg(g) ➔ Mg+(g) + e-
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Why is the ionisation energy of boron less than that of beryllium?
the outer electron in boron is paired in a 2s orbital
the outer electron in boron is in a lower energy subshell
the outer electron in boron is in a higher energy subshell
the outer electron in boron is unpaired in a 2s orbital
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