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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. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
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
3.0x108m/s
sulfate
voltaic cells

2. ClO3²?
entropy
Law of Conservation of Mass
Molecular Compounds
chlorate

3. If Q<Ksp
no precipitate forms
critical point
1/2mv²
carbohydrates

4. Describe various properties of one orbital
STP
3.0x108m/s
Quantum Numbers
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

5. Solid to liquid
Molal BP Elevation Constant
melting
-al
Molar Mass of Element/ Total Molar Mass %

6. Oxidation # of Polyatomic Ions
sulfide
charge
k=Ae^(-Ea/RT)
1/2mv²

7. Ester suffix
London dispersion forces
-oate
red/orange
3/2RT

8. 1 sigma bond - 1 pi bond
Integrated Rate Law
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
double bond
Calorimetry

9. Matter can't be created nor destroyed
Valence Electrons(assigned)
Law of Multiple Proportions
Barometer
Law of Conservation of Mass

10. A device in which chemical energy is changed to electrical energy
Aufbau Principle
catalyst
P1= X1P1°
Galvanic Cell

11. Composition Formula
Molar Mass of Element/ Total Molar Mass %
q
M = square root (3RT/mm)
-oate

12. 1/[A] vs. time is a ...-order reaction
second
paramagnetic
0
red

13. Speed per molecule of gas
v3kT/m
Constant Pressure
Matter
period

14. Change without heat transfer between the system and its surroundings
Weight
Colligative properties
Increase Temperature
adiabatic

15. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
carbohydrates
cohesion
soluble
q

16. MnO4¹?
Net Ionic Equation
Law of Conservation of Mass
1 atm
permanganate

17. All _________ compounds are electrolytes
blue-violet
wavelength
electrolyte
Ionic

18. Thickness
Le Chatelier's Principle
strong acid strong base rxn
viscosity
permanganate

19. l=1
p
blue-violet
8.31J/Kmol
Metalliods

20. Ideal Gas Law Formula
PV=nRT
-one
5% rule
rate law

21. For significant digits - leading zeros ____ significant
1/2mv²
are not
Law of Multiple Proportions
Law of Conservation of Mass

22. Occupies the space above and below a sigma bond
Bond Order
heat of vaporization
oxidation
Pi Bond

23. These orbitals are perpendicular
p orbitals
?Hvap
Colligative properties
freezing

24. Gas to solid
Law of Definite Proportion
deposition
Coordination Compound
Linear

25. pH=
log[H+]
n (first quantum number)
Valence Electrons(assigned)
dichromate

26. Cr2O7²?
mol Fraction
cathode
dichromate
Temperature

27. A single substance that may be an acid or a base (i.e. water)
Amphoteric
prop-
p+
s

28. Raoult's Law - relations between vapor pressure and concentrations
Chemical Bonds
Ag+ - Pb2+ - Hg2+
P1= X1P1°
Closed System

29. Gain of electrons - decrease in oxidation #
d orbitals
Amphoteric
reduction
Theoretical yield

30. Electron pairs found in the space between the atoms
Bonding Pairs
blue
Integrated First-Order Rate Law
allotrope

31. (organics) six carbons
Matter
hex-
Antibonding Molecular Orbital
-al

32. The minimum energy that molecules must possess for collisions to be effective - Ea
double bond
Adding
activation energy
conjugate acid

33. The weighted average of all the isotopes that an atom can have (in g/mol)
Net Ionic Equation
Pressure
Joule
Atomic Mass Unit

34. ?Hsoln=?H1+?H2+?H3+...
Average KE = 1/2(mass)(average speed of all particles)
dec-
Law of Conservation of Mass
Enthalpy of Solution

35. n+m (these are orders of reactants)
London dispersion forces
Overall Reaction Order
rate gas A/rate gas B = square root (mm A/ mm B)
oxidation

36. F¹?
-al
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
flouride
surroundings

37. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
van't Hoff Factor
s orbitals
3.0x108m/s

38. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
square planar
Second-Order Half Life
Kinetic Molecular Theory - for ideal gases
Boltzmann distribution

39. The rest of the universe (in thermodynamics)
Kinetic Molecular Theory - for ideal gases
Colligative properties
alkyne
surroundings

40. H?+NH3?NH4
Strong acid weak base rxn
Bond enthalpy
Bond Energy
Chemical Kinetics

41. Dirrect Method Formula
Limiting reactant
phosphate - sulfide - carbonate - sulfate
Bonding Pairs
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

42. High-energy light
22.4L
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
Gamma Ray-
not spontaneous

43. Colors of Reaction when (MnO4 -) --> (Mn2+)
purple --> pink
deposition
Its element
soluble

44. When n=3 ->2 - color=
chromate
red
Ampere
Bonding Pairs

45. Amount of product produced when limiting reactant is used up
Oxidation is Loss Reduction is Gain
Theoretical yield
P1V1/N1T1=P2V2/N2T2
chloride

46. Carboxylic acid ending
Equilibrium constant
0.0826Latm/Kmol
-oic acid
trigonal planar

47. Weakest IMFs - found in all molecules
high pressure - low temperature
London dispersion forces
precipitate
trigonal planar

48. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
AE = q + w
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
melting

49. Oxidation # of Hydrogen
Van't Hoff factor
Le Chatelier's Principle
hex-
+1 - except if bonded to Alkali Metal -1

50. IMF that exists in polar molecules
rate law
Bond Order
Dipole-dipole forces
Solute