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Chapter 2: Problem 67

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

Short Answer

Expert verified
The chemical formulas for the given compounds are: (a) \(\text{Al(OH)}_{3}\), (b) \(\text{K}_{2}\text{SO}_{4}\), (c) \(\text{Cu}_{2}\text{O}\), (d) \(\text{Zn(NO}_{3}\text{)}_{2}\), (e) \(\text{HgBr}_{2}\), (f) \(\text{Fe}_{2}(\text{CO}_{3})_{3}\), and (g) \(\text{NaBrO}\).

Step by step solution

01

Identify elements and their charges

Aluminum (Al) has a charge of +3. Hydroxide (OH) has a charge of -1.
02

Combine elements

To balance the charges, we need 3 hydroxide groups for each aluminum atom. Therefore, the chemical formula is \(\text{Al(OH)}_{3}\). #b) Potassium sulfate#
03

Identify elements and their charges

Potassium (K) has a charge of +1. Sulfate (SO₄) has a charge of -2.
04

Combine elements

To balance the charges, we need 2 potassium atoms for each sulfate group. Therefore, the chemical formula is \(\text{K}_{2}\text{SO}_{4}\). #c) Copper(I) oxide#
05

Identify elements and their charges

Copper (Cu) has a charge of +1 (denoted by I). Oxygen (O) has a charge of -2.
06

Combine elements

To balance the charges, we need 2 copper atoms for each oxygen atom. Therefore, the chemical formula is \(\text{Cu}_{2}\text{O}\). #d) Zinc nitrate#
07

Identify elements and their charges

Zinc (Zn) has a charge of +2. Nitrate (NO₃) has a charge of -1.
08

Combine elements

To balance the charges, we need 2 nitrate groups for each zinc atom. Therefore, the chemical formula is \(\text{Zn(NO}_{3}\text{)}_{2}\). #e) Mercury(II) bromide#
09

Identify elements and their charges

Mercury (Hg) has a charge of +2 (denoted by II). Bromine (Br) has a charge of -1.
10

Combine elements

To balance the charges, we need 2 bromine atoms for each mercury atom. Therefore, the chemical formula is \(\text{HgBr}_{2}\). #f) Iron(III) carbonate#
11

Identify elements and their charges

Iron (Fe) has a charge of +3 (denoted by III). Carbonate (CO₃) has a charge of -2.
12

Combine elements

To balance the charges, we need 2 iron atoms for each 3 carbonate groups. Therefore, the chemical formula is \(\text{Fe}_{2}(\text{CO}_{3})_{3}\). #(g) Sodium hypobromite#
13

Identify elements and their charges

Sodium (Na) has a charge of +1. Hypobromite (BrO) has a charge of -1.
14

Combine elements

To balance the charges, we need 1 sodium atom for each hypobromite group. Therefore, the chemical formula is \(\text{NaBrO}\).

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Most popular questions from this chapter

The compound cyclohexane is an alkane in which six carbon atoms form a ring. The partial structural formula of the compound is as follows: (a) Complete the structural formula for cyclohexane. (b) Is the molecular formula for cyclohexane the same as that for \(n\) -hexane, in which the carbon atoms are in a straight line? If possible, comment on the source of any differences. (c) Propose a structural formula for cyclohexanol, the alcohol derived from cyclohexane.

Provide the name or chemical formula, as appropriate, for each of the following acids: (a) hydroiodic acid, (b) chloric acid, (c) nitrous acid, \((\mathrm{d}) \mathrm{H}_{2} \mathrm{CO}_{3},(\mathrm{e}) \mathrm{HClO}_{4},\) (f) \(\mathrm{CH}_{3} \mathrm{COOH}\)

Because many ions and compounds have very similar names, there is great potential for confusing them. Write the correct chemical formulas to distinguish between (a) calcium sulfide and calcium hydrogen sulfide, (b) hydrobromic acid and bromic acid, (c) aluminum nitride and aluminum nitrite, (d) iron(II) oxide and iron(III) oxide, (e) ammonia and ammonium ion, (f) potassium sulfite and potassium bisulfite, (g) mercurous chloride and mercuric chloride, (h) chloric acid and perchloric acid.

Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (a) \(33^{7} X\), (b) \(\frac{127}{53} \mathrm{X}\), (c) \(\frac{152}{63} \mathrm{X}\) (d) \({ }_{83}^{209} \mathrm{X}\).

The element lead (Pb) consists of four naturally occurring isotopes with atomic masses 203.97302,205.97444,206.97587 , and 207.97663 amu. The relative abundances of these four isotopes are 1.4,24.1,22.1 , and \(52.4 \%\), respectively. From these data, calculate the atomic weight of lead.
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