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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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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. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
melting point
experimental yield
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
Atmospheric Pressure

2. The heat changed in a chemical reaction.
Thermochemistry
t-shape
red/orange
n0

3. These orbitals are spherical
s orbitals
AE= AH - RTAn
first
rate

4. 90° - d^2sp^3
insoluble
electrolyte
Le Chatelier's Principle
Octahedral

5. Happens at lines in phase change charts
-ol
Law of Conservation of Mass
Constant Volume
equilibrium

6. The chemical formed when a base accepts a proton
equivalence point
conjugate acid
Sigma Bond
heat capacity

7. The mixing of native atomic orbitals to form special orbitals for bonding
Hybridization
Dipole Moment
6.63x10?³4Js
square planar

8. Each orbital can hold two e?s each w/ opposite spins
standard solution
Pauli Exclusion Principle
London dispersion forces
Calorimeter

9. The actual amount of product produced in an experiment
activation energy
Anode
Kinetic Molecular Theory - for ideal gases
experimental yield

10. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
log[H+]
voltaic cells
Electronegativity
purple --> pink

11. When gas compresses ...
d
Bond Order
Reaction Quotient (Q)
Positive work value; work done on system

12. A monoatomic cation takes name from...
Tetrahedral
Pressure
Its element
Cg=kPg

13. [A] vs. time is a ...-order reaction
p
Barometer
zero
Density

14. Ptotal=Pa+Pb+Pc....

15. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Kinetic Molecular Theory - for ideal gases
second
Reaction Quotient (Q)
CAT

16. These orbitals are perpendicular
Monoprotic
like
p orbitals
-ic acid

17. Aldehyde suffix
London Dispersion Forces
precipitate
-al
entropy

18. AX4E
seesaw
voltaic cells
alcohol
8.31J/Kmol

19. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
0 degrees C - 1 atm
Arrhenius Acid
Its root and adding -ide

20. The line running between the atoms
blue
Reaction Quotient (Q)
Decrease Volume and Increase Temperature
Sigma Bond

21. STP
wavelength
heat of fusion
0 degrees C - 1 atm
Boltzmann distribution

22. (organics) five carbons
Equilibrium constant
pent-
electrolyte
adhesion

23. IMF that occurs with FON
carbonate
London dispersion forces
Hydrogen bonding
Chemical Kinetics

24. Substance in which something is dissolved in a solution (higher [ ])
E
alkyne
Solvent
dec-

25. Phase change from solid to gas
complex ions
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
deposition
sublimation

26. A monoatomic anion is named by taking...
Bases
iodide
Its root and adding -ide
(moles of products that are gasses) - (moles of reactants that are gasses)

27. Variable for energy of e- - goes from 1 -2 -3 on up
trigonal planar
n (first quantum number)
end point
0.0821 atm L/mol K

28. 96 -485 C/mol e-
Faraday
Volt
M1V1=M2V2
blue-violet

29. #NAME?
Electronegativity
supercritical fluid
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
E

30. Calculation from K to C
C + 273
% error
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Enthalpy of Solution

31. (A) - C/s
Overall Reaction Order
Covalently w/in themselves - Ionicly bonded w/ each other
Ampere
Increase Temperature

32. ln[A]=-kt + ln[A]0
q/moles
msAT
not spontaneous
Integrated First-Order Rate Law

33. Cl¹?
chloride
square pyramidal
Normality
Hess's Law

34. The reactant that is being oxidized - brings about reduction
Solubility Product (Ksp)
Ionic
blue-green
reduction agent

35. CrO4²?
chloride
Solubility Product (Ksp)
oxidizing agent
chromate

36. Gain of electrons - decrease in oxidation #
reduction
Atomic Mass Unit
Molecular Orbitals (MOs)
Bronsted-Lowry acid

37. l=1
end point
p
-ic acid
Octahedral

38. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
deposition
London Dispersion Forces
Thermochemistry
Reducing Agent

39. Color of Ca (flame test)
Specific Heat (s)
red/orange
entropy
Pressure

40. (organics) four carbons
but-
Arrhenius Acid
q
non-

41. Diatomic Molecules
surroundings
Equilibrium constant
Ionic Compounds
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

42. Energy needed to break a bond
alkene
first
rate gas A/rate gas B = square root (mm A/ mm B)
bond energy

43. Only contains ions that change in reaction
pi=(nRT)/v
Net Ionic Equation
iodide
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

44. kf of water
Molar Mass of Element/ Total Molar Mass %
entropy (S)
oxide
1.86°C

45. .69/k
(moles of products that are gasses) - (moles of reactants that are gasses)
P1= X1P1°
Matter
First-Order Half Life

46. An element with several different forms - each with different properties (i.e. graphite & diamond)
Arrhenius Base
Allotrope
Its root and adding -ide
Hydrogen bonding

47. A given compound always has exactly the same proportion of elements by mass
k=Ae^(-Ea/RT)
+1 - except if bonded to Alkali Metal -1
Law of Definite Proportion
octahedral

48. AP doesn't deal with ...-order reaction - don't pick it!
paramagnetic
bond energy
third
Solution

49. Ability of an atom in a molecule to attract shared electrons to itself
Electronegativity
pent-
Density
Average KE = 1/2(mass)(average speed of all particles)

50. (msubs) Can only be +1/2 or -1/2
Dipole Moment
red/orange
Its root and adding -ide
Electron Spin Quantum Number