Lesson 13A.2
13A.2 Polarisation of ions Quiz: Pearson Edexcel Chemistry, Unit 13
20 questions
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Lesson 13A.2, Polarisation of ions: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 13: Energetics II, written with Revision Ninja.
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The 20 questions
-
What process occurs when a cation distorts the electron cloud of a nearby anion?
- Polarisation
- Hydration
- Ionisation
- Atomisation
-
Which property of a cation determines its polarising power?
- Charge density
- Mass number
- Electronegativity
- Electron affinity
-
Which type of anion is the most easily polarised?
- Large, singly charged
- Large, highly charged
- Small, highly charged
- Small, singly charged
-
Which of these cations has the highest polarising power?
- K+
- Al3+
- Na+
- Mg2+
-
Which of these halide ions is the most polarisable?
- F-
- Br-
- Cl-
- I-
-
What effect does polarisation of ions have on an ionic lattice?
- Increases ionic character
- Adds covalent character
- Reduces covalent character
- Adds metallic character
-
Which compound shows the greatest covalent character due to ion polarisation?
- Potassium fluoride
- Sodium fluoride
- Sodium chloride
- Silver iodide
-
Which group 1 chloride has the greatest covalent character?
- Lithium chloride
- Potassium chloride
- Rubidium chloride
- Sodium chloride
-
Why does aluminium chloride have greater covalent character than sodium chloride?
- Smaller anion radius
- Higher charge density
- Lower charge density
- Larger anion charge
-
Which change to a halide anion increases the covalent character of a sodium salt?
- Increasing anion radius
- Decreasing anion radius
- Increasing electronegativity
- Decreasing anion charge
-
An experimental lattice energy is much more exothermic than its theoretical ionic value. Why?
- Perfect ionic bonding
- Significant covalent character
- Significant metallic character
- Exothermic hydration energy
-
Arrange the sizes of the cations Na+ (about 102 pm), Mg2+ (about 72 pm) and Al3+ (about 53 pm) in order of increasing polarising power.
- Al3+ < Na+ < Mg2+
- Al3+ < Mg2+ < Na+
- Mg2+ < Na+ < Al3+
- Na+ < Mg2+ < Al3+
-
What happens to the theoretical lattice energy value when significant covalent character is present in a compound?
- It remains unchanged
- It becomes endothermic
- It is more exothermic
- It is less exothermic
-
Why is lithium iodide more covalent than lithium fluoride?
- Iodide is smaller
- Fluoride is larger
- Iodide is larger
- Fluoride is uncharged
-
Why does the theoretical ionic model underestimate lattice energy for some compounds?
- Nuclei repel cations
- Polarisation occurs
- Complete electron transfer
- Delocalised electrons form
-
Which cation has a higher polarising power: Mg2+ or Ca2+?
- Both are equal
- Neither polarises
- Ca2+
- Mg2+
-
Which combination of ionic properties gives the greatest covalent character?
- Small cation, small anion
- Large cation, small anion
- Large cation, large anion
- Small cation, large anion
-
Which compound has greater covalent character: AgCl or NaCl?
- AgCl
- NaCl
- Both are equal
- Neither is covalent
-
Which magnesium halide exhibits the greatest covalent character?
- Magnesium chloride
- Magnesium fluoride
- Magnesium bromide
- Magnesium iodide
-
Which cation has the higher charge density and polarising power?
- Equal polarising power
- 3+ ion (60 pm)
- Neither ion polarises
- 2+ ion (70 pm)
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