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Chapter 8: Problem 12

Define valence electrons. For representative elements, the number of yalence electrons of an element is equal to its group number. Show that this is true for the following elements: \(\mathrm{Al}, \mathrm{Sr}, \mathrm{K}, \mathrm{Br}, \mathrm{P}, \mathrm{S}, \mathrm{C}\).

Short Answer

Expert verified
The number of valence electrons for the representative elements $\mathrm{Al}$, $\mathrm{Sr}$, $\mathrm{K}$, $\mathrm{Br}$, $\mathrm{P}$, $\mathrm{S}$, $\mathrm{C}$ equals their group numbers: 3, 2, 1, 7, 5, 6, and 4 respectively.

Step by step solution

01

Defining Valence Electrons

Valence electrons are the electrons present in the outermost shell of an atom that can participate in chemical reactions.
02

Finding the Group Number for Aluminum (Al)

Aluminum belongs to the group 13 in the periodic table. Therefore, it has 3 valence electrons, which equals its group number.
03

Finding the Group Number for Strontium (Sr)

Strontium belongs to the group 2 in the periodic table. Therefore, it has 2 valence electrons, which equals its group number.
04

Finding the Group Number for Potassium (K)

Potassium belongs to the group 1 in the periodic table. Therefore, it has 1 valence electron, which equals its group number.
05

Finding the Group Number for Bromine (Br)

Bromine belongs to the group 17 in the periodic table. Therefore, it has 7 valence electrons, which equals its group number.
06

Finding the Group Number for Phosphorus (P)

Phosphorus belongs to the group 15 in the periodic table. Therefore, it has 5 valence electrons, which equals its group number.
07

Finding the Group Number for Sulfur (S)

Sulfur belongs to the group 16 in the periodic table. Therefore, it has 6 valence electrons, which equals its group number.
08

Finding the Group Number for Carbon (C)

Carbon belongs to the group 14 in the periodic table. Therefore, it has 4 valence electrons, which equals its group number.

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Most popular questions from this chapter

Write ground-state electron configurations for these ions: (a) \(\mathrm{Li}^{+},\) (b) \(\mathrm{H}^{-}\), (c) \(\mathrm{N}^{3-},\) (d) \(\mathrm{F}^{-},\) (e) \(\mathrm{S}^{2-}\) (f) \(\mathrm{Al}^{3+},(\mathrm{g}) \mathrm{Se}^{2-}\) (h) \(\mathrm{Br}^{-}\) (i) \(\mathrm{Rb}^{+},(\mathrm{j}) \mathrm{Sr}^{2+},(\mathrm{k}) \mathrm{Sn}^{2+}\)

The first four ionization energies of an element are approximately \(738 \mathrm{~kJ} / \mathrm{mol}, \quad 1450 \mathrm{~kJ} / \mathrm{mol}, 7.7 \times\) \(10^{3} \mathrm{~kJ} / \mathrm{mol}\), and \(1.1 \times 10^{4} \mathrm{~kJ} / \mathrm{mol}\). To which periodic group does this element belong? Why?

Explain why the first electron affinity of sulfur is \(200 \mathrm{~kJ} / \mathrm{mol}\) but the second electron affinity is \(-649 \mathrm{~kJ} / \mathrm{mol}\),

Arrange the following atoms in order of decreasing atomic radius: \(\mathrm{Na}, \mathrm{Al}, \mathrm{P}, \mathrm{Cl}, \mathrm{Mg}\).

In the periodic table, the element hydrogen is sometimes grouped with the alkali metals (as in this book) and sometimes with the halogens. Explain why hydrogen can resemble the Group \(1 \mathrm{~A}\) and the Group 7A elements.
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