Studied by 17 peopleionic bonding
transfer of electrons from a metal to a nonmetal, forming cations and anions
covalent bonding
sharing of one or more pairs of electrons between two nonmetals
metallic bonding is between a
metal and metal
How are electrons shared in metallic bonding?
valence electrons are donated into a vast electron pool
Why do metals conduct energy?
delocalization
Why are noble gases stable?
they have a filled valence electron
isoelectronic
having the same number and arrangements of electrons as the closest noble gas
Lewis electron-dot structures
method of representing an element and its valence electrons
Lewis electron-dot structures are not useful for:
transition and inner transition metals
cations
postively charged ions
anions
negatively charged ions
Ionic bonds are formed the
attraction between opposite charges
Atoms lose or gain the amount electrons needed for them to form a
full octet
crisscross rule
the numerical value of the superscript charge becomes the subscript on the other ion
nonpolar covalent bond
bond between two atoms in which the attraction is the same
polar covalent bond
bond between two atoms with different levels of attraction
electronegativity (EN)
measure of the attractive force an atom exerts on a bonding pair of electrons
electronegativities increase from ________ and decrease going __________
left to right; top to bottom
what element is the most electronegative?
flourine
formal charge
charge associated with the most reasonable Lewis structure
formal charge equation
formal charge = (# of valence electrons) - (# of nonbonding electrons - 1/2 # of bonding electrons)
Formal charges of a favorable Lewis structure
small numbers, no like charges adjacent to each other, low formal charges on electronegative elements, totals to the harge on the ion or 0 for a compound
valence-shell electron-pair repulsion theory (VSPER)
valence electrons pairs surrounding a central pair will try to move away from each other to minimize repulsion
electron-group geometry
all electron groups are considered
molecular geometry
only bonding electrons are considered
linear geometry
two bonding pairs
trigonal planar geometry
three bonding pairs
bent geometry
two bonding pairs, one to two lone pairs
tetrahedral geometry
four bonding pairs
trigonal pyramidal geometry
three bonding pairs, one lone pair
trigonal bipyramidal geometry
five bonding pairs
irregular tetrahedral (see-saw) geometry
four bonding pairs, one lone pair
t-shaped geometry
three bonding pairs, two lone pairs
linear geometry (5 pairs)
two bonding pairs, three lone pairs
octahedral geometry
six bonding pairs
square pyramidal geometry
five bonding pairs, one lone pair
square planar geometry
four bonding pairs, two lone pairs
valence bond theory
the mixing of covalent atomic orbitals to form a new kind of orbital
hybrid orbitals
mixed atomic orbitals in covalent bonding
sp hybridization
overlap of an s and p orbital with linear orientation
sp^2 hybridization
overlap of an s orbital and two p orbitals with a trigonal planar orientation
sp^3 hybridization
overlap of an s orbital and three p orbitals with tetrahedral orientation
sigma (σ) bonds
overlap orbitals occuring on a line between atoms involved in covalent bond
pi (π) bonds
overlap of orbitals occuring above and below the line through the two nuclei of the bonding atoms
resonance
more than one Lewis structure can be written for a Lewis structure
how does the actual structure of a molecule compare to its resonance structure?
the actual structure is an average of the resonance structure; all the bonds in the molecule are the same
a bond with a higher order is:
stronger and shorter
paramagnetism
attraction to a magnetic field
diamagnetism
slight repulsion from a magnetic field
Note 
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