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Chapter 8: Problem 9

Write the electron configuration for phosphorus. Identify the valence electrons in this configuration and the nonvalence electrons. From the standpoint of chemical reactivity, what is the important difference between them?

Short Answer

Expert verified
The electron configuration of phosphorus (atomic number 15) is \(1s^2 2s^2 2p^6 3s^2 3p^3\). It has 5 valence electrons (in the third energy level: \(3s^2 3p^3\)) and 10 nonvalence (core) electrons (\(1s^2 2s^2 2p^6\)). The important difference in chemical reactivity is that valence electrons participate in chemical reactions and bond formation, determining an element's chemical properties, while nonvalence electrons do not directly participate.

Step by step solution

01

Write the electron configuration

The electron configuration of an element is the distribution of its electrons among the atomic orbitals, following the Aufbau principle, Pauli Exclusion principle, and Hund's rule. For phosphorus, which has an atomic number of 15, the electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p鲁
02

Identify valence electrons

Valence electrons are the electrons in the outermost energy level (shell) of an atom. For phosphorus, the outermost shell is the third energy level (n=3). Therefore, the valence electrons are: 3s虏 3p鲁 Phosphorus has a total of 5 valence electrons.
03

Identify nonvalence electrons

Nonvalence electrons, also known as core electrons, are the electrons located in the inner energy levels (shells) of an atom. For phosphorus, the core electrons are: 1s虏 2s虏 2p鈦� Phosphorus has a total of 10 nonvalence electrons.
04

Explain the importance of valence and nonvalence electrons in chemical reactivity

The important difference between valence and nonvalence electrons in terms of chemical reactivity is that valence electrons are involved in chemical reactions and bond formation with other atoms, whereas nonvalence electrons do not participate in chemical reactions directly. Valence electrons determine the chemical properties of an element, as they are responsible for the attractive forces between atoms when forming bonds. In the case of phosphorus, its 5 valence electrons make it capable of forming 5 covalent bonds with other atoms, depending on the element it reacts with, and these bonds ultimately determine the reactivity and properties of the resulting compounds.

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Most popular questions from this chapter

Explain the following trends in lattice energy: (a) \(\mathrm{CaF}_{2}>\mathrm{BaF}_{2} ;\) (b) \(\mathrm{NaCl}>\mathrm{RbBr}>\mathrm{CsBr} ;\) (c) \(\mathrm{BaO}>\mathrm{KF}\).

(a) Construct a Lewis structure for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\), in which each atom achieves an octet of electrons. (b) Do you expect the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{H}_{2} \mathrm{O}_{2}\) to be longer or shorter than the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{O}_{2}\) ?

Based on data in Table \(8.2\), estimate (within \(30 \mathrm{~kJ} / \mathrm{mol}\) ) the lattice energy for (a) LiBr, (b) \(\mathrm{CsBr}\), (c) \(\mathrm{CaCl}_{2}\).

(a) Write a Lewis structure for the phosphorus trifluoride molecule, \(\mathrm{PF}_{3}\). Is the octet rule satisfied for all the atoms in your structure? (b) Determine the oxidation numbers of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms. (c) Determine the formal charges of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms. (d) Is the oxidation number for the \(\mathrm{P}\) atom the same as its formal charge? Explain why or why not.

For the following collection of nonmetallic elements, \(\mathrm{O}\), \(\mathrm{P}, \mathrm{Te}, \mathrm{I}, \mathrm{B},(\mathrm{a})\) which two would form the most polar single bond? (b) Which two would form the longest single bond? (c) Which two would be likely to form a compound of formula \(\mathrm{XY}_{2}\) ? (d) Which combinations of elements would likely yield a compound of empirical formula \(\mathrm{X}_{2} \mathrm{Y}_{3} ?\) In each case explain your answer.
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