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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. Gas to solid
period
Root Mean Square Velocity
deposition
endothermic
2. kb of water
0.512°C
Formal Charge
hydroxide
M = square root (3RT/mm)
3. pH=
log[H+]
deposition
22.4L
green/yellow
4. Organic w/ -O-
high pressure - low temperature
complex ions
insoluble
ether
5. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
Le Chatelier's Principle
alkene
Ampere
6. 1/([A]0*k)
Q>K
standard solution
work
Second-Order Half Life
7. Substance being dissolved in a solution (lower [ ])
Solute
strong acids
pent-
Counterions
8. Positive enthalpy - heat flows into system
Galvanic Cell
endothermic
Sigma Bond
activated complex (transition state)
9. (organics) nine carbons
non-
Molarity
rate gas A/rate gas B = square root (mm A/ mm B)
Bronsted-Lowry Base
10. Ionizes to produce H+ ions
square planar
Arrhenius Acid
Heat Capacity (C)
eth-
11. 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)
ether
period
Molecular Compounds
Oxidizing Agent
12. Peak of energy diagram
Normality
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
activated complex (transition state)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
13. Oxidation # of Compounds
-ol
0
Pressure
Zero-Order Half Life
14. Substances that form H+ when dissolved in water; proton donors
triple point
excess reactant
Acids
Oxidizing Agent
15. Group 1 and heavier Group 2 bases
strong bases
Strong acid weak base rxn
vapor pressure
Sigma Bond
16. Substance in which something is dissolved in a solution (higher [ ])
Antibonding Molecular Orbital
Solvent
Root Mean Square Velocity
Amino-
17. Effusion of a gas is inversely proportional to the square root of the molar mass
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18. Heat capacity formula
p
Strong acid weak base rxn
C=(mass)(specific heat)
entropy (S)
19. Type of system in which the energy may escape - but the mass is conserved
Closed System
Endothermic
condensation
Bond Energy
20. Amine prefix
Acid + Base --> Salt + Water
Bronsted-Lowry acid
Amino-
prop-
21. Generally insoluble anions (names)
-1
salt bridge
phosphate - sulfide - carbonate - sulfate
Colligative properties
22. Oxidation # of Polyatomic Ions
strong bases
Coordination Compound
0
charge
23. High-energy light
Gamma Ray-
high pressure - low temperature
oxalate
Equilibrium constant
24. CO3²?
Law of Conservation of Mass
carbonate
m (third quantum number)
nitrite
25. (organics) three carbons
specific heat
C + 273
amine
prop-
26. 180° - sp
Octahedral
Manometer
Q<K
Linear
27. MnO4¹?
red
heat capacity
permanganate
catalyst
28. AX3E2
Molarity
Covalently w/in themselves - Ionicly bonded w/ each other
T-shape
cohesion
29. Speed of Diffusion/Effusion formula
triple bond
rate gas A/rate gas B = square root (mm A/ mm B)
a precipitate forms
hydrocarbons
30. Volume of gas @STP
22.4L
dichromate
octahedral
nu
31. #NAME?
strong bases
E
22.4L
n0
32. The actual amount of product produced in an experiment
Hund's Rule
Enthalpy of Solution
Balmer Series
experimental yield
33. Planck's constant - used to calculate energy w/frequency
Surroundings
6.63x10?³4Js
phosphate - sulfide - carbonate - sulfate
Entropy (S)
34. Connects the 2 half cells in a voltaic cell
chromate
salt bridge
Counterions
Boltzmann distribution
35. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
viscosity
Buffer
Ionic Compounds
end point
36. Point at which vapor pressure=air pressure above
Balmer Series
Osmotic Pressure
Arrhenius equation
boiling point
37. (organics) double-bonded compound
Closed System
alkene
heat capacity
pi=(nRT)/v
38. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Amount of atoms present
rate
Density
Aufbau Principle
39. frequency symbol
nu
heat of fusion
first
Arrhenius Base
40. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
Aufbau Principle
condensation
Barometer
41. Carboxylic acid ending
London dispersion forces
(moles of products that are gasses) - (moles of reactants that are gasses)
Its element
-oic acid
42. Elements on staircase on periodic table
Metalliods
catalyst
+1 - except if bonded to Alkali Metal -1
Specific Heat Capacity
43. Tools NEEDED for dilution
Volume Metric Flask & Pipet
purple
3/2RT
force x distance = work done
44. 760 mmHg - 760 torr
Amount of atoms present
Molality
1 atm
violet
45. Mol/L - concentration of a solution
Molarity
s orbitals
cathode
increasing
46. The measurement of heat changes
conjugate acid
Ionic Compounds
Calorimetry
Pressure of H2O must be Subtracted
47. CrO4²?
chromate
Bronsted-Lowry Acid
geometric isomers
high pressure - low temperature
48. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Pressure of H2O must be Subtracted
pent-
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
insoluble
49. AX3E
dichromate
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Anion
trigonal pyramidal
50. Unit of electrical potential; J/C
Thermochemistry
Volt
London dispersion forces
Multiplying