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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. Symbol for Total Heat absorbed or released
3/2RT
q
melting point
Counterions

2. The driving force for a spontaneous is an increase in entropy of the universe
Temperature
Integrated Zero-Order Rate Law
Weight
Entropy (S)

3. Everything in the universe that is not defined by you as part of the system
1.38x10?²³J/K
Trigonal Bipyramidal
X of a = moles a/total moles
Surroundings

4. Color of Cs (flame test)
cyanide
ammonium
condensation
blue

5. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
-oic acid
Atmospheric Pressure
g solute/g solvent x 100
Reducing Agent

6. (organics) single-bonded compound
q/moles
Polar Covalent
Weight
alkane

7. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
Bond Order
Buffered Solution
msAT

8. (organics) one carbon
Molecular
Endothermic
meth-
soluble

9. Equation to find Ea from reaction rate constants at two different temperatures
dec-
Multiplying
condensation
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

10. Pure metal or metal hydride + H20 ->
base and hydrogen gas
g solute/g solvent x 100
first
red

11. OIL RIG
-(P)(Change in V)
boiling point
e-
Oxidation is Loss Reduction is Gain

12. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
Finding Empirical Formulas
Adding
0

13. When n=4 ->2 - color=
Cell Potential (Ecell)
cathode
rate
blue-green

14. A method of investigation involving observation and theory to test scientific hypotheses
AE = q + w
Polar Covalent
Pauli Exclusion Principle
Scientific Method

15. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
P of a =(X of a)(total pressure)
reduction
Cg=kPg
non-

16. Group 2 metals
endless
pent-
Alkaline earth metals
Monoprotic

17. 2 or more covalently bonded atoms
but-
0
3rd law of thermodynamics
Molecule

18. Group 1 and heavier Group 2 bases
dichromate
rate
Tetrahedral
strong bases

19. q rxn = ?
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
tetrahedral
entropy (S)
-(q of H2O + q of cal)

20. R=
0.0826Latm/Kmol
Hydrogen bonding
Hydrogen bonding
Hund's Rule

21. K
Ligand
pi=(nRT)/v
p orbitals
Equilibrium constant

22. Point at which liquid?gas occurs
boiling point
Diffusion
purple --> pink
Law of Multiple Proportions

23. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
End Point
system
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

24. IMF that exists in polar molecules
Aufbau Principle
Equivalence Point
System
Dipole-dipole forces

25. Arrhenius equation
k=Ae^(-Ea/RT)
1.38x10?²³J/K
Alkali metals
Arrhenius equation

26. Involves quantum numbers
Quantum Mechanical Model
increasing
Dalton's Law of Partial Pressures
Bond enthalpy

27. ln[A]=-kt + ln[A]0
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Arrhenius Acid
Integrated First-Order Rate Law
-al

28. Experimental yield/theoretical yieldx100
Isolated System
Hess's Law
Trigonal Planar
% yield

29. Cl¹?
Aufbau Principle
chloride
Closed System
0

30. Mixing of gases
Diffusion
iodide
Octahedral
condensation

31. Connects the 2 half cells in a voltaic cell
Constant Volume
Principal Quantum Number
salt bridge
rate law

32. Molality =
Aufbau Principle
Exothermic
Graham's Law
moles solute/kg solvent

33. l=2
Specific Heat (s)
d
diamagnetic
Equilibrium constant

34. Formula used when diluting stock solution (to find amount of water or stock needed)
M1V1=M2V2
work
oxidation
Amount of atoms present

35. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
Its root and adding -ide
l (second quantum number)
First-Order Rate Law

36. C2O4²?
oxalate
prop-
red
Heat

37. Ka=[products]^m/[reactants]^n
base
M1V1=M2V2
Acid Dissociation Constant
Solubility Product (Ksp)

38. Temperature-pressure point after which gas can no longer form liquid
Weight
0.512°C
Atmospheric Pressure
critical point

39. Non-Ideal Gas Conditions
AH
Heat Capacity (C)
Net Ionic Equation
high pressure - low temperature

40. Organic reaction in which two functional groups come together - resulting in the release of water
condensation
anode
purple
Density

41. Hydroxides are soluble or insoluble?
M1V1=M2V2
insoluble
+1 - except if bonded to Alkali Metal -1
Ideal Gas Law

42. 1/([A]0*k)
Molality
-ic acid
M1V1=M2V2
Second-Order Half Life

43. AP doesn't deal with ...-order reaction - don't pick it!
third
Hund's Rule
Atomic Mass Unit
Oxidation is Loss Reduction is Gain

44. Half-life equation
Ag+ - Pb2+ - Hg2+
N=N.(0.5)^time/time half-life
conjugate acid
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

45. Isotope
l (second quantum number)
-al
different # of neutrons
Hydrogen bonding

46. Color of Ca (flame test)
charge
Thermochemistry
Constant Pressure
red/orange

47. AX3
Specific Heat Capacity
Faraday
Molar Mass of Element/ Total Molar Mass %
trigonal planar

48. 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
oxidation
Counterions
E
LE Model

49. For significant digits - leading zeros ____ significant
are not
Ligand
s (fourth quantum number)
Pressure of H2O must be Subtracted

50. 2+ charge
increasing
purple --> pink
Alpha Particles-
Counterions