Podcast
Questions and Answers
Which statement about lithium peroxide and lithium superoxide is true?
Which statement about lithium peroxide and lithium superoxide is true?
- They do not exist. (correct)
- They can be easily synthesized in a laboratory setting.
- They are commonly found in nature
- They are both highly reactive compounds.
Which of the following is true about the chemical properties of BeO?
Which of the following is true about the chemical properties of BeO?
- It reacts with water to form M(OH)2 like the other MO oxides.
- It is an ionic compound
- It dissolves in strongly acidic solutions to form [Be(OH)4]2-.
- It does not react with water. (correct)
Which alkali metal salt is least likely to be anhydrous?
Which alkali metal salt is least likely to be anhydrous?
- Sodium
- Lithium
- Rubidium (correct)
- Potassium
Which of the following statements is true about BeCl2 and BeF2 in the molten state?
Which of the following statements is true about BeCl2 and BeF2 in the molten state?
Which statement about lithium's ionization energy is true?
Which statement about lithium's ionization energy is true?
What is the reason behind the unusual chemical behavior of Be?
What is the reason behind the unusual chemical behavior of Be?
Flashcards
Lithium peroxide/superoxide existence?
Lithium peroxide/superoxide existence?
Lithium peroxide (Liâ‚‚Oâ‚‚) and lithium superoxide (LiOâ‚‚) do not exist.
BeO reaction with water?
BeO reaction with water?
Beryllium oxide (BeO) is inert and does not react with water.
Anhydrous alkali salt - least likely?
Anhydrous alkali salt - least likely?
Rubidium salts are least likely to be anhydrous due to rubidium's large ionic radius and lower charge density, resulting in weaker lattice energy and a greater tendency to form hydrates.
BeCl2/BeF2 molten state property?
BeCl2/BeF2 molten state property?
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Lithium ionization energy?
Lithium ionization energy?
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Reason for Be's unusual behavior?
Reason for Be's unusual behavior?
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Study Notes
- Lithium does not form peroxide or superoxide.
- Lithium ion has high polarizing power due to its small size.
- Lithium peroxide and lithium superoxide do not exist.
- Majority of alkali metal salts are anhydrous.
- Lithium and sodium salts are most likely to exist as hydrated salts.
- Lithium has an unusually large hydration energy.
- Lithium ion is hard to reduce but easy to oxidize.
- The small size of the Li+ ion allows a close approach to surrounding water molecules.
- Lithium has the highest first ionization energy.
- Oxidation to produce Li+(aq) is different from ionization energy.
MCQ Questions:
- Why does lithium not form peroxide or superoxide? A) Due to its high polarizing power B) Due to its large size C) Due to its low polarizing power D) Due to its large electron cloud
Answer: A
- Why are lithium and sodium salts most likely to exist as hydrated salts? A) Due to their small size B) Due to their large size C) Due to their high polarizing power D) Due to their low polarizing power
Answer: A
- Why is lithium ion hard to reduce but easy to oxidize? A) Due to its large size B) Due to its small size C) Due to its low polarizing power D) Due to its high polarizing power
Answer: D
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