- 188.8.131.52.25: In what ways are polyatomic ions like simple ions? In what ways are...
- 184.108.40.206.26: Why must roman numerals be used when naming certain ionic compounds?
- 220.127.116.11.27: What do the endings -ite and -ate indicate about a polyatomic ion?
- 18.104.22.168.28: Explain how calcium, Ca2+, and phosphate, PO4 3, can make a compoun...
- 22.214.171.124.29: Name the compounds represented by the following formulas. a. Ca(NO2...
- 126.96.36.199.30: Write the formulas for the following ionic compounds made of simple...
- 188.8.131.52.31: Name the following binary ionic compounds. If the metal forms more ...
- 184.108.40.206.32: Write formulas for the following compounds. a. mercury(II) sulfate ...
Solutions for Chapter 5.3: Names and Formulas of Ionic Compounds
Full solutions for Modern Chemistry: Student Edition 2006 | 1st Edition
A reaction involving the addition of two groups to a conjugated p system in which one group is installed at the C1 position and the other group is installed at the C2 position.
An unsaturated hydrocarbon that contains one or more carbon-carbon triple bonds.
Hydrocarbon compounds that contain a planar, cyclic arrangement of carbon atoms linked by both s and delocalized p bonds. (Section 24.2)
beta (b) rays.
A ligand in which two linked coordinating atoms are bound to a metal. (Section 23.3)
A system that enables the exchange of energy (usually in the form of heat) but not mass with its surroundings. (6.2)
A voltaic cell containing the same electrolyte and the same electrode materials in both the anode and cathode compartments. The emf of the cell is derived from a difference in the concentrations of the same electrolyte solutions in the compartments. (Section 20.6)
A mode of radioactive decay in which an inner-shell orbital electron is captured by the nucleus. (Section 21.1)
elimination (of radicals)
In radical reaction mechanisms, a step in which a bond forms between the alpha (a) and beta (b) positions. As a result, a single bond at the b position is cleaved, causing the compound to fragment into two pieces.
A crystal lattice in which the lattice points are located at the faces and corners of each unit cell. (Section 12.2)
The practice in which water laden with sand and other materials is pumped at high pressure into rock formations to release natural gas and other petroleum materials. (Section 18.4)
When orbitals of equal energy are available but there are not enough electrons to fi ll all of them completely, one electron is put in each before a second electron is added to any
Naturally occurring compoundsthat can be extracted from cells usingnonpolar organic solvents.
An allowed energy state of an electron in the quantum mechanical model of the atom; the term orbital is also used to describe the spatial distribution of the electron. An orbital is defined by the values of three quantum numbers: n, l, and ml (Section 6.5)
An insoluble substance that forms in, and separates from, a solution. (Section 4.2)
In NMR spectroscopy, a signal that is comprised of four peaks.
A high-energy species formed between two successive reaction steps, that lies in an energy minimum between the two transition states
second law of thermodynamics
A statement of our experience that there is a direction to the way events occur in nature. When a process occurs spontaneously in one direction, it is nonspontaneous in the reverse direction. It is possible to state the second law in many different forms, but they all relate back to the same idea about spontaneity. One of the most common statements found in chemical contexts is that in any spontaneous process the entropy of the universe increases. (Section 19.2)
valence bond theory
A theory that treats a bond as the sharing of electrons that are associated with individual atoms, rather than being associated with the entire molecule.
A reagent used to perform a Wittig reaction.
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