Test your basic knowledge |

AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Pairs of electrons localized on an atom
zero
Lone Pair
Law of Definite Proportion
Theory of Relativity

2. Rate of Diffusion/Effusion formula
Second-Order Half Life
Equilibrium constant
lambda
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

3. Amount of heat needed to change a system by 1°C
equilibrium
complex ions
heat capacity
octahedral

4. frequency symbol
First-Order Half Life
v3kT/m
v3RT/M(in kg)
nu

5. A homogeneous mixture with 1 phase
nitrate
Solution
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Manometer

6. AX4E
seesaw
electron affinity
Speed of light
permanganate

7. Thickness
viscosity
Force = mass x acceleration
Speed of light
# protons + # neutrons

8. When n=3 ->2 - color=
Buffer
red
0 degrees C - 1 atm
LE Model

9. Degree of disorder in a system
1/2mv²
entropy (S)
Bronsted-Lowry base
methoxy-

10. The entropy of a pure perfectly formed crystal @0K is 0
deposition
3rd law of thermodynamics
Speed of light
Manometer

11. Amount of gravitational force exerted on an object
actual yield/theoretical yield x 100%
square planar
trigonal planar
Weight

12. Atoms combine in fixed whole # ratios
6.63x10?³4Js
boiling point
Negative work value; work done by system
Law of Multiple Proportions

13. A solution that resists a change in its pH
Buffered Solution
Increase Temperature
insoluble
melting

14. Substances w/ critical temperatures below 25°C
Law of Conservation of Energy
permanent gases
trigonal bipyramidal
second

15. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
insoluble
base
oct-
M = square root (3RT/mm)

16. If heat capacity isn't mentioned - you can assume that q of cal is = ?
0
Joule
Temperature
-(P)(Change in V)

17. Change in moles (An) =?
Hydrogen bonding
strong acid strong base rxn
(moles of products that are gasses) - (moles of reactants that are gasses)
Molality

18. Does the same as equilibrium expression - except it uses initial concentrations
Second-Order Rate Law
Reaction Quotient (Q)
# protons + # neutrons
oxidation

19. C2H3O2¹?
oxide
acetate
insoluble
1atm=?mmHg/Torr

20. Verticals on the periodic table
Its element
Molecular Compounds
zero
group

21. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
non-
no precipitate forms
Average KE = 1/2(mass)(average speed of all particles)

22. Point at which the titrated solution changes color
conjugate base
Ideal Gas Law
end point
Law of Multiple Proportions

23. (# of lone pair e-)+1/2(# of shared e-)
d
Anode
permanganate
Valence Electrons(assigned)

24. Resistance to flow
Kinetic Molecular Theory - for ideal gases
Isotopes
viscosity
Equilibrium constant

25. O²?
oxide
Multiplying
Nodes
Aufbau Principle

26. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Hund's Rule
Buffer
Molality
hydrolysis

27. If needed - indicate charge of metal(cation) by...
catalyst
A Roman numeral
n0
experimental yield

28. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
k=Ae^(-Ea/RT)
Chemical Bonds
permanganate

29. kf of water
Anode
1.86°C
Calorimetry
acid

30. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
hydro-ic acid
Colligative properties
alcohol
hydrocarbons

31. Osmotic pressure=MRT
Osmotic Pressure
Amount of atoms present
rate gas A/rate gas B = square root (mm A/ mm B)
blue-green

32. 1/[A]=kt + 1/[A]0
Acid + Base --> Salt + Water
not spontaneous
titrant buret
Integrated Second-Order Rate Law

33. Increase Volume
deposition
Increase Temperature
3.0x108m/s
triple point

34. ?H when 1 mol of bonds is broken in the gaseous state
Bond enthalpy
Endothermic
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
mol

35. IMF that occurs with FON
Molecule
Hydrogen bonding
Joule
Molal BP Elevation Constant

36. The driving force for a spontaneous is an increase in entropy of the universe
Theoretical yield
Beta Particles-
see-saw
Entropy (S)

37. AX4
rate law
Diffusion
ionic
tetrahedral

38. Instrument used to measure the pressure of atmospheric gas
d
Barometer
equivalence point
Law of Conservation of Mass

39. Newton's Second Law
Force = mass x acceleration
Quantum Model
Oxidation is Loss Reduction is Gain
3/2RT

40. AX3E2
Zero-Order Half Life
t-shape
nu
are

41. Electron pairs found in the space between the atoms
chloride
Bonding Pairs
Equivalence Point
Hydrogen bonding

42. Group 1 metals
pent-
k=Ae^(-Ea/RT)
Magnetic Quantum Number (ml)
Alkali metals

43. Idea Gas Law (actual rules)
Pi Bond
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
trigonal planar
-one

44. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Force = mass x acceleration
wavelength
Formal Charge
dec-

45. J/°Cmol or J/Kmol
dec-
insoluble
Delta H or Enthalpy Change
Molar Heat Capacity

46. Color of Ca (flame test)
Limiting reactant
-al
red/orange
X of a = moles a/total moles

47. Substance that - when dissolved - is conductive
electrolyte
1.86°C
Percent Yield
Ag+ - Pb2+ - Hg2+

48. Elements on staircase on periodic table
Metalliods
alcohol
Specific Heat (s)
-(P)(Change in V)

49. Elements which have all electrons paired and relatively unaffected by magnetic fields
q/moles
diamagnetic
s orbitals
3/2RT

50. Similar to atomic orbitals - except between molecules
# protons + # neutrons
Molecular Orbitals (MOs)
log[H+]
bent