Chemistry Flashcards
1
Q
Titration end point
A
When indicator changes color
2
Q
Titration equivalence point
A
amount of titrant has neutralized analyte (moles of acid= moles of base) - vertical on curve
3
Q
electronegativity
A
atom attraction of electron to self
4
Q
heiseberg uncertainty principle
A
cant know position and momentum at the same time
5
Q
principal quantum number
A
n, main energy level
6
Q
angular momentum quantum number
(Azimuthal)
A
l, shape, 0 to n-1, 0=s, 1=p
7
Q
magnetic quantum number
A
ml, orientation of orbital, -l to l
8
Q
spin quantum number
A
ms, +1/2 or -1/2
9
Q
Total orbitals
A
Total= n^2
10
Q
Number of electrons in an orbital
A
2 max
11
Q
Number of electrons in a shell
A
2n^2
12
Q
Afbau principle
A
fill lowest to highest energy
13
Q
pauli exclusion
A
no 2 electrons can have the same 4 quantum numbers
14
Q
paramagnetism
A
one or more unpaired electrons- pulled into external magnetic field
15
Q
diamagentism
A
all electrons are paired. repelled by magnetic field
16
Q
atomic number
A
Z, number of protons
17
Q
mass number
A
A, protons and neutrons in the nucleus
18
Q
atomic mass
A
average mass of all isotopes
19
Q
Mass defect
A
difference between predicted and actual mass.. mass is converted through energy when nucleus is made…. E=Mc^2 is energy released
20
Q
Nuclear binding energy
A
energy to break nucleus or form nucleus (causes mass defect)
21
Q
Nuclear strong force
A
holds nucleus, stable, stronger than electrostatics of repelling protons
22
Q
Nucleons
A
protons and neutrons in nucleus
23
Q
Visible spectrum ranges
A
red= longer and lower frequency, violet= shorter wavelength, higher frequency
24
Q
Common ion effect
A
move system away from extra ion, will decrease solubility
25
How does pH affect solubility
increasing H+/OH alters other ions, increasing H will alter baisic anions and decrease it so shift towards basic anion
26
Sigma vs. pi bonds
head on orbital overlap, pi bonds are side by side unhybridized p
27
formal charge
number of valence electrons in free atom - number of bonds - number of nonbonded electrons
28
VSEPR
negative charges repel, forces molecule to a shape - form to move electrons far apart
29
sp3 hybrid
109.5, tetradhedral
30
sp2 hybrid
120, trigonal planar
31
Triple bonds
shortest and strongest
32
intermolecular bonds
between molecules
33
Dipole- dipole bonds
electrostatic via permanent dipole
34
hydrogen bonds
dipole-dipole, hydrogen with an EN atom (F,O,N)
35
Dispersion
weak, transient dipole due to EN difference. Temporary induced dipole
36
Constitutional isomers
differ in connectivty and structure
37
Chiral
non superimposable mirror images, 4 different groups
38
Achiral
superimposable miror images
39
stereoisomers
differ in 3D arrangements
40
Enantiomers
chiral mirror images, not superimposable, opposite configuration at all chiral centers
41
How to tell R vs. S
prioritize (Higher priority is higher atomic number), then out lower priority in the back, Clockwise is R
42
Optical activity
plane polarized light rotates
43
diastereomers
non-superimposable, non mirror images, opposite configuration at some chiral centers
44
number of stereoisomers
2^n where n=chiral centers
45
cis isomer
same group on same side of double bond
46
E/Z system
Z= high priority on same side of double bond
47
Atomic radius
increases down group (due to more electrons) and increases from right to left (less protons) shielding is due to electrons
48
Zeff
Charge felt by added electrons. Increases from left to right (more protons) and bottom to top (further away from protons at bottom)
49
Ionization energy
energy to remove electrons (increases left to right and bottom to top) - farther away feels less protons, and at right has more protons
50
electronegativity
tendency of atoms to attract a bonding pair of electrons, increases left to right and up a group
51
Electron affinity
accept electrons, increases left to right and up a group (increase in affinity means more exothermic)
52
Huckels rule
planar monocyclic rings with pi electrons 4n+2 are aromatic
53
nucleophillic functional groups
lewis base, amines, negative charges, lower EN, more EDG
54
electrophillic functional groups
positive, carbonyl C, lewis acid
55
conformational isomers
different spatial arrangment, different energy levels due to strain
56
Polar protic solvents
stabilize nucleophile. Increase rate of SN1
57
EWG
stabilize negative charge and increase acidity
58
EDG examples
OH, NR2, OR, R
59
How do mesylate and tosylate act as protecting groups
they protect alcohol from being nucleophile or acid
60
tautomer
shift carbonyl (keto) to alkene (enol)
61
How do acetals/ ketals protect
protect aldehydes or ketones from nucleophillic reaction
62
hemi vs. full acetal or ketal
hemi has an OH, full has 2 OR
63
furanose vs. pyranose
furanose has 5 membered ring, pyranose has 6 membered ring
64
triglyceride synthesis
OH on glycerol is nucleophile, attack carbonyl on carboxylic acid. Makes ester bond
65
anomeric carbon
old carbonyl carbon, attatched to 2 oxygen, OH up is alpha, OH down is beta
66
Zero reaction order
rate is independent of concentration, slope=-kf
67
first reaction order
rate is proportional to concentration, graph ln[A], slope=-kf
68
second reaction order
rate is proportional to reactant, graph 1/[A], slope kf
69
Kinetics
how fast a reaction is, rate
70
Thermodynamics
spontaneity, stability
71
zero law of thermodynamics
temperature is a state function, in contact means in equilibrium
72
first law of thermodynamics
energy of isolated systems is conserved, delta U= Q+W (if work done on gas then add, if by gas then subtract)
73
second law of thermodynamics
entropy of isolated systems wont decrease, heat flows hot to cold
74
third law of thermodynamics
entropy increases with temperature, volume
75
La Chetllier
move to less concentration, lower P, and heat removed
76
Boyles Law
PV= constant
77
Charles Law
V/T= constant
78
Avagadros Law
V/n= constant
79
Isovolumetric
delta v=0, w=0, delta U= q- vertical line
80
adiabatic
delta T=0, q=0, delta U=w , NO HEAT EXCHANGED
81
isothermal
delta U= 0, delta E=0, 0=q+ w, PV=0
82
isobaric
constant P, delta U= Q + (-PdeltaV)
83
Ideal gas law
pV=nRT
84
STP
1 mol= 22.4L, 1 atm, 273K
85
When does real has deviate from ideal
when close together, high P, low temp
86
normality
number of equivalents per L solution
87
Ksp
solubility constant, shows how inclined compound is to dissolve, only include aq and gas
88
Balance Redox
make hald reaction, balance all except HO, then add H2O to balance O and H+ ti balance H, add electrons to balance charge
89
acidic
more acidic= more polar, more oxygenated.
90
weak acid
HF, HCN, acetic acid
91
weak base
NH3, ammonia
92
pKa of amino acids
amino group is 9, carboxyl is 2 (acidic). pI is 5.5
93
purpose of acetyl coA
TCA cycle, produces fatty acid when ATP is high
94
anomers
epimers that are in their cyclic state
95
Epimers
stereoisomers that differ in stereochem configuration at only ONE stereocenter
96
Max number of stereoisomers
2^n where n= number of chiral centers
97
Fischer projection
horizontal is wedged, out of page. Vertical is dashed, into page
98
How does optical activity relate to configuration
Positive =d, negative=s
99
What affects acidity
EWG - (stabilize the negative charge to increase acidity), more polar, more oxidized
100
How does reduction occur
hydride attacks carbonyl (hydrogen has lone pair)
101
Amino acid synthesis
amine is nucleophile, and carbonyl is electrophule. Can be gabriel or strecker
102
Reaction quotient
Q, at some point in time to reach equilibrium
103
Redox titration
strong oxiding agent is titrated and the change in voltage is measured. equivalence is when all of the reducing agent is oxidized
104
Velocity
displacement over time
105
Acceleration
Change in velocity over time, has force, can change in magnitude or direction
106
Negative acceleration
slowing down when velocity is positive, speeding up when velocity is negative
107
Hydrophobic effect
hydrophobic layer moves closer together and becomes ordered, making a smaller hydrophillic layer of water- allows higher entropy for water
108
Vmax
shows enzyme concentration
109
Kcat
Vmax / [Et] , lower kM means tight fit
110
X intercept on Michaelis Menten
1/km
111
Y intercept on Michaelis Menten
1/Vmax
112
Slope on Michaelis Menten
Km/Vmax
113
Bronsted acid vs. base
acid is proton donor, base is proton acceptor
114
Lewis acid vs. base
acid is electron pair acceptor, base is electron pair donor
115
geometric isomers
isomers that differ in orientation across a double bond
116
coordinate covalent
both electrons come from same atom
117
heat of formation
larger is favored (more release)
118
Ka
Acid dissociation constant, how well something dissociates
119
amplitude
maximum magnitude of displacement from equilibrium
120
period
time for entire cycle, T=1/f
121
how do electrochemical cells work
reduction at cathode, oxidation at anode
122
direction of electron flow in electrochemical cells
electrons flow from anode to cathode
123
What can oxidizing agent oxidize?
Any reducing agent below it on standard reduction table
124
How to tell if redox is spontaneous?
add redox standard redox potentials - + potential is spontaneous
125
ceoncentration cell
same electrode on both sides, different concentrations
126
isotopes
same atom, differ in number of neutrons
127
alpha particle
two protons and two neutrons bound, positive
128
beta particles
high energy electrons or positrons
129
beta radiation
protons turns into a neutron, release electron
130
positron
electron counter part, +1
