## Chemistry: Molecular Approach (4th Edition)

a. Tin can form $Sn^{2+}$ or $Sn^{4+}$. Calculate the charge of the Sn ion: Oxygen has a charge of $-2$. To balance that, Sn must have a charge of $+2$. According to table 3.2, the anion name for oxygen is 'oxide'. Therefore: $SnO$: Tin (II) oxide. b. Chromium can form $Cr^{3+}$ or $Cr^{2+}$ Determine its charge: Sulfide has a charge of $-2$. In this molecule: $3 \times -2 = -6$. To balance that, each Cr must have a charge of $+3$. According to table 3.2, the anion name for sulfur is 'sulfide'. Therefore: $Cr_2S_3$: Chromium (III) sulfide. c. Rb can only form $Rb^{+}$ (First column of periodic table). According to table 3.2, the anion name for iodine is 'iodide'. Therefore: RbI: Rubidium iodide. d. Ba can only form $Ba^{2+}$ (Second column of periodic table). According to table 3.2, the anion name for bromine is 'bromide'. Therefore: $BaBr_2$: Barium bromide.