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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. Reactant which doesn't get used up completely in a chemical reaction
% error
blue
excess reactant
Law of Conservation of Mass

2. Lowers activation energy
-2 - with peroxide -1
moles of solute/ L of solution
catalyst
surroundings

3. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
Hund's Rule
C + 273
heat capacity
voltaic cells

4. O²?
?Tb= kb x molality
oxide
Boltzmann distribution
PV=nRT

5. l=2
square pyramidal
Bronsted-Lowry Acid
d
22.4L

6. Where oxidation occurs
charge
Anode
insoluble
yellow

7. Type of system in which nothing is transfered (no mass or energy); ideal
Isolated System
Dalton's Law
-one
Second-Order Half Life

8. Color of Li (flame test)
linear
p+
adhesion
red

9. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
LE Model
22.4L
alkane
?Tf= kf x molality

10. Kinetic Energy per molecule
1/2mv²
Integrated First-Order Rate Law
Net Ionic Equation
pent-

11. (organics) one carbon
bond energy
Overall Reaction Order
meth-
spontaneity

12. Color of Sr (flame test)
d
(moles of products that are gasses) - (moles of reactants that are gasses)
Pressure of H2O must be Subtracted
red

13. C=2.9979*10^8 m/s
-al
chlorite
Joule
Speed of light

14. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
soluble
Molecule
Magnetic Quantum Number (ml)
moles of solute/ L of solution

15. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
1/2mv²
0
d orbitals

16. The measurement of heat changes
Calorimetry
London dispersion forces
?Tf= kf x molality
Acids

17. The actual amount of product produced in an experiment
N=N.(0.5)^time/time half-life
titrant buret
cohesion
experimental yield

18. Where reduction occurs
trigonal planar
Quantum Model
Cathode
?Hvap

19. n+m (these are orders of reactants)
H
Strong acid weak base rxn
Overall Reaction Order
CAT

20. pH=
log[H+]
s orbitals
boiling point
Molecular Orbitals (MOs)

21. Boltzmann constant - used in calculating speed of gas per molecule
a precipitate forms
carbohydrates
Solution
1.38x10?²³J/K

22. Phase change from solid to gas
Work
AE = q + w
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
sublimation

23. Describe various properties of one orbital
Chemical Bonds
permanganate
non-
Quantum Numbers

24. #NAME?
Molarity
first
E
m (third quantum number)

25. Forward rxn occurs when
Molar Heat Capacity
Q<K
blue
carbonate

26. A solid or gas that can be formed when 2 or more aqueous reactants come together
Sigma Bond
Bronsted-Lowry acid
Arrhenius Acid
precipitate

27. Ptotal=P1+P2+P3+...

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28. H + donor
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
effects of IMF
Bronsted-Lowry Acid
bent

29. Measure of the change in enthalpy
Scientific Method
moles solute/kg solvent
Delta H or Enthalpy Change
hept-

30. The chemical formed when a base accepts a proton
n0
Magnetic Quantum Number (ml)
conjugate acid
Arrhenius base

31. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
complex ions
Equilibrium Expression
work
force x distance = work done

32. Determined by the formula h/m(in kg)v - (v=velocity)
wavelength
8.314 J/K mol
sulfide
excess reactant

33. Degree of disorder in a system
entropy (S)
0
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
Bronsted-Lowry Acid

34. Point where acid completely neutralizes base
Equilibrium Expression
Cathode
Pi Bond
equivalence point

35. How to Find an Empirical Formula Given Percentages
Trigonal Bipyramidal
heat of vaporization
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Arrhenius Base

36. Isotope
First-Order Half Life
# protons + # neutrons
Pressure
different # of neutrons

37. SI unit of energy; Kg*m^2/s^2
different # of neutrons
Joule
M = square root (3RT/mm)
0

38. Variable for type of orbital
Electronegativity
Scientific Method
Quantum Mechanical Model
l (second quantum number)

39. J/°Cmol or J/Kmol
Molar Heat Capacity
8.314 J/K mol
Density
endless

40. H?+OH??H2O
increasing
Aufbau Principle
strong acid strong base rxn
1atm=?Pa

41. These orbitals are perpendicular
n0
s (fourth quantum number)
STP
p orbitals

42. How to Find an Empirical Formula Given Grams
but-
STP
Overall Reaction Order
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

43. Puts H? into solution
q/moles
Arrhenius acid
Amino-
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

44. AX5
trigonal bipyramidal
equilibrium
Molecular Compounds
red

45. Speed of Diffusion/Effusion formula
AH
rate gas A/rate gas B = square root (mm A/ mm B)
non-
hydrolysis

46. The reactant that is being oxidized - brings about reduction
reduction agent
eth-
London Dispersion Forces
activated complex (transition state)

47. 1 sigma bond - 1 pi bond
Law of Multiple Proportions
double bond
purple --> pink
dichromate

48. When n=5 ->2 - color=
0.0821 atm L/mol K
Counterions
rate
blue-violet

49. A given compound always has exactly the same proportion of elements by mass
triple bond
Closed System
Law of Definite Proportion
96500

50. Happens at lines in phase change charts
equilibrium
Boltzmann distribution
Heisenberg Uncertainty Principle
system