What is the mass of one ${ }^{16} \mathrm{O}$ atom, in grams?

In the molecules $CO, C O_2$, and $C H_2 O$, which $C—O$ bond is the shortest? Which C—O bond is the strongest?

Which of the following statements about renewable resources is TRUE?
(A) They are found only in tropical climates.
(B) They can never be depleted.
(C ) They are replaceable by natural means.
(D) They regenerate quickly.

Indicate the hybridization of the central atom in

$$AlCl_4^-$$

Which molecule should have the strongest carbon-carbon bond? The strongest carbon-oxygen bond?

F2 and Cl2 are produced by electrolytic oxidation, whereas Br2 and I2 are produced by chemical oxidation of the halide ions in a concentrated aqueous solution (brine) by a more electronegative halogen. Give two reasons why Cl2 isn't prepared this way.

Why are the alkaline-earth metals less reactive than the alkali metals?

Name each of the following compounds and indicate which ones are best described as ionic:\

$$\mathrm{SrSO}_4$$

Which of the following processes will likely result in a precipitation reaction?
Mixing an $\mathrm{NaNO}_3$ solution with a $\mathrm{CuSO}_4$ solution.

Which of the following processes will likely result in a precipitation reaction?
Mixing a $\mathrm{BaCl}_2$ solution with a $\mathrm{K}_2 \mathrm{SO}_4$ solution. Write a net ionic equation for the precipitation reaction.

A sample of iron ore weighing $0.2792 \mathrm{~g}$ was dissolved in an excess of a dilute acid solution. All the iron was first converted to $\mathrm{Fe}$ (II) ions. The solution then required $23.30 \mathrm{~mL}$ of $0.0194~M\mathrm{~KMnO}_4$ for oxidation to $\mathrm{Fe}$ (III) ions. Calculate the percent by mass of iron in the ore.

A sample of iron ore weighing $0.2792 \mathrm{~g}$ was dissolved in an excess of a dilute acid solution. All the iron was first converted to Fe(II) ions. The solution then required $23.30 \mathrm{~mL}$ of $0.0194 \mathrm{M}$ $\mathrm{KMnO}_4$ for oxidation to $\mathrm{Fe}$ (III) ions. Calculate the percent by mass of iron in the ore.

A sample of iron ore weighing $0.2792 \mathrm{~g}$ was dissolved in an excess of a dilute acid solution. All the iron was first converted to $\mathrm{Fe}$ (II) ions. The solution then required $23.30 \mathrm{~mL}$ of $0.0194 M$ $\mathrm{KMnO}_4$ for oxidation to $\mathrm{Fe}$(III) ions. Calculate the percent by mass of iron in the ore.

A volume of $35.2 \mathrm{~mL}$ of a $1.66 M \mathrm{KMnO}_4$ solution is mixed with $16.7 \mathrm{~mL}$ of a $0.892 M \mathrm{KMnO}_4$ solution. Calculate the concentration of the final solution.