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Chapter 8: Problem 30

Name the ions with +3 charges that have these electron configurations: (a) \([\mathrm{Ar}] 3 d^{3},(\mathrm{~b})[\mathrm{Ar}],\) (c) \([\mathrm{Kr}] 4 d^{6}\) (d) \([\mathrm{Xe}] 4 f^{14} 5 d^{6}\)

Short Answer

Expert verified
The ions with a +3 charge for their respective electron configurations are: (a) V+3, (b) None, (c) Ag+3, and (d) Au+3.

Step by step solution

01

Identifying Atom for Configuration (a)

Electron configuration \([\mathrm{Ar}] 3 d^{3}\) refers to the atom whose electron configuration is like that of Argon (Ar) plus an extra 3 electrons in the 3d orbital. That atom is Vanadium (V) because neutral Vanadium has 5 electrons in its 3d orbital. Thus, losing 2 electrons will have this configuration. Therefore, the ion with a +2 charge and this electron configuration is V+3.
02

Identifying Atom for Configuration (b)

The electron configuration \([\mathrm{Ar}]\) refers to the atom Argon (Ar) itself. It cannot lose any electrons since it is already at full electron capacity for its energy level, meaning it is not an ion with a +3 charge. So there are no ions with a +3 charge for this electron configuration.
03

Identifying Atom for Configuration (c)

Electron configuration \([\mathrm{Kr}] 4 d^{6}\) refers to the atom which equates to the configuration of Krypton (Kr) plus an extra 6 electrons in the 4d orbital. That atom is Silver (Ag) because neutral Silver has 10 electrons in its 4d orbital. Thus, losing 4 electrons will have this configuration. Therefore, the ion with a +3 charge for this electron configuration is Ag+3.
04

Identifying Atom for Configuration (d)

Electron configuration \([\mathrm{Xe}] 4 f^{14} 5 d^{6}\) refers to the atom equating to the configuration of Xenon (Xe) plus 14 extra electrons in the 4f orbital and an extra 6 electrons in the 5d orbital. That atom is Gold (Au) because neutral Gold has 10 electrons in its 5d orbital. Thus, losing 4 electrons will have this configuration. The ion with a +3 charge for this electron configuration is Au+3.

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Most popular questions from this chapter

A neutral atom of a certain element has 17 electrons. Without consulting a periodic table, (a) write the ground-state electron configuration of the element, (b) classify the element, (c) determine whether the atoms of this element are diamagnetic or paramagnetic.

Write the formulas and names of the oxides of the second-period elements (Li to \(\mathrm{N}\) ). Identify the oxides as acidic, basic, or amphoteric.

Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions.

When magnesium metal is burned in air, it forms two products \(A\) and \(B\). A reacts with water to form a basic solution. B reacts with water to form a similar solution as that of A plus a gas with a pungent odor. Identify \(A\) and \(B\) and write equations for the reactions.

Without referring to a periodic table, write the electron configurations of elements with these atomic numbers: (a) \(9,\) (b) \(20,\) (c) \(26,\) (d) 33. Classify the elements.
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