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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. [A]0/2k
96500
Zero-Order Half Life
Alkaline earth metals
% error

2. Proton acceptors - must have an unshared pair of e?s
Chemical Kinetics
Polar Covalent
Bronsted-Lowry base
Dalton's Law of Partial Pressures

3. CO3²?
anode
carbonate
Bond Energy
sulfate

4. A weak acid that changes color at or near the equivalence point
electrolyte
Magnetic Quantum Number (ml)
indicator
% yield

5. Force acting over distance
electrolyte
End Point
Anode
Work

6. Variable for spin of electron (+.5 or -.5)
First-Order Rate Law
red/orange
Heat
s (fourth quantum number)

7. 6.022x10^23
permanent gases
tetrahedral
mol
Scientific Method

8. 2+ charge
weak acid strong base rxn
0
Alpha Particles-
non-

9. Mol/kg of solvent - used in calculating colligative properties
equilibrium
Molality
no precipitate forms
linear

10. ?T=k*m(solute)
excess reactant
Effusion
Polar Covalent
Molal BP Elevation Constant

11. Half cell in which reduction occurs
Ideal Gas Law
cathode
Open System
dichromate

12. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
A Roman numeral
Atmospheric Pressure
Density
freezing

13. Proton (symbol)
Open System
equilibrium
p
p+

14. pH=
but-
diamagnetic
Q<K
log[H+]

15. Solid to gas
3rd law of thermodynamics
sublimation
1atm=?Pa
Barometer

16. Expresses how the concentrations depend on time
Isolated System
Integrated Rate Law
?Hvap
Quantum Mechanical Model

17. 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)
Molecular Compounds
Faraday
moles of solute/ L of solution
System

18. U(rms)=(3RT/M)^1/2
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Root Mean Square Velocity
trigonal pyramidal
cohesion

19. Similar to atomic orbitals - except between molecules
spontaneous
Solute
Molecular Orbitals (MOs)
pi=(nRT)/v

20. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
96500
conjugate acid
Boltzmann distribution
rate

21. Does the same as equilibrium expression - except it uses initial concentrations
weak acid strong base rxn
Reaction Quotient (Q)
reduction agent
ionic

22. (organics) three carbons
3rd law of thermodynamics
Ag+ - Pb2+ - Hg2+
prop-
effects of IMF

23. #NAME?
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
E
oxidation
% yield

24. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
heat capacity
Closed System
blue
not spontaneous

25. Like dissolves...
Integrated Zero-Order Rate Law
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
like
red

26. Donates a single H+ Ion (... other prefixes also)
Increase Temperature
Colligative properties
prop-
Monoprotic

27. Positive enthalpy - heat flows into system
pent-
endothermic
Integrated Second-Order Rate Law
-ous acid

28. For significant digits - leading zeros ____ significant
-(q of H2O + q of cal)
are not
rate
Specific Heat (s)

29. (organics) double-bonded compound
Faraday
bromate
alkene
Equilibrium constant

30. Mass reactants= mass products
Law of Conservation of Mass
Calorimetry
Acids
Law of Conservation of Energy

31. Substance that - when dissolved - is conductive
flouride
electrolyte
Quantum Numbers
experimental yield

32. Actual Yield/Theoretical Yield*100%
Faraday
-one
Percent Yield
nitrite

33. (organics) triple-bonded compound
-oate
alkyne
single bond
are

34. Substances that form OH- when dissolved in water; proton acceptors
Anode
electron affinity
like
Bases

35. Newton's Second Law
Force = mass x acceleration
Mass
Electronegativity
AE= AH - RTAn

36. Ether prefix
methoxy-
oxide
amine
equilibrium

37. In covalent bonds - prefixes are used to tell...
Molal FP Depression Constant
sulfite
Resonance
Amount of atoms present

38. NH4¹?
Surroundings
ammonium
Reducing Agent
Temperature

39. (organics) five carbons
chromate
pent-
Cathode
square pyramidal

40. Work = ?
sulfate
-(P)(Change in V)
end point
Dalton's Law

41. 1 sigma bond - 2 pi bonds
melting point
adhesion
triple bond
Adding

42. Raoult's Law - relations between vapor pressure and concentrations
boiling point
Scientific Method
nitrate
P1= X1P1°

43. IMF that occurs with FON
Hydrogen bonding
-ol
mol Fraction
tetrahedral

44. Each orbital can hold two e?s each w/ opposite spins
insoluble
melting point
cohesion
Pauli Exclusion Principle

45. Occupies the space above and below a sigma bond
oxalate
vapor pressure
Pi Bond
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

46. Non-Ideal Gas Conditions
Transition metals
0
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
high pressure - low temperature

47. Mass #
# protons + # neutrons
Nernst Equation
M1V1=M2V2
hydroxide

48. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Delta H or Enthalpy Change
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Chemical Kinetics
Equilibrium Expression

49. AX5E
Oxidizing Agent
square pyramidal
meth-
square planar

50. Type of system in which the energy and mass may leave or enter
Open System
Second-Order Half Life
pi=(nRT)/v
% yield