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polarity
(of a bond) expresses how equally electrons are shared between two atoms
ΔEN
shows the absolute value of the difference in electronegativity of two bonded atoms that provides a rough measure of the polarity to be expected in the bond, and thus, the bond type
nonpolar covalent bonds
electrons shared equally between atoms
mostly diatomic molecues and C—H
polar covalent molecules
unequal sharing of electrons
different nonmetals
ionic bonds
metal gives electrons to a nonmetal
metal and nonmetal
polar covalent bonds
form between atoms whose electronegativities differ, resulting in an unequal sharing of electrons
closer to the more electronegative element
in a polar covalent bond, where do the electrons lie?
δ+
signifies the atom that is being deprived of electrons
δ-
signifies the atom that is hogging the electrons
positive
the cross end of the arrow represents the ____ end of the dipole
negative
the arrowhead points toward the ______ end of the dipole
dipole moment
describes the strength of a dipole
bond order
the number of bonding electron pairs shared by two atoms
bond length
the distance between the nuclei of two bonded atoms
bond dissociation energy
the energy required to break a bond
bond order
the number of chemical bonds between a pair of atoms
typically a value of 1 (single bond), 2 (double bond), or 3 (triple bond)
in molecules with resonance structures
when does a fractional bond occur?
the shorter the bond and the stronger the bond
the greater the bond order (more bonds holding two atoms together)…
the longer the bond length and the weaker the bond
the lesser the bond order (less bonds holding two atoms together)…
bond length
the distance between the nuclei of two bonded atoms
atomic size and bond order
what does bond length depend on?
a larger atom
for atomic size in bond length, what has a longer bond?
a higher bond order
for bond order in bond length, what has a shorter bond?
bond energy
the energy required to break 1 mole of a chemical bond in the gas phase
bond energy
the strength of a bond is measured by the…
the higher the bond strength and the shorter the bond
the greater the number of bonds…
stronger and shorter
more bonds =
weaker and longer
fewer bonds =
decreases
bond order increases while bond length…
single
a double bond is stronger than a ____ bond
shorter
a double bond is ___ than a single bond
molecular shape
chemical/physical properties are related to…
active site
biomolecules will interact with molecules that fit into their…
lewis structures and ball-and-stick models
what are the two ways to show molecular shape?
ball-and-stick model
atoms and bonds are shown in three dimensions, showing the structure, including the bond angles
valence shell electron pair repulsion theory (VSEPR)
the 3D shape of a molecule can be predicted using this
main ideas of VSEPR
electron clouds are regions of negative charge
electron clouds will repel each other
electron clouds will, therefore, try to get as far away from each other as possible. this minimizes repulsive forces
VSEPR
states that the repulsion between these electron pairs is the most important factor in determining the geometry (or shape) of a molecule
their electron pair repulsions
molecules adopt the shape that minimizes…
far apart
valence electrons, whether present in bond pairs or lone pairs, seek to be as _______ _______ from each other as possible
steric number
the number of electrons
steric number
(present as lone pairs or as bonding electrons) around a central atom fundamentally controls the shape of the molecule
