Question

The formulas and common names for several substances are given below. Give the systematic names for these substances. a. sugar of lead \(\quad \operatorname{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) b. blue vitrol \(\quad\) CuSO \(_{4}\) c. quicklime \(\quad \mathrm{CaO}\) d. Epsom salts \(\quad\mathrm{MgSO}_{4}\) e. milk of magnesia \(\quad \operatorname{Mg}(\mathrm{OH})_{2}\) f. gypsum \(\quad \mathrm{CaSO}_{4}\) g. laughing gas \(\quad \mathrm{N}_{2} \mathrm{O}\)

Short answer

a. lead(II) acetate b. copper(II) sulfate c. calcium oxide d. magnesium sulfate e. magnesium hydroxide f. calcium sulfate g. dinitrogen monoxide

Step-by-step solution

a. Sugar of lead (Pb(C₂H₃O₂)₂)

: The given formula contains lead (Pb) and acetate (C₂H₃O₂). The compound has two acetate ions bound to one lead ion. Therefore, the systematic name is lead(II) acetate.

b. Blue vitrol (CuSO₄)

: The given formula contains copper (Cu) and sulfate (SO₄). Therefore, the systematic name is copper(II) sulfate.

c. Quicklime (CaO)

: The given formula contains calcium (Ca) and oxygen (O). Therefore, the systematic name is calcium oxide.

d. Epsom salts (MgSO₄)

: The given formula contains magnesium (Mg) and sulfate (SO₄). Therefore, the systematic name is magnesium sulfate.

e. Milk of magnesia (Mg(OH)₂)

: The given formula contains magnesium (Mg) and hydroxide (OH). There are two hydroxide ions bound to one magnesium ion. Therefore, the systematic name is magnesium hydroxide.

f. Gypsum (CaSO₄)

: The given formula contains calcium (Ca) and sulfate (SO₄). Therefore, the systematic name is calcium sulfate.

g. Laughing gas (N₂O)

: The given formula contains nitrogen (N) and oxygen (O). There are two nitrogen atoms for every one oxygen atom. Therefore, the systematic name is dinitrogen monoxide.

Key concepts

Systematic Naming of Compounds

In chemistry, the systematic naming of compounds is a method to bring uniformity and clarity to chemical nomenclature. This ensures that chemists around the world can accurately identify and utilize these substances. The process of naming a compound systematically involves recognizing the elements present in the compound and determining the appropriate prefixes, root names, and suffixes based on established rules. For example, lead(II) acetate is determined by acknowledging the presence of lead (Pb) and acetate ions (\(\text{C}_2\text{H}_3\text{O}_2^-\)), with the "(II)" indicating the charge or oxidation state of the lead ion.

Rules such as these enable consistent communication, especially important in scientific research and industrial chemistry. The systematic approach eliminates ambiguity and prevents errors that could arise from using common names alone.

Inorganic Chemistry

Inorganic chemistry is the branch of chemistry concerned with inorganic compounds, which encompass a wide array of substances that are not based on carbon-hydrogen bonds, distinguishing them from organic chemistry. Inorganic chemistry includes a vast range of compounds such as salts, metals, minerals, and many others.

• Examples include simple salts like calcium oxide (\(\text{CaO}\)), known as quicklime, which is widely used in construction.
• Another example is copper(II) sulfate (\(\text{CuSO}_4\)), used in agriculture and art, reflecting the diversity of applications for inorganic compounds.

The systematic naming of inorganic compounds follows specific guidelines that help chemists specify compositions clearly. This can include coordination compounds, nonmetals, and complete complexes.

Common Names of Chemical Compounds

In everyday practice, many chemical compounds are known by common names rather than their systematic names. These common names often derive from historical or traditional uses of the substances, or their appearances.

Such names, like Epsom salts (\(\text{MgSO}_4\)), which is magnesium sulfate systematically, have origins in the locations they were first discovered or prominent uses. For instance, Epsom salts were named after the English town of Epsom where the mineral was first extracted.

• Quicklime is another example, referring to calcium oxide (\(\text{CaO}\)), named for its historical use in making lime plaster.
• Laughing gas, referring to dinitrogen monoxide (\(\text{N}_2\text{O}\)), is so named for its euphoric effects when inhaled.

While these common names are useful in casual or historical contexts, they lack the precision required for scientific communication, where the systematic names provide clarity.

Chemical Formulas

Chemical formulas represent the proportions of atoms that make up a particular chemical compound. These formulas provide crucial insights into the composition and structure of the compound, which is essential for understanding its properties and potential reactions.

• For inorganic compounds, these formulas often include notations that indicate the number of atoms of each element present in the compound, such as in \(\text{Pb(C}_2\text{H}_3\text{O}_2\text{)}_2\), which is lead(II) acetate.
• Similarly, the formula \(\text{Mg(OH)}_2\) describes magnesium hydroxide, indicating each magnesium ion is bonded to two hydroxide ions.

Formulas help in balancing chemical equations and understanding the ratios of different elements, aiding in practical applications like reactions, formulation of medicines, or synthesis of materials. Understanding these formulas is foundational to mastering more advanced topics in both inorganic and organic chemistry.