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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. Occupies the space above and below a sigma bond
Decrease Volume and Increase Temperature
freezing
Pi Bond
Cation

2. Spectrum of light when an electron drops to energy level n=2
Balmer Series
methoxy-
8.314 J/K mol
are not

3. When n=4 ->2 - color=
blue-green
equivalence point
not spontaneous
weak acid strong base rxn

4. If anion ends in -ate - acid name ends in...
endothermic
p orbitals
-ic acid
m (third quantum number)

5. Molality =
Chemical Bonds
End Point
moles solute/kg solvent
Calorimetry

6. Weakest IMFs - found in all molecules
Positive work value; work done on system
London dispersion forces
Molal BP Elevation Constant
Monoprotic

7. Osmotic pressure formula
alkane
Bond Order
-ous acid
pi=(nRT)/v

8. 0°C and 1 atm
Molal FP Depression Constant
STP
lambda
l (second quantum number)

9. Oxidation # of Oxygen
supercritical fluid
-2 - with peroxide -1
linear
iodide

10. Point where acid completely neutralizes base
van't Hoff Factor
heat capacity
equivalence point
Bronsted-Lowry base

11. Change in Energy = ? (in terms of constant pressure; for gasses)
Alkali metals
AE= AH - RTAn
a precipitate forms
increasing

12. A measure of resistance of an object to a change in its state of motion
conjugate base
Mass
0.0826Latm/Kmol
isothermal

13. Variable for energy of e- - goes from 1 -2 -3 on up
but-
LeChatelier's Principle
n (first quantum number)
Bases

14. Group 1 and heavier Group 2 bases
strong bases
Coordination Compound
3rd law of thermodynamics
different # of neutrons

15. PV=nRT
-ic acid
alcohol
Trigonal Planar
Ideal Gas Law

16. How to Balance a Redox Equation
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
moles of solute/ L of solution
d orbitals
s (fourth quantum number)

17. Positive ion
ammonium
adhesion
Cation
Cell Potential (Ecell)

18. Point at which solid?liquid occurs
hydroxide
Alpha Particles-
d
melting point

19. Raoult's Law - relations between vapor pressure and concentrations
London dispersion forces
melting point
purple
P1= X1P1°

20. A single substance that may be an acid or a base (i.e. water)
1st law of thermodynamics
d
Amphoteric
k=Ae^(-Ea/RT)

21. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Specific Heat (s)
1.38x10?²³J/K
Ionic Compounds
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

22. Non-Ideal Gas Conditions
Percent Yield
high pressure - low temperature
blue-green
Tetrahedral

23. Only contains ions that change in reaction
s
viscosity
Net Ionic Equation
r1/r2

24. H + donor
cohesion
Increase Temperature
Matter
Bronsted-Lowry Acid

25. NH4¹?
System
Isolated System
ammonium
n0

26. The minimum energy that molecules must possess for collisions to be effective - Ea
Antibonding Molecular Orbital
T-shape
activation energy
d

27. pH=
base and hydrogen gas
log[H+]
Molality
Radioactivity

28. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
LE Model
?Tb= kb x molality
n0
Molecular Compounds

29. When n=6 ->2 - color=
Speed of light
Calorimeter
Gamma Ray-
violet

30. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Second-Order Half Life
Diffusion
# protons + # neutrons
yellow --> green

31. (organics) triple-bonded compound
Oxidizing Agent
alkyne
diamagnetic
Nodes

32. J/°Cmol or J/Kmol
Joule
carbohydrates
Molar Heat Capacity
Naming Binary Ionic Compounds

33. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
different # of neutrons
blue-green
exothermic
spontaneous

34. The reactant in the reduction reaction that forces the oxidation reaction to occur
-oate
period
Oxidizing Agent
0.512°C

35. Force that holds atoms together
Chemical Bonds
Enthalpy of Solution
meth-
0 degrees C - 1 atm

36. Boltzmann constant - used in calculating speed of gas per molecule
surroundings
s (fourth quantum number)
iodide
1.38x10?²³J/K

37. Verticals on the periodic table
Zero-Order Half Life
Joule
Atomic Mass Unit
group

38. When gas compresses ...
PV=nRT
surroundings
Positive work value; work done on system
endless

39. R in ideal gas law
-(q of H2O + q of cal)
0.0821 atm L/mol K
(moles of products that are gasses) - (moles of reactants that are gasses)
Bronsted-Lowry base

40. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
E
Alkali metals
insoluble
A Roman numeral

41. Melting
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
viscosity
fusion
Alkali metals

42. Instrument used to measure the pressure of atmospheric gas
spontaneity
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
different # of neutrons
Barometer

43. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
Molal FP Depression Constant
purple
Constant Pressure

44. AP doesn't deal with ...-order reaction - don't pick it!
third
Reaction Quotient (Q)
rate law
oxide

45. [A] vs. time is a ...-order reaction
zero
Equilibrium constant
Pressure
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

46. Actual Yield/Theoretical Yield*100%
6.63x10?³4Js
Percent Yield
prop-
phosphate

47. Substances w/ critical temperatures below 25°C
Beta Particles-
methoxy-
Electron Spin Quantum Number
permanent gases

48. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
?Hvap
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
hydrolysis
work

49. A solid or gas that can be formed when 2 or more aqueous reactants come together
methoxy-
Ag+ - Pb2+ - Hg2+
precipitate
Entropy (S)

50. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Integrated First-Order Rate Law
trigonal bipyramidal
% error
Cg=kPg