Terms : Hide Images
| 11051310872 | Valence Electrons | electrons located in the outermost shell (valence shell) of the atom, that can be transferred to or shared with another atom |  | 0 |
| 11051310873 | Covalent Bond | a chemical bond resulting from the sharing of an electron pair(s) between atoms |  | 1 |
| 11051310874 | Ionic Bond | a chemical bond resulting from electrical attraction between cations and anions |  | 2 |
| 11051310875 | Non-Polar Covalent Bond | a covalent bond in which the bonding electrons are shared equally by the bonded atoms |  | 3 |
| 11051310876 | Electronegativity | a measure of the tendency of an atom to attract electrons |  | 4 |
| 11051310877 | Bond Energy | the energy required to break a chemical bond and form neutral isolated atoms |  | 5 |
| 11051310878 | Bond Length | The distance between bonded atoms |  | 6 |
| 11051310879 | Chemical Formula | a formula that indicates the relative numbers of atoms of each kind in a chemical compound by using chemical symbols and numerical subscripts |  | 7 |
| 11051310880 | Binary Compound | a compound composed of only two elements |  | 8 |
| 11051310881 | Diatomic Molecule | a molecule containing only two atoms |  | 9 |
| 11051310882 | Lewis Structure | a diagram in which chemical symbols represent nuclei and inner-shell electrons, dot pairs or dashes between two chemical symbols represent shared electron pairs, and dots adjacent to only one chemical symbol represent unshared electron pairs |  | 10 |
| 11051310883 | Lone Pair | a pair of electrons that is not involved in bonding |  | 11 |
| 11051310884 | Molecule | a neutral group of atoms that are held together by covalent bonds |  | 12 |
| 11051310885 | Single Bond | a bond produced by the sharing of one pair of electrons between two atoms. represented in lewis structures by a straight line. |  | 13 |
| 11051310886 | VSEPR Theory | Valence Shell Electron Pair Repulsion Theory: repulsion between the sets of valence level electrons surrounding an atom causes these sets to be oriented as far apart as possible |  | 14 |
| 11051310887 | Polar Covalent Bond | having an uneven distribution of electrical charge |  | 15 |
| 11051310888 | Oxidation Number | a number assigned to an element in chemical combination that represents the number of electrons lost or gained by an atom of that element in the compound. |  | 16 |
| 11051310889 | Cation | a positively charged ion |  | 17 |
| 11051310890 | Anion | a negatively charged ion |  | 18 |
| 11051310891 | Monatomic Ion | an ion made of only one element |  | 19 |
| 11051310892 | Polyatomic Ion | a charged group of covalently bonded atoms |  | 20 |
| 11051310893 | Double Bond | bond produced by the sharing of two pairs of electrons (4 electrons) between two bonded atoms. Represented in lewis structures as two straight lines. |  | 21 |
| 11051310894 | Triple Bond | bond produced by the sharing of three pairs of electrons (6 electrons) between two bonded atoms. represented in lewis structures by three straight lines. |  | 22 |
| 11051310895 | bond strength | determined by bond energy and related to bond length, the stronger the bond, the shorter its length. | | 23 |
| 11051310896 | atomic radius | a measure of the size of an atom. |  | 24 |
| 11051310897 | ionization energy | a measure of the amount of energy necessary to remove an electron from an atom. |  | 25 |
| 11053820500 | lattice energy | the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions | 26 | |
| 11053851678 | Electrolyte | An ionic compound whose aqueous solution conducts an electric current | 27 | |
| 11053904196 | delocalized electrons | the electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom | 28 | |
| 11053912532 | metallic bond | the attraction of a metallic cation for delocalized electrons | 29 |
