/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 73 Write the chemical formulas for ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 2: Problem 73

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

Short Answer

Expert verified
(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) \(\text{Fe}_2(\text{CO}_3)_3\), (g) \(\text{NaOBr}\).

Step by step solution

01

Understanding Chemical Formulas

Chemical formulas are written based on the cation and anion present in a compound and their respective charges. The formula is balanced to ensure that the total positive and negative charges in the compound equal zero.
02

Writing Aluminum Hydroxide Formula

Aluminum has a charge of +3 and the hydroxide ion is OH鈦� with a charge of -1. To balance the charges, three hydroxide ions are needed for each aluminum ion, resulting in the formula \(\text{Al(OH)}_3\).
03

Writing Potassium Sulfate Formula

Potassium has a charge of +1 and the sulfate ion \(\text{SO}_4^{2-}\) has a charge of -2. To balance the charges, two potassium ions are needed for each sulfate ion, giving the formula \(\text{K}_2\text{SO}_4\).
04

Writing Copper(I) Oxide Formula

Copper(I) indicates a +1 charge for copper. Oxygen typically has a -2 charge. For charge balance, two copper ions are needed for each oxide ion, resulting in the formula \(\text{Cu}_2\text{O}\).
05

Writing Zinc Nitrate Formula

Zinc has a +2 charge and the nitrate ion \(\text{NO}_3^-\) has a -1 charge. Thus, two nitrate ions are required to balance the charge of one zinc ion, giving the formula \(\text{Zn(NO}_3\text{)}_2\).
06

Writing Mercury(II) Bromide Formula

Mercury(II) indicates a +2 charge for mercury, and bromide has a -1 charge. Two bromide ions are needed for each mercury ion, resulting in the formula \(\text{HgBr}_2\).
07

Writing Iron(III) Carbonate Formula

Iron(III) indicates a +3 charge for iron, and the carbonate ion \(\text{CO}_3^{2-}\) has a -2 charge. To balance these charges, two iron ions and three carbonate ions are used, resulting in \(\text{Fe}_2(\text{CO}_3)_3\).
08

Writing Sodium Hypobromite Formula

Sodium carries a +1 charge, and hypobromite \(\text{OBr}^-\) carries a -1 charge. A simple one-to-one ratio is needed, resulting in the formula \(\text{NaOBr}\).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Compound Nomenclature
Understanding compound nomenclature is key to mastering chemistry. Nomenclature is the system used to give compounds a unique and systematic name. Let's focus on chemical compounds, which are substances consisting of two or more elements chemically combined in fixed ratios.
The nomenclature system involves identifying the cations (positive ions) and anions (negative ions) that make up the compound. Elements like metals typically form cations, whereas nonmetals often form anions.

For example:
  • Aluminum hydroxide: "Aluminum" is the cation, while "hydroxide" is the polyatomic anion.
  • Potassium sulfate: Here, "potassium" serves as the cation and "sulfate" as the anion.
  • Copper(I) oxide: Indicates copper with a +1 charge (indicated by Roman numeral I), forming a compound with oxygen.
The name of each compound gives clues about its chemical formula, often reflecting the ratio required to balance charge. Understanding these names helps in writing precise chemical formulas.
Cation and Anion Charges
Cations and anions are really important in chemistry. They determine how elements combine to form compounds.

  • Cations: These are positive ions. Metals generally lose electrons to form cations. Their charge is positive and reflects the number of electrons lost. For example, aluminum ( ext{Al}^{3+}) loses three electrons to become positively charged.
  • Anions: These are negative ions. Nonmetals tend to gain electrons to form anions, resulting in a negative charge. For instance, the sulfate ion ( ext{SO}_4^{2-}) carries a -2 charge due to gaining electrons.
When writing chemical formulas, balance is crucial. This means the total positive charge from cations equals the total negative charge from anions. If a compound has a cation of +2 and an anion of -1, you would need two anions to balance one cation. Mastering this concept is essential for crafting the correct chemical formula.
Balancing Chemical Equations
Balancing chemical equations assures that matter is conserved in a chemical reaction. This also applies when writing chemical formulas, as each formula must reflect a balanced charge.

The goal is to adjust the compound's ratio such that all positive and negative charges cancel each other out. Consider some examples from the exercise:
  • For aluminum hydroxide, you have aluminum ( ext{Al}^{3+}) and hydroxide ( ext{OH}^-). You'll need three hydroxide units to balance one aluminum ion, forming ext{Al(OH)}_3.
  • For potassium sulfate, the sulfate ion ( ext{SO}_4^{2-}) requires two potassium ( ext{K}^+) ions to balance, leading to ext{K}_2 ext{SO}_4.
Each step in balancing involves identifying the charges of each involved ion and finding the smallest whole-number ratio that achieves neutrality in charge. Understanding this principle helps students correctly derive chemical formulas from given compound names, a crucial skill in chemistry.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

From the following list of elements \(-\mathrm{Mg}, \mathrm{Li}, \mathrm{Tl}, \mathrm{Pb}, \mathrm{Se}, \mathrm{Cl}, \mathrm{Xe}, \mathrm{Si},\) C-pick the one that best fits each description. Use each element only once: \((\mathbf{a})\) an alkali metal, \((\mathbf{b})\) an alkaline earth metal, \((\mathbf{c})\) a noble gas, \((\mathbf{d})\) a halogen, \((\mathbf{e})\) a metalloidin group \(14,(\mathbf{f})\) a nonmetal listed in group \(14,(\mathbf{g})\) a metal that forms a \(3+\) ion, \((\mathbf{h})\) a nonmetal that forms a \(2-\) ion, \((\mathbf{i})\) an element that is used as radiation shielding.

(a) What is a functional group? (b) What functional group characterizes an alcohol? (c) Write a structural formula for 1-pentanol, the alcohol derived from pentane by making a substitution on one of the carbon atoms.

Chloropropane is derived from propane by substituting \(\mathrm{Cl}\) for \(\mathrm{H}\) on one of the carbon atoms. (a) Draw the structural formulas for the two isomers of chloropropane. (b) Suggest names for these two compounds.

Mass spectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. The mass spectrum of \(\mathrm{H}_{2}\) is taken under conditions that prevent decomposition into \(\mathrm{H}\) atoms. The two naturally occurring isotopes of hydrogen are \({ }^{1} \mathrm{H}\) (atomic mass \(=1.00783 \mathrm{u}\); abundance \(\left.99.9885 \%\right)\) and \({ }^{2} \mathrm{H}(\) atomic mass \(=2.01410 \mathrm{u} ;\) abundance \(0.0115 \%)\). (a) How many peaks will the mass spectrum have? (b) Give the relative atomic masses of each of these peaks. (c) Which peak will be the largest, and which the smallest?

Millikan determined the charge on the electron by studying the static charges on oil drops falling in an electric field (Figure 2.5 ). A student carried out this experiment using several oil drops for her measurements and calculated the charges on the drops. She obtained the following data: $$ \begin{array}{lc} \hline \text { Droplet } & \text { Calculated Charge (C) } \\ \hline \text { A } & 1.60 \times 10^{-19} \\ \text {B } & 3.15 \times 10^{-19} \\ \text {C } & 4.81 \times 10^{-19} \\ \text {D } & 6.31 \times 10^{-19} \\ \hline \end{array} $$ (a) What is the significance of the fact that the droplets carried different charges? (b) What conclusion can the student draw from these data regarding the charge of the electron? (c) What value (and to how many significant figures) should she report for the electronic charge?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.