3.E.1:Periodic Variations in Element Properties

Exercise 3.E.2

Based on their positions in the periodic table, predict which has the largest atomic radius: Li, Rb, N, F, I.

Answer

Rb

Exercise 3.E.3

Based on their positions in the periodic table, predict which has the largest first ionization energy: Mg, Ba, B, O, Te.

Answer

O

Exercise 3.E.4

Based on their positions in the periodic table, predict which has the smallest first ionization energy: Li, Cs, N, F, I.

Answer

Cs

Exercise 3.E.5

Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: F, Li, N, Rb

Answer

Rb < Li < N < F

Exercise 3.E.6

Based on their positions in the periodic table, rank the following atoms or compounds in order of increasing first ionization energy: Mg, O, S, Si

Answer

Mg < Si < S < O

Exercise 3.E.7

Atoms of which group in the periodic table have a valence shell electron configuration of ns²np³?

Answer

15 (5A)

Exercise 3.E.8

Atoms of which group in the periodic table have a valence shell electron configuration of ns²?

Answer

2

Exercise 3.E.9

Based on their positions in the periodic table, list the following atoms in order of increasing radius: Mg, Ca, Rb, Cs.

Answer

Mg < Ca < Rb < Cs

Exercise 3.E.10

Based on their positions in the periodic table, list the following atoms in order of increasing radius: Sr, Ca, Si, Cl.

Answer

Cl < Si < Ca < Sr

Exercise 3.E.11

Based on their positions in the periodic table, list the following ions in order of increasing radius: K⁺, Ca²⁺, Al³⁺, Si⁴⁺.

Answer

Si⁴⁺ < Al³⁺ < Ca²⁺ < K⁺

Exercise 3.E.12

List the following ions in order of increasing radius: Br^–, Li⁺, Te^2–, Mg²⁺.

Answer

Li⁺ < Mg²⁺ < Br^– < Te^2–

Exercise 3.E.13

Which atom and/or ion is (are) isoelectronic with Br⁺: Se²⁺, Se, As^–, Kr, Ga³⁺, Cl^–?

Answer

Se, As⁻

Exercise 3.E.14

Which of the following atoms and ions is (are) isoelectronic with S²⁺: Si⁴⁺, Cl³⁺, Ar, As³⁺, Si, Al³⁺?

Answer

Si, Cl³⁺

Exercise 3.E.15

Compare both the numbers of protons and electrons present in each to rank the following ions in order of increasing radius: As^3–, Br^–, K⁺, Mg²⁺.

Answer

Mg²⁺ < K⁺ < Br^– < As^3–

Exercise 3.E.16

Of the five elements Al, Cl, I, Na, Rb, which has the most exothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? Hint: note the process depicted does not correspond to electron affinity

[latex]\ce{E+}(g)+\ce{e-}⟶\ce{E}(g)[/latex]

Answer

Add texts here. Do not delete this text first.

Exercise 3.E.17

Of the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction?

[latex]\ce{E}(g)⟶\ce{E+}(g)+\ce{e-}[/latex]

Answer

O, IE₁

Exercise 3.E.18

The ionic radii of the ions S^2–, Cl^–, and K⁺ are 184, 181, 138 pm respectively. Explain why these ions have different sizes even though they contain the same number of electrons.

Answer

Add texts here. Do not delete this text first.

Exercise 3.E.19

Which main group atom would be expected to have the lowest second ionization energy?

Answer

Ra

Exercise 3.E.20

Explain why Al is a member of group 13 rather than group 3?

Answer

Add texts here. Do not delete this text first.Exercise 3.E.1