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Chapter 3: Problem 55

Give three ions that are isoelectronic with neon. Place these ions in order of increasing size.

Short Answer

Expert verified
The three ions that are isoelectronic with neon are Na^+, F^-, and Al^3+. In order of increasing size, these ions are: Al^3+ < Na^+ < F^-.

Step by step solution

01

Determine the number of electrons in neon

Neon (Ne) is a noble gas, and its atomic number is 10. This means that it has 10 protons and 10 electrons.
02

Identify ions with the same number of electrons as neon

To find ions that are isoelectronic with neon, we should look for ions that have 10 electrons. Some examples are: 1. Sodium ion (Na^+): Sodium has 11 electrons, but when it loses 1 electron, it will have 10 electrons (Na^+). 2. Fluoride ion (F^-): Fluorine has 9 electrons, but when it gains 1 electron, it will have 10 electrons (F^-). 3. Aluminum ion (Al^3+): Aluminum has 13 electrons, but when it loses 3 electrons, it will have 10 electrons (Al^3+).
03

Order the ions based on their size

Let's compare the sizes of these ions based on their nuclear charge and electron configuration. 1. Na^+: Sodium ion has 11 protons and 10 electrons. It has lost its valence electron, making its outermost electron shell closer to the nucleus. 2. F^-: Fluoride ion has 9 protons and 10 electrons. It has gained an extra electron in its outermost shell, making it a little larger than neon. 3. Al^3+: Aluminum ion has 13 protons and 10 electrons. It has lost 3 electrons, making its outermost electron shell much closer to the nucleus. When an ion has more protons, its nucleus attracts electrons more strongly, making the ion smaller. Based on this information, we can order these ions in terms of increasing size: Al^3+ < Na^+ < F^-

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Most popular questions from this chapter

Without using Fig. \(3-4,\) predict which bond in each of the following groups will be the most polar. a. \(\mathrm{C}-\mathrm{H}, \mathrm{Si}-\mathrm{H}, \mathrm{Sn}-\mathrm{H}\) \(\mathbf{b .}\) Al- \(\mathbf{B r}, \mathbf{G a}-\mathbf{B r}, \operatorname{In}-\mathbf{B r}, \mathbf{T}-\mathbf{B r}\) c. \(C-O\) or \(S i-O\) d. \(\mathrm{O}-\mathrm{F}\) or \(\mathrm{O}-\mathrm{Cl}\)

Consider the following bond lengths: \(\begin{array}{cccccc}\mathbf{C}-\mathbf{O} & 143 \mathrm{pm} & \mathbf{C}=\mathbf{O} & 123 \mathrm{pm} & \mathbf{C} \equiv \mathbf{O} & 109 \mathrm{pm}\end{array}\) In the \(\mathrm{CO}_{3}^{2-}\) ion, all three \(\mathrm{C}-\mathrm{O}\) bonds have identical bond lengths of \(136 \mathrm{pm}\). Why?

Nitrous oxide \(\left(\mathrm{N}_{2} \mathrm{O}\right)\) has three possible Lewis structures: $$\therefore N=N=O^{\cdot} \leftrightarrow: N \equiv N-\vec{O}: \longleftrightarrow: N-N \equiv 0$$ Given the following bond lengths, $$\begin{aligned} &\mathrm{N}-\mathrm{N} \quad 167 \mathrm{pm} \quad \mathrm{N}=\mathrm{O} \quad 115 \mathrm{pm}\\\ &\mathrm{N}=\mathrm{N} \quad 120 \mathrm{pm} \quad \mathrm{N}-\mathrm{O} \quad 147 \mathrm{pm}\\\ &\mathrm{N} \equiv \mathrm{N} \quad 110 \mathrm{pm} \end{aligned}$$ rationalize the observations that the \(\mathrm{N}-\mathrm{N}\) bond length in \(\mathrm{N}_{2} \mathrm{O}\) is \(112 \mathrm{pm}\) and that the \(\mathrm{N}-\mathrm{O}\) bond length is \(119 \mathrm{pm}\). Assign formal charges to the resonance structures for \(\mathrm{N}_{2} \mathrm{O}\). Can you eliminate any of the resonance structures on the basis of formal charges? Is this consistent with observation?

Write the formula for each of the following compounds: a. sodium oxide b. sodium peroxide c. potassium cyanide d. copper(II) nitrate e. selenium tetrabromide f. iodous acid g. lead(IV) sulfide h. copper(I) chloride I. gallium arsenide J. cadmium selenide k. zinc sulfide I. nitrous acid m. diphosphorus pentoxide

Write Lewis structures that obey the octet rule for the following species. Assign the formal charge for each central atom. a. \(\mathrm{POCl}_{3}\) b. \(\mathrm{SO}_{4}^{2-}\) c. \(\mathrm{ClO}_{4}\) d. \(\mathrm{PO}_{4}^{3-}\) e. \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) f. \(\quad X \in O_{4}\) g. \(\mathrm{ClO}_{3}\) h. \(\mathrm{NO}_{4}^{3-}\)
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