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AP Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Volume of gas @STP
Metalliods
22.4L
Solute
-oic acid

2. Oxidation # of Ions
trigonal pyramidal
Equilibrium constant
Atmospheric Pressure
charge

3. Kinetic Energy per molecule
nu
1/2mv²
chromate
Amphoteric

4. IMF that occurs with FON
-(q of H2O + q of cal)
Hydrogen bonding
standard solution
End Point

5. Proton acceptors - must have an unshared pair of e?s
Bronsted-Lowry base
Calorimetry
Arrhenius Acid
methoxy-

6. q cal = ?
CAT
Pauli Exclusion Principle
Work
Covalently w/in themselves - Ionicly bonded w/ each other

7. We cannot simultaneously determine an atom's exact path or location
Calorimeter
v3kT/m
Heisenberg Uncertainty Principle
single bond

8. C2O4²?
Van't Hoff factor
Cation
Principal Quantum Number
oxalate

9. The measurement of heat changes
Calorimetry
Octahedral
3.0x108m/s
violet

10. Melting
Alkali metals
fusion
Open System
square planar

11. Mass reactants= mass products
Dipole Moment
Law of Conservation of Mass
v3kT/m
rate law

12. Energy required to break a bond
p
Bond Energy
sulfite
Solubility Product (Ksp)

13. 6.022x10^23
mol
Molecular Orbitals (MOs)
Equivalence Point
Hydrogen bonding

14. Average Kinetic Energy Formula
8.314 J/K mol
-one
Molal BP Elevation Constant
Average KE = 1/2(mass)(average speed of all particles)

15. Boiling point elevation formula
Law of Conservation of Mass
Dipole Moment
Acids
?Tb= kb x molality

16. neutron (symbol)
square pyramidal
n0
l (second quantum number)
period

17. x can be ignored when % ionization is <5%
Nernst Equation
E
Molarity
5% rule

18. Freezing point depression formula
Allotrope
condensation
Chemical Bonds
?Tf= kf x molality

19. (organics) nine carbons
non-
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
22.4L
-ol

20. Color of Ba (flame test)
Valence Electrons(assigned)
green/yellow
endothermic
Radioactivity

21. Arrhenius equation
0.0826Latm/Kmol
red
Positive work value; work done on system
k=Ae^(-Ea/RT)

22. Substances w/ critical temperatures below 25°C
Quantum Model
Density
surroundings
permanent gases

23. A molecule having a center of positive charge and a center of negative charge
Dipole Moment
oxide gas and water
d
l (second quantum number)

24. Liquid to gas
hept-
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
vaporization
eth-

25. OH¹?
Theory of Relativity
Galvanic Cell
Buffer
hydroxide

26. Kinetic Energy per mol
3/2RT
Oxidizing Agent
% error
increasing

27. ... compounds are most conductive
heat of fusion
lambda
4.184
ionic

28. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
0
Equivalence Point
First-Order Rate Law
Molality

29. AX4E2
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
M = square root (3RT/mm)
square planar
sulfite

30. Color of K (flame test)
critical point
purple
zero
sublimation

31. R=
acetate
8.31J/Kmol
tetrahedral
conjugate acid

32. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Theoretical yield
Standard Temperature and Pressure
l (second quantum number)
yellow --> green

33. These orbitals are perpendicular
t-shape
exothermic
p orbitals
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

34. Different form of same element
Valence Electrons(assigned)
allotrope
eth-
T-shape

35. Phase change from solid to gas
methoxy-
soluble
-(P)(Change in V)
sublimation

36. Delta H (AH) = ?
Chemical Kinetics
Theory of Relativity
Coordination Compound
q/moles

37. Point at which the titrated solution changes color
X of a = moles a/total moles
end point
Hydrogen bonding
Zero-Order Half Life

38. ClO3²?
chlorate
purple --> pink
-one
strong bases

39. Universal IMF for nonpolar molecules
London dispersion forces
-al
Ag+ - Pb2+ - Hg2+
Magnetic Quantum Number (ml)

40. Determined by the formula h/m(in kg)v - (v=velocity)
?Tf= kf x molality
wavelength
dichromate
not spontaneous

41. kb of water
Molality
electrolyte
seesaw
0.512°C

42. Experimental yield/theoretical yieldx100
% yield
single bond
Molal BP Elevation Constant
-oate

43. n+m (these are orders of reactants)
double bond
flouride
Anion
Overall Reaction Order

44. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Alkaline earth metals
(moles of products that are gasses) - (moles of reactants that are gasses)
dichromate
Law of Multiple Proportions

45. Energy (definition)
group
force x distance = work done
Pressure of H2O must be Subtracted
Ionic

46. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
-ol
are not
salt bridge
Chemical Kinetics

47. Significant Digits of Conversion Factors
endless
Coordination Compound
green/yellow
Surroundings

48. Two molecules with identical connectivity but different geometries
condensation
base and hydrogen gas
M1V1=M2V2
geometric isomers

49. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
Heisenberg Uncertainty Principle
nitrite
sublimation

50. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
Bond enthalpy
Cation
square pyramidal
spontaneous