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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. q rxn = ?
third
Resonance
-(q of H2O + q of cal)
-2 - with peroxide -1

2. Degree of disorder in a system
reduction
bromate
heat capacity
entropy (S)

3. The rest of the universe (in thermodynamics)
Barometer
surroundings
n0
but-

4. Mol/L - concentration of a solution
entropy (S)
solid CO2
dichromate
Molarity

5. Force that holds atoms together
Specific Heat Capacity
Chemical Bonds
boiling point
oxide gas and water

6. To find activation energy use the...
conjugate base
Arrhenius equation
log[H+]
Bronsted-Lowry acid

7. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
first
Cg=kPg
Boltzmann distribution
Root Mean Square Velocity

8. frequency symbol
carbonate
nu
conjugate acid
Reaction Quotient (Q)

9. Phase change from gas to solid
deposition
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Equilibrium Expression
p+

10. Gas to liquid
condensation
Law of Multiple Proportions
-(q of H2O + q of cal)
Monoprotic

11. CO3²?
Molecular
carbonate
1/2mv²
voltaic cells

12. ?T=k*m(solute)
London dispersion forces
Molal BP Elevation Constant
see-saw
?Tb= kb x molality

13. Faraday's constant
Hund's Rule
System
96500
Allotrope

14. Mol of solute/kg of solvent
-ous acid
Multiplying
Molality
London Dispersion Forces

15. Variable for energy of e- - goes from 1 -2 -3 on up
First-Order Half Life
Hydrogen bonding
n (first quantum number)
Heat

16. l=2
Aufbau Principle
-(P)(Change in V)
red/orange
d

17. Color of Li (flame test)
C + 273
red
m (third quantum number)
Root Mean Square Velocity

18. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
Magnetic Quantum Number (ml)
charge
ether

19. We cannot simultaneously determine an atom's exact path or location
Quantum Numbers
Heisenberg Uncertainty Principle
Principal Quantum Number
Atomic Mass Unit

20. 1/([A]0*k)
Heat Capacity (C)
Weight
Second-Order Half Life
carbohydrates

21. Oxidation # of Halogens
Dalton's Law of Partial Pressures
Magnetic Quantum Number (ml)
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
-1

22. Like dissolves...
CAT
square planar
First-Order Rate Law
like

23. A measure of randomness or disorder
weak acid strong base rxn
PV=nRT
entropy
reduction agent

24. Thickness
Molecule
viscosity
van't Hoff Factor
hydrocarbons

25. Energy can't be created nor destroyed
London dispersion forces
Anode
Law of Conservation of Energy
Molality

26. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
catalyst
3/2RT
alkane
Cg=kPg

27. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Temperature
Chemical Kinetics
Molecular
Heisenberg Uncertainty Principle

28. Gain of electrons - decrease in oxidation #
Bond enthalpy
purple
Buffered Solution
reduction

29. These orbitals are spherical
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
s orbitals
Solution
Molarity

30. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
not spontaneous
equilibrium
mol

31. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
alcohol
Quantum Model
are not

32. (organics) single-bonded compound
alkane
purple --> pink
insoluble
Arrhenius acid

33. The chemical formed when an acid donates a proton
conjugate base
see-saw
Temperature
boiling point

34. Mass percent
Linear
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
g solute/g solvent x 100
Amphoteric

35. Moles of solute/volume of soln(L)
Q<K
prop-
4.184
Molarity

36. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
oxide
AE = q + w
s orbitals

37. O²?
oxide
Mass
paramagnetic
yellow

38. The weighted average of all the isotopes that an atom can have (in g/mol)
phosphate
Atomic Mass Unit
isothermal
are not

39. 1 sigma bond - 1 pi bond
22.4L
n (first quantum number)
double bond
equivalence point

40. negative ion
Oxidizing Agent
critical point
Anion
Chemical Bonds

41. Resistance to flow
adiabatic
Linear
viscosity
Gamma Ray-

42. Ptotal=P1+P2+P3+...

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43. Freezing point depression formula
specific heat
?Tf= kf x molality
Osmotic Pressure
Molal BP Elevation Constant

44. Involves quantum numbers
Heat
Quantum Mechanical Model
base
ether

45. Calculation from K to C
C + 273
Open System
Bronsted-Lowry base
Pauli Exclusion Principle

46. Molality =
LeChatelier's Principle
are
Endothermic
moles solute/kg solvent

47. l=1
-ous acid
sublimation
Dipole-dipole forces
p

48. Carboxylic acid ending
Adding
charge
-oic acid
Arrhenius acid

49. Two molecules with identical connectivity but different geometries
different # of neutrons
square pyramidal
Temperature
geometric isomers

50. Newton's Second Law
Force = mass x acceleration
Buffered Solution
d orbitals
boiling point