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Chapter 2: Problem 107

Fill in the blanks in the following table: $$ \begin{array}{l|l|l|l|} \hline \text { Cation } & \text { Anion } & \text { Formula } & \text { Name } \\\ \hline \mathrm{Ni}^{2+} & \mathrm{CH}_{3} \mathrm{COO} & & \text { Sodium carbonate } \\ & & & \\ \mathrm{Ca}^{2+} & \mathrm{F}^{-} & & \\ & & \mathrm{Cu}\left(\mathrm{ClO}_{4}\right)_{2} & \\ & & & \\ & & & \\ \hline \end{array} $$

Short Answer

Expert verified
The completed table is: $$ \begin{array}{l|l|l|l|} \hline \text { Cation } & \text { Anion } & \text { Formula } & \text { Name } \\ \hline \mathrm{Ni}^{2+} & \mathrm{CH}_{3} \mathrm{COO} & \mathrm{Ni(CH_3COO)_2} & \text { Nickel(II) acetate } \\ \mathrm{Ca}^{2+} & \mathrm{F}^{-} & \mathrm{CaF_2} & \text { Calcium fluoride } \\ \mathrm{Cu}^{2+} & \mathrm{ClO}_{4}^{-} & \mathrm{Cu(ClO_4)_2} & \text { Copper(II) perchlorate } \\ \hline \end{array} $$

Step by step solution

01

Fill in the first formula

Write the ionic formula for \(\mathrm{Ni}^{2+}\) and \(\mathrm{CH}_{3} \mathrm{COO}\). Since these have charges of +2 and -1 respectively, we need two acetate anions for every one nickel cation to make the electric charge neutral. So the ionic formula is: $$ \mathrm{Ni(CH_3COO)_2} $$
02

Correct the first name

The name mentioned in the first row is incorrect. Since the compound consists of Nickel and Acetate ions, the correct name should be: $$ \text{Nickel(II) acetate} $$
03

Fill in the second cation and name

The given formula in the second row is: $$ \mathrm{CaF_2} $$ So, we can determine that the missing cation is \(\mathrm{Ca}^{2+}\), and the name of this compound is: $$ \text{Calcium fluoride} $$
04

Fill in the third name

In the third row, the given formula is $$ \mathrm{Cu(ClO_4)_2} $$ It is a compound consisting of Copper and Perchlorate ions. Since Copper has a charge of +2, the correct name is: $$ \text{Copper(II) perchlorate} $$
05

Fill in the complete table

Now, let's fill in the completed table: $$ \begin{array}{l|l|l|l|} \hline \text { Cation } & \text { Anion } & \text { Formula } & \text { Name } \\ \hline \mathrm{Ni}^{2+} & \mathrm{CH}_{3} \mathrm{COO} & \mathrm{Ni(CH_3COO)_2} & \text { Nickel(II) acetate } \\ \mathrm{Ca}^{2+} & \mathrm{F}^{-} & \mathrm{CaF_2} & \text { Calcium fluoride } \\ \mathrm{Cu}^{2+} & \mathrm{ClO}_{4}^{-} & \mathrm{Cu(ClO_4)_2} & \text { Copper(II) perchlorate } \\ \hline \end{array} $$

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Most popular questions from this chapter

Suppose a scientist repeats the Millikan oil-drop experiment but reports the charges on the drops using an unusual (and imaginary) unit called the warmomb (wa). The scientist obtains the following data for four of the drops: $$ \begin{array}{lc} \hline \text { Droplet } & \text { Calculated Charge (wa) } \\ \hline \text { A } & 3.84 \times 10^{-8} \\ \text {B } & 4.80 \times 10^{-8} \\ \text {C } & 2.88 \times 10^{-8} \\ \text {D } & 8.64 \times 10^{-8} \\ \hline \end{array} $$ (a) If all the droplets were the same size, which would fall most slowly through the apparatus? (b) From these data, what is the best choice for the charge of the electron in warmombs? (c) Based on your answer to part (b), how many electrons are there on each of the droplets? (d) What is the conversion factor between warmombs and coulombs?

Give the names and charges of the cation and anion in each of the following compounds: (a) CuS, (b) \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3}\) (d) \(\mathrm{Co}(\mathrm{OH})_{2}\) (e) \(\mathrm{PbCO}_{3}\).

Write the chemical formulas for the following compounds: (a) aluminum hydroxide, \((\mathbf{b})\) potassium sulfate, \((\mathbf{c})\) copper(I) oxide, \((\mathbf{d})\) zinc nitrate, \((\mathbf{e})\) mercury(II) bromide, (f) iron(III) carbonate, \((\mathbf{g})\) sodium hypobromite.

The oxides of nitrogen are very important components in urban air pollution. Name each of the following compounds: (a) \(\mathrm{N}_{2} \mathrm{O}\) \(,(\mathbf{b}) \mathrm{NO}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (e) $\mathrm{N}_{2} \mathrm{O}_{4}$

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