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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. l=2
electron affinity
blue
d
Bronsted-Lowry Base

2. The actual amount of product produced in an experiment
experimental yield
oxide gas and water
soluble
k=Ae^(-Ea/RT)

3. Point at which liquid?gas occurs
boiling point
5% rule
alkyne
bond energy

4. IMF that exists in polar molecules
yellow --> green
v3RT/M(in kg)
Dipole-dipole forces
melting point

5. AP doesn't deal with ...-order reaction - don't pick it!
third
voltaic cells
Increase Temperature
Molecular

6. Change without heat transfer between the system and its surroundings
violet
blue-violet
adiabatic
blue-green

7. The reactant that is being oxidized - brings about reduction
A Roman numeral
reduction agent
p orbitals
Molality

8. Kinetic Energy per molecule
1/2mv²
H
sulfide
zero

9. Mass/volume
a precipitate forms
Strong acid weak base rxn
Density
Hybridization

10. A weak acid that changes color at or near the equivalence point
v3RT/M(in kg)
group
Temperature
indicator

11. Organic w/ -NH2
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
hydroxide
amine
AE= AH - RTAn

12. 760 mmHg - 760 torr
system
octahedral
M = square root (3RT/mm)
1 atm

13. Heat capacity formula
Quantum Mechanical Model
group
C=(mass)(specific heat)
sulfide

14. CN¹?
cyanide
wavelength
Buffered Solution
Pi Bond

15. Arrhenius equation
-1
chlorite
Faraday
k=Ae^(-Ea/RT)

16. Calculation from K to C
alkene
Formal Charge
C + 273
Q<K

17. Carbon & hydrogen compounds
Pauli Exclusion Principle
critical point
hydrocarbons
isothermal

18. A method of investigation involving observation and theory to test scientific hypotheses
rate
Calorimetry
Scientific Method
cyanide

19. The chemical formed when a base accepts a proton
but-
reduction
C + 273
conjugate acid

20. All forms of energy except for heat
work
-2 - with peroxide -1
excess reactant
no precipitate forms

21. R in instances that pertain to energy
log[H+]
Pressure of H2O must be Subtracted
8.314 J/K mol
zero

22. [A]0/2k
Zero-Order Half Life
A Roman numeral
2nd law of thermodynamics
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

23. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
alcohol
P of a =(X of a)(total pressure)
State Functions
phosphate - sulfide - carbonate - sulfate

24. Amount of product produced when limiting reactant is used up
Theoretical yield
entropy
Molecule
cathode

25. Point at which the titrated solution changes color
methoxy-
carbohydrates
end point
endothermic

26. Degree of disorder in a system
entropy (S)
eth-
activation energy
acid

27. Coffee Cup Calorimeter
Normality
Constant Pressure
cyanide
Zero-Order Rate Law

28. Proton (symbol)
Law of Multiple Proportions
Its element
p+
LeChatelier's Principle

29. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
trigonal bipyramidal
complex ions
n0
carbonate

30. If anion ends in -ide - acid name ends in
hydro-ic acid
Formal Charge
Its element
third

31. Type of system in which the energy and mass may leave or enter
s orbitals
Open System
96500
-ous acid

32. Variable for type of orbital
Solute
LE Model
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
l (second quantum number)

33. r=k[A]^2
second
zero
Standard Temperature and Pressure
Second-Order Rate Law

34. J/°Cg or J/Kg
AE= AH - RTAn
Counterions
Specific Heat Capacity
third

35. Half cell in which oxidation occurs
0
anode
isothermal
condensation

36. Half-life equation
freezing
Hund's Rule
1/2mv²
N=N.(0.5)^time/time half-life

37. Metal oxide + H20 ->
Gamma Ray-
base
Dipole-dipole forces
Trigonal Planar

38. AX2E - AX2E2
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Valence Electrons(assigned)
hydrolysis
bent

39. Ionizes to produce H+ ions
Arrhenius Acid
triple bond
deposition
Multiplying

40. .69/k
strong acids
bond energy
First-Order Half Life
-oate

41. A device in which chemical energy is changed to electrical energy
first
not spontaneous
Galvanic Cell
end point

42. AX3E2
boiling point
entropy (S)
T-shape
Hess's Law

43. K
Osmotic Pressure
Theory of Relativity
van't Hoff Factor
Equilibrium constant

44. Increase Pressure
Equilibrium Expression
Decrease Volume and Increase Temperature
mol
8.31J/Kmol

45. AX3
Constant Pressure
trigonal planar
blue-green
0.0821 atm L/mol K

46. Forward rxn occurs when
Q<K
Graham's Law
lambda
1 atm = 760 mmHg = 101.3 kPa

47. Change that occurs at constant temperature
single bond
isothermal
diamagnetic
Arrhenius acid

48. High-speed electrons
increasing
-oic acid
electrolyte
Beta Particles-

49. Larger molecules which have higher mass and therefore electron density have stronger...
l (second quantum number)
Ionic
Molal FP Depression Constant
London dispersion forces

50. Reactant which doesn't get used up completely in a chemical reaction
melting point
like
charge
excess reactant