Answers to Chapter 02 Study Questions
- Page ID
- 14619
\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\)
-
- law of multiple proportions
- law of conservation of mass
- law of definite proportion
- Rutherford’s experiment supported the ideas that atoms contain a small dense center (nucleus) and are mostly empty space.
Nuclear Symbol | Atomic Number | Mass Number | Number of Protons | Number of Electrons | Number of Neutrons | Charge |
\(\mathrm{^{40}_{18}Ar}\) | 18 | 40 | 18 | 18 | 22 | 0 |
\(\mathrm{^{39}_{19}K^+}\) | 19 | 39 | 19 | 18 | 20 | +1 |
\(\mathrm{^{36}_{16}S^{2-}}\) | 16 | 36 | 16 | 18 | 20 | -2 |
- \(\mathrm{^{20}_{10}Ne}\) and \(\mathrm{^{22}_{10}Ne}\)
-
- MG, Group 2, metal, Period 5
- MG, Group 17, nonmetal, Period 4
- TM, Period 5
- MG, Group 15, nonmetal, Period 3
- MG, Group 13, metalloid, Period 2
- ITM, Period 7
- MG, Group 14, metal, Period 5
- TM, Period 6
- Group 1 = alkali metals; Group 2 = alkaline earth metals; Group 17 = halogens; Group 18 = noble gases.
- Elements: \(\ce{O2}\), \(\ce{N2}\), \(\ce{Cl2}\), or any other diatomic element. Compounds: \(\ce{CO2}\), \(\ce{H2O}\), \(\ce{NH3}\), or any other covalent compound.
-
- positive, +1
- positive, +2
- negative, -1
- negative, -2
- positive, +1
-
- covalent, dinitrogen oxide or dinitrogen monoxide
- ionic, potassium oxide
- covalent, phosphorus trichloride
- ionic, aluminum phosphate
- covalent, hydrochloric acid
- ionic, ammonium fluoride
- ionic, lead(II) nitrite
- covalent, sulfurous acid
-
- calcium carbonate
- zinc sulfide
- copper(I) hydroxide
- magnesium perchlorate
-
- \(\ce{K3PO4}\)
- \(\ce{(NH4)2SO4}\)
- \(\ce{Co(OH)2}\)
- \(\ce{FeN}\)
-
- \(\ce{PI3}\)
- \(\ce{N2O5}\)
- \(\ce{HClO3}\)