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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. Raoult's Law - relations between vapor pressure and concentrations
Equilibrium Expression
P1= X1P1°
Thermochemistry
adiabatic
2. PO4³?
see-saw
Cathode
moles of solute/ L of solution
phosphate
3. Increase Pressure
Covalently w/in themselves - Ionicly bonded w/ each other
Decrease Volume and Increase Temperature
violet
strong bases
4. Planck's constant - used to calculate energy w/frequency
Mass
Arrhenius Base
6.63x10?³4Js
Isolated System
5. Ending for alcohols
n (first quantum number)
Molal BP Elevation Constant
Boltzmann distribution
-ol
6. ClO2¹?
chlorite
trigonal bipyramidal
Chemical Kinetics
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
7. Polyatomic Ions (bonding)
octahedral
Buffered Solution
Covalently w/in themselves - Ionicly bonded w/ each other
effects of IMF
8. Within a sublevel - place one e? per orbital before pairing them
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9. ?T=k*m(solute)
hydro-ic acid
chlorate
Molal BP Elevation Constant
1atm=?mmHg/Torr
10. Color of Ba (flame test)
London dispersion forces
+1 - except if bonded to Alkali Metal -1
green/yellow
Buffer
11. Energy required for liquid?gas
mol Fraction
London dispersion forces
heat of vaporization
Specific Heat Capacity
12. Volume of gas @STP
Dalton's Law
22.4L
Arrhenius acid
-oate
13. Amine prefix
purple
Polar Covalent
Alpha Particles-
Amino-
14. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
Polar Covalent
different # of neutrons
prop-
15. Anions or cations as needed to produce a compound with non net charge
Nodes
Counterions
Volume Metric Flask & Pipet
condensation
16. Atomic #
n (first quantum number)
seesaw
# protons (atom is defined by this)
Balmer Series
17. A weak acid that changes color at or near the equivalence point
Law of Conservation of Mass
indicator
Allotrope
Solubility Product (Ksp)
18. Similar to atomic orbitals - except between molecules
oxide gas and water
1.38x10?²³J/K
CAT
Molecular Orbitals (MOs)
19. When n=6 ->2 - color=
Galvanic Cell
Force = mass x acceleration
violet
work
20. Symbol for Total Heat absorbed or released
q
hex-
oxidizing agent
Chemical Bonds
21. 1/[A]=kt + 1/[A]0
spontaneity
Integrated Second-Order Rate Law
trigonal bipyramidal
End Point
22. 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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23. Freezing point depression formula
-(q of H2O + q of cal)
?Tf= kf x molality
paramagnetic
entropy (S)
24. We cannot simultaneously determine an atom's exact path or location
Law of Multiple Proportions
electron affinity
Heisenberg Uncertainty Principle
Open System
25. SO4²?
ammonium
square pyramidal
sulfate
Bond enthalpy
26. R in ideal gas law
Law of Definite Proportion
Hund's Rule
0.0821 atm L/mol K
q/moles
27. CO3²?
carbonate
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Chemical Bonds
oxide gas and water
28. Carbon - hydrogen - oxygen compounds
Oxidizing Agent
P of a =(X of a)(total pressure)
carbohydrates
Aufbau Principle
29. 760mmHg/Torr
1/2mv²
Reducing Agent
Equilibrium constant
1atm=?mmHg/Torr
30. The part of the universe one is focused upon (in thermodynamics)
system
Principal Quantum Number
octahedral
Volume Metric Flask & Pipet
31. Oxidation # of Compounds
P1= X1P1°
oxidation
Work
0
32. 1/[A] vs. time is a ...-order reaction
Root Mean Square Velocity
second
Overall Reaction Order
voltaic cells
33. The chemical formed when an acid donates a proton
v3kT/m
cohesion
perchlorate
conjugate base
34. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
P1V1/N1T1=P2V2/N2T2
analyte
Amino-
35. Heat capacity formula
lambda
analyte
C=(mass)(specific heat)
Arrhenius equation
36. Oxidation # of Ions
sublimation
charge
Q<K
Chemical Bonds
37. 1 sigma bond - 2 pi bonds
soluble
?Tf= kf x molality
triple bond
Speed of light
38. Proton (symbol)
Heat Capacity (C)
Delta H or Enthalpy Change
Hund's Rule
p+
39. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Allotrope
First-Order Half Life
alkene
insoluble
40. 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
octahedral
Pauli Exclusion Principle
Law of Multiple Proportions
complex ions
41. Substances w/ critical temperatures below 25°C
group
Solute
Buffered Solution
permanent gases
42. (# of lone pair e-)+1/2(# of shared e-)
acetate
Hydrogen bonding
bond energy
Valence Electrons(assigned)
43. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
fusion
strong acids
Nernst Equation
-one
44. AX3
trigonal planar
condensation
Graham's Law
Q>K
45. AX2E - AX2E2
bent
CAT
hydrocarbons
Polar Covalent
46. Horizontals on the periodic table
Effusion
period
bond energy
LeChatelier's Principle
47. Liquid to gas
p+
-ic acid
Ag+ - Pb2+ - Hg2+
vaporization
48. 0.00°C - 1 atm
Standard Temperature and Pressure
boiling point
1.86°C
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
49. Work = ?
deposition
+1 - except if bonded to Alkali Metal -1
Quantum Mechanical Model
-(P)(Change in V)
50. Wavelength symbol
-oate
lambda
van't Hoff Factor
96500