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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. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
Positive work value; work done on system
Law of Multiple Proportions
Ionic

2. Elements in groups 3-12
ionic
Transition metals
Bond enthalpy
deposition

3. Speed of Diffusion/Effusion formula
% yield
rate gas A/rate gas B = square root (mm A/ mm B)
bromate
sulfide

4. Average speed of gas
Magnetic Quantum Number (ml)
v3RT/M(in kg)
q
green/yellow

5. Force per unit area
different # of neutrons
Dipole Moment
Pressure
N=N.(0.5)^time/time half-life

6. C2H3O2¹?
acetate
Second-Order Rate Law
Radioactivity
Integrated Rate Law

7. Mass #
bond energy
group
Reducing Agent
# protons + # neutrons

8. SI unit of energy; Kg*m^2/s^2
methods of increasing rate
oxalate
green/yellow
Joule

9. Effusion of a gas is inversely proportional to the square root of the molar mass

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10. l=0
second
Force = mass x acceleration
Nernst Equation
s

11. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium

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12. Chemical composition of dry ice
solid CO2
Aufbau Principle
Exothermic
A Roman numeral

13. AX5E
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
msAT
square pyramidal
0 degrees C - 1 atm

14. AX4E
precipitate
see-saw
excess reactant
0.0826Latm/Kmol

15. Where there are no electrons
Nodes
not spontaneous
Chemical Kinetics
chlorate

16. Variable for orientation of orbital (-1 through +1)
indicator
zero
m (third quantum number)
Trigonal Planar

17. 1/([A]0*k)
a precipitate forms
Dipole-dipole forces
Law of Definite Proportion
Second-Order Half Life

18. Temperature-pressure combination at which solid - liquid - and gas states appear
endless
1 atm
triple point
hydroxide

19. The driving force for a spontaneous is an increase in entropy of the universe
Entropy (S)
0
square pyramidal
q/moles

20. Mixing of gases
Diffusion
seesaw
analyte
Molality

21. Oxidation # of Hydrogen
prop-
+1 - except if bonded to Alkali Metal -1
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
hydroxide

22. The part of the universe one is focused upon (in thermodynamics)
moles of solute/ L of solution
acid
heat of vaporization
system

23. Dirrect Method Formula
blue-violet
Counterions
alkene
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

24. Boiling point elevation formula
Metalliods
Pressure
?Tb= kb x molality
-one

25. A molecule having a center of positive charge and a center of negative charge
charge
Dipole Moment
C + 273
5% rule

26. # bonding e- - # antibonding e-/2
Arrhenius base
Bond Order
s (fourth quantum number)
electrolyte

27. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
insoluble
Thermochemistry
hydrolysis
Sigma Bond

28. Color of K (flame test)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
purple
Arrhenius Base
Molecular Orbitals (MOs)

29. A method of investigation involving observation and theory to test scientific hypotheses
Scientific Method
freezing
Octahedral
d orbitals

30. Expresses how the concentrations depend on time
square planar
Integrated Rate Law
Ag+ - Pb2+ - Hg2+
msAT

31. Proton acceptors - must have an unshared pair of e?s
1 atm
Chemical Bonds
Bronsted-Lowry base
Alkaline earth metals

32. Increase Pressure
Decrease Volume and Increase Temperature
Limiting reactant
Density
Its element

33. Heat needed to change 1 g of substance to 1°C
Molarity
charge
# protons (atom is defined by this)
specific heat

34. The chemical formed when an acid donates a proton
conjugate base
0.0821 atm L/mol K
Constant Pressure
Specific Heat (s)

35. Type of system in which the energy and mass may leave or enter
non-
Open System
hept-
Metalliods

36. AX4
tetrahedral
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
n0
Q>K

37. l=1
p
Net Ionic Equation
2nd law of thermodynamics
end point

38. U(rms)=(3RT/M)^1/2
titrant buret
Root Mean Square Velocity
green/yellow
First-Order Rate Law

39. When n=6 ->2 - color=
Effusion
spontaneous
violet
A Roman numeral

40. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Calorimetry
Cg=kPg
8.31J/Kmol
electrolyte

41. Actual Yield/Theoretical Yield*100%
Valence Electrons(assigned)
1atm=?mmHg/Torr
Percent Yield
96500

42. pH=
Volume Metric Flask & Pipet
log[H+]
rate gas A/rate gas B = square root (mm A/ mm B)
System

43. AX3E
AE= AH - RTAn
trigonal pyramidal
Molarity
-ic acid

44. Elements which have all electrons paired and relatively unaffected by magnetic fields
-oate
Dipole-dipole forces
diamagnetic
Pressure of H2O must be Subtracted

45. Carbon - hydrogen - oxygen compounds
Arrhenius equation
carbohydrates
specific heat
Acids

46. AX4E
seesaw
London dispersion forces
actual yield/theoretical yield x 100%
1 atm

47. These orbitals are perpendicular
melting point
d orbitals
p orbitals
Hybridization

48. When n=4 ->2 - color=
blue-green
viscosity
mol
chlorate

49. Ending for alcohols
-ol
Delta H or Enthalpy Change
g solute/g solvent x 100
s orbitals

50. Organic reaction in which two functional groups come together - resulting in the release of water
Density
Beta Particles-
paramagnetic
condensation