Textbook Question
Give systematic names for the following compounds: (f) (NH4)2SO4
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Ch.2 - Atoms, Molecules & Ions
Chapter 2, Problem 155
What are the formulas of the compounds formed from the following ions? (a) Na+ and NO3- (b) K+ and SO42- (c) Sr2+ and Cl-
Verified step by step guidance1
Step 1: Identify the charges on each ion. For (a) Na+ has a charge of +1 and NO3- has a charge of -1. For (b) K+ has a charge of +1 and SO42- has a charge of -2. For (c) Sr2+ has a charge of +2 and Cl- has a charge of -1.
Step 2: Determine the ratio of ions needed to balance the charges. For (a), since both ions have charges of +1 and -1, they combine in a 1:1 ratio. For (b), since K+ is +1 and SO42- is -2, two K+ ions are needed to balance one SO42- ion. For (c), since Sr2+ is +2 and Cl- is -1, two Cl- ions are needed to balance one Sr2+ ion.
Step 3: Write the chemical formula by combining the ions in the ratio determined. For (a), the formula is NaNO3. For (b), the formula is K2SO4. For (c), the formula is SrCl2.
Step 4: Ensure that the total positive charge equals the total negative charge in each compound. For (a), Na+ and NO3- each have charges that cancel each other out. For (b), 2 K+ ions (2 x +1) balance the -2 charge of SO42-. For (c), 1 Sr2+ ion (+2) balances with 2 Cl- ions (2 x -1).
Step 5: Verify that the formulas are written in the simplest whole number ratio of ions. For (a) NaNO3, (b) K2SO4, and (c) SrCl2, all formulas are already in their simplest form.
Related Practice
Textbook Question
Name the following ions: (a) Ba2+ (b) Cs+ (c) V3+ (d) HCO3- (e) NH4 (f) Ni2+ (g) NO2- (h) ClO2- i) Mn2+ (j) ClO4-
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Textbook Question
What are the formulas of the compounds formed from the following ions? (a) Ca2+ and Br- (b) Ca2+ and SO42- (c) Al3+ and SO42-
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Open Question
What are the charges on the positive ions in the following compounds? (a) Zn(CN)2 (b) Fe(NO2)3 (c) Ti(SO4)2 (d) Sn3(PO4)2 (e) Hg2S (f) MnO2 (g) KIO (h) Cu(CH3CO2)2
Textbook Question
Ammonia (NH3) and hydrazine (N2H4) are both compounds of nitrogen and hydrogen. Based on the law of multiple pro-portions, how many grams of hydrogen would you expect 2.34 g of nitrogen to combine with to yield ammonia? To yield hydrazine?
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Open Question
If 3.670 g of nitrogen combines with 0.5275 g of hydrogen to yield compound X, how many grams of nitrogen would combine with 1.575 g of hydrogen to make the same compound? Is X ammonia (NH3) or hydrazine (N2H4)?