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41 Cards in this Set
- Front
- Back
Chemical Bond
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A link between atoms that results from the mutual attraction between the nuclei and valence electrons of both atoms
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Ionic Bond
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a chemical bond resulting from electrical attraction between large numbers of positive and negative ions, cations & anions
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Covalent Bond
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a chemical bond resulting from the sharing of electron pairs between two atoms
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Polar Covalent Bond
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a covalent bond where the united atoms have an unequal attraction for the shared electrons
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Nonpolar Covalent Bond
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a covalent bond in which the bonding electrons are shared equally by bonded atoms with a resulting balanced distribution of charges
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Ionic Compound
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composed of positive and negative ions combined so that the positive and negative charges are equal
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Formula Unit
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simplest collection of atoms from which a compound's formula can be established
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Crystal Lattice
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an orderly arrangement of ions
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Lattice energy
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the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
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Molecule
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the smallest unit quanity of matter which can exist by itself and retain all the properties of the original substance
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Molecular Compound
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a chemical compound whose simplest units are molecules
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The 7 diatomic molecules
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hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine
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Bond Energy
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the energy required to break a chemical bond and fomr neutral atoms
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Bond Length
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the average distance between two bonded atoms
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Octet Rule
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chemical compounds will form so that each atom, by gaining, losing or sharing electrons, has an octet of electrons in its highest occupied energy level
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Unshared Pair
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a pair of electrons that is not involved in bonding, but instead belongs exclusively to one atom
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Structural Formula
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indicates the kind, number, arrangement, and bonds, but not the unshared pairs, of the atoms in the molecule
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Isomers
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compounds with the same formula but a different arrangement of atoms
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Chemical Formula
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indicates the relative numbers of each kind of atom in a chemical compound by using atomic symbols and numerical subscripts
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Molecular Formula
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shows the types and numbers of atoms combined in a single molecule
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Single Bond
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covalent bond produced by sharing one pair of electrons between 2 atoms
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Double Bond
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a covalent bond between 2 atoms produced by the sharing of two pairs of electrons
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Covalent Networking Bond
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a continuous, 3D network of covalently bonded atoms
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Coordinate Covalent Bond
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a bond where just one atom contributes electrons
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Triple Bond
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a covalent bond with the sharing of three pairs of electrons
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Polyatomic Ion
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a charged group of covalently bonded atoms
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Resonance
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refers to bonding in molecules that cannot be correctly represented by a single lewis structure
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Delocalized Electrons
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valence electrons that are free to move about
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Metallic Bond
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a chemical bond resulting from the attraction between metal atoms and surrounding mobile electrons
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Heat of Vaporization
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the amount of heat needed to change a metal in solid state to a gas
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VSEPR Theory
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used for predicting molecular geometry
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Main assumption of the VSEPR Theory
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electrons in molecules will repel one another; therefore causing the bonds and long pairs of electrons to orient themselves as they do
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VSEPR Theory
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states that repulsion between the sets of valence-level electorn pairs surrounding an atom causes these sets to be oriented as far apart as possible
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Hybridization
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the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energy
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Hybrid Orbitals
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orbitals of equal energy produced by the combination of two or more orbitals on the same atom
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Intermolecular Forces
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the forces of attraction between molecules
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Intramolecular Forces
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the forces of attraction within a molecule
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Dipole
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equal, but opposite charges separated by a short distance
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Dipole-Dipole Forces
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forces of attraction between polar molecules
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Hydrogen Bonding
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an intermolecular attraction between a hydrogen atom and an unshared pair of electrons on a strongly electronegative atom in another molecule
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London Dispersion Forces
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intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles and induced dipoles
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