Chapter 8
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18 terms
Terms | Definitions |
|---|---|
 Ionic Bond | electrostatic forces that exist between ions of opposite charge, usually result from the interaction of metals on the left side with nonmetals (excluding group 8A) |
| Covelant Bond | sharing of electrons between two atoms, nometallic elements with one another |
| Metallic Bond | found in metals |
| Lewis Dot Structure | simple way of showing valence electrons in an atom, bond formations. the lewis symbol for an element consists of the chemical symbol for the element plus a dot for each valence electron |
| Octet Rule | atoms tends to gain, lose, or share electrons until they are surrounded by eight valence electrons, full s and p subshells |
| Lattice Energy | the energy required to completely separate a mole of a solid ionic compound into its gaseous ions |
| Lattice Energy Formula | Eel = kQ₁Q₂ / d k = 8.99x10⁹ J-m/C² |
| Electronegativity | the ability of an atom in a molecule to attract electrons to itself |
| Electron Affinity | measure of how strongly an atom attracts additional electrons |
| Ionization Energy | how strongly a gaseous atom holds onto its electrons |
| Dipole Moment | the quantitative measure of the magnitude of a dipole |
| Dipole | a distance separates two electrical charges of equal magnitude but opposite signs |
| Steps to drawing lewis structures | 1. Sum the valence electrons from all atoms, 2. write the symbols for the atoms to show which atoms are attached to which and connect them with a single bond, 3. complete the octets around all the atoms bonded to the central atom. 4. place any leftover electrons on the central atom 5. if there are not enough to give the central atom an octet, try multiple bonds |
| Formal Charge | any atom in a molecule is the charge the atom would have if all the atoms in the molecule had the same electronegativity |
| Exception to the Octet Rule | molecules and polyatomic ions containing odd number of electrons, fewer than an octet of valence electrons, atom with more than an octet of valence electrons |
| Bond Enthalpy | enthalpy change in reactions in which bonds are broken, the bond enthalpy is always a positive quantity, |
| C-m in D | 3.34 x 10⁻³⁰ |
| A in m | 10⁻¹⁰ |
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