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Chemical Bonding
Terms Important for Understanding Chemical Bonding
42
Chemistry
11th Grade
06/16/2009

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Term
Alloy
Definition
A mixture composed of two or more elements, at least one of which is a metal.
Term
Chemical Formula
Definition
An expression that indicates the number and type of atoms present in the smallest representative unit of a substance.
Term
Coordination Number
Definition
The number of ions of opposite charge that surround each ion in a crystal.
Term
Electron Dot Structure (or Lewis Dot Diagram)
Definition
A notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the nucleus and the inner shell electrons.
Term
Formula Unit
Definition
The lowest whole number ratio of ions in an ionic compound; in calcium fluoride, the ratio of calcium cations to fluoride anions is 1:2 and the formula unit is CaF2
Term
Halide Ion
Definition
A negative ion formed when a halogen atom gains an electron
Term
Ionic Bonds
Definition
The electrostatic attraction that binds oppositely charge ions together. Typically ionic bonds from between a metal and a nonmetal or a metal and an anionic polyatomic ion.
Term
Ionic Compounds
Definition
A compound composed of positive and negative charges.
Term
Metallic Bonds
Definition
The force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions.
Term
Octet Rule
Definition
Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons.
Term
Valence Electron
Definition
An electron in the highest occupied energy level of an atom.
Term
Bond Dissociation Energy
Definition
The energy required to break the bond between two covalently bonded atoms.
Term
Bonding Orbital
Definition
A molecular orbital that can be occupied by two electrons of a covalent bond.
Term
Covalent Bond
Definition
A bond formed by the sharing of electrons between atoms. These bonds are typically between nonmetal atoms.
Term
Coordinate Covalent Bond
Definition
A covalent bond in which one atom contributes both bonding electrons.
Term
Diatomic Molecule
Definition
A molecule consisting of two and only two atoms.
Term
Dipole
Definition
A molecule that has two poles, or regions with opposite charges.
Term
Dipole-Dipole Forces (or Dipole Interactions)
Definition
Intermolecular forces that result from the attraction of oppositely charged regions of polar molecules.
Term
London Dispersion Forces
Definition
Weakest intermolecular forces that occur between two nonpolar molecules.
Term
Double Covalent Bond
Definition
A bond in which two atoms share two pairs of electrons.
Term
Hydrogen Bonds
Definition
Attractive forces between covalently bonded molecules. This type of intermolecular force occurs when hydrogen is covalently bonded to a highly electronegative atom (like Fluorine or Oxygen). The hydrogen is then attracted to an unshared electron pair on an atom of a different molecule.
Term
Molecular Compound
Definition
A compound that is composed of covalently bonded molecules.
Term
Molecular Formula
Definition
A chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound.
Term
Molecular Orbital
Definition
An orbital that applies to the entire molecule.
Term
Molecule
Definition
A neutral group of atoms that is joined together by covalent bonds.
Term
Network Solids
Definition
A solid in which all of the atoms are covalently bonded to each other.
Term
Nonpolar Covalent Bond
Definition
A covalent bond in which the electrons are shared equally by the two atoms.
Term
Nonpolar Molecule
Definition
A molecule that does not contain two oppositely charged regions.
Term
Pi Bond
Definition
A covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms.
Term
Polar Covalent Bond
Definition
A covalent bond between atoms in which the electrons are shared unequally.
Term
Polar Molecule
Definition
A molecule in which one side of the molecule is slightly positive and the opposite side is slightly negative.
Term
Polyatomic Ion
Definition
A tightly bound, covalently-bonded group of atoms that behaves as a unit and has a positive or negative charge.
Term
Lewis Structure
Definition
A convention for drawing molecules in which the atomic symbol stands for the nucleus and inner-shell electrons of an atom, dots represent unshared electrons, and dashes represent shared electron pairs.
Term
Single Covalent Bond
Definition
A bond formed when two atoms share one pair of electrons.
Term
Triple Covalent Bond
Definition
A covalent bond in which two atoms share three pairs of electrons.
Term
Unshared Pair
Definition
A pair of valence electrons that is not shared between atoms of a molecule.
Term
van der Waals Forces
Definition
Collectively, the two weakest intermolecular forces of attraction: London Dispersion Forces and Dipole-Dipole Forces.
Term
VSEPR Theory
Definition
The Valence Shell Electron Pair Repulsion Theory, which states that because electrons repel each other, molecules will adjust their shapes so that valence electron pairs are as far apart as possible.
Term
Sigma Bond
Definition
A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei.
Term
Hybridization
Definition
A mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.
Term
Resonance Structure
Definition
One of the two or more equally valid Lewis structures of a molecule or a polyatomic ion.
Term
Structural Formula
Definition
An abbreviated form of a Lewis structure in which the shared pairs of electrons are shown as dashes, but no unshared pairs of electrons are shown.
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