- Lesson 19.1: Explain the difference between an anion and a cation.
- Lesson 19.2: Explain what is meant by noble gas envy
- Lesson 19.3: How many electrons, protons, and neutrons does Li1 have?
- Lesson 19.4: Give two similarities and two differences between Cl and Cl2.
- Lesson 19.5: Give two similarities and two differences between Be and Be21.
- Lesson 19.6: Which noble gas is closest to magnesium, Mg, on the periodic table?...
- Lesson 19.7: Which noble gas is closest to sulfur, S, on the periodic table? Wha...
- Lesson 19.8: List four ions that have the same number of electrons as neon, Ne.
- Lesson 19.9: List four ions that have the same number of electrons as argon, Ar.
- Lesson 19.10: What charge would an arsenic, As, ion have?
- Lesson 19.11: What is the symbol of an ion with 22 protons, 24 neutrons, and 18 e...
- Lesson 19.12: When chlorine gains an electron to become a chloride ion with a 21 ...
- Lesson 19.13: Explain why the elements on the right side of the periodic table ga...
- Lesson 19.14: What periodic patterns do you notice for the charges on the ions?
- Lesson 19.15: Which of these ions have the correct charge? Choose all that apply....
- Lesson 19.16: Which of these ions have the same number of electrons as S22? Choos...
Solutions for Chapter Lesson 19: Ions
Full solutions for Living by Chemistry | 2nd Edition
Hydrocarbons containing one or more carbon–carbon triple bonds. (Section 24.2)
A conformation about a single bond in which two groups on adjacent carbons lie at a dihedral angle of 180°.
In UV-Vis spectroscopy, an equation describing the relationship between molar absorptivity (e), absorbance (A), concentration (C), and path length (l): e = A (C Ž l)
The volume of a fixed amount of gas maintained at constant temperature is inversely proportional to the gas pressure. (5.3)
The amount of fissionable material necessary to maintain a nuclear chain reaction. (Section 21.7)
The mass of a substance divided by its volume. (1.6)
dissolving metal reduction
A reaction in which an alkyne is converted into a trans alkene.
Incorporation of a hetero atom into a solid to change its electrical properties. For example, incorporation of P into Si. (Section 12.7)
A crystal lattice in which the lattice points are located at the faces and corners of each unit cell. (Section 12.2)
The steric interaction that results when two groups in a Newman projection are separated by a dihedral angle of 60°.
A compound with hydroxyl (!OH) groups on adjacent carbons.
Water that contains appreciable concentrations of Ca2 + and Mg 2 + ; these ions react with soaps to form an insoluble material. (Section 18.4)
Bonding that results from intermolecular attractions between molecules containing hydrogen bonded to an electronegative element. The most important examples involve OH, NH, and HF. (Section 11.2)
The ratio of the number of moles of one component of a mixture to the total moles of all components; abbreviated X, with a subscript to identify the component. (Section 10.6)
Valence electrons not involved in forming covalent bonds. Also called unshared pairs or lone pairs.
When used in the context of fats and oils, a mixture of triglycerides that is liquid at room temperature
Principle of microscopic reversibility
This principle states that the sequence of transition states and reactive intermediates in the mechanism of any reversible reaction must be the same, but in reverse order, for the reverse reaction as for the forward reaction
The difference in energy between a resonance hybrid and the most stable of its hypothetical contributing structures in which electrons are localized on particular atoms and in particular bonds.
sigma (s) bond
A bond that is characterized by circular symmetry with respect to the bond axis.
Atomic orbitals that are achieved by mathematically averaging one s orbital with only one p orbital to form two hybridized atomic orbitals.