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Chapter 8: Problem 10

(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons. (b) How many electrons must a sulfur atom gain to achieve an octet in its valence shell? (c) If an atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{3},\) how many electrons must it gain to achieve an octet?

Short Answer

Expert verified
(a) False, the hydrogen atom is stable with only 2 electrons in its 1s orbital. (b) A sulfur atom must gain 2 electrons to achieve an octet in its valence shell. (c) The atom with the given electron configuration, \(1s^{2}2s^{2}2p^{3}\), must gain 3 electrons to achieve an octet in its valence shell.

Step by step solution

01

Determine the stability of a hydrogen atom

The statement claims that the hydrogen atom is most stable when it has a full octet of electrons. However, the hydrogen atom needs only two electrons in its 1s orbital to achieve a stable electron configuration, as it has only one electron shell (the first shell) which can hold a maximum of just 2 electrons. Therefore, the statement is false. #b#
02

Determining the number of electrons a sulfur atom needs to gain for an octet

To find out how many electrons a sulfur atom must gain to achieve an octet in its valence shell, we must first understand its electron configuration. Sulfur is in Group 16 of the periodic table, which means it has six valence electrons (the electron configuration of sulfur is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}\)). To achieve an octet, sulfur needs to have a total of eight valence electrons. By subtracting its current number of valence electrons (6) from the desired octet (8), we find out that sulfur must gain 2 electrons.
03

Answer for part (b)

So, a sulfur atom must gain 2 electrons to achieve an octet in its valence shell. #c#
04

Determining the number of electrons an atom needs to gain for an octet given an electron configuration

The given electron configuration for the atom is \(1s^{2}2s^{2}2p^{3}\). The valence shell is the last shell with electrons and in this case, it is the second shell (2s and 2p orbitals). The second shell can hold a maximum of 8 electrons.
05

Calculate missing electrons to achieve an octet

By summing the electrons present in the second shell (2 + 3 = 5) and comparing it against the desired octet (8), we can calculate the number of electrons needed to achieve an octet: 8 - 5 = 3.
06

Answer for part (c)

Therefore, the atom with the given electron configuration must gain 3 electrons to achieve an octet in its valence shell.

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Most popular questions from this chapter

The substance chlorine monoxide, ClO(g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of \(1.24 \mathrm{D},\) and the \(\mathrm{Cl}-\) O bond length is 1.60 \(\mathrm{A}\) . (a) Determine the magnitude of the charges on the Cl and O atoms in units of the electronic charge, \(e\) (b) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the Clo molecule? (c) Using formal charges as a guide, propose the dominant Lewis structure for the molecule. (d) The anion \(\mathrm{ClO}^{-}\) exists. What is the formal charge on the Cl for the best Lewis structure for \(\mathrm{ClO}^{-}\) ?

(a) Construct a Lewis structure for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\) in which each atom achieves an octet of electrons. (b) How many bonding electrons are between the two oxygen atoms? (c) 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 \(\mathrm{O}_{2} ?\) Explain.

Based on Lewis structures, predict the ordering, from shortest to longest, of \(N-O\) bond lengths in \(N O^{+}, N O_{2}^{-},\) and \(N O_{3}^{-} .\)

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