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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. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
bent
strong bases
Chemical Kinetics
Manometer

2. If anion ends in -ite - acid name ends in...
not spontaneous
-ous acid
moles of solute/ L of solution
P1V1/N1T1=P2V2/N2T2

3. Amount of product produced when limiting reactant is used up
Theoretical yield
0
1/2mv²
Force = mass x acceleration

4. A given compound always has exactly the same proportion of elements by mass
Principal Quantum Number
Standard Temperature and Pressure
square planar
Law of Definite Proportion

5. 1 sigma bond - 1 pi bond
double bond
violet
specific heat
Alkaline earth metals

6. Only contains ions that change in reaction
Net Ionic Equation
Graham's Law
Lone Pair
permanganate

7. 760mmHg/Torr
acetate
1atm=?mmHg/Torr
insoluble
Hydrogen bonding

8. Puts H? into solution
Atmospheric Pressure
Arrhenius acid
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
sulfide

9. 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)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Molecular Compounds
Linear
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

10. negative ion
Anion
H
Zero-Order Half Life
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

11. Reactant which doesn't get used up completely in a chemical reaction
hydrolysis
excess reactant
d orbitals
Enthalpy of Solution

12. (organics) single-bonded compound
X of a = moles a/total moles
alkane
Atomic Mass Unit
q

13. AX4E2
-(q of H2O + q of cal)
Acid Dissociation Constant
square planar
0

14. Force acting over distance
Anode
Work
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
sulfite

15. Proton donors
Galvanic Cell
Bronsted-Lowry acid
Bond Order
Law of Conservation of Energy

16. Molecules' tendency to stick to the container
exothermic
phosphate
Electron Spin Quantum Number
adhesion

17. Increase Pressure
cyanide
Decrease Volume and Increase Temperature
1 atm = 760 mmHg = 101.3 kPa
Cell Potential (Ecell)

18. A method of investigation involving observation and theory to test scientific hypotheses
Resonance
Scientific Method
Ag+ - Pb2+ - Hg2+
exothermic

19. ClO3²?
chlorate
0
Average KE = 1/2(mass)(average speed of all particles)
Pressure

20. r=k[A]
m (third quantum number)
group
First-Order Rate Law
Dipole-dipole forces

21. PO4³?
Ionic
condensation
amine
phosphate

22. For significant digits - leading zeros ____ significant
-oic acid
Isotopes
wavelength
are not

23. (organics) triple-bonded compound
insoluble
iodide
0.0821 atm L/mol K
alkyne

24. AX3
boiling point
trigonal planar
chromate
oxide gas and water

25. The part of the universe one is focused upon (in thermodynamics)
Speed of light
Metalliods
system
cathode

26. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
purple --> pink
Cg=kPg
Cathode
Multiplying

27. AX3E
trigonal pyramidal
Law of Multiple Proportions
Buffered Solution
f

28. The chemical formed when an acid donates a proton
-ol
Electronegativity
Lone Pair
conjugate base

29. Color of K (flame test)
Adding
moles solute/kg solvent
purple
m (third quantum number)

30. Phase change from solid to gas
Constant Pressure
-2 - with peroxide -1
sublimation
STP

31. Effusion of a gas is inversely proportional to the square root of the molar mass

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32. Elements which have all electrons paired and relatively unaffected by magnetic fields
oxidation
diamagnetic
critical point
Molarity

33. Substance that - when dissolved - is conductive
precipitate
Dipole Moment
electrolyte
N=N.(0.5)^time/time half-life

34. Donates a single H+ Ion (... other prefixes also)
yellow
Monoprotic
Calorimeter
pi=(nRT)/v

35. n+m (these are orders of reactants)
Chemical Kinetics
s (fourth quantum number)
Transition metals
Overall Reaction Order

36. Oxidation # of Hydrogen
Strong acid weak base rxn
double bond
+1 - except if bonded to Alkali Metal -1
allotrope

37. Universal IMF for nonpolar molecules
strong acid strong base rxn
actual yield/theoretical yield x 100%
end point
London dispersion forces

38. S²?
sulfide
prop-
First-Order Rate Law
Integrated Second-Order Rate Law

39. Has values from 0 to (n-1); tells shape of atomic orbitals
Cation
Galvanic Cell
Angular Momentum Quantum Number
e-

40. How to Find an Empirical Formula Given Percentages
equilibrium
exothermic
acetate
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

41. AX6
Law of Multiple Proportions
?Hvap
Allotrope
octahedral

42. J/°Cmol or J/Kmol
msAT
Molar Heat Capacity
M1V1=M2V2
Acid + Base --> Salt + Water

43. Phase change from gas to solid
Effusion
deposition
Manometer
wavelength

44. Work = ?
Ampere
-(P)(Change in V)
precipitate
Quantum Numbers

45. Liquid to gas
Oxidation is Loss Reduction is Gain
fusion
sulfide
vaporization

46. Isotope
Q>K
Solution
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
different # of neutrons

47. Actual Yield/Theoretical Yield*100%
Nernst Equation
Percent Yield
red
Temperature

48. Change without heat transfer between the system and its surroundings
Bronsted-Lowry base
geometric isomers
adiabatic
M = square root (3RT/mm)

49. When n=5 ->2 - color=
Antibonding Molecular Orbital
chloride
blue-violet
viscosity

50. Mole Fraction
X of a = moles a/total moles
boiling point
Equilibrium Expression
Barometer