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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. 120° - sp^2
Calorimetry
hydro-ic acid
Trigonal Planar
E

2. Change in moles (An) =?
Diffusion
seesaw
Cg=kPg
(moles of products that are gasses) - (moles of reactants that are gasses)

3. Releases/gives off heat (negative value)
Integrated Second-Order Rate Law
Exothermic
0
surroundings

4. Larger molecules which have higher mass and therefore electron density have stronger...
6.63x10?³4Js
London dispersion forces
non-
red

5. Significant Digits of Conversion Factors
-ol
endless
N=N.(0.5)^time/time half-life
k=Ae^(-Ea/RT)

6. Composition Formula
Molar Mass of Element/ Total Molar Mass %
Ag+ - Pb2+ - Hg2+
standard solution
Volt

7. AX4E2
Nernst Equation
square planar
s
State Functions

8. Raoult's Law - relations between vapor pressure and concentrations
q/moles
P1= X1P1°
like
Acids

9. The transfer of energy between two objects due to temperature difference
Graham's Law
M1V1=M2V2
f
Heat

10. Negative enthalpy - heat flows into surroundings
rate
exothermic
96500
3/2RT

11. An equilibrium expression
Solubility Product (Ksp)
Dipole-dipole forces
Amount of atoms present
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

12. Rate of Diffusion/Effusion formula
Buffered Solution
Negative work value; work done by system
ether
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

13. Significant Digits of counted things
Endothermic
electrolyte
endless
Molality

14. Molecules' tendency to stick to the container
vaporization
adhesion
Entropy (S)
tetrahedral

15. A device used to measure Delta H
Calorimeter
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
trigonal bipyramidal
Heat

16. These orbitals are spherical
s orbitals
?Hvap
2nd law of thermodynamics
vaporization

17. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Second-Order Half Life
n (first quantum number)
Angular Momentum Quantum Number
Manometer

18. If heat capacity isn't mentioned - you can assume that q of cal is = ?
catalyst
0
Ionic Compounds
g solute/g solvent x 100

19. Nonmetal oxide + H2O ->
sulfide
blue
acid
Aufbau Principle

20. Mass #
work
Colligative properties
Arrhenius equation
# protons + # neutrons

21. l=3
Average KE = 1/2(mass)(average speed of all particles)
X of a = moles a/total moles
n0
f

22. Each orbital can hold two e?s each w/ opposite spins
trigonal bipyramidal
Pauli Exclusion Principle
actual yield/theoretical yield x 100%
g solute/g solvent x 100

23. NH4¹?
ammonium
Molecular
Law of Definite Proportion
Integrated Zero-Order Rate Law

24. AX4E
0.0821 atm L/mol K
see-saw
paramagnetic
Bases

25. The reactant that is being oxidized - brings about reduction
Linear
reduction agent
Heisenberg Uncertainty Principle
l (second quantum number)

26. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Cg=kPg
Molarity
Aufbau Principle
London dispersion forces

27. Ecell= E°cell -RT/nF x lnQ
0
rate
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
Nernst Equation

28. Formula used when diluting stock solution (to find amount of water or stock needed)
nitrate
force x distance = work done
0.0821 atm L/mol K
M1V1=M2V2

29. Where oxidation occurs
non-
nitrate
charge
Anode

30. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
methoxy-
Atomic Mass Unit
Molecular
Magnetic Quantum Number (ml)

31. Color of Ca (flame test)
vapor pressure
Heat
red/orange
X of a = moles a/total moles

32. 1/[A] vs. time is a ...-order reaction
Diffusion
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
red
second

33. Absorbs/takes in heat (positive value)
T-shape
5% rule
A Roman numeral
Endothermic

34. Spectrum of light when an electron drops to energy level n=2
nitrite
alkyne
Balmer Series
trigonal planar

35. IMF that occurs with FON
base
Hydrogen bonding
Galvanic Cell
complex ions

36. Coffee Cup Calorimeter
Alkaline earth metals
Constant Pressure
chlorate
Magnetic Quantum Number (ml)

37. Group 1 and heavier Group 2 bases
no precipitate forms
q
strong bases
Solvent

38. Heat required to raise the system 1°C
pent-
heat capacity
endothermic
isothermal

39. A solution that resists a change in its pH
spontaneity
Buffered Solution
AE= AH - RTAn
vaporization

40. The reactant in the reduction reaction that forces the oxidation reaction to occur
Its root and adding -ide
Hybridization
Oxidizing Agent
Negative work value; work done by system

41. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
sulfite
End Point
Integrated Second-Order Rate Law
p+

42. Ester suffix
London dispersion forces
-oate
Equivalence Point
Acids

43. In ideal gas law problem - when it says "atmospheric" ...
M = square root (3RT/mm)
Dipole-dipole forces
double bond
Pressure of H2O must be Subtracted

44. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
Pressure of H2O must be Subtracted
Calorimeter
boiling point

45. Cr2O7²?
Radioactivity
dichromate
5% rule
viscosity

46. Only contains ions that change in reaction
insoluble
Heat
v3kT/m
Net Ionic Equation

47. Ability of an atom in a molecule to attract shared electrons to itself
Octahedral
strong acid strong base rxn
Electronegativity
alkyne

48. 2+ charge
indicator
Bases
phosphate
Alpha Particles-

49. 760 mmHg - 760 torr
1 atm
Trigonal Planar
s (fourth quantum number)
-1

50. We cannot simultaneously determine an atom's exact path or location
Aufbau Principle
Delta H or Enthalpy Change
(moles of products that are gasses) - (moles of reactants that are gasses)
Heisenberg Uncertainty Principle