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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. [A] vs. time is a ...-order reaction
trigonal planar
zero
-ic acid
Oxidizing Agent

2. J/°Cg or J/Kg
Specific Heat Capacity
Dalton's Law of Partial Pressures
Chemical Kinetics
trigonal pyramidal

3. Polyatomic Ions (bonding)
Amphoteric
Finding Empirical Formulas
Covalently w/in themselves - Ionicly bonded w/ each other
rate

4. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Law of Definite Proportion
meth-
Buffered Solution
yellow --> green

5. Temperature-pressure point after which gas can no longer form liquid
critical point
activated complex (transition state)
Atomic Mass Unit
oxide

6. A given compound always has exactly the same proportion of elements by mass
Valence Electrons(assigned)
reduction
Law of Definite Proportion
Enthalpy of Solution

7. Osmotic pressure=MRT
Osmotic Pressure
freezing
Magnetic Quantum Number (ml)
red

8. CO3²?
0
1 atm = 760 mmHg = 101.3 kPa
see-saw
carbonate

9. Group 2 metals
Alkaline earth metals
Barometer
Q<K
Equilibrium constant

10. Pure metal or metal hydride + H20 ->
1.86°C
Integrated First-Order Rate Law
base and hydrogen gas
Ligand

11. 1 sigma bond
3.0x108m/s
reduction agent
single bond
Molar Heat Capacity

12. Calculation from K to C
nu
C + 273
soluble
insoluble

13. Matter can't be created nor destroyed
Law of Conservation of Mass
?Tf= kf x molality
Reaction Quotient (Q)
t-shape

14. Organic w/ -NH2
amine
Work
Linear
-2 - with peroxide -1

15. Different form of same element
acid
allotrope
amine
Increase Temperature

16. Change that occurs at constant temperature
isothermal
Electron Spin Quantum Number
96500
yellow

17. Force per unit area
C=(mass)(specific heat)
Pressure
0
increasing

18. 1/[A]=kt + 1/[A]0
critical point
msAT
Integrated Second-Order Rate Law
8.31J/Kmol

19. Color of Na (flame test)
(moles of products that are gasses) - (moles of reactants that are gasses)
no precipitate forms
Adding
yellow

20. Substance that - when dissolved - is conductive
lambda
0.0821 atm L/mol K
electrolyte
X of a = moles a/total moles

21. The amount of energy/heat required to raise some substance 1 degree C
Heat Capacity (C)
condensation
third
equilibrium

22. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
exothermic
Manometer
3rd law of thermodynamics
LeChatelier's Principle

23. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
Q>K
End Point
Ionic

24. A solution that resists a change in pH - contains both a weak acid and its conjugate base
M = square root (3RT/mm)
Arrhenius Base
Buffer
sulfate

25. q rxn = ?
Negative work value; work done by system
ether
Endothermic
-(q of H2O + q of cal)

26. When gas expands ...
double bond
oxidizing agent
Negative work value; work done by system
nitrate

27. IMF that occurs with FON
Heat Capacity (C)
tetrahedral
Hydrogen bonding
weak acid strong base rxn

28. The part of the universe one is focused upon (in thermodynamics)
system
red
0
endless

29. This MUST be determined experimentally
Faraday
rate law
lambda
analyte

30. If anion ends in -ate - acid name ends in...
rate
0
London Dispersion Forces
-ic acid

31. R=
Integrated Second-Order Rate Law
8.31J/Kmol
salt bridge
% error

32. Positive ion
Ampere
eth-
Manometer
Cation

33. Variable for spin of electron (+.5 or -.5)
Molar Mass of Element/ Total Molar Mass %
1 atm = 760 mmHg = 101.3 kPa
s (fourth quantum number)
charge

34. Connects the 2 half cells in a voltaic cell
msAT
1.38x10?²³J/K
salt bridge
van't Hoff Factor

35. Releases/gives off heat (negative value)
Counterions
Osmotic Pressure
Dalton's Law
Exothermic

36. .69/k
Pressure
indicator
moles solute/kg solvent
First-Order Half Life

37. kb of water
Cation
0.512°C
Overall Reaction Order
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

38. Electron (symbol)
sublimation
5% rule
phosphate
e-

39. Actual Yield/Theoretical Yield*100%
-oate
Law of Conservation of Mass
Percent Yield
Specific Heat Capacity

40. pH=
log[H+]
Net Ionic Equation
Its element
6.63x10?³4Js

41. H?+NH3?NH4
Strong acid weak base rxn
p+
# protons + # neutrons
seesaw

42. Amount of product produced when limiting reactant is used up
blue-green
activation energy
Integrated Second-Order Rate Law
Theoretical yield

43. Energy needed to vaporize a mole of a liquid
?Hvap
dichromate
Heat
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions

44. The entropy of a pure perfectly formed crystal @0K is 0
oxalate
3rd law of thermodynamics
0
-ic acid

45. Mass reactants= mass products
indicator
viscosity
Heisenberg Uncertainty Principle
Law of Conservation of Mass

46. Theoretical yield-experimental yield/theoretical yieldx100
-al
% error
T-shape
Molecule

47. Stronger IMF= lower... weaker IMF= higher...
Ampere
vapor pressure
X of a = moles a/total moles
Normality

48. (organics) one carbon
vapor pressure
Bond Order
Metalliods
meth-

49. Carbon - hydrogen - oxygen compounds
carbohydrates
alkene
Calorimeter
oxalate

50. I=moles of particles/moles of solute dissolved

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