- 11.2.1: What force holds NaCl units together?
- 11.2.2: Describe dipole-dipole forces.
- 11.2.3: What force gives water unique properties?
- 11.2.4: Why does ice have a lower density than liquid water does?
- 11.2.5: Explain why oxygen, nitrogen, and fluorine are elements in molecule...
- 11.2.6: How is the strength of London dispersion forces related to the numb...
- 11.2.7: How do intermolecular forces affect whether a substance is a solid ...
- 11.2.8: a. Which is nonpolar: CF4 or CH2F2? b. Which substance likely has a...
- 11.2.9: Are the London dispersion forces between water molecules weaker or ...
- 11.2.10: NH3 has a much higher boiling point than PH3 does. Explain.
- 11.2.11: Why does argon boil at a higher temperature than neon does?
- 11.2.12: Which will have the higher melting point, KF or KNO3? Explain your ...
Solutions for Chapter 11.2: Intermolecular Forces
Full solutions for Modern Chemistry: Student Edition 2006 | 1st Edition
In IR spectroscopy as well as UV-VIS spectroscopy, a plot that measures the percent transmittance or absorption as a function of frequency.
alkaline earth metals
Members of group 2A in the periodic table. (Section 7.7)
alpha (a) anomer
The cyclic hemiacetal of an aldose in which the hydroxyl group at the anomeric position is trans to the CH2OH
Particles that are identical to helium-4 nuclei, consisting of two protons and two neutrons, symbol 4 2He or 4 2a. (Section 21.1)
A reaction in which two species are involved in the rate-determining step.
A law stating that at constant temperature, the product of the volume and pressure of a given amount of gas is a constant. (Section 10.3)
conjugate acid–base pair
An acid and a base, such as H2O and OH-, that differ only in the presence or absence of a proton. (Section 16.2)
A drawing style that is often used when dealing with compounds bearing multiple chirality centers, especially for carbohydrates. (See also Sect. 5.7.)
A five-membered cyclic hemiacetal form of a carbohydrate.
The energy that an object possesses by virtue of its motion. (Section 5.1)
A solid whose dimensions range from 1 to 100 nm and whose properties differ from those of a bulk material with the same composition. (Section 12.1)
A compound containing an electron-rich atom that is capable of donating a pair of electrons.
An isotope that is radioactive; that is, it is undergoing nuclear changes with emission of radiation. (Section 21.1)
A conformational change in which one chair conformation is converted into the other.
A compound that contains no p bonds.
sp Hybrid orbitaL
A hybrid atomic orbital formed by the combination of one s atomic orbital and one 2p atomic orbital.
specific heat 1Cs2
The heat capacity of 1 g of a substance; the heat required to raise the temperature of 1 g of a substance by 1 °C. (Section 5.5)
An intermediate with tetrahedral geometry. This type of intermediate is formed when a nucleophile attacks the carbonyl group of a carboxylic acid derivative.
The difference in energy between staggered and eclipsed conformations (for example, in ethane).
van der Waals forces
A group of intermolecular attractive forces including dipole-dipole, dipole-induced dipole, and induced dipole-induced dipole (dispersion) forces