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34 Cards in this Set

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Axial
in the trigonal bipyramidal electron-pair geometry, the two positions directly acoss from each other
Bent
the molecular geometry of a triatomic molecule or ion in which the bond angle is less than 180 degrees
bond angle
the angle formed between two bond axes.
bond axis
an imaginary line connecting the nuclei of two bonded atoms
bond dissociation enthalpy
the enthalpy change for breaking a bond in a molecule with the reactants and products in the gas phase.
bond length
the distance between the nuclei of two bonded atoms.
bond order
the number of bonding electron pairs shared by two atoms in a molecule or polyatomic ion.
bonding pair
a pair of electrons that is shared betweeen two atoms.
bonding
describes the forces that hold adacent atoms together
chemical bond
an attractive force between two atoms that causes the atoms to be attached together.
coordinate covalent bond
a covalent bond in which both electrons in the bond were contributed by one atom.
core electrons
all of the electrons in atom except for the valence electrons
covalent bond
a force of attraction between two atoms that results from the sharing of electrons in the valence shells of two atoms
dipole moment
the product of the magnitude of the partial charges on a molecule and the distnace by which they are separated. The dipole moment is a vector quantity having both a magnitude and a direction
double bond
a double bond exists when four eletrons are shared by two atoms; two pairs of electrons are shared.
eleelectronegativity
a measure of the ability of an atom in a molecule to attract electrons to itself
electroneutrality principle
electrons in a molecule or polyatomic ion will be distributed in such a way that the charges on all atoms are as close to zero as possible
Electron-pair geometry
the geometry taken up by the valence electron pairs around a central atom
equatorial
in the trigonal bipyramidal electron-pair geometry, the three politions in a plase midway between the two axial positions
Formal Charge
Formal Charge = group number - [Lone pair electrons + 1/2 bonding electrons]
Free radical
a chemcial species containing an unpaired electron; these tend to be very reactive.
Ionic Bond
the electrostatic attraction between two oppositely charged ions. Ion formation results from the tranfer of electrons from one atom to another
Isoelectronic
containing the same number and arrangement of electrons
Isostructural
having the same structure
Lewis electron dot symbol
in a lewis dot symbol for an atom, the chemical symbol is used to represent the nucleus and core electrons of an atom; the valence electrons are represnted by dots place around the symbol
Lewis structure
a representation of a covalenty bonded species in which the chemical symbol is used to represent the nucleus and core electrons of each atoms; a lone pair belonging solely to one atom is represented by two dots. and a pair of electrons that is shared between two atoms is represented by a line connecting two atoms
Resonace Structure/ Formal Charges
To predict formal charge for a resonace structure. take the sum of the outer atoms/ it by the amount of outer atoms
Bond order
For Valence Bond Theory
Bond order = Number of shared pairs in all X-Y Bonds/ Number X-Y links in the molecule or ion
Bond order
For MO theory
Add up full orbitals and half full orbitals fractonal bonding is allowed
paramagnetic
MO Theory
Unpaired Electron
Diamagnetic
all electrons are paired
HEOMO
Highest energy occupied molecular orbital
the hieghts occupied orbital on the diagram
sigma bond
a sigma bond is a bond in which electrons density is greatest along the axis of the bond
pi pond
a covalent bond that resluts from the sidways overlap of unhbridized p orbital on two different atoms. a pi bond concentrates electron density above and below the bond axis