- 22.214.171.124.1: Describe the attractive forces and repulsive forces that exist betw...
- 126.96.36.199.2: Compare a bond between two atoms to a spring between two students.
- 188.8.131.52.3: In what two ways can two atoms share electrons when forming a coval...
- 184.108.40.206.4: What happens in terms of energy and stability when a covalent bond ...
- 220.127.116.11.5: How are the partial charges shown in a polar covalent molecule?
- 18.104.22.168.6: What information can be obtained by knowing the electronegativity d...
- 22.214.171.124.7: Why do molecular compounds have low melting points and low boiling ...
- 126.96.36.199.8: Why does the distance between two nuclei in a covalent bond vary?
- 188.8.131.52.9: How does a molecular orbital differ from an atomic orbital?
- 184.108.40.206.10: How does the strength of a covalent bond relate to bond length?
- 220.127.116.11.11: Compare the degree of polarity in HF, HCl, HBr, and HI.
- 18.104.22.168.12: Given that it has the highest electronegativity, can a fluorine ato...
- 22.214.171.124.13: What does a small electronegativity difference reveal about the str...
- 126.96.36.199.14: Based on electronegativity values, which bond has the highest degre...
Solutions for Chapter 6.1: Covalent Bonds
Full solutions for Modern Chemistry: Student Edition 2006 | 1st Edition
absolute temperature scale.
A temperature scale that uses the absolute zero of temperature as the lowest temperature. (5.3)
A reaction in which a reagent adds to the two carbon atoms of a carbon–carbon multiple bond. (Section 24.3)
Organic bases that have the functional group —NR2, where R may be H, an alkyl group, or an aromatic group. (24.4)
A substance (molecule or ion) that acts as a proton acceptor. (Section 16.2)
An object that is not superimposable on its mirror image.
A compound inwhich two carbon-carbon p bonds are separated from each other by exactly one s bond.
Polymers that return to their original shape after being stretched.
In the VSEPR model, a region about a central atom in which an electron pair is concentrated. (Section 9.2)
A reaction in which the Gibbs free energy of the products is higher than that of the reactants. The position of equilibrium for an endergonic reaction favors starting materials
The mixing of different types of atomic orbitals to produce a set of equivalent hybrid orbitals. (Section 9.5)
A compound that possesses chirality centers and an internal plane of symmetry.
metathesis (exchange) reaction
A reaction in which two substances react through an exchange of their component ions: AX + BY ¡ AY + BX. Precipitation and acid–base neutralization reactions are examples of metathesis reactions. (Section 4.2)
A solid, inorganic substance occurring in nature, such as calcium carbonate, which occurs as calcite. (Section 23.1)
A ligand in which two or more donor atoms can coordinate to the same metal ion. (Section 23.3)
Primary (1°) amine
An amine in which nitrogen is bonded to one carbon and two hydrogens
A unimolecular nucleophilic substitution reaction.
Specifi c rotation
The observed rotation of the plane of polarized light when a sample is placed in a tube 1.0 dm in length and at a concentration of 1 g/mL for a solution. For a pure liquid, concentration is expressed in g/mL (density).
An ether (R!O!R) where both R groups are identical.
Valence Shell Electron Pair Repulsion theory, which can be used to predict the geometry around an atom.
Williamson ether synthesis
A method for preparing an ether from an alkoxide ion and an alkyl halide (via an SN2 process).