Question 1

Compared to the Group 1 elements, the Group 2 elements&#10;A) are stronger reducing agents.&#10;B) have higher hardness.&#10;C) are more reactive.

Accepted Answer

Group 2 elements are generally harder than Group 1 elements because they have a higher charge density due to their smaller atomic radii and the presence of two valence electrons, which leads to stronger metallic bonds.

Question 2

The extraction from molten chlorides is important process for isolation of:&#10;A) Be&#10;B) Ra&#10;C) Mg

Accepted Answer

Magnesium (Mg) is commonly extracted from molten chlorides through a process called electrolysis.

Question 3

What is peculiar about BeH₂? A) It can be formed directly from the elements. B) It is the most reactive Group 2 hydride C) It is only non-saline hydride of the Group 2.

Accepted Answer

BeH2 is the only non-saline (covalent) hydride among the Group 2 elements. The others form ionic (saline) hydrides.

Question 4

Select the correct statement:&#10;A) Be forms covalent halides.&#10;B) All Group 2 halides are soluble in water.&#10;C) All Group 2 halides are strong Lewis acids.

Accepted Answer

Be forms covalent halides due to its small size and high ionization energy, which makes it difficult for Be to lose electrons to form ionic bonds. Instead, it shares electrons to form covalent bonds.

Question 5

What can be said about general properties of the Group 2 compounds with oxygen?&#10;A) All oxides are basic.&#10;B) These elements do not form peroxides.&#10;C) A convenient way of obtaining oxides of Mg, Ca and Ba is thermal decomposition of their carbonates.

Accepted Answer

The answer of What can be said about general properties...

Question 6

What is(are) the product(s) of reaction between the Group 2 nitride and water?&#10;A) Metal oxide and ammonia&#10;B) Metal hydroxide and ammonia&#10;C) Metal hydroxide and nitride

Accepted Answer

When a Group 2 nitride reacts with water, it forms the corresponding metal hydroxide and ammonia.

Question 7

The decomposition temperature of the Group 2 carbonates:&#10;A) increases down the group.&#10;B) decreases down the group&#10;C) shows no group trends.

Accepted Answer

The decomposition temperature of Group 2 carbonates increases down the group. This is because the cations become larger and their charge density decreases, making it harder to polarize the carbonate ion and thus requiring more energy (higher temperature) to decompose the carbonate.

Question 8

In comparison to the Group 1 compounds, compounds of the Group 2 are&#10;A) less soluble in water.&#10;B) more soluble in water.&#10;C) equally soluble.

Accepted Answer

Group 2 compounds are generally less soluble in water compared to Group 1 compounds due to their higher lattice energies, which require more energy to overcome for dissolution.

Question 9

Which cations of the Group 2 form the least stable complexes? (i) Be²⁺ and Mg²⁺ (ii) Ca²⁺ (iii) Sr²⁺ and Ba²⁺ A) (i) B) (ii) C) (iii)

Accepted Answer

Sr²⁺ and Ba²⁺ form the least stable complexes among Group 2 cations due to their larger ionic sizes and lower charge density, which result in weaker interactions with ligands.

Question 10

Select the correct statement.&#10;A) The Group 2 organometallic compounds are not very reactive.&#10;B) The ionic character of metal-carbon bond increases down the group.&#10;C) Beryllium organometallics are the least stable in the group.

Accepted Answer

The ionic character of the metal-carbon bond increases down the group because the metals become more electropositive, leading to a greater difference in electronegativity between the metal and carbon.

Deck 12: The Group 2 Elements