- Ch.1 - Chemical Tools: Experimentation & Measurement167
- Ch.2 - Atoms, Molecules & Ions145
- Ch.3 - Mass Relationships in Chemical Reactions162
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms91
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory66
- Ch.7 - Covalent Bonding and Electron-Dot Structures59
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy114
- Ch.10 - Gases: Their Properties & Behavior121
- Ch.11 - Liquids & Phase Changes52
- Ch.12 - Solids and Solid-State Materials72
- Ch.13 - Solutions & Their Properties70
- Ch.14 - Chemical Kinetics84
- Ch.15 - Chemical Equilibrium70
- Ch.16 - Aqueous Equilibria: Acids & Bases86
- Ch.17 - Applications of Aqueous Equilibria101
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium77
- Ch.19 - Electrochemistry137
- Ch.20 - Nuclear Chemistry82
- Ch.21 - Transition Elements and Coordination Chemistry126
- Ch.22 - The Main Group Elements92
- Ch.23 - Organic and Biological Chemistry11
Chapter 22, Problem 22.3
Which of the following elements (X) will form a covalent hydride with the formula XH3 that is a gas at room temperature? (LO 22.4)
(a) Al (b) As (c) Ba (d) Se
Video transcript
Look at the location of elements A, B, C, and D in the following periodic table:
(e) Which of these oxides has the highest melting point? Which has the lowest melting point?
Consider the six second- and third-row elements in groups 4A–6A of the periodic table:
Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.
(a) Identify the nonfluorine atom in each case, and write the molecular formula of each fluoride.
Consider the six second- and third-row elements in groups 4A–6A of the periodic table:
Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.
(b) Explain why the fluorides of nitrogen and phosphorus have different molecular structures but the fluorides of carbon and silicon have the same molecular structure.
The following pictures represent various silicate anions. Write the formula and charge of each anion.
Which element in each of the following pairs has more nonmetallic character?
(a) Se or Te
Which compound in each of the following pairs is more ionic?
(b) P4O6 or Ga2O3