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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. Oxidation # of free elements
3/2RT
0
Chemical Bonds
Transition metals

2. Reverse rxn occurs when
boiling point
v3RT/M(in kg)
Q>K
Finding Empirical Formulas

3. Where oxidation occurs
Anode
k=Ae^(-Ea/RT)
entropy
% error

4. 109.5° - sp^3
heat of vaporization
excess reactant
Tetrahedral
alcohol

5. Mass percent
Surroundings
g solute/g solvent x 100
Dipole Moment
Temperature

6. 760 mmHg - 760 torr
1 atm
p orbitals
Atmospheric Pressure
?Hvap

7. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Speed of light
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Atmospheric Pressure
voltaic cells

8. Connects the 2 half cells in a voltaic cell
cathode
excess reactant
Coordination Compound
salt bridge

9. In a given atom no two electrons can have the same set of four quantum numbers
Quantum Numbers
1st law of thermodynamics
Molarity
Pauli Exclusion Principle

10. Pairs of electrons localized on an atom
Lone Pair
boiling point
Law of Multiple Proportions
iodide

11. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
blue-violet
Increase Temperature
Its element

12. Ionizes to produce OH- Ions
Arrhenius Acid
Arrhenius Base
deposition
?Hvap

13. AX4E2
Molality
% yield
square planar
endless

14. 0°C and 1 atm
cathode
STP
viscosity
Molar Mass of Element/ Total Molar Mass %

15. When n=6 ->2 - color=
% yield
adiabatic
wavelength
violet

16. Expresses how the concentrations depend on time
Quantum Numbers
Integrated Rate Law
permanganate
2nd law of thermodynamics

17. (A) - C/s
Ampere
k=Ae^(-Ea/RT)
cyanide
-(q of H2O + q of cal)

18. Group 1 and heavier Group 2 bases
heat of vaporization
strong bases
Bond enthalpy
London dispersion forces

19. 1 sigma bond - 2 pi bonds
Delta H or Enthalpy Change
triple bond
k=Ae^(-Ea/RT)
endless

20. Change in Energy = ? (in terms of constant pressure; for gasses)
(moles of products that are gasses) - (moles of reactants that are gasses)
AE= AH - RTAn
permanent gases
critical point

21. 760mmHg/Torr
E
1atm=?mmHg/Torr
AE= AH - RTAn
Bases

22. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
3/2RT
d
iodide
supercritical fluid

23. Resistance to flow
Oxidation is Loss Reduction is Gain
oxide
Arrhenius Base
viscosity

24. Speed per molecule of gas
v3kT/m
Heat
adhesion
triple point

25. q H2O = ?
Constant Pressure
London dispersion forces
msAT
bent

26. When _____ significant digits - round answer to least significant digit
hydrocarbons
Van't Hoff factor
Multiplying
Reaction Quotient (Q)

27. The energy required to raise 1 g of substance 1 degree C
Barometer
Resonance
Specific Heat (s)
Boltzmann distribution

28. Increase Volume
Anode
Bonding Pairs
Increase Temperature
Atmospheric Pressure

29. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
conjugate acid
Chemical Kinetics
(moles of products that are gasses) - (moles of reactants that are gasses)
1.86°C

30. Larger molecules which have higher mass and therefore electron density have stronger...
Pauli Exclusion Principle
London dispersion forces
Molar Mass of Element/ Total Molar Mass %
period

31. Atoms with the same number of protons but a different number of neutrons
no precipitate forms
but-
Isotopes
nitrite

32. Elements in groups 3-12
Ideal Gas Law
eth-
Transition metals
Law of Definite Proportion

33. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
1.38x10?²³J/K
Ionic Compounds
Ideal Gas Law

34. OIL RIG
2nd law of thermodynamics
isothermal
l (second quantum number)
Oxidation is Loss Reduction is Gain

35. Color of Li (flame test)
moles solute/kg solvent
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
red
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

36. Group 1 metals
sulfate
Delta H or Enthalpy Change
log[H+]
Alkali metals

37. (organics) six carbons
red
Colligative properties
triple point
hex-

38. Newton's Second Law
Theoretical yield
hydrocarbons
Le Chatelier's Principle
Force = mass x acceleration

39. AX4E
moles of solute/ L of solution
seesaw
AH
-(P)(Change in V)

40. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
soluble
cohesion
Dipole Moment

41. C=2.9979*10^8 m/s
equilibrium
flouride
Speed of light
Metalliods

42. U(rms)=(3RT/M)^1/2
Normality
Solubility Product (Ksp)
Root Mean Square Velocity
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

43. pH=
Gamma Ray-
Ligand
log[H+]
Q>K

44. AX5E
System
# protons (atom is defined by this)
square pyramidal
End Point

45. Substances that form OH- when dissolved in water; proton acceptors
Tetrahedral
N=N.(0.5)^time/time half-life
Bases
State Functions

46. Temperature-pressure combination at which solid - liquid - and gas states appear
triple point
6.63x10?³4Js
Nodes
Allotrope

47. Energy required for liquid?gas
Molal BP Elevation Constant
heat of vaporization
0
sulfate

48. The transfer of energy between two objects due to temperature difference
charge
96500
Coordination Compound
Heat

49. Color of Cs (flame test)
Monoprotic
group
blue
Osmotic Pressure

50. A solid or gas that can be formed when 2 or more aqueous reactants come together
analyte
precipitate
Anion
equilibrium