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Chapter 2: Problem 101

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

Expert verified
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

01

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.
02

b. Blue vitrol (CuSO₄)

: The given formula contains copper (Cu) and sulfate (SO₄). Therefore, the systematic name is copper(II) sulfate.
03

c. Quicklime (CaO)

: The given formula contains calcium (Ca) and oxygen (O). Therefore, the systematic name is calcium oxide.
04

d. Epsom salts (MgSO₄)

: The given formula contains magnesium (Mg) and sulfate (SO₄). Therefore, the systematic name is magnesium sulfate.
05

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.
06

f. Gypsum (CaSO₄)

: The given formula contains calcium (Ca) and sulfate (SO₄). Therefore, the systematic name is calcium sulfate.
07

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.

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Most popular questions from this chapter

You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: \(30.43 \% \mathrm{X}, 69.57 \% \mathrm{Y}\) Compound \(\mathrm{II} : 63.64 \% \mathrm{X}, 36.36 \% \mathrm{Y}\) In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react “gas X” with “gas Y” to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas \(\mathrm{X}^{\prime \prime}+2\) volumes "gas $\mathrm{Y}^{\prime \prime} \longrightarrow$ 2 volumes compound I 2 volumes \(^{4}\) gas \(\mathrm{X}^{\prime \prime}+1\) volume "gas \(\mathrm{Y}^{\prime \prime} \longrightarrow\) 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.

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Dalton assumed that all atoms of the same element were identical in all their properties. Explain why this assumption is not valid.

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