Chem 111- Test 3- St. Thomas Flashcards
absorbance
+
emission
-
orbital diagram
the thing w the lines
electron configuration
[the last nobel gas in row 18] and then the d, s, and p’s
what doesn’t need 8 around central atom
B and Be
principle quantum number
n. the shells
angular momentum or azimuthal quantum number
L, subshell (shape of orbital)
l=what on s orbital
0
l=what on p orbital
1
l=what on d orbital
2
magnetic quantum number
m(l), orientation of orbital (d- -2 to 2; s= 0, p= -1 to 1)
l=what on f orbital
3
spin quantium number
direction of the spin (+1/2 or -1/2)
transition metals in electron configuration
s and d orbitals only. also electron is removed from s orbital first
negative ion
= MORE electrons
positive ion
= LESS electrons
atomic radius
smaller left to right, larger top to bottom
ionization energy
energy required to move one elctron from an atom. higher left to right, lower top to bottom.
electron affinity
increase left to right, lower top to bottom
nonpolar covalent
electrons shared equally
polar covalent
electrons not shared equally
polar and nonpolar depend on what
electronegativity
electronegativity
increasing left to right, decreasing top to bottom
pure covalent number
less than 0.4
polar covalent number
between 0.4 and 1.8
ionic number
greater than 1.8
formal charge
valence electrons- (lone pair electrions + 1/2 bonding electrons)
bond order
sum of indiviedual bond orders/ mumber of bond groups
individual bond order
of bonds connecting atoms
breaking bonds ____ energy
requires (endothermic)
building bonds ____ energy
releases (exothermic)
size pattern
decreases up and decreases left to right
ionic bond strength
- charge
- size
charge ionic bond strength
higher charge= higher bond strength (aka lattice energy)
size bond strength
smaller ion = higher bond strength (lattice energy)
____ bonds = higher melting points
stronger
covalent bond strength
- # of bonds
- size
reaction enthalpy
Ebonds broken- Ebonds formed
bonds broken are the ____
reactants
bonds formed are the____
products
more bonds = ____ length
shorter
electronic geometry-2 bonds + lone pairs
linear, 180 angle
electronic geometry-3 bonds + lone pairs
trigonal planar, 120 degrees
electronic geometry- 4 bonds + lone pairs
tetrahedral, all 109.5 degrees
electronic geometry- 5 bonds + lone pairs
trigonal bipyramidal , angles of 90 or 120
electronic geometry- 6 bonds + lone pairs
octahedral, angles 90 or 180
trigonal planar with 1 lone pair
bent, angles left are less than 120 degrees
tetrahedral one lone pair
trigonal pyramid, angles left are less than 109
tetrahedral with 2 lone pairs
bent, but angles are less than 109
trigonal bipyramid, one lone pair
seesaw, angles of less than 90 (straight to bottom) and less than 120 (between bottom 2)
trigonal bipyramid, 2 lone pairs
t shape, angles of less than 90 degrees
trigonal bipyramid, 3 lone pairs
linear, 180 degrees
octahedral, 1 lone pair
square pyramid, ALL angles less than 90
octahedral, 2 lone pair
square planar, 90 degrees
octahedral, 3 lone pair
t shaped, less than 90 degrees
octahedral, 4 lone pair
linear, 180 degrees
localized
electrons in bonds. they take up less space because they are shared
delocalized
lone pair electrons. they take more space because they are not shared
angle distortion
lone pairs on central atoms will distort bond angles
when is a it polar
when EG and MG are NOT the same. (this means there IS a dipole moment), OR if there are different bond types, it is also polar
when is it nonpolar
when EG and MG are the same (no dipole moment)
be able to write the s, d, and p orbitals
s on left (1 on top + helium on left), d in middle (3 on top (NOT 4)), p on right, (2 on top- not including helium)
EG= linear, what is hybridization?
sp
EG= trigonal planar, what is hybridization?
sp2
EG= tetrahedral, what is hybridization?
sp3
EG= trigonal bipyramidal, what is hybridization?
sp3d
EG= octahedral, what is hybridization?
sp3d2
hybrid orbital what do you do
the hybridization = the # of regions (i.e. sp2= 3 regions), then valence electrons = the spins (start with up, then go back with the extras as down spins)
single bond (sigma and pi)
sigma bond
double bond (sigma and pi)
1 sigma, 1 pi
triple bond (sigma and pi)
1 sigma and 2 pi
when can molecules rotate?
only in a single bond
energy units
J/photon
energy symbol
change in E
wavelength
(the weird one)
frequency
v
when does it come out of s orbital first?
transition metals
what takes 1 s and 10 d (the exceptions)
Cr and Cu
shielding
electrons are repelled by other electrons in lower shells (so when its up vs down idk)
the more negative energy is…
the higher electron affinity it has
a high electron affinity has ____ energy value
negative
