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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. Bomb Calorimeter
red/orange
Pauli Exclusion Principle
Constant Volume
Ligand

2. AX4E
Cation
see-saw
-(q of H2O + q of cal)
Theoretical yield

3. Puts OH? into solution
are
v3kT/m
Arrhenius base
vaporization

4. Amount of gravitational force exerted on an object
PV=nRT
precipitate
1 atm
Weight

5. The line running between the atoms
weak acid strong base rxn
Sigma Bond
conjugate base
Entropy (S)

6. Unit of electrical potential; J/C
Work
Integrated Rate Law
Volt
Average KE = 1/2(mass)(average speed of all particles)

7. F¹?
PV=nRT
flouride
r1/r2
mol

8. Energy required for melting to occur
heat of fusion
X of a = moles a/total moles
-(P)(Change in V)
Bronsted-Lowry Base

9. Electron (symbol)
M1V1=M2V2
e-
N=N.(0.5)^time/time half-life
Solute

10. Actual Yield/Theoretical Yield*100%
Weight
Percent Yield
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
yellow --> green

11. CrO4²?
non-
chromate
Theory of Relativity
-1

12. Heat needed to change 1 g of substance to 1°C
different # of neutrons
s orbitals
heat of fusion
specific heat

13. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
(moles of products that are gasses) - (moles of reactants that are gasses)
moles solute/kg solvent
pent-

14. Cr2O7²?
1atm=?Pa
22.4L
dichromate
electrolyte

15. When _____ significant digits - round answer to least significant digit
Quantum Model
hex-
Multiplying
Anode

16. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
s
methoxy-
complex ions
First-Order Half Life

17. Substances w/ critical temperatures below 25°C
s (fourth quantum number)
permanent gases
entropy
Volt

18. Specific heat of water
Arrhenius equation
Aufbau Principle
4.184
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

19. We cannot simultaneously determine an atom's exact path or location
T-shape
Heisenberg Uncertainty Principle
endless
a precipitate forms

20. Carboxylic acid ending
chlorite
-oic acid
Increase Temperature
Q>K

21. H?+OH??H2O
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
tetrahedral
Boltzmann distribution
strong acid strong base rxn

22. Ketone suffix
oxalate
-one
boiling point
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

23. 2+ charge
Alpha Particles-
oxide
Limiting reactant
X of a = moles a/total moles

24. Proton donors
permanganate
Bronsted-Lowry acid
H
third

25. The entropy of a pure perfectly formed crystal @0K is 0
0.512°C
acid
ammonium
3rd law of thermodynamics

26. Like dissolves...
red
0
d orbitals
like

27. How to Find a Weighted Average
conjugate base
3rd law of thermodynamics
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
m (third quantum number)

28. Energy involved in gaining an electron to become a negative ion
electron affinity
moles solute/kg solvent
carbonate
mol

29. 90° - d^2sp^3
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Octahedral
Thermochemistry
system

30. Liquid to gas
geometric isomers
vaporization
Amino-
Sigma Bond

31. High-speed electrons
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
Beta Particles-
Hund's Rule
Valence Electrons(assigned)

32. Work = ?
Solvent
Calorimeter
-(P)(Change in V)
are

33. Force per unit area
Pressure
meth-
1st law of thermodynamics
Electron Spin Quantum Number

34. (organics) six carbons
hex-
M1V1=M2V2
iodide
specific heat

35. C2O4²?
Amphoteric
oxalate
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
strong bases

36. Happens at lines in phase change charts
Adding
Law of Multiple Proportions
8.31J/Kmol
equilibrium

37. 0.00°C - 1 atm
vaporization
purple
0.0826Latm/Kmol
Standard Temperature and Pressure

38. Expresses how the concentrations depend on time
heat of fusion
-oate
Principal Quantum Number
Integrated Rate Law

39. [A] vs. time is a ...-order reaction
Amino-
zero
LE Model
Molecular Orbitals (MOs)

40. A solution used in titrations whose concentration is known
Aufbau Principle
bent
standard solution
6.63x10?³4Js

41. R=
0.512°C
endothermic
anode
0.0826Latm/Kmol

42. To find activation energy use the...
Normality
Arrhenius equation
Hydrogen bonding
Reducing Agent

43. Hydroxides are soluble or insoluble?
condensation
insoluble
n (first quantum number)
Q<K

44. Speed of light - C
Isotopes
3.0x108m/s
Law of Conservation of Mass
Alkali metals

45. Elements which have unpaired electrons and highly affected by magnetic fields
q/moles
paramagnetic
Cg=kPg
square pyramidal

46. (organics) one carbon
Molality
ether
meth-
no precipitate forms

47. 180° - sp
Linear
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
LeChatelier's Principle
Alkaline earth metals

48. # bonding e- - # antibonding e-/2
Bond Order
yellow
Molar Heat Capacity
Isotopes

49. Energy (definition)
Coordination Compound
Magnetic Quantum Number (ml)
force x distance = work done
cyanide

50. ... compounds are most conductive
moles of solute/ L of solution
period
complex ions
ionic