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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. All forms of energy except for heat
work
0
C=(mass)(specific heat)
v3kT/m

2. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
Dalton's Law
methoxy-
lambda

3. [A]0/2k
anode
Zero-Order Half Life
Dalton's Law
Anode

4. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Open System
prop-
Ionic Compounds
tetrahedral

5. Kinetic Energy of an individual particle formula
tetrahedral
(moles of products that are gasses) - (moles of reactants that are gasses)
M = square root (3RT/mm)
Law of Conservation of Mass

6. Oxidation # of Polyatomic Ions
charge
e-
like
paramagnetic

7. Mol of solute/kg of solvent
Molality
equilibrium
Naming Binary Ionic Compounds
violet

8. Larger molecules which have higher mass and therefore electron density have stronger...
London dispersion forces
Temperature
Molarity
Le Chatelier's Principle

9. Unit of electrical potential; J/C
Solute
Volt
p+
Exothermic

10. The entropy of a pure perfectly formed crystal @0K is 0
cathode
3rd law of thermodynamics
are
Decrease Volume and Increase Temperature

11. ln[A] vs. time is a ...-order reaction
prop-
first
Alpha Particles-
End Point

12. Ptotal=P1+P2+P3+...

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13. Oxidation # of Hydrogen
Hund's Rule
Chemical Kinetics
+1 - except if bonded to Alkali Metal -1
Valence Electrons(assigned)

14. 96 -485 C/mol e-
Molecular Orbitals (MOs)
Faraday
spontaneous
q/moles

15. Variable for orientation of orbital (-1 through +1)
soluble
Theoretical yield
M1V1=M2V2
m (third quantum number)

16. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
Electron Spin Quantum Number
% yield
melting

17. ClO3²?
Cg=kPg
chlorate
1/2mv²
Angular Momentum Quantum Number

18. Pure metal or metal hydride + H20 ->
cyanide
base and hydrogen gas
CAT
Volume Metric Flask & Pipet

19. Instrument used to measure the pressure of atmospheric gas
Adding
msAT
Law of Multiple Proportions
Barometer

20. NO3¹?
Amphoteric
allotrope
nitrate
Standard Temperature and Pressure

21. AX2 - AX2E3
linear
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Gamma Ray-
6.63x10?³4Js

22. Volume of gas @STP
1 atm
heat capacity
22.4L
deposition

23. The likelihood that a rxn will occur "by itself"
Graham's Law
heat of vaporization
sublimation
spontaneity

24. (A) - C/s
Delta H or Enthalpy Change
Amino-
Ampere
phosphate - sulfide - carbonate - sulfate

25. How to Balance a Redox Equation
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
Isotopes
Diffusion
London dispersion forces

26. J/°Cg or J/Kg
Weight
work
analyte
Specific Heat Capacity

27. Expresses how the concentrations depend on time
Bond Order
green/yellow
Integrated Rate Law
Pressure of H2O must be Subtracted

28. Molecules' tendency to stick to the container
triple point
bond energy
adhesion
Solution

29. IMF that exists in polar molecules
?Tf= kf x molality
Law of Definite Proportion
Dipole-dipole forces
oxalate

30. AX6
entropy (S)
octahedral
hydrolysis
-oic acid

31. Higher in energy than the atomic orbitals of which it is composed
Equilibrium constant
strong acids
Antibonding Molecular Orbital
Bronsted-Lowry Base

32. Osmotic pressure formula
d orbitals
pi=(nRT)/v
viscosity
red

33. The reactant that is being oxidized - brings about reduction
reduction agent
Enthalpy of Solution
Cell Potential (Ecell)
hex-

34. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
acid
Pressure of H2O must be Subtracted
are not

35. A monoatomic anion is named by taking...
Temperature
Its root and adding -ide
Zero-Order Half Life
Hund's Rule

36. Color of Ca (flame test)
red/orange
Scientific Method
s orbitals
Faraday

37. Mole Fraction
X of a = moles a/total moles
Bronsted-Lowry acid
deposition
LeChatelier's Principle

38. 760mmHg/Torr
London dispersion forces
Monoprotic
1atm=?mmHg/Torr
Hess's Law

39. A molecule having a center of positive charge and a center of negative charge
Force = mass x acceleration
acid
Dipole Moment
Thermochemistry

40. Variable for spin of electron (+.5 or -.5)
nitrite
s (fourth quantum number)
Quantum Numbers
square planar

41. The mixing of native atomic orbitals to form special orbitals for bonding
Angular Momentum Quantum Number
acid
Hybridization
1.38x10?²³J/K

42. Each orbital can hold two e?s each w/ opposite spins
Theoretical yield
Oxidizing Agent
are
Pauli Exclusion Principle

43. Anything occupying space and with mass
Constant Pressure
Matter
-2 - with peroxide -1
boiling point

44. Ending for alcohols
-ol
Barometer
adhesion
Ampere

45. NO2¹?
Radioactivity
nitrite
Bond Order
% error

46. Type of system in which nothing is transfered (no mass or energy); ideal
Le Chatelier's Principle
Isolated System
-al
electron affinity

47. Consists of a complex ion - a transition metal with attached ligands - and counterions
Bronsted-Lowry base
LE Model
Coordination Compound
Law of Conservation of Mass

48. Anions or cations as needed to produce a compound with non net charge
Counterions
Effusion
phosphate - sulfide - carbonate - sulfate
blue-violet

49. Passage of gas through tiny orifice
London Dispersion Forces
alkyne
Second-Order Rate Law
Effusion

50. The reactant that is being reduced - brings about oxidation
oxidizing agent
C + 273
Density
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+