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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. To find activation energy use the...
Arrhenius equation
Molal FP Depression Constant
endless
electron affinity

2. Increase Volume
Increase Temperature
Hybridization
CAT
Overall Reaction Order

3. R in ideal gas law
0.0821 atm L/mol K
Alpha Particles-
Heat
electron affinity

4. Significant Digits of counted things
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
endless
trigonal planar
Osmotic Pressure

5. Involves quantum numbers
end point
Quantum Mechanical Model
Acids
hydrolysis

6. Resistance to flow
van't Hoff Factor
square planar
viscosity
heat of fusion

7. Mass/volume
d
red/orange
Density
Valence Electrons(assigned)

8. O²?
chloride
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
oxide
diamagnetic

9. For significant digits - leading zeros ____ significant
0
s (fourth quantum number)
Ideal Gas Law
are not

10. Point at which vapor pressure=air pressure above
N=N.(0.5)^time/time half-life
Equilibrium Expression
CAT
boiling point

11. All _________ compounds are electrolytes
Scientific Method
0
Ionic
Calorimetry

12. Donates a single H+ Ion (... other prefixes also)
Anion
Law of Conservation of Mass
Le Chatelier's Principle
Monoprotic

13. AX2E - AX2E2
Bases
bent
weak acid strong base rxn
solid CO2

14. If Q<Ksp
octahedral
soluble
no precipitate forms
electron affinity

15. 90° - d^2sp^3
Octahedral
0
e-
like

16. 760mmHg/Torr
nu
Molality
Amount of atoms present
1atm=?mmHg/Torr

17. Carboxylic acid ending
Hund's Rule
sublimation
-oic acid
Speed of light

18. Ionizes to produce OH- Ions
Arrhenius Base
# protons (atom is defined by this)
0
% error

19. H?+OH??H2O
Graham's Law
22.4L
strong acid strong base rxn
Heisenberg Uncertainty Principle

20. Color of Cs (flame test)
Atmospheric Pressure
AE= AH - RTAn
Molarity
blue

21. Instrument used to measure the pressure of atmospheric gas
flouride
rate
Barometer
Quantum Numbers

22. AX4E2
square planar
no precipitate forms
P1= X1P1°
Equilibrium constant

23. Nonmetal oxide + H2O ->
acid
octahedral
-ol
Ideal Gas Law

24. Puts OH? into solution
Positive work value; work done on system
Density
specific heat
Arrhenius base

25. The chemical formed when a base accepts a proton
Bond enthalpy
conjugate acid
Arrhenius base
melting point

26. Peak of energy diagram
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
-ous acid
methods of increasing rate
activated complex (transition state)

27. Proton (symbol)
5% rule
p+
oxidizing agent
n (first quantum number)

28. This MUST be determined experimentally
endothermic
are
rate law
second

29. Kinetic Energy per molecule
Barometer
Anode
red
1/2mv²

30. When gas expands ...
oxidizing agent
Negative work value; work done by system
equivalence point
perchlorate

31. High-speed electrons
Acids
Beta Particles-
Transition metals
viscosity

32. A monoatomic cation takes name from...
Its element
second
Net Ionic Equation
Coordination Compound

33. Lowers activation energy
catalyst
Alkaline earth metals
Isolated System
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

34. A solid or gas that can be formed when 2 or more aqueous reactants come together
p orbitals
precipitate
melting
Van't Hoff factor

35. Gas to solid
# protons + # neutrons
deposition
excess reactant
strong acids

36. Raising heat - adding catalyst - heighten concentration - bigger surface area
chlorate
equilibrium
methods of increasing rate
supercritical fluid

37. Heat capacity formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
H
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
C=(mass)(specific heat)

38. R=
Isolated System
activation energy
0.0826Latm/Kmol
Nodes

39. S²?
Hund's Rule
sulfide
cyanide
pent-

40. 0.00°C - 1 atm
mol
cohesion
adiabatic
Standard Temperature and Pressure

41. Positive ion
but-
Cation
entropy
Ideal Gas Law

42. High-energy light
Gamma Ray-
-(P)(Change in V)
mol
m (third quantum number)

43. Everything in the universe that is not defined by you as part of the system
Coordination Compound
Speed of light
are not
Surroundings

44. The heat changed in a chemical reaction.
Thermochemistry
Law of Conservation of Mass
system
Equivalence Point

45. Ka=[products]^m/[reactants]^n
Adding
Acid Dissociation Constant
Temperature
Metalliods

46. Gas to liquid
London dispersion forces
cathode
Q>K
condensation

47. Negative enthalpy - heat flows into surroundings
specific heat
exothermic
dichromate
Nodes

48. These orbitals are spherical
Law of Conservation of Mass
e-
s orbitals
Alkali metals

49. C2H3O2¹?
alkyne
acetate
standard solution
Calorimetry

50. Energy involved in gaining an electron to become a negative ion
exothermic
N=N.(0.5)^time/time half-life
electron affinity
-ous acid