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Chapter 10: Problem 59

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{N}_{2}\); (b) HCN; (c) \(\mathrm{NH}_{4}^{+} ;\) (d) \(\mathrm{NO}_{3}^{-} ;\) (e) NSF.

Short Answer

Expert verified
The shapes of the molecules and ions are as follows: (a) \(\mathrm{N}_{2}\) - Linear; (b) HCN - Linear; (c) \(\mathrm{NH}_{4}^{+} ;\) - Tetrahedral; (d)\(\mathrm{NO}_{3}^{-} ;\) - Trigonal Planar; (e) NSF - Bent or V-Shaped.

Step by step solution

01

Calculate Steric Number for N2

As nitrogen (N) has five valence electrons, N2 means that each nitrogen shares three electrons with each other. Thus, the steric number becomes 3 and the shape is Linear.
02

Predict Shape for HCN

Carbon (C), the central atom here, has 4 valence electrons. In HCN, it forms a double bond with Nitrogen (N) and a single bond with Hydrogen (H). Total bonded electrons = 4, so the steric number is 4 (3 from N and 1 from H). Hence, the shape is Linear.
03

Predict Shape for NH4+

Nitrogen (N) has 5 valence electrons. In Ammonium ion (NH4+), it forms 4 bonds with Hydrogens so total bonded electrons = 8 (4x2 from each H). The steric number is 4, which leads to a Tetrahedral shape.
04

Predict Shape for NO3-

In Nitrate ion (NO3-), Nitrogen (N) is the central atom with 5 valence electrons. It forms three bonds (2 with one Oxygen and 1 with two others). In total, bonded electrons = 6 (2x3 from each O). The steric number is 3, hence the shape is Trigonal Planar.
05

Predict Shape for NSF

In NSF, Sulphur (S) is the central atom with 6 valence electrons. It forms 2 single bonds with Nitrogen and Fluorine, so total bonded electrons = 4 (2x2 from each N, F). The steric number is 4, therefore the shape is Bent or V-Shaped.

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Most popular questions from this chapter

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures. (a) \(\mathrm{Al}(\mathrm{OH})_{3}\); (c) \(\mathrm{NH}_{4} \mathrm{F}\); (d) \(\mathrm{KClO}_{3}\); (b) \(\mathrm{Ca}(\mathrm{CN})_{2}\); (e) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\).

Write plausible Lewis structures for the following molecules that contain only single covalent bonds. (a) \(\mathrm{FCl} ;\) (b) \(\mathrm{I}_{2} ;\) (c) \(\mathrm{SF}_{2} ;\) (d) \(\mathrm{NF}_{3} ;\) (e) \(\mathrm{H}_{2} \mathrm{Te}\).

Comment on the similarities and differences in the molecular structure of the following four-atom species: \(\mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}, \mathrm{SO}_{3}^{2-},\) and \(\mathrm{ClO}_{3}^{-}\).

Represent the following ionic compounds by Lewis structures: (a) barium hydroxide; (b) sodium nitrite; (c) magnesium iodate; (d) aluminum sulfate.

In which of the following molecules would you expect the oxygen-to-oxygen bond to be the shortest: (a) \(\mathrm{H}_{2} \mathrm{O}_{2},\) (b) \(\mathrm{O}_{2},\) (c) \(\mathrm{O}_{3} ?\) Explain.
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