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34 Cards in this Set
- Front
- Back
Axial
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in the trigonal bipyramidal electron-pair geometry, the two positions directly acoss from each other
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Bent
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the molecular geometry of a triatomic molecule or ion in which the bond angle is less than 180 degrees
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bond angle
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the angle formed between two bond axes.
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bond axis
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an imaginary line connecting the nuclei of two bonded atoms
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bond dissociation enthalpy
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the enthalpy change for breaking a bond in a molecule with the reactants and products in the gas phase.
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bond length
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the distance between the nuclei of two bonded atoms.
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bond order
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the number of bonding electron pairs shared by two atoms in a molecule or polyatomic ion.
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bonding pair
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a pair of electrons that is shared betweeen two atoms.
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bonding
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describes the forces that hold adacent atoms together
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chemical bond
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an attractive force between two atoms that causes the atoms to be attached together.
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coordinate covalent bond
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a covalent bond in which both electrons in the bond were contributed by one atom.
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core electrons
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all of the electrons in atom except for the valence electrons
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covalent bond
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a force of attraction between two atoms that results from the sharing of electrons in the valence shells of two atoms
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dipole moment
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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
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double bond
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a double bond exists when four eletrons are shared by two atoms; two pairs of electrons are shared.
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eleelectronegativity
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a measure of the ability of an atom in a molecule to attract electrons to itself
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electroneutrality principle
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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
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Electron-pair geometry
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the geometry taken up by the valence electron pairs around a central atom
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equatorial
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in the trigonal bipyramidal electron-pair geometry, the three politions in a plase midway between the two axial positions
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Formal Charge
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Formal Charge = group number - [Lone pair electrons + 1/2 bonding electrons]
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Free radical
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a chemcial species containing an unpaired electron; these tend to be very reactive.
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Ionic Bond
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the electrostatic attraction between two oppositely charged ions. Ion formation results from the tranfer of electrons from one atom to another
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Isoelectronic
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containing the same number and arrangement of electrons
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Isostructural
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having the same structure
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Lewis electron dot symbol
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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
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Lewis structure
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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
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Resonace Structure/ Formal Charges
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To predict formal charge for a resonace structure. take the sum of the outer atoms/ it by the amount of outer atoms
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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
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Bond order
For MO theory |
Add up full orbitals and half full orbitals fractonal bonding is allowed
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paramagnetic
MO Theory |
Unpaired Electron
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Diamagnetic
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all electrons are paired
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HEOMO
Highest energy occupied molecular orbital |
the hieghts occupied orbital on the diagram
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sigma bond
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a sigma bond is a bond in which electrons density is greatest along the axis of the bond
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pi pond
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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
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