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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. l=0
Pi Bond
Metalliods
s
trigonal pyramidal

2. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
Second-Order Rate Law
high pressure - low temperature
l (second quantum number)

3. Half-life equation
Pauli Exclusion Principle
Normality
Temperature
N=N.(0.5)^time/time half-life

4. Ionizes to produce H+ ions
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
X of a = moles a/total moles
Molality
Arrhenius Acid

5. 96 -485 C/mol e-
Amount of atoms present
heat capacity
Speed of light
Faraday

6. 1/([A]0*k)
0
Second-Order Half Life
C + 273
3rd law of thermodynamics

7. (organics) four carbons
# protons (atom is defined by this)
3.0x108m/s
are not
but-

8. Anions or cations as needed to produce a compound with non net charge
solid CO2
Counterions
Alkali metals
Density

9. C2O4²?
Theoretical yield
conjugate base
oxalate
carbonate

10. A device used to measure Delta H
bond energy
T-shape
Calorimeter
Bond enthalpy

11. AX2 - AX2E3
Percent Yield
linear
chlorate
C=(mass)(specific heat)

12. Group 1 and heavier Group 2 bases
Metalliods
strong bases
(moles of products that are gasses) - (moles of reactants that are gasses)
melting

13. AX5
Hydrogen bonding
acetate
Equilibrium constant
trigonal bipyramidal

14. Kinetic Energy per mol
Linear
5% rule
3/2RT
N=N.(0.5)^time/time half-life

15. When gas compresses ...
end point
Positive work value; work done on system
q/moles
single bond

16. The rest of the universe (in thermodynamics)
insoluble
Cathode
sublimation
surroundings

17. Faraday's constant
Heisenberg Uncertainty Principle
Amphoteric
96500
l (second quantum number)

18. Variable for energy of e- - goes from 1 -2 -3 on up
Equilibrium constant
Molar Mass of Element/ Total Molar Mass %
n (first quantum number)
triple bond

19. Oxoacid solution (such as HSO4-) forms...
Ideal Gas Law
oxide gas and water
Volt
soluble

20. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
vapor pressure
Open System
Acid + Base --> Salt + Water
group

21. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Bonding Pairs
oct-
strong acids
London Dispersion Forces

22. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
LE Model
melting point
complex ions
hydrolysis

23. CrO4²?
Constant Volume
chromate
?Tf= kf x molality
complex ions

24. Half cell in which reduction occurs
C=(mass)(specific heat)
Integrated Second-Order Rate Law
-oic acid
cathode

25. Puts H? into solution
Arrhenius acid
Delta H or Enthalpy Change
Average KE = 1/2(mass)(average speed of all particles)
Cathode

26. Point at which vapor pressure=air pressure above
Pi Bond
-(q of H2O + q of cal)
boiling point
Ag+ - Pb2+ - Hg2+

27. Atoms combine in fixed whole # ratios
oct-
Osmotic Pressure
Trigonal Bipyramidal
Law of Multiple Proportions

28. The minimum energy that molecules must possess for collisions to be effective - Ea
London dispersion forces
London dispersion forces
activation energy
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

29. IMF that exists in polar molecules
sulfide
Dipole-dipole forces
Surroundings
trigonal bipyramidal

30. Type of system in which nothing is transfered (no mass or energy); ideal
Isolated System
amine
melting
sulfide

31. Melting
spontaneous
fusion
Zero-Order Rate Law
end point

32. Involves quantum numbers
Ideal Gas Law
square planar
Quantum Mechanical Model
Hund's Rule

33. The part of the universe one is focused upon (in thermodynamics)
Specific Heat Capacity
system
Dipole-dipole forces
red

34. r=k
Zero-Order Rate Law
Specific Heat Capacity
Bronsted-Lowry acid
Counterions

35. Solid to liquid
melting
Overall Reaction Order
adhesion
0 degrees C - 1 atm

36. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Integrated Rate Law
Calorimeter
different # of neutrons

37. 101 -325 Pa
1atm=?Pa
Boltzmann distribution
Overall Reaction Order
purple

38. All cations are soluble with sulfate EXCEPT
cyanide
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
P of a =(X of a)(total pressure)
conjugate acid

39. Change in Energy (AE) = ? (in terms of work)
AE = q + w
geometric isomers
v3kT/m
increasing

40. Instrument used to measure the pressure of atmospheric gas
boiling point
Barometer
permanganate
P of a =(X of a)(total pressure)

41. Reactant that's completely used up in a chemical reaction
Limiting reactant
Bond Energy
Pauli Exclusion Principle
Positive work value; work done on system

42. Organic w/ -NH2
trigonal bipyramidal
non-
amine
Diffusion

43. The total energy of the universe is constant - all systems tend towards minimum energy
salt bridge
1.38x10?²³J/K
1st law of thermodynamics
0

44. Proton donors
3/2RT
Bronsted-Lowry acid
Aufbau Principle
Resonance

45. Point where acid completely neutralizes base
Cell Potential (Ecell)
?Hvap
equivalence point
n (first quantum number)

46. Solution in flask being titrated
Hydrogen bonding
C=(mass)(specific heat)
van't Hoff Factor
analyte

47. OH¹?
hydroxide
Octahedral
Ideal Gas Law
condensation

48. The heat changed in a chemical reaction.
4.184
van't Hoff Factor
first
Thermochemistry

49. Anything occupying space and with mass
Atmospheric Pressure
Acids
freezing
Matter

50. Generally insoluble anions (names)
t-shape
C + 273
phosphate - sulfide - carbonate - sulfate
Electron Spin Quantum Number