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Chapter 8: Problem 7

(a) What are valence electrons? (b) How many valence electrons does a nitrogen atom possess? (c) An atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2} .\) How many valence electrons does the atom have?

Short Answer

Expert verified
(a) Valence electrons are the outermost electrons in an atom that participate in chemical bonding, usually in the highest energy level. (b) A nitrogen atom has 5 valence electrons. (c) The atom with electron configuration \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{2}\) has 4 valence electrons.

Step by step solution

01

Definition of Valence Electrons

Valence electrons are the outermost electrons in an atom that participate in chemical bonding. They are usually the electrons in the highest energy level (highest principal quantum number) of an atom.
02

Valence Electrons in a Nitrogen Atom

A nitrogen atom has an atomic number of 7. Therefore, its electron configuration follows the order 1s虏, 2s虏, 2p鲁. The electrons in the highest energy level (n = 2) are 2s虏 and 2p鲁. So, a nitrogen atom has 5 valence electrons.
03

Valence Electrons in the Given Atom

The given electron configuration is 1s虏 2s虏 2p鈦� 3s虏 3p虏. The highest energy level (principal quantum number) is n = 3. In this energy level, there are 3s虏 and 3p虏 electrons. So, the atom has 2 + 2 = 4 valence electrons.

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Most popular questions from this chapter

(a) What is meant by the term covalent bond? (b) Give three examples of covalent bonding. (c) A substance \(X Y\), formed from two different elements, boils at \(-33^{\circ} \mathrm{C}\). Is XY likely to be a covalent or an ionic substance? Explain.

Which of the following molecules or ions contain polar bonds: (a) \(\mathrm{P}_{4}\), (b) \(\mathrm{H}_{2} \mathrm{~S}\), (c) \(\mathrm{NO}_{2}^{-}\), (d) \(\mathrm{S}_{2}{ }^{2-}\) ?

Consider benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) in the gas phase. (a) Write the reaction for breaking all the bonds in \(\mathrm{C}_{6} \mathrm{H}_{6}(g)\), and use data in Appendix \(C\) to determine the enthalpy change for this reaction. (b) Write a reaction that corresponds to breaking all the carbon-carbon bonds in \(\mathrm{C}_{6} \mathrm{H}_{6}(g) .\) (c) By combining your answers to parts (a) and (b) and using the average bond enthalpy for \(C-H\) from Table \(8.4\), calculate the average bond enthalpy for the carbon-carbon bonds in \(\mathrm{C}_{6} \mathrm{H}_{6}(\mathrm{~g}) .\) (d) Comment on your answer from part (c) as compared to the values for \(C-C\) single bonds and \(C=C\) double bonds in Table \(8.4 .\)

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Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: (a) \(\mathrm{NO}^{+}\), (b) \(\mathrm{POCl}_{3}\) (P is bonded to the three \(\mathrm{Cl}\) atoms and to the \(\mathrm{O}\) ), (c) \(\mathrm{ClO}_{4}^{-}\), (d) \(\mathrm{HClO}_{3}(\mathrm{H}\) is bonded to \(\mathrm{O})\).
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