Gen Chem 1 Flashcards
1
Q
change in heat of isothermal
A
non-zero
2
Q
are standard state and standard temperature and pressure the same
A
no
3
Q
half-life
A
amount of time required for exactly one half of the mass of the substance to disappear due to radioactive decay
4
Q
work
A
energy transfer via force or via change in volume at a constant pressure
5
Q
what happens below pH 7
A
[H+] > [OH-]
6
Q
equation for bom calorimeter
A
q=C(deltaT)
7
Q
group 2
A
alkaline earth metals
8
Q
conjugate base
A
acid without its H+
9
Q
beta decay
A
neutron to a proton, ejection of electron
10
Q
covalent bonds
A
between non-metals and involves the sharing of electrons
11
Q
work
A
energy transfer via force or via change in volume at a constant pressure
12
Q
percent mass
A
mass of an element/ mass of the compound *100%
13
Q
units of entropy
A
J/K
14
Q
reaction rate
A
change in molarity of reactants per second
15
Q
attractive electrons in or out of phase
A
in phase
16
Q
work done by a system
A
negative
17
Q
strong acids have a ____ Ka and a ____ pKa
A
large, small
18
Q
change in temperature of isothermal
A
zero
19
Q
bronsted-lowry acid
A
donate H+
20
Q
endothermic change in enthalpy for fromation
A
positive
21
Q
the horizontal regions on a titration curve
A
buffer
22
Q
how does change in enthalpy of reaction change with a reaction in reverse
A
negative
23
Q
second law of thermodynamics
A
entropy of a system is always increasing
24
Q
what is the reverse of vaporization
A
condensation
25
area under the P vs V graph
work
26
atomic radius and the periodic table
increases down and left
27
molecular formula
same as or multiple of the empirical formula
28
bicarbonate
HCO3-
29
Q
reaction proceeds to the right
30
enzymes
catalyze biochemical reactions
31
symbol for specific heat capacity
c (lowercase)
32
Chlorite
ClO2(2-)
33
Permanganate
MnO4-
34
magnetic quantum number
orbital orientation
| -l to l
35
Q>K
reaction proceeds to the left
36
pKw is equal to
pH=pOH=14
37
What is needed for a reaction to occur (2 things)
enough energy to overcome the activation energy
AND
the correct spatial orientation
38
pH equals
-log[H+]
39
A
mass number
| number of protons and neutrons
40
negative change in entropy
decrease randomness
41
heisenberg uncertainty principle
the more precisely one property is measured the less precisely the other can be known
42
what happens above pH 7
[H+]
43
second quantum number
azimuthal (l)
44
actual yield
how much product is actually made
45
the only elements to produce a magnetic field
Fe, Co, Ni
46
when is maximum entropy
equilibrium
47
Chlorate
ClO3-
48
first order
ln[A] versus time
| -k slope
49
Noble gases
+/-0
| Stable
50
equation for bom calorimeter
q=C(deltaT)
51
q=change in enthalpy is only true at
constant pressure
52
is a lewis acid an electrophile or nucleophile
electrophile
53
Metals
Loosely held electrons
54
isotopes
atoms with the same number of protons and different numbers of neutrons
different forms of an element
55
calorimeters are used to calculate
change in enthalpy
56
do light or dark colors radiate more?
dark
57
phenylphtalien
9.3
58
amphoteric
can act as an acid or base
59
enthalpy
energy contained within chemical bonds
60
le-chatelier's principle
systems at equilibrium that experience change will shift to reduce the effects of that change
61
strong bases (8)
```
Group IA hydroxides
NH2-
H-
Ca(OH)2
CaO
Sr(OH)2
Ba(OH)2
Na2O
```
62
titration
drop by drop mixing of an acid and a base with an indicator
63
bond dissociation energy
bond energy
64
group 17
halogens
65
example of amphoteric molecule
water
66
spin quantum number
+/-1/2
67
electronegativity and the periodic table
increases up and across
68
pOH equals
-log[OH-]
69
Kw is equal to
10^-14=[H30+][OH-]
70
what happens at pH of 7
[H+]=[OH-]
71
hypochlorite
ClO-
72
periods
rows of the periodic table
| elements have the same valence shell
73
ways to increase entropy (5)
```
more particles
form a gas
increase volume
increase temperature
increase complexity/disorder
```
74
pKa of strong acids
below 0
75
fourth quantum number
spin (ms)
76
q=change in enthalpy is only true at
constant pressure
77
negative work
done by the system
78
is bonding or anitbonding higher in energy
antibonding
79
is 3d or 4s higher in energy?
3d
80
isobaric
constant pressure
81
what is the pH at equivalence for weak base/strong acid
below 7
82
units of energy
J or cal
83
radioactive decay
process by which unstable atoms change their chemical composition over time
84
titrant
being added, known concentration
85
how many electrons in all shells after the first
8
86
What is the Bohr model?
Atomic structure
+ nucleus with orbits of electrons
87
double displacement reaction is also known as
metathesis
88
molecular weight
mass of the elements in a molecule summed together
89
perchlorate
ClO4-
90
metallic character and the periodic table
increases down and left
91
an increase in temperature of an exothermic reaction
decreases the equilibrium constant
92
increase in entropy is spontaneous or nonspontaneous
spontaneous
93
enthalpy
energy contained within chemical bonds
94
relative heat of combustion
+1 for C
| -0.5 for O
95
How does metallic character change with size?
smaller are less metallic
96
reverse of fusion
melting
97
is 5s or 4p higher in energy?
5s
98
electrolytes
compounds that fully dissociate in water
99
electron capture
proton to neutron, capture of electron
100
what is the pH at equivalence for weak acid/strong base
above 7
101
how many electrons in the first shell
two
102
lewis acid
accept electron pair
103
lewis base
donate electron pair
104
by what mechanism are covalent bonds broken and reformed?
radical reaction
105
heat capacity
amount of energy a system must absorb to give a unit change in temperature
106
change in energy is equal to
q+w
107
standard state
reference point for measurement
108
what equation shows that kinetic energy and temperature are directly proportional
KE=(3/2)KbT
109
Ka=
[H+][A-]/[HA]
110
unit of enthalpy
J
111
what two measures does the uncertainty principle refer to?
position and momentum
112
equation for specific heat capacity
c=q/m(deltaT)
| q-mc(deltaT)
113
change in heat of adiabatic
zero
114
henderson-hasselbach
pH=pKa+log(A-/HA)
115
does a catalyst change the equilibrium constant
no
116
energy levels
represent the energies of the electrons in an atom
117
theoretical yield
prediction of yield under ideal conditions
118
what is the pH at equivalence for strong base/strong acid
7
119
unit of enthalpy
J
120
half equivalence opint
pH=pKa
121
symbol for heat capacity
C (capital)
122
what is the pH at equivalence for strong acid/strong base
7
123
alkali metals
+1
| reactive, soft, explode when exposed to water
124
equilibrium
reactants and products are at concentrations that have no further tendency to change with time
forward and reverse reactions proceed at the same rates
125
change in enthalpy of vaporization
enthalpy of change from liquid to gas
126
electron configuration
set of quantum numbers and the number of electrons in each
127
order the subatomic particles by size
protons=neutrons>>>electrons
128
change in enthalpy of formation
formation of a compound from elements in their standard states
129
does an anion have more or less electrons than protons
more
130
manganite
MnO
131
how to determine a formula from the percent mass
change % to mass in g
convert to moles
divide all by the lowest number of moles (coefficient)
132
work equation
W=P(deltaV)
133
NH3 and NH4+
base and conjugate acid
134
HCl and Cl-
acid and conjugate base
135
hydrolysis of salts
conjugate acid/base combined with a cation/anion
136
one equivalent
amount of acid or base necessary to produce or consume one mole of H+ ions
137
percent yield
actual/theoretical *100%
138
examples of good electrolytes
ionic compounds
| strong acids/bases
139
work on a system
positive
140
indicators
weak acids that change color when dissociating
141
how does change in enthalpy of reaction change with a reaction in reverse
negative
142
catalyst
any substance that increases reaction rate without being consumed in the reaction
143
does a cation have more or less electrons than protons?
less
144
do light or dark colors absorb more?
dark
145
standard state
reference point for measurement
146
units of specific heat capacity
J/g*°C or cal/g*°C
147
zero order
[A] versus time
| -k slope
148
third law of thermodynamics
pure crystalline substances at absolute zero have zero entropy
149
hydroxide
OH-
150
Z
atomic number
| number of protons
151
third law of thermodynamics
pure crystalline substances at absolute zero have zero entropy
152
what type of solution will require a high condosity
more metallic character than NaCl
153
pauli exclusion principle
no two electrons in a single atom can have the same four quantum numbers
154
first law of thermodynamics
energy cannot be created or destroyed
155
equation for coffee cup calorimeter
q=mc(deltaT)
156
alkaline earth metals
+2
| reactive
157
methyl orange
3.7
158
positron emmision
emitted as a byproduct
159
conversion from C to K
°C+273=K
160
principal quantum number
shell and relative energy of the electron in the shell
161
conjugate acid
base plus a H+
162
does adding the salt of a weak acid raise and lower the pH and why
raise because the weak acid reforms, taking away H+
163
how to find Ka of a weak acid
Ka=(x^2)/([HA]-x)
164
coulombs law
F=(kqq)/r^2
165
nitrate
NO3-
166
Phosphate
PO4(3-)
167
condosity
concentration of NaCl solution that will conduct the same electronegativity as the solution in question
168
azimuthal quantum number
subshell of the orbital
| s=0 p=1 d=2 f=3
169
double displacement reaction
AB + CD--> AD +CB
170
adiabatic
no heat exchange
171
sign of change in enthalpy for making bonds
negative
172
Na2CO3
salt of a weak acid (bicarbonate)
173
second law of thermodynamics
entropy of a system is always increasing
174
Group 1
alkali metals
175
positive change in gibbs free energy
non-spontaneous
176
second order
1/[A] versus time
| k slope
177
non-metals
tightly held electrons
178
what is always true at the equivalence point
[titrant]=[analyte]
179
what type of heat exchange is analogous to current through w wire
conduction
180
change in temperature of adiabatic
non-zero
181
units of gibbs free energy
J
182
First quantum number
Principal (n)
183
pH+pOH=
14
184
Carbonate
CO3(2-)
185
Cyanide
CN-
186
with what variable does the equilibrium constant change
temperature
187
third quantum number
magnetic (Ml)
188
can you take ln(-x)
no
189
how many electrons in a d orbital?
ten
190
Kb=
[OH-][HA]/[A-]
191
strong bases have a ____ Kb and a ____ pKb
large, small
192
what equation shows that kinetic energy and temperature are directly proportional
KE=(3/2)KbT
193
energy is required to ____ bonds
break
194
zeroth law of thermodynamics
if A and B are in equilibrium and B and C are in equilibrium, then A and C must be in equilibrium
195
analyte
in beaker, unknown concentration
196
change in enthalpy of formation
formation of a compound from elements in their standard states
197
what are the condition for standard state
changes by table, reference
198
molar mass
mass of a given substance divided by the amount of substance
199
litmus
6.5
200
ionic character
measure of the polarity of a bond
| the greater the difference between electronegativity means more ionic character
201
positive work
done on the system
202
arrheius base
give up OH- ions
203
what are the condition for standard state
changes by table, reference
204
change in standard enthalpy of formation of elements
0
205
Ka*Kb=
Kw
206
Balancing reactions
Carbons
Hydrogens
Oxygens
(Others)
207
single displacement reaction
A + BC--> AC +B
208
F block
lanthanides and actinides
209
change in enthalpy of solution
dissolution of a species in solution
210
Sulfuric acid
H2SO4
211
buffer solution
weak acid and weak base, often conjugates of one another
212
quantum mechanics
every electron in an atom has 4 numbers to define shell, subshell, orbital, and spin
213
ln(0.5)
negative
214
increase pressure
towards less molecules of gas
215
bronsted-lowry base
accept H+
216
does the indicator impact pH
no
217
zeroth law of thermodynamics
if A and B are in equilibrium and B and C are in equilibrium, then A and C must be in equilibrium
218
Manganate
MnO4(2-)
219
an increase in temperature of an endothermic reaction
increases the equilibrium constant
220
endothermic change in enthalpy for fromation
positive
221
relationship between size and charge stability
increases with size
222
negative change in gibbs free energy
spontaneous
223
lustrous
shiny
224
which halogens are gas at room temperature
Fl
| Cl
225
Characteristics of metals
shiny, malleable, ductile, conductors, ionic bonds
226
NH4NO3
salt of a weak base (ammonium)
227
at what pH should an indicator change color
pH of equivalence
228
fundamental thermodynamic relation
deltaG=deltaH-T(deltaS)
229
groups
families
columns of the periodic table
same number of valence electrons
230
do non-metals form positive or negative ions
negative
231
arrhenius acid
give up H+ ions
232
relation between change in gibbs energy and Keq
deltaG= -RTln(Keq)
233
constant pressure implies
open container
234
which halogens are solid at room temperature
I
| As
235
f=
v/lamda
236
area under the P vs V graph
work
237
positive work
done on the system
238
carbonic acid
H2CO3
239
how many electrons in a p orbital
six
240
strong acids (8)
```
HI
HBr
HCl
H2SO4
HNO3
HClO4
HClO3
H3O+
```
241
what property defines an element
atomic number
242
electron affinity and the periodic table
increases up and across
243
specific heat capacity
heat capacity for an individual substance per unit mass
244
empirical formula
simplest formula for a compound
245
units of heat capacity
J/K or cal/°C
246
do bonding have attractive or unattractive electrons
attractive
247
sign of change in enthalpy for breaking bonds
positive
248
isothermal
constant temperature
249
ionic bonds
between a metal and a non-metal due to electrostatic attraction
formation of cations and anions
250
first law of thermodynamics
energy cannot be created or destroyed
251
are standard state and standard temperature and pressure the same
no
252
Ammonium
NH4+
253
calorimeters are used to calculate
change in enthalpy
254
at constant pressure, enthalpy change is equal to
q
255
energy (KE) of the ejected electron
energy minus the work function
256
anion
negative
257
Nitrite
NO2-
258
decrease pressure
towards more molecules of gas
259
effective nuclear charge
more electrons and more electron shells shield the outer electrons from the positive nucleus
260
do metals form positive or negative ions
positive
261
Naming acids
ate-->ic
| ite-->ous
262
do metals or non-metals have lower melting points
non-metals
263
does a more stable bond have more or less energy than a less stable bond?
more energy
264
does forming bonds use or release energy?
releases
| bonds form that result in a decrease in energy
265
change in enthalpy of reaction
products-reactants
266
halogens
-1
| non-metallic
267
characteristics of non-metals
low melting points, covalent bonds
268
What charge does the nucleus have?
positive
269
change in enthalpy of fusion
enthalpy of change from liquid to solid
270
does [H+]=[OH-] always hold true at the equivalence point?
no, only strong acid and strong base titration
271
ionization energy and the periodic table
increases up and across
272
E=
hf
hv/lamda
hc/lamda
273
limiting reagent problems
balance reaction
| determine how much product can be made with each reactant
274
entropy
measure of randomness or disorder in a system
275
what makes up the nucleus
protons and electrons
276
pKa+pKb=
14
277
is a cation smaller or lager than its neutral counterpart
smaller
278
groups 3-12
transition metals
279
work done by a system
negative
280
conduction
molecular collisions carry heat along a conduit such that high energy molecules collide with their neighbors, which in turn collide with their neighbors and spread the energy throughout
281
how many electrons in an s orbital
two
282
change in enthalpy of combustion
enthalpy value for combustion of a compound with oxygen to form carbon dioxide and water
283
coordinate covalent bond
covalent bond in which both electrons shared are donated by the same atom
284
change in enthalpy of reaction
products-reactants
285
transition metals
ductile, malleable, conduct electricity and heat, multiple oxidation states
286
heat of combustion
amount of energy released when a molecule is combustion with oxygen
287
temperature
average kinetic energy of molecules
288
decomposition reaction
AB--> A + B
289
equation for heat capacity
C=g/(deltaT)
290
convection
hotter portions rise and cooler portions sink in a fluid
291
when is the maximum buffering strength
[HA]=[A-]
292
cation
positive
293
negative natural log
between 0 and 1
294
work equation
W=P(deltaV)
295
Group 18
noble gases
296
negative work
done by the system
297
equation for coffee cup calorimeter
q=mc(deltaT)
298
exothermic change in enthalpy of formation
negative
299
sulfurous acid
H2SO3
300
exothermic change in enthalpy of formation
negative
301
conversion from C to K
°C+273=K
302
more energy available to do work with what change in entropy
positive
303
change in energy is equal to
q+w
304
Atomic weight
average weight of an element based on the relative abundance of isotopes
305
at constant pressure, enthalpy change is equal to
q
306
which halogens are liquid at room temperature
Br
307
gibbs free energy
amount of free or useful energy available to do work
308
unstable molecule has a _____ heat of combustion
high
309
black body radiator
perfect theoretical radiator
310
Sulfate
SO4(2-)
311
work function
energy required to eject an electron from the outermost shell
312
does a more stable molecule have a higher or lower heat of combustion?
lower
313
work on a system
positive
314
how to increase yield
use more reactants
| shift equilibrium to the right (often by removing product as it forms)
315
mole
6.02e23 of anything
316
positive change in entropy
increase randomness
317
constant volume implies
rigid walls
318
change in standard enthalpy of formation of elements
0
319
radiation
electromagnetic waves emitted from a hot body into surrounding environment
320
alpha decay
loss of one He nucleus
| A: 4 Z: 2
321
is an anion smaller or larger than its neutral counterparts
larger
322
ln(10)
positive
323
stable molecule has a _____ heat of combustion
low
