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21 Cards in this Set

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  • Back
The enthalpy change accompanying the breakage of a given bond in a mole of gaseous molecules.
Bond Energy
The distance between the nuclei of two bonded atoms.
Bond Length
The number of electrons pairs shared by two bonded atoms.
Bond Order
An electron pair shared by two nuclei; the mutual attraction between the nuclei and the electron pair forms a covalent bond.
Bonding Pair
The idealized bonding type that is based on localized electron-pair sharing between two atoms with little difference in their tendencies to lose or gain electrons(usually nonmetals).
Covalent Bonding
A covalent bond that consists of two bonding pairs; two atoms sharing four electrons in the form of one sigma and one pie bond.
Double Bond
The relative ability of a bonded atom to attract shared electrons.
The difference in electronegativities between the atoms of a bond.
Electronegativity Difference
The hypothetical charge on an atom in a molecule or ion.
Formal Charge
The idealized bonding type based on the attraction of oppositely charged atoms with large differences in their tendencies to lose or gain electrons(usually between metals and nonmetals)
Ionic Bonding
A notation in which the element symbol represents the nucleus and inner elctrons, and surrounding dots represent the valence electrons.
Lewis electron-dot symbol
A structural formula consisting of electron-dot symbols, with lines as bonding pairs and dot pairs as lone pairs.
Lewis structure
An electron pair that is part of an atom's valence shell but not involved in covalent bonding.
Lone Pair
An idealized type of bonding based on the attraction between metal ions and their delocalized valence electrons.
Metallic Bonding
A covalent bond between identical atoms such that the bonding pair is shared equally.
Nonpolar Covalent Bond
The observation that when atoms bond, they often lose, gain, or share electrons to attain a filled outer shell of eight electrons.
Octet Rule
A covalent bond in which the electon pair is shared unequally, so the bond has partially negative and partially positive poles.
Polar Covalent Bond
One of two or more Lewis structures for a molecule that cannot be adequately describe by a single structure. These differ only in the position of electron pairs.
Resonance Structure
The weighted average of the resonance structures of a molecule.
Resonance Hybrid
A bond that consists of one electron pair.
Single Bond
A covalent bond that consists of three bonding pairs, two atoms sharing six electrons; one sigma and two pie bonds.
Triple Bond