Chapter 2: Atoms, Molecules, and Ions Homework #2
2.14 Indicate the number of protons, neutrons, and electrons in each of these species: 15 7 N, 33 16 S, 24 12 Mg, 25 12 Mg, 48 22 Ti, 79 35 Br, 195 78 Pt 2.24 Group these elements in pairs that you would expect to show similar chemical properties: K, F, P, Na, Cl, and N. 2.34 Give the number of protons and electrons in each of the following common ions: K+, Mg2+, Fe3+, Br-, Mn2+, C4-, and Cu2+. 2.42 What are the empirical formulas of the following compounds? (a) Al2Br6, (b) Na2S2O4, (c) N2O5, and (d) K2Cr2O7. 2.46 Which of the following compounds are likely to be ionic? Which are likely to be molecular? CH4, NaBr, BaF2, CCl4, ICl, CsCl, and NF3. 2.48 Name these species: (a) KClO, (b) Ag2CO3, (c) FeCl2, (d) KMnO4, (e) CsClO3, (f) HIO, (g) FeO, (h) Fe2O3, (i) TiCl4, (j) NaH, (k) Li3N, (l) Na2O, (m) Na2O2, (n) FeCl3 • 6H2O, (o) (AsO4)3-, and (p) (HSO3)-. 2.50 Write the formulas for these compounds: (a) copper(I) cyanide, (b) strontium chlorite, (c) perchloric acid, (d) hydroiodic acid, (e) disodium ammonium phosphate, (f) lead(II) carbonate, (g) tin(II) fluoride, (h) tetraphosphorus decasulfide, (i) mercury(II) oxide, (j) mercury(I) iodide, and (k) cobalt(II) chloride hexahydrate.
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