Chem1 - Gen Chem Flashcards
1
Q
cation has a _ charge
A
positive
2
Q
anion has a _ charge
A
negative
3
Q
what is a salt?
A
a cation+ anion
4
Q
periodic table group 1
A
alkali metals
5
Q
periodic table group 2
A
alkaline earth metals
6
Q
periodic table group 16
A
oxygen group
7
Q
periodic table group 17
A
halogens
8
Q
periodic table group 18
A
noble gases
9
Q
metals tend to __ electrons
A
lose
10
Q
qualities of metals?
A
luster, ductility, malleabilty, conductivity
11
Q
nonmetals tend to __ electron
A
gain
12
Q
which groups are the transition metals?
A
3-12(the middle shit)
13
Q
what do alkali metals (group 1) easily form?
A
+1 cations
14
Q
what do alkaline earth metals form?
A
+2 cations
15
Q
noble gases are inert, T/F?
A
True
16
Q
atomic radius ____ DOWN and LEFT on the periodic table
A
INCREASES
17
Q
ionization energy, electron affinity, and electrongative ____ UP and RIGHT on the periodic table
A
INCREASE
18
Q
what is ionization energy?
A
energy needed to detach electrons from the atom(1st, 2nd, 3rd form +1 +2 and +3 cation respectively)
19
Q
what is electronegativity?
A
tendency to attractelectrons
20
Q
what is electron affinity?
A
willingness to accept new electrons
21
Q
what is principal quantum number?
A
shell level of electron
22
Q
what is azimuthal quantum number?
A
subshell and subshell SHAPE0=s, 1=p, 2=d, 3=f
23
Q
what is the heisenburg uncertainty principle?
A
cannot know exact momentum or position of electron
24
Q
s-orbital
A
groups 1-2, spherical
25
p orbital?
dumbbell shaped, groups 13-18
26
d orbital in which groups?
3-12(middle shit)
27
f subshell in which groups?
the bottom 2 row things
28
electron configuration
list shells and subshells from lowest to highest energy levelEx: Na= 1s22s22p63s1
Na+=1s22s23p6
29
what is hund's rule?
electrons will not share orbitals until all other orbitals are filled
30
what is the photoelectric effect?
electrons ejected by shining light on a metal. increasing FREQUENCY of photons is what increases intensity
31
differences in electronegativity give a bond __
partial ionic character
32
if YUGE difference in electronegativity
forms ionic bond
33
what is a dipole moment?
when a center of positive charge is displaced from center of negative chargeLondon dispersion/van der waals: weakest dipoles
34
mega(M)
106
35
kilo
103
36
deci
10-1
37
centi
10-2
38
milli
10-3
39
micro
10-6
40
nano
10-9
41
pico
10-12
42
thermodynamic product?
more stable, higher energy required, slower, favored by high temp
43
kinetic product
less stable, less energy required, faster, favored by low temp
44
what is the arrhenius equation?
relates collision frequency with spatial orientation & fraction of collisions with sufficient relative energy to give a rate constant
45
what is the limiting reactant?
the thing that is completely used up when the reaction runs to completion
46
what are the units for reaction rate?
Ms-1 or molL-1s-1
47
how do you determine the rate law given experimental data?
find 2 trials where only 1 reactant changes concentration, see what happens to the measured rate. if the rate doubles or halves, its first order, if it quadruples, its second order. etc etc.
48
what is half life?
time it takes for 1/2 of substance to decay. results in exponential decay and a semi-log plot.
49
what is alpha decay?
loss of alpha particle/helium nucleuschanges mass number, and loses 2 protons.
50
what is beta decay?
Beta minus: atomic # increasesejects electron
Beta plus: atomic # decrease
emits positron(positron emission)
mass # remains same for both
51
what is electron capture?
captures electron, creates neutron by combining it with a proton
52
what is gamma decay?
emission of a massless gamma particle
53
lower Rf factor means it is ___ polar because the plate itself is ___
more, polar
54
what does it mean to be paramagnetic?
basically, if it has unpaired electrons it is paramagnetic. odd # of electrons means its always paramagnetic
55
at room temperature all ionic compounds exist as ___
solids
56
Zeff increases __ the periodic table
down
57
higher Ksp means it is (more/less) soluble
more
58
what is a colloidal mixture?
microscopic suspension of particles. stuff does not dissolve completely. (ex: milk)
59
NMR only provides information about ____ H atoms in a molecule
NONEQUIVALENT
60
what is the unit for a first order reaction?
reciprocal seconds (s-1)
61
an increase in oxidation number means the compound was
oxidized
62
a decrease in oxidation number means the compound was
reduced
63
what is ionization constant?
extent to which something dissociates in water.
64
Ksp describes what?
amount of a compound that will dissolve in water
65
what will happen if Ksp is exceeded?
ppt will form
66
alkali metals have an oxidation number of
1
67
how many electrons does a radical have?
an odd number
68
what is a coordination complex?
covalently bonded complexes between nonmetal ligands and a transition metal ion
69
what is a bohr atom?
one that only has one electron
70
what does a lewis base do?
donates electrons
71
.33e15when moving decimal to right, what happens to exponent?
DECREASES
72
what is 10^-2?
equivalent to 1/10^2
73
what is effective nuclear charge?
charge felt by the outermost electrons in the outermost shell FROM the strength of the protons (so, more protons=more charge)
74
what is a divalent ion?
2
75
when all ions have the same # of electrons, the atomic size depends on
effective nuclear charge (more protons=smaller radius)
76
what kinds of bonds are ionic and covalent?
INTRAmolecular (between atoms in a molecule)
77
what does it mean to be dibasic/tribasic?
can acccept 2 or 3 protons
78
what is the solubility of oxides in water?
insoluble, except for those with group 1 cations
79
what is the solubility of group 1 cations?
all water soluble
80
london dispersion forces rely mostly on
molecular mass
81
in gas liquid chromatography, which will have the highest retention rate?
whichever has the highest boiling point
82
if an equation releases 45j/mol of energy, what is the enthalpy change?
-45j/mol
83
when a transition metal is ionized, where are the electrons removed from?
the highest energy subshell
84
if there is a lone pair of electrons in an sp3 hybridized molecule, what is the geometry?
trigonal PYRAMIDAL
85
positron emission is favored when
there are more protons than neutrons
86
what is nitrogens preferred oxidation state?
-3
87
what is the equation specific heat
heat capacity/mass
88
what is a heterogeneous catalyst?
one that has different phase than the thing it catalyzes
89
if pKa less than current pH
it will be deprotonated
90
why is the sodium ion smaller than potassium or chloride?
its highest subshell is 4s, which is lower than the other two (4p, 5s)
91
what charged particle is emitted during beta- decay?
an electron
92
how do you calculate Rf factor?
distance traveled by thing/ solvent distance
93
how do enzymes lower the Ea?
stabilizing transition state
94
tera
10^12
95
what is the orbital configuration for octahedral compounds?
d2sp3
96
what is the entropy sign for the formation of a gaseous product?
POSITIVE
97
ft*lb/s=
J/s=Watts(W)
98
a compound with a high reduction potential is likely to be a good
oxidizer
99
the only way to change the value of Ksp is to change
the temperature
100
which layer would an amide be found in?
ether layer
101
what is silica gel and its significance in chromatography?
silica gel is a polar stationary phase, so more polar compounds will elute slower and have lower Rf
102
reduction always takes place at the
cathode
103
a large equilibrium constant means what about deltaG?
it is very negative (spontaneous)
104
an interaction between a metal cation and an electron pair donor is considered a:
coordinate covalent interaction
105
how much of a sample would remain after 2 half lives?
25%
106
what is the rate constant for a unimolecular mechanism
s-1
