Give the formula of the oxide that reacts with water to form [latex]H_{3}PO_{3}[/latex], HClO, and [latex]H_{2}SO_{3}[/latex]. STRATEGY Refer to Table 21.3. Find an oxide in which the central atom has the same oxidation number as the acid.

[latex]H_{3}PO_{3}[/latex] oxidation number: +3; oxide with oxidation number +3: [latex]P_{4}O_{6}[/latex] HClO oxidation number: +1; oxide with oxidation number +1: [latex]Cl_{2}O[/latex] [latex]H_{2}SO_{3}[/latex] oxidation number: +4; oxide with oxidation number +4: [latex]SO_{2}[/latex]

Question 21.6: Give the formula of the oxide that reacts with water to form...

Chemistry: Principles and Reactions

Give the formula of the oxide that reacts with water to form $H_{3}PO_{3}$ , HClO, and $H_{2}SO_{3}$ .

STRATEGY

Refer to Table 21.3. Find an oxide in which the central atom has the same oxidation number as the acid.

Table 21.3 Nonmetal Oxides*
Group 15	Group 16	Group 17
$N_2O_5(s), N_2O_4(g), NO_2(g)$		$OF_2(g), O_2F_2(g)$
$N_2O_3(d), NO(g), N_2O(g)$
$P_4O_{10}(s), P_4O_6(s)$	$SO_3(l), SO_2(g)$	$Cl_{2}O_{7}(l), Cl_{2}O_{6}(l)$
		$ClO_{2}(g), Cl_{2}O(g)$
		$BrO_2(d), Br_2O(d)$
		$I_2O_5(s), I_4O_9(s), I_2O_4(s)$

*The states listed are those observed at 25°C and 1 atm. Compounds that decompose below 25°C are listed as (d).
Oxides shown in boldface are discussed in the text

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