CHEM 1127Q: 3RD EXAM
44 Cards in this Set
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Name all of the geometric shapes that stem from trigonal bipyramidal (in order) and how many terminal atoms it has, and the bond angle
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trigonal bipyramidal (5 terminal atoms) <90,120,180>
Seesaw (4 terminal atoms) <90,120,180>
T-Shaped (3 terminal atoms) <90,180>
Linear (2 terminal atoms) <180>
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Name all of the geometric shapes that stem from an octahedral (in order) and how many terminal atoms it has, and the bond angle
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Octahedral (6 terminal atoms) <90,180)
Square Pyramidal (5 terminal atoms) <90,180>
Square Planar (4 terminal atoms) <90,180>
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Name all of the geometric shapes that stem from trigonal planar (in order) and how many terminal atoms it has, and the bond angle
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Trigonal Planar (3 terminal atoms) <120>
Bent (2 terminal atoms <120>
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Name all of the geometric shapes that stem from tetrahedral (in order) and how many terminal atoms it has, and the bond angle
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Tetrahedral (4 terminal atoms) <109>
Trigonal Pyramidal (3 terminal atoms) <109>
Bent (2 terminal atoms) <109>
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Lowest hybridization number and its geometry
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sp
(linear)
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Highest hybridization number and its geometry
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sp3d2
(octahedral)
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List all hybridization numbers from least to greatest
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sp
sp2
sp3
sp3d
sp3d2
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difference between polar and nonpolar
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Polar: (unsymmetrical)
Has dipoles
Nonpolar: (symmetrical)
Has no dipoles
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important note about lone pairs
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They are used to determine polarity and write hybridization numbers
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what is (n-1) used for?
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to give you the max of (l), which is the sublevels
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what are the quantum numbers
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1.) Principal energy level (n)
2.) Sublevel (l) {n-1}
3.) Orbitals (ml) {ml -> -1 ......+l}
4.) Electron spins (ms) {+ 1/2}
Left sides are positive spins of each sublevel
Right sides are negative spins of each sublevel
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What atoms can't have multiple bonds?
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Fluorine
Chlorine
Hydrogen
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Which atoms make multiple bonds?
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{PONCS}
Phosphorus
Oxygen
Nitrogen
Carbon
Sulfur
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Distinguish between sigma bonds and pi bonds
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Sigma = Single bond
(strong bond)
Actually overlaps p orbitals (horizontal)
Pi = Double bond
(weak bond)
Shares electrons by vertical orbitals
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What orbitals can a sigma bond have
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S orbital
P orbital
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what orbitals can a pi bond have?
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P orbitals
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Atomic Radius Trend
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(-) ! < -----------------
! (+) (-)
!
!
(+) v
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Electronegativity Trend
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(+) ^ ------------------- >
i (-) (+)
i
(-) i
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Ionization Trend
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(+) ^ ------------------- >
i (-) (+)
i
(-) i
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S Orbital Shape
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Spherical
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P Orbital Shape
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(figure 8 on x, y, z axis)
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Constant "C" value
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C = 2.998 x 10^8 m/s
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Value of "RH" constant
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RH= 2.180 x 10^18 J
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Value of "h" constant
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h= 6.626 x 10^ -34 m^2kg/s
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Excited state
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electron moves from a lower orbital to a higher one
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ground state
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when the electrons are most stable
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paramagnetic
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atoms is unstable and valences are NOT full
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diamagnetic
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atom is most stable and all valences are full
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Nonideal bond angle of bent molecule
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104 degrees
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what is heat formation of an element in their "MOST STABLE STATE" under standard conditions
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0
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how to convert from Celsius to kelvin
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add 273 to C
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Convert from Celsius to Fahrenheit
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C x (9/5) + 32 = F
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what is the specific heat of water
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4.18 j/g c
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What does evolved refer to?
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exothermic (release)
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what is the magnitude of q and delta H for EXOTHERMIC reactions
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-q
- delta H
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what is the magnitude of q and delta H for ENDOTHERMIC reactions
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+q
+ delta H
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What is Hess's Law?
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...
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what is are gas equations?
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pv = nrt
pv = grt
MM
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value of "r" constant
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r = 0.0821
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Ionization Energy
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the measure of how difficult it is to remove an electron from a gaseous atom
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how many meters are in 1 nm
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1.0 x 10^ -9 m = 1 nm
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how many joules are in 1 kj
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1,000 J = 1 kj
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what atoms has the greatest Electronegativity
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Fluorine (F)
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what element has the largest atomic radius
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Cesium (Cs)
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CHEM 1127Q: 3RD EXAM