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Chapter 8: Problem 14

What is the Lewis symbol for each of the following atoms or ions: (a) \(K,(b) A s,(c) S n^{2+},\left(\right.\) d) \(N^{3-} ?\)

Short Answer

Expert verified
The Lewis symbols for the given atoms or ions are: (a) K: \[\mathrm{K \cdot}\], (b) As: \[\mathrm{As:}\], (c) Sn²⁺: \[\mathrm{Sn^{2+}::}\], and (d) N³⁻: \[\mathrm{N^{3-}:::}\].

Step by step solution

01

(a) Lewis symbol for K (Potassium)

Potassium is an alkali metal with an atomic number of 19. Its electron configuration is 1s²2s²2p⁶3s²3p⁶4s¹, meaning it has one valence electron. The Lewis symbol for potassium would be the chemical symbol 'K' surrounded by one dot. So the Lewis symbol for potassium is \[\mathrm{K \cdot}\]
02

(b) Lewis symbol for As (Arsenic)

Arsenic has an atomic number of 33, with an electron configuration of 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³. Arsenic has 5 valence electrons, present in the 4p orbitals. The Lewis symbol for arsenic will have the chemical symbol 'As' surrounded by 5 dots. So the Lewis symbol for arsenic is \[\mathrm{As:}\]
03

(c) Lewis symbol for Sn²⁺ (Tin ion with a +2 charge)

Tin is a metal with an atomic number of 50. Its electron configuration is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p². In its 2+ ionic form, tin loses two electrons from the 5p orbital. Consequently, its electron configuration becomes 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰. With 4 valence electrons left, the Lewis symbol for Sn²⁺ has four dots around the symbol 'Sn'. So the Lewis symbol for Sn²⁺ is \[\mathrm{Sn^{2+}::}\]
04

(d) Lewis symbol for N³⁻ (Nitrogen ion with a -3 charge)

Nitrogen is a non-metal with an atomic number of 7. Its electron configuration is 1s²2s²2p³, which gives it 5 valence electrons. In its 3- ionic form, nitrogen gains 3 additional electrons in the 2p orbital to complete the octet. The electron configuration for N³⁻ is 1s²2s²2p⁶ with 8 valence electrons. The Lewis symbol for N³⁻ has 8 dots surrounding 'N'. So the Lewis symbol for N³⁻ is \[\mathrm{N^{3-}:::}\]

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Most popular questions from this chapter

A common form of elemental phosphorus is the tetrahedral \(\mathrm{P}_{4}\) molecule, where all four phosphorus atoms are equivalent: At room temperature phosphorus is a solid. (a) Do you think there are any unshared pairs of electrons in the \(\mathrm{P}_{4}\) molecule? (b) How many \(\mathrm{P}-\mathrm{P}\) bonds are there in the molecule? (c) Can you draw a Lewis structure for a linear \(\mathrm{P}_{4}\) molecule that satisfies the octet rule? (d) Using formal charges, what can you say about the stability of the linear molecule versus that of the tetrahedral molecule?

(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 \(\mathrm{O}_{2} ?\)

Which of these elements are unlikely to form covalent bonds: \(\mathrm{S}, \mathrm{H}, \mathrm{K}, \mathrm{Ar},\) Si? Explain your choices.

The chlorine oxides, in which a chlorine atom is bonded to one or more oxygen atoms, are important molecules in the chemistry of the atmosphere. Will any of the chlorine oxides obey the octet rule? Why or why not?

Draw the Lewis structures for each of the following ions or molecules. Identify those that do not obey the octet rule, and explain why they do not: (a) \(\mathrm{SO}_{3}^{2-}\), (b) \(\mathrm{AlH}_{3}\) (c) \(\mathrm{N}_{3}^{-}\) (d) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (e) \(\mathrm{SbF}_{5}\)
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