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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Ch.2 - Atoms, Molecules & Ions
Chapter 2, Problem 159
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
Verified step by step guidance1
Step 1: Identify the overall charge of the compound. Since these are neutral compounds, the sum of the charges of the positive and negative ions must equal zero.
Step 2: Determine the charge of the negative ion (anion) in each compound. Use the known charges of common polyatomic ions and monatomic ions. For example, CN^- has a charge of -1, NO2^- has a charge of -1, SO4^2- has a charge of -2, PO4^3- has a charge of -3, S^2- has a charge of -2, O^2- has a charge of -2, IO^- has a charge of -1, and CH3CO2^- has a charge of -1.
Step 3: Calculate the total negative charge in each compound by multiplying the charge of the anion by the number of anions present in the formula. For example, in Zn(CN)2, there are 2 CN^- ions, so the total negative charge is 2(-1) = -2.
Step 4: Determine the charge on the positive ion (cation) by ensuring the total positive charge balances the total negative charge to make the compound neutral. For example, in Zn(CN)2, the total negative charge is -2, so the charge on Zn must be +2 to balance it.
Step 5: Repeat the process for each compound, ensuring the sum of the charges of the cations and anions equals zero for each compound.
Related Practice
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 formulas of the compounds formed from the following ions? (a) Na+ and NO3- (b) K+ and SO42- (c) Sr2+ and Cl-
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)?
Textbook Question
Prior to 1961, the atomic mass unit (amu) was defined as 1/16 the mass of the atomic weight of oxygen; that is, the atomic weight of oxygen was defined as exactly 16. What was the mass of a 12C atom prior to 1961 if the atomic weight of oxygen on today's scale is 15.9994?
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