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Chapter 11: Problem 31

Nonmetals form negative ions by (losing/gaining) enough electrons to achieve the electron configuration of the next noble gas.

Short Answer

Expert verified
Nonmetals form negative ions by \(gaining\) enough electrons to achieve the electron configuration of the next noble gas.

Step by step solution

01

Understand the formation of negative ions

Negative ions, also known as anions, are formed when an atom gains extra electrons. This results in having more electrons than protons, giving the ion an overall negative charge.
02

Identify nonmetal behavior with electrons

Nonmetals have a higher affinity for the negatively charged electrons compared to metals. They tend to gain electrons in reactions and form negative ions, or anions, to achieve stability.
03

Compare electron configuration to the nearest noble gas

The noble gases are located on the far right of the periodic table, and they have a full set of electrons in their outermost shell. This electron configuration is highly stable and unreactive. Nonmetals aim to achieve a similar electron configuration to be more stable. To do this, they will gain electrons and fill their outermost shell until they reach the electron configuration of the next closest noble gas.
04

Conclude the correct option

Based on the analysis, nonmetals form negative ions by gaining enough electrons to achieve the electron configuration of the next noble gas. So the correct option is "gaining."

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Most popular questions from this chapter

Although both the \(\mathrm{BF}_{3}\) and \(\mathrm{NF}_{3}\) molecules contain the same number of atoms, the \(\mathrm{BF}_{3}\) molecule is flat, whereas the \(\mathrm{NF}_{3}\) molecule is trigonal pyramidal. Explain.

Explain the difference between a covalent bond formed between two atoms of the same element and a covalent bond formed between atoms of two different elements.

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. a. \(\mathrm{PH}_{3}\) b. \(\mathrm{SF}_{2}\) C. HBr d. \(\mathrm{CCl}_{4}\)

In each case, which of the following pairs of bonded elements forms the more polar bond? a. \(\mathrm{S}-\mathrm{F}\) or \(\mathrm{S}-\mathrm{Cl}\) b. \(\mathrm{N}-\mathrm{O}\) or \(\mathrm{P}-\mathrm{O}\) c. \(\mathrm{C}-\mathrm{H}\) or \(\mathrm{Si}-\mathrm{H}\)

Is the formula we write for an ionic compound the molecular formula or the empirical formula? Why?
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