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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. Entropy in the universe is always...
Magnetic Quantum Number (ml)
melting point
Hund's Rule
increasing

2. Determined by the formula h/m(in kg)v - (v=velocity)
trigonal pyramidal
Isotopes
wavelength
viscosity

3. OIL RIG
Angular Momentum Quantum Number
Oxidation is Loss Reduction is Gain
first
p orbitals

4. Increase Volume
red
exothermic
STP
Increase Temperature

5. Temperature-pressure combination at which solid - liquid - and gas states appear
cathode
triple point
Anode
see-saw

6. Color of Cs (flame test)
blue
endless
Nernst Equation
-(P)(Change in V)

7. neutron (symbol)
period
cohesion
n0
end point

8. The reactant in the reduction reaction that forces the oxidation reaction to occur
Van't Hoff factor
0
soluble
Oxidizing Agent

9. These orbitals are spherical
bond energy
triple bond
s orbitals
strong bases

10. Similar to atomic orbitals - except between molecules
mol
Antibonding Molecular Orbital
Anode
Molecular Orbitals (MOs)

11. An element with several different forms - each with different properties (i.e. graphite & diamond)
0.0826Latm/Kmol
Allotrope
Isolated System
alkene

12. Type of system in which the energy and mass may leave or enter
catalyst
Open System
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
are not

13. Two molecules with identical connectivity but different geometries
geometric isomers
Pauli Exclusion Principle
Increase Temperature
Ideal Gas Law

14. Moles of solute/volume of soln(L)
Theory of Relativity
Integrated Rate Law
oxide
Molarity

15. 90°&120° - dsp^3
viscosity
cohesion
96500
Trigonal Bipyramidal

16. The line running between the atoms
s (fourth quantum number)
Temperature
Sigma Bond
end point

17. All cations are soluble with bromide - chloride and iodide EXCEPT
Percent Yield
-oate
# protons + # neutrons
Ag+ - Pb2+ - Hg2+

18. Equation to find Ea from reaction rate constants at two different temperatures
blue-green
chloride
System
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

19. All forms of energy except for heat
see-saw
square pyramidal
work
not spontaneous

20. (A) - C/s
Ampere
fusion
alkene
Molal FP Depression Constant

21. U(rms)=(3RT/M)^1/2
surroundings
Root Mean Square Velocity
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
wavelength

22. If anion ends in -ite - acid name ends in...
-ous acid
hydrolysis
Equivalence Point
melting

23. Resistance to flow
0
k=Ae^(-Ea/RT)
complex ions
viscosity

24. 1 sigma bond - 2 pi bonds
Ideal Gas Law
mol
triple bond
Finding Empirical Formulas

25. A measure of resistance of an object to a change in its state of motion
octahedral
Mass
Bonding Pairs
sublimation

26. Non-Ideal Gas Conditions
Magnetic Quantum Number (ml)
methoxy-
high pressure - low temperature
seesaw

27. Amount of gravitational force exerted on an object
Weight
square pyramidal
solid CO2
Electronegativity

28. If Q<Ksp
no precipitate forms
Alkali metals
Equilibrium Expression
d orbitals

29. 1/[A] vs. time is a ...-order reaction
Hybridization
Arrhenius Acid
Increase Temperature
second

30. Nonmetal oxide + H2O ->
Overall Reaction Order
charge
3/2RT
acid

31. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
permanganate
allotrope
cathode

32. Matter can't be created nor destroyed
Surroundings
Bond Order
Law of Conservation of Mass
are

33. Spontaneous emission of radiation
Radioactivity
Cell Potential (Ecell)
Nodes
rate law

34. Reactant which doesn't get used up completely in a chemical reaction
Graham's Law
excess reactant
end point
second

35. Polyatomic Ions (bonding)
deposition
Solute
?Tf= kf x molality
Covalently w/in themselves - Ionicly bonded w/ each other

36. 760mmHg/Torr
dichromate
LeChatelier's Principle
1atm=?mmHg/Torr
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

37. STP
deposition
Mass
0 degrees C - 1 atm
Solubility Product (Ksp)

38. IMF that occurs with FON
Hydrogen bonding
Coordination Compound
melting
Pauli Exclusion Principle

39. AX4E2
square planar
a precipitate forms
Alkali metals
3/2RT

40. The heat changed in a chemical reaction.
Naming Binary Ionic Compounds
First-Order Rate Law
strong acids
Thermochemistry

41. For significant digits - leading zeros ____ significant
purple --> pink
+1 - except if bonded to Alkali Metal -1
Average KE = 1/2(mass)(average speed of all particles)
are not

42. q H2O = ?
Endothermic
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
msAT
p orbitals

43. A method of investigation involving observation and theory to test scientific hypotheses
Cg=kPg
Amount of atoms present
Scientific Method
Hybridization

44. Group 2 metals
bent
Manometer
Alkaline earth metals
s (fourth quantum number)

45. How to Balance a Redox Equation
q
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
Integrated First-Order Rate Law
pent-

46. AX3E
trigonal pyramidal
Arrhenius Acid
3rd law of thermodynamics
violet

47. The rest of the universe (in thermodynamics)
Integrated First-Order Rate Law
triple bond
Zero-Order Rate Law
surroundings

48. Molality =
C + 273
moles solute/kg solvent
Octahedral
AH

49. Oxidation # of Oxygen
-2 - with peroxide -1
Ionic
Law of Conservation of Mass
-one

50. kf of water
seesaw
Dalton's Law of Partial Pressures
1.86°C
Solution