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Test your basic knowledge |
AP Chemistry
Start Test
Study First
Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.
This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
spontaneous
Nernst Equation
blue
1atm=?Pa
2. Color of Ca (flame test)
red/orange
Balmer Series
heat capacity
0
3. Lowers activation energy
Magnetic Quantum Number (ml)
catalyst
# protons + # neutrons
Quantum Model
4. What is defined by you taken from the whole universe
System
Molarity
Q>K
Theoretical yield
5. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
0 degrees C - 1 atm
Aufbau Principle
Decrease Volume and Increase Temperature
Acid + Base --> Salt + Water
6. PO4³?
group
condensation
phosphate
CAT
7. CO3²?
carbonate
Specific Heat Capacity
trigonal planar
different # of neutrons
8. (# of lone pair e-)+1/2(# of shared e-)
p+
Valence Electrons(assigned)
2nd law of thermodynamics
3rd law of thermodynamics
9. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Buffer
weak acid strong base rxn
Law of Multiple Proportions
Cation
10. AX6
blue
octahedral
Bond enthalpy
standard solution
11. (organics) nine carbons
non-
melting point
Transition metals
zero
12. These orbitals are spherical
Q>K
blue
oct-
s orbitals
13. Heat needed to change 1 g of substance to 1°C
Cation
specific heat
Integrated Second-Order Rate Law
Hess's Law
14. J/°Cg or J/Kg
AE= AH - RTAn
Specific Heat Capacity
Pressure of H2O must be Subtracted
are
15. Bomb Calorimeter
Dipole Moment
p
Strong acid weak base rxn
Constant Volume
16. AP doesn't deal with ...-order reaction - don't pick it!
Strong acid weak base rxn
p orbitals
LeChatelier's Principle
third
17. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Molecule
Boltzmann distribution
Chemical Kinetics
Molecular
18. Stronger IMF= lower... weaker IMF= higher...
Oxidizing Agent
p orbitals
vapor pressure
carbonate
19. Osmotic pressure formula
pi=(nRT)/v
f
red
Aufbau Principle
20. r=k[A]^2
adiabatic
Electronegativity
deposition
Second-Order Rate Law
21. ln[A] vs. time is a ...-order reaction
Calorimetry
g solute/g solvent x 100
square pyramidal
first
22. IMF that occurs with FON
are
Hydrogen bonding
-(q of H2O + q of cal)
spontaneous
23. SO4²?
Van't Hoff factor
Cation
sulfate
1 atm = 760 mmHg = 101.3 kPa
24. Symbol for Enthalpy
Standard Temperature and Pressure
H
-ous acid
1.86°C
25. The reactant that is being oxidized - brings about reduction
adiabatic
methods of increasing rate
spontaneous
reduction agent
26. Group 1 metals
Entropy (S)
strong acids
Alkali metals
E
27. AX4E
A Roman numeral
first
see-saw
single bond
28. Ionizes to produce OH- Ions
t-shape
linear
supercritical fluid
Arrhenius Base
29. Mass/volume
Density
Surroundings
v3RT/M(in kg)
Strong acid weak base rxn
30. Spontaneous emission of radiation
Radioactivity
different # of neutrons
activated complex (transition state)
1atm=?Pa
31. (organics) double-bonded compound
titrant buret
surroundings
oct-
alkene
32. The part of the universe one is focused upon (in thermodynamics)
system
oct-
Ag+ - Pb2+ - Hg2+
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
33. When gas compresses ...
AE = q + w
Positive work value; work done on system
Weight
Ag+ - Pb2+ - Hg2+
34. The amount of energy/heat required to raise some substance 1 degree C
phosphate
Heat Capacity (C)
8.314 J/K mol
End Point
35. All _________ compounds are electrolytes
Ionic
pi=(nRT)/v
alkene
1.38x10?²³J/K
36. How to Balance a Redox Equation
group
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
1 atm = 760 mmHg = 101.3 kPa
cohesion
37. Gain of electrons - decrease in oxidation #
Zero-Order Rate Law
reduction
Buffered Solution
M1V1=M2V2
38. Where oxidation occurs
e-
deposition
equivalence point
Anode
39. 96 -485 C/mol e-
STP
square planar
Faraday
H
40. Positive enthalpy - heat flows into system
permanent gases
blue-green
endothermic
Effusion
41. 6.022x10^23
-one
triple point
alkene
mol
42. Oxidation # of Compounds
linear
0
hept-
3.0x108m/s
43. Energy required for melting to occur
Finding Empirical Formulas
Amphoteric
Pauli Exclusion Principle
heat of fusion
44. The minimum energy that molecules must possess for collisions to be effective - Ea
5% rule
Molal BP Elevation Constant
activation energy
hex-
45. C2O4²?
Arrhenius equation
Quantum Model
Theoretical yield
oxalate
46. Colors of Reaction when (MnO4 -) --> (Mn2+)
8.314 J/K mol
C + 273
purple --> pink
hex-
47. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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on line
183
48. O²?
red/orange
Matter
Integrated First-Order Rate Law
oxide
49. If heat capacity isn't mentioned - you can assume that q of cal is = ?
0
sublimation
purple --> pink
Molar Mass of Element/ Total Molar Mass %
50. BrO3¹?
bromate
geometric isomers
isothermal
T-shape