Chemistry Ch 8-9 Voc

Front 1

bond energy

Back 1

energy required to break the bond

Front 2

ionic bonding

Back 2

formed when an atom that looses electrons easily reacts with an atom that has a high affinity for electrons

Front 3

coulumb's law

Back 3

energy of interaction between a pair of ions

Front 4

bond length

Back 4

distance where the energy is minimal

Front 5

covalent bonding

Back 5

electrons are shared by the nuclei

Front 6

polar covalent bond

Back 6

unequal sharing of electrons

Front 7

electronegativity

Back 7

the ability of an atom in a molecule to attract shared electrons to itself

Front 8

dipole moment

Back 8

molecule that has a center of positive charge and a center of negative charge

Front 9

isoelectronic ions

Back 9

ions containing the same number of electrons

Front 10

lattice energy

Back 10

the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid

Front 11

localized electron model

Back 11

a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms

Front 12

lewis structure

Back 12

shows valence electron arranged among the atoms in the molecule

Front 13

resonance

Back 13

invoked when more than one valid lewis structure can be written for a particular molecule

Front 14

formal charge

Back 14

difference between the number of valence electrons on the free atom and the number of valence electrons assigned to the atom in the molecule

Front 15

molecular structure

Back 15

three dimensional arrangement of atoms in the molecule

Front 16

VSEPR model

Back 16

the structure around a given atom is determined principally by minimizing electron-pair replusions

Front 17

hybridization

Back 17

the mixing of native atomic orbitals to form special orbitals for bonding

Front 18

hybrid orbitals

Back 18

when a atom adopts a different set of atomic orbitals from those it has in the free state

Front 19

sigma bond

Back 19

covalent bond where the electron pair is shared in an area centered on a line running between the atoms

Front 20

pi bond

Back 20

parallel p orbitals can share an electron pair which occupies the space above and below a line joining the atoms

Front 21

molecular orbitals

Back 21

can hold tow electrons with opposite spins and the square of the molecule wave function indicates electron probability

Front 22

sigma molecular orbitals

Back 22

MO1 and MO2, bonding, and antibonding

Front 23

bonding molecular orbital

Back 23

lower in energy than the atomic orbitals of which it is composed

Front 24

antibonding molecular orbital

Back 24

higher in energy than the atomic orbitals of which it is composed

Front 25

bond order

Back 25

difference between the number of bonding electrons and the number of antibonding electrons divided by two

Front 26

pi molecular orbitals

Back 26

designated as pi2p for the bonding MO and pi2p* for the antibonding MO

Front 27

paramagnetism

Back 27

causes the substance to attracted into the inducing magnetic field

Front 28

diamagnetism

Back 28

causes the substance to be repelled from the inducing magnetic field