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Chapter 8: Problem 8

Write formulas for each of the following compounds: a. potassium hydroxide b. calcium nitrate c. sodium carbonate d. carbon tetrachloride e. magnesium bromide

Short Answer

Expert verified
a. KOH, b. Ca(NO鈧�)鈧�, c. Na鈧侰O鈧�, d. CCl鈧�, e. MgBr鈧�

Step by step solution

01

Identify the Ions

For each compound, identify the cation (positive ion) and the anion (negative ion). This will help in writing the correct formula.
02

Write the Formula for Potassium Hydroxide

Potassium (K) has a +1 charge and hydroxide (OH) has a -1 charge. The formula is obtained by balancing these charges: KOH
03

Write the Formula for Calcium Nitrate

Calcium (Ca) has a +2 charge and nitrate (NO鈧�) has a -1 charge. To balance these charges, two nitrate ions are needed: Ca(NO鈧�)鈧�
04

Write the Formula for Sodium Carbonate

Sodium (Na) has a +1 charge and carbonate (CO鈧�) has a -2 charge. To balance the charges, two sodium ions are needed: Na鈧侰O鈧�
05

Write the Formula for Carbon Tetrachloride

Carbon tetrachloride is a molecular compound, consisting of one carbon atom covalently bonded to four chlorine atoms: CCl鈧�
06

Write the Formula for Magnesium Bromide

Magnesium (Mg) has a +2 charge and bromide (Br) has a -1 charge. To balance these charges, two bromide ions are needed: MgBr鈧�

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Key Concepts

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

ionic compounds
Ionic compounds are formed when elements transfer electrons to achieve a full outer shell, resulting in the formation of ions. These ions have positive (cation) and negative (anion) charges. For example, in potassium hydroxide (KOH), potassium (K) is the cation with a +1 charge, and hydroxide (OH) is the anion with a -1 charge. The resulting compound balances these charges, producing a stable ionic structure.
molecular compounds
Molecular compounds are formed when atoms share electrons through covalent bonds. This process leads to the formation of molecules rather than ions. An example is carbon tetrachloride (CCl鈧�), where one carbon atom shares electrons with four chlorine atoms, creating covalent bonds. Molecular compounds often have distinct properties such as lower melting points and the ability to form gases, unlike ionic compounds.
chemical charges
Chemical charges arise from the loss or gain of electrons by atoms. Cations are positively charged as they lose electrons, while anions are negatively charged as they gain electrons. For instance, magnesium (Mg) becomes a cation with a +2 charge upon losing two electrons, while bromide (Br) becomes an anion with a -1 charge upon gaining one electron. These charges are essential in forming stable compounds by balancing positive and negative forces.
balancing charges
Balancing charges is crucial in writing correct chemical formulas. The total positive charge must equal the total negative charge. For calcium nitrate (Ca(NO鈧�)鈧�), calcium (Ca) has a +2 charge, and nitrate (NO鈧�) has a -1 charge. To balance these charges, two nitrate ions are required to offset the +2 charge of one calcium ion, resulting in a balanced formula. This rule ensures the stability of ionic compounds.
cation
A cation is an atom or molecule with a net positive charge due to the loss of one or more electrons. Cations are typically metals like sodium (Na), which loses one electron to become Na鈦�, or magnesium (Mg), which loses two electrons to become Mg虏鈦�. Cations are attracted to anions in ionic compounds, resulting in the formation of stable ionic bonds. The type and number of electrons lost determine the charge on the cation.
anion
An anion is an atom or molecule with a net negative charge due to the gain of one or more electrons. For example, bromine (Br) gains one electron to become Br鈦�, while hydroxide (OH) is a polyatomic ion with a -1 charge. Anions pair with cations to form ionic compounds, maintaining the balance of charges. The process of gaining electrons and the resultant charge depend on the element's position in the periodic table and its tendency to attract electrons.

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Most popular questions from this chapter

List the three requirements for a correctly written chemical equation.

a. What is meant by the activity of an element? b. How does this description differ for metals and nonmetals?

Ammonia reacts with oxygen to yield nitrogen and water. \(4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)\) Given this chemical equation, as well as the number of moles of the reactant or product indicated below, determine the number of moles of all remaining reactants and products. \(\begin{array}{ll}{\text { a. } 3.0 \mathrm{mol} \mathrm{O}_{2}} & {\text { c. } 1.0 \mathrm{mol} \mathrm{N}_{2}} \\ {\text { b. } 8.0 \mathrm{mol} \mathrm{NH}_{3}} & {\text { d. } 0.40 \mathrm{mol} \mathrm{H}_{2} \mathrm{O}}\end{array}\)

Aqueous sodium hydroxide is produced commercially by the electrolysis of aqueous sodium chloride. Hydrogen and chlorine gases are also produced. Write the balanced chemical equation for the production of sodium hydroxide. Include the physical states of the reactants and products.

How many atoms of each type are represented in each of the following? \(\begin{array}{ll}{\text { a. } 3 \mathrm{N}_{2}} & {\text { f. } 5 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}} \\ {\text { b. } 2 \mathrm{H}_{2} \mathrm{O}} & {\text { g. } 4 \mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}} \\ {\text { c. } 4 \mathrm{HNO}_{3}} & {\text { h. } 2\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}}\end{array}\) \(\begin{array}{ll}{\text { d. } 2 \mathrm{Ca}(\mathrm{OH})_{2}} & {\text { i. } 6 \mathrm{Al}_{2}\left(\mathrm{SeO}_{4}\right)_{3}} \\ {\text { e. } 3 \mathrm{Ba}\left(\mathrm{ClO}_{3}\right)_{2}} & {\text { j. } 4 \mathrm{C}_{3} \mathrm{H}_{8}}\end{array}\)
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