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CHM152L-C02
Ch.9&10
Question | Answer |
---|---|
Lewis theory | A simple model of chemical bonding using diagrams that represent bonds between atoms as lines or pairs of dots. |
ionic bond | A chemical bond formed between two oppositely charged ions, generally a metallic cation and a nonmetallic anion that are attracted to one another by electrostatic forces. |
covalent bond | A chemical bond in which two atoms share electrons that interact with the nuclei of both atoms, lowering the potential energy of each through electrostatic interactions. |
metallic bonding | The type of bonding that occurs in metal crystals, in which metal atoms donate their electrons to an electron sea, delocalized over the entire crystal lattice. |
octet | A Lewis structure with eight dots, signifying a filled outer electron shells for s and p block elements. |
octet rule | The tendency for most bonded atoms to possess or share eight electrons in their outer shell to obtain stable electron configurations and lower their potential energy. |
bonding electrons | A pair of electrons shared between two atoms. |
lone pair electrons | A pair of electrons associated with only one atom. |
bond order | For a molecule, the number of electrons in bonding orbitals minus the number of electrons in nonbonding orbitals divided by two-a positive bond order implies that the molecule is stable. |
single bond | The bond that forms when one electron pair is shared between two atoms. |
double bond | The bond that forms when two electron pairs are shared between two atoms. |
triple bond | The bond that forms when three electron pairs are shared between two atoms. |
electronegativity | The ability of an atom to attract electrons to itself in a covalent bond. |
non-polar covalent bond | Two atoms sharing electrons equally. |
polar covalent bond | Two atoms sharing electrons unequally. |
dipole moment | A measure of the separation of positive and negative charge in a molecule. |
resonance | Two or more valid Lewis structures that are shown with double-headed arrows between them to indicate that the actual structure of the molecule is intermediate between them. |
resonance hybrid | The actual structure of a molecule that is intermediate between two or more resonance structures. |
formal charge | The charge that an atom in a Lewis structure would have if all the bonding electrons were shared equally between the bonded atoms. |
free radical | A molecule or ion with an odd number of electrons in its Lewis structure. |
VSEPR theory | (Valence Shell Electron Pair Repulsion) A theory that allows prediction of the shapes of molecules based on the idea that electrons-either as lone pairs or as bonding pairs-repel one another. |
electron pair geometry | The geometrical arrangement of electron groups in a molecule. |
molecular geometry | The geometrical arrangement of atoms in a molecule. |
valence bond theory | An advanced model of chemical bonding in which electrons reside in quantum-mechanical orbitals localized on individual atoms that are a hybridized blend of standard atomic orbitals - chemical bonds result from an overlap of these orbitals. |
hybridization | A mathematical procedure in which standard atomic orbitals are combined to form new, hybrid orbitals. |
hybrid orbitals | Orbitals formed from the combination of standard atomic orbitals that correspond more closely to the actual distribution of electrons in a chemically bonded atom. |
sigma bond | The resulting bond that forms between a combination of any two s, p, or hybridized orbitals that overlap end to end. |
pi bond | The bond that forms between two p orbitals that overlap side to side. |