Lesson 1.2.1
1.2.1 First and successive ionisation energies Quiz: Pearson Edexcel Chemistry, Unit 1
20 questions
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Lesson 1.2.1, First and successive ionisation energies: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 1: Atomic Structure and the Periodic Table, written with Revision Ninja.
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The 20 questions
-
Which state of matter must atoms be in for first ionisation energy?
- Liquid
- Solid
- Aqueous
- Gaseous
-
Which equation represents the first ionisation energy of sodium?
- Na(g) -> Na+(g) + e-
- Na(g) + e- -> Na-(g)
- Na+(g) -> Na2+(g) + e-
- Na(s) -> Na+(s) + e-
-
Which equation represents the second ionisation energy of magnesium?
- Mg(g) -> Mg2+(g) + 2e-
- Mg2+(g) -> Mg3+(g) + e-
- Mg(s) -> Mg+(s) + e-
- Mg+(g) -> Mg2+(g) + e-
-
Why are successive ionisation energies always larger than the previous one?
- Weaker nuclear charge
- More positive ion
- Larger atomic radius
- Fewer total protons
-
Which factor does NOT directly increase first ionisation energy?
- Neutron number
- Nuclear charge
- Electron shielding
- Atomic radius
-
Which element in Period 3 has the lowest first ionisation energy?
- Magnesium
- Sodium
- Argon
- Aluminium
-
Successive ionisation energies (kJ/mol) of an element are 578, 1817, 2745, 11578. How many electrons are in its outer shell?
- 4
- 3
- 2
- 1
-
Successive ionisation energies (kJ/mol) of an element X are 738, 1451, 7733, 10540. Which group does X belong to?
- Group 1
- Group 2
- Group 4
- Group 3
-
Successive ionisation energies (kJ/mol) of X are 496, 4562, 6910, 9543. What is the most likely group of X?
- Group 2
- Group 1
- Group 3
- Group 7
-
Successive ionisation energies measure the removal of electrons from what species?
- Gaseous ions
- Aqueous atoms
- Solid metals
- Liquid molecules
-
Why is the first ionisation energy of boron lower than that of beryllium?
- Paired 2s electrons
- Higher 2p energy
- Fewer inner shells
- Greater nuclear charge
-
Why is the first ionisation energy of lithium higher than that of sodium?
- Smaller atomic radius
- More inner shielding
- Larger mass number
- Lower nuclear charge
-
What is the general trend in first ionisation energy across Period 2?
- Constant value
- General decrease
- General increase
- Random fluctuation
-
Which element has the greatest first ionisation energy?
- Fluorine
- Neon
- Oxygen
- Sodium
-
Why is the first ionisation energy of oxygen lower than that of nitrogen?
- Orbital pair repulsion
- Extra shielding shell
- Higher nuclear charge
- Smaller atomic radius
-
A large jump in successive ionisation energies between electrons 4 and 5 indicates what?
- Isotope change
- Sub-shell change
- Neutral atom loss
- New inner shell
-
Why is the second ionisation energy of an element greater than the first?
- Decreased nuclear charge
- More electron shielding
- Increased net attraction
- Larger ionic radius
-
Why is the first ionisation energy of aluminium lower than that of magnesium?
- Smaller atomic radius
- Outer 3s electron
- Outer 3p electron
- Higher nuclear charge
-
Why is potassium's first ionisation energy lower than lithium's?
- Smaller atomic radius
- Increased atomic shielding
- Higher nuclear charge
- Fewer inner shells
-
Which factor directly causes an increase in first ionisation energy?
- Greater nuclear charge
- More inner shells
- Increased shielding
- Larger atomic radius
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