Chemistry Chapter 6 Vocab.
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pigsthefreak on October 30, 2007
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29 terms
Terms | Definitions |
|---|---|
 Chemical Bond | a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
| Ionic Bonding | Chemical bonding that results from the electrical attraction between cations and anions |
| Covalent Bonding | the sharing of electron pairs between two atoms |
| Non-Polar Covalent Bond | a covalent in which the bonding electrons are shared equally be the bonded atoms, resulting in a balanced distribution of electrical charge |
| Polar | uneven distribution of charge |
| Molecule | a neutral group of atoms that are held together by covalent bonds |
| Molecular Compound | a chemical compound whose simplest units are molecules |
| Chemical Formula | the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts |
| Molecular Formula | shows the types and numbers of atoms combined in a single molecule of a molecular compound |
| Bond Energy | the energy required to break a chemical bond and form neutral isolated atoms |
| Electron-dot Notation | an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol |
| Lewis Structures | formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron paris in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons |
| Structural Formulas | indicates the kind, number, arrangement, and bonds but not the unshared pairs of hte atoms in a molecule |
| Single Bond | a covalent bond in which one pair of electrons is shared between two atoms |
| Multiple Bonds | double and triple bonds |
| Resonance | refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
| Ionic Compound | composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal |
| Formula Unit | the simplest collection of atoms from which an ionic compund's formula can be established |
| Lattice Energy | the energy released when one mole of an ionic crystalline compound is formed from gaseous ions |
| Polyatomic Ion | a charged group of covalently bonded atoms |
| Metallic Bonding | the chemical bonding that results form the attraction between metal atoms and the surrounding sea of electrons |
| Malleablility | the ability of a substance to be hammered or beaten into thin sheets |
| Ductility | the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire |
| VSEPR Theory | states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible |
| Hybridization | the mixing to two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of ezual energies |
| Hybrid Orbitals | orbitals of equal energy produced by the combination of two or more orbitals on the same atom |
| Dipole | created by equal but opposite charges that are separated by a short distance |
| Hydrogen Bonding | the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule |
| London Dispersion Forces | the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles |
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