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Chapter 6: Problem 25

Name the following covalent compounds. a. \(\mathrm{SF}_{4}\) b. \(\mathrm{XeF}_{4}\) c. \(\mathrm{PBr}_{5}\) d. \(\mathrm{N}_{2} \mathrm{O}_{5}\) e. \(\mathrm{Si}_{3} \mathrm{N}_{4}\)

Short Answer

Expert verified
The covalent compounds are named as follows: a. Sulfur tetrafluoride, b. Xenon hexafluoride, c. Phosphorus pentabromide, d. Dinitrogen pentoxide, e. Trisilicon tetranitride.

Step by step solution

01

Naming SF4

SF4 stands for sulfur tetrafluoride. 'Tetra' is the prefix used for four of an element, in this case Fluorine.
02

Naming XeF4

XeF4 stands for xenon hexafluoride. 'Hexa' is the prefix used for six of an element, in this case Fluorine.
03

Naming PBr5

PBr5 stands for phosphorus pentabromide. 'Penta' is the prefix used for five of an element, in this case Bromine.
04

Naming N2O5

N2O5 stands for dinitrogen pentoxide. 'Di' is the prefix used for two of an element, in this case Nitrogen, and 'penta' is for five of an element, in this case Oxygen.
05

Naming Si3N4

Si3N4 stands for Trisilicon tetranitride. 'Tri' is the prefix used for three of an element, in this case Silicon, and 'tetra' is for four of an element, in this case Nitrogen.

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Most popular questions from this chapter

Two molecules have different shapes but the same composition. Can you conclude that they have the same physical and chemical properties? Explain you answer.

Why is the electronegativity of an element important?

Name the following compounds, draw their Lewis structures, and determine their shapes. a. \(\mathrm{SiCl}_{4}\) b. \(\mathrm{BCl}_{3}\) c. \(\mathrm{NBr}_{3}\)

Draw Lewis structures for the following polyatomic ions. a. \(\mathrm{OH}^{-}\) b. \(\mathrm{O}_{2}^{2-}\) c. \(\mathrm{NO}^{2-}\) d. \(\mathrm{NO}^{2+}\) e. \(\mathrm{AsO}_{4}^{3-}\)

Why does \(F\) generally form covalent bonds with great polarity?
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