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Test your basic knowledge |
AP Chemistry
Start Test
Study First
Subjects
:
science
,
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. Moles of solute/volume of soln(L)
Molarity
Work
Quantum Model
blue-green
2. (organics) eight carbons
Anode
Multiplying
Bases
oct-
3. Substances w/ critical temperatures below 25°C
moles solute/kg solvent
Temperature
endless
permanent gases
4. CrO4²?
Hydrogen bonding
red
endothermic
chromate
5. Atomic #
First-Order Half Life
Bonding Pairs
# protons (atom is defined by this)
Finding Empirical Formulas
6. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
m (third quantum number)
Resonance
Acid Dissociation Constant
alkene
7. r=k
Zero-Order Rate Law
Pauli Exclusion Principle
oct-
Sigma Bond
8. AX4
strong acid strong base rxn
tetrahedral
rate law
activation energy
9. Rate of Diffusion/Effusion formula
permanent gases
heat of fusion
Radioactivity
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
10. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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11. ln[A] vs. time is a ...-order reaction
Finding Empirical Formulas
Cation
first
Law of Multiple Proportions
12. 1 sigma bond - 2 pi bonds
1.38x10?²³J/K
insoluble
triple bond
are not
13. J/°Cmol or J/Kmol
Molar Heat Capacity
phosphate - sulfide - carbonate - sulfate
Anion
Temperature
14. (organics) two carbons
lambda
Law of Multiple Proportions
eth-
1.86°C
15. Oxidation # of free elements
standard solution
cohesion
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
0
16. Oxidation # of Polyatomic Ions
Faraday
permanent gases
Solubility Product (Ksp)
charge
17. Liquid to solid
insoluble
Dalton's Law
freezing
Alpha Particles-
18. Expresses how the concentrations depend on time
Hund's Rule
mol
Integrated Rate Law
Q>K
19. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Arrhenius equation
Heat Capacity (C)
# protons (atom is defined by this)
Equivalence Point
20. 90°&120° - dsp^3
Naming Binary Ionic Compounds
Work
M = square root (3RT/mm)
Trigonal Bipyramidal
21. When n=3 ->2 - color=
red
Van't Hoff factor
adhesion
Arrhenius acid
22. negative ion
Q<K
Anion
spontaneity
Mass
23. (A) - C/s
Ampere
hydrolysis
Weight
PV=nRT
24. The entropy of a pure perfectly formed crystal @0K is 0
condensation
phosphate
Effusion
3rd law of thermodynamics
25. Mass reactants= mass products
triple bond
cohesion
Law of Conservation of Mass
alkane
26. Phase change from gas to solid
deposition
M = square root (3RT/mm)
bent
Heisenberg Uncertainty Principle
27. (organics) triple-bonded compound
Speed of light
chlorate
phosphate - sulfide - carbonate - sulfate
alkyne
28. C=2.9979*10^8 m/s
-ol
Aufbau Principle
Kinetic Molecular Theory - for ideal gases
Speed of light
29. [A]0/2k
Zero-Order Half Life
Equivalence Point
d
X of a = moles a/total moles
30. AP doesn't deal with ...-order reaction - don't pick it!
Resonance
third
Valence Electrons(assigned)
Second-Order Rate Law
31. Mass/volume
melting
Density
Arrhenius Acid
Zero-Order Half Life
32. An equilibrium expression
Galvanic Cell
Ag+ - Pb2+ - Hg2+
charge
Solubility Product (Ksp)
33. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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34. 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)
Molecular Compounds
precipitate
Polar Covalent
C=(mass)(specific heat)
35. Energy needed to break a bond
period
strong bases
bond energy
Monoprotic
36. Energy required to break a bond
LE Model
Bond Energy
Atomic Mass Unit
Bond enthalpy
37. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
force x distance = work done
Graham's Law
Force = mass x acceleration
38. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
f
hydrolysis
trigonal bipyramidal
Pi Bond
39. Puts OH? into solution
first
increasing
Arrhenius base
catalyst
40. Positive enthalpy - heat flows into system
endothermic
Volt
analyte
Scientific Method
41. Proton donors
-ous acid
Theory of Relativity
Bronsted-Lowry acid
96500
42. Solid to gas
sublimation
Hess's Law
Zero-Order Rate Law
Nodes
43. AX3E2
rate law
exothermic
Octahedral
T-shape
44. Increase Volume
nu
P of a =(X of a)(total pressure)
Reducing Agent
Increase Temperature
45. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
Ligand
acetate
Pi Bond
46. Two molecules with identical connectivity but different geometries
Trigonal Bipyramidal
Calorimetry
p orbitals
geometric isomers
47. Involves quantum numbers
Acids
Faraday
22.4L
Quantum Mechanical Model
48. Heat capacity formula
AH
Constant Volume
Principal Quantum Number
C=(mass)(specific heat)
49. Spontaneous emission of radiation
hydro-ic acid
Constant Pressure
Radioactivity
Arrhenius Acid
50. Atoms combine in fixed whole # ratios
CAT
Electronegativity
Law of Multiple Proportions
phosphate