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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. Oxidation # of Oxygen
5% rule
supercritical fluid
-2 - with peroxide -1
oxidizing agent
2. Substances w/ critical temperatures below 25°C
oct-
Amount of atoms present
Arrhenius equation
permanent gases
3. E?s fill the lowest energy orbital first - then work their way up
dec-
Scientific Method
freezing
Aufbau Principle
4. For significant digits - trailing zeros _____ significant
first
Specific Heat Capacity
are
Exothermic
5. A molecule having a center of positive charge and a center of negative charge
2nd law of thermodynamics
Dipole Moment
force x distance = work done
?Hvap
6. High-energy light
Thermochemistry
Gamma Ray-
-one
Positive work value; work done on system
7. Universal IMF for nonpolar molecules
standard solution
London dispersion forces
methoxy-
are
8. Metal oxide + H20 ->
diamagnetic
carbonate
base
Valence Electrons(assigned)
9. (# of lone pair e-)+1/2(# of shared e-)
strong bases
Dalton's Law
Valence Electrons(assigned)
v3kT/m
10. The transfer of energy between two objects due to temperature difference
Solubility Product (Ksp)
Surroundings
analyte
Heat
11. This MUST be determined experimentally
Le Chatelier's Principle
Lone Pair
rate law
m (third quantum number)
12. In ideal gas law problem - when it says "atmospheric" ...
Its root and adding -ide
Pressure of H2O must be Subtracted
Molality
Molecular
13. Force per unit area
Pressure
Density
Equilibrium constant
Closed System
14. Carbon - hydrogen - oxygen compounds
carbohydrates
salt bridge
1 atm
melting
15. Symbol for Total Heat absorbed or released
q
Diffusion
blue
critical point
16. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
k=Ae^(-Ea/RT)
cathode
Calorimeter
17. Mass #
alcohol
base
First-Order Half Life
# protons + # neutrons
18. E=mc^2
Angular Momentum Quantum Number
Theory of Relativity
chloride
trigonal bipyramidal
19. Expresses how the concentrations depend on time
chromate
Integrated Rate Law
Specific Heat Capacity
geometric isomers
20. Point at which liquid?gas occurs
boiling point
t-shape
ether
high pressure - low temperature
21. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
0
sulfide
bond energy
LE Model
22. AP doesn't deal with ...-order reaction - don't pick it!
sulfide
Monoprotic
third
Hybridization
23. PO4³?
Molecular Compounds
8.31J/Kmol
phosphate
Limiting reactant
24. Average Kinetic Energy Formula
group
Trigonal Bipyramidal
Average KE = 1/2(mass)(average speed of all particles)
rate law
25. Organic w/ -OH group
alcohol
Dipole-dipole forces
Buffered Solution
Decrease Volume and Increase Temperature
26. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
melting point
reduction agent
cyanide
27. Amount of product produced when limiting reactant is used up
s (fourth quantum number)
Antibonding Molecular Orbital
P1V1/N1T1=P2V2/N2T2
Theoretical yield
28. When gas expands ...
equilibrium
London Dispersion Forces
carbohydrates
Negative work value; work done by system
29. Ptotal=Pa+Pb+Pc....
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30. A single substance that may be an acid or a base (i.e. water)
Nernst Equation
activation energy
Amphoteric
insoluble
31. r=k[A]
First-Order Rate Law
P1V1/N1T1=P2V2/N2T2
Zero-Order Half Life
zero
32. These orbitals are spherical
Hydrogen bonding
Arrhenius acid
s orbitals
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
33. Raising heat - adding catalyst - heighten concentration - bigger surface area
high pressure - low temperature
Solution
methods of increasing rate
experimental yield
34. q H2O = ?
msAT
k=Ae^(-Ea/RT)
System
Molecule
35. Ending for alcohols
Speed of light
Bond Order
Octahedral
-ol
36. Half cell in which oxidation occurs
Q>K
First-Order Half Life
anode
+1 - except if bonded to Alkali Metal -1
37. Gas to liquid
Decrease Volume and Increase Temperature
melting point
condensation
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
38. Color of Na (flame test)
Sigma Bond
yellow
octahedral
Colligative properties
39. Ester suffix
Molar Heat Capacity
-oate
solid CO2
Law of Conservation of Energy
40. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
geometric isomers
electron affinity
rate
oxidizing agent
41. Atomic #
Molality
# protons (atom is defined by this)
Hund's Rule
triple point
42. Group 2 metals
Alkaline earth metals
heat of fusion
Manometer
Hund's Rule
43. Energy needed to vaporize a mole of a liquid
Bases
?Tf= kf x molality
n0
?Hvap
44. Cation first - anion second
Naming Binary Ionic Compounds
sulfite
Le Chatelier's Principle
Delta H or Enthalpy Change
45. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
permanganate
Molecular
Thermochemistry
Ionic
46. Coffee Cup Calorimeter
Standard Temperature and Pressure
Constant Pressure
Delta H or Enthalpy Change
Radioactivity
47. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
n (first quantum number)
k=Ae^(-Ea/RT)
Boltzmann distribution
adhesion
48. Entropy in the universe is always...
Formal Charge
Hund's Rule
increasing
spontaneity
49. These orbitals are diagonal
Molality
Endothermic
electron affinity
d orbitals
50. 101 -325 Pa
1atm=?Pa
Pauli Exclusion Principle
CAT
chlorate