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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. PO4³?
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
-al
phosphate
trigonal pyramidal

2. AX4E
seesaw
Boltzmann distribution
third
allotrope

3. ClO2¹?
Tetrahedral
system
chlorite
hydro-ic acid

4. Energy required for liquid?gas
heat of vaporization
0.0821 atm L/mol K
Dipole-dipole forces
Integrated Second-Order Rate Law

5. Point at which vapor pressure=air pressure above
Amino-
Ionic
boiling point
electrolyte

6. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
third
Manometer
vaporization
Molality

7. Variable for type of orbital
l (second quantum number)
equilibrium
insoluble
-ol

8. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium

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9. Donates a single H+ Ion (... other prefixes also)
yellow
Calorimeter
second
Monoprotic

10. AX4E2
blue
% yield
endothermic
square planar

11. 101 -325 Pa
Ideal Gas Law
1atm=?Pa
activation energy
base and hydrogen gas

12. AX5E
square pyramidal
carbohydrates
Molarity
phosphate - sulfide - carbonate - sulfate

13. ... compounds are most conductive
Hund's Rule
Kinetic Molecular Theory - for ideal gases
H
ionic

14. All cations are soluble with sulfate EXCEPT
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
London dispersion forces
Molality
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

15. Aldehyde suffix
insoluble
-al
Molecular
96500

16. H?+NH3?NH4
Strong acid weak base rxn
log[H+]
1.38x10?²³J/K
mol

17. Temperature-pressure point after which gas can no longer form liquid
Isotopes
critical point
oxidizing agent
Joule

18. AX5
indicator
Valence Electrons(assigned)
trigonal bipyramidal
Manometer

19. Ionizes to produce OH- Ions
Arrhenius Base
Nodes
log[H+]
Bond Order

20. STP
0 degrees C - 1 atm
System
Hydrogen bonding
s orbitals

21. IMF that occurs with FON
Trigonal Bipyramidal
Entropy (S)
Hydrogen bonding
mol Fraction

22. Dalton's Law of Partial Pressures (to find partial pressure formula)
P of a =(X of a)(total pressure)
amine
8.314 J/K mol
end point

23. 0°C and 1 atm
First-Order Rate Law
Naming Binary Ionic Compounds
Zero-Order Half Life
STP

24. This MUST be determined experimentally
period
Alpha Particles-
rate law
purple

25. Tools NEEDED for dilution
Force = mass x acceleration
msAT
Volume Metric Flask & Pipet
AE= AH - RTAn

26. S²?
sulfide
Volt
trigonal bipyramidal
chlorite

27. Ending for alcohols
v3RT/M(in kg)
-ol
Nodes
Weight

28. (organics) ten carbons
are not
Average KE = 1/2(mass)(average speed of all particles)
dec-
hex-

29. Loss of electrons - increase in oxidation #
1.38x10?²³J/K
base
Scientific Method
oxidation

30. The amount of energy/heat required to raise some substance 1 degree C
Heat Capacity (C)
Molecular
chloride
C=(mass)(specific heat)

31. The reactant that is being oxidized - brings about reduction
Arrhenius base
equilibrium
reduction agent
-oate

32. Energy required to break a bond
hydro-ic acid
Zero-Order Rate Law
Bond Energy
Isolated System

33. [A] vs. time is a ...-order reaction
g solute/g solvent x 100
Manometer
zero
log[H+]

34. Unusually strong dipole forces found when H is bonded to N - O - or F
like
Bond Energy
Hydrogen bonding
Acid + Base --> Salt + Water

35. A single substance that may be an acid or a base (i.e. water)
log[H+]
Reaction Quotient (Q)
Positive work value; work done on system
Amphoteric

36. Significant Digits of Conversion Factors
activated complex (transition state)
work
Speed of light
endless

37. AX4E
cathode
see-saw
Its element
Allotrope

38. Oxidation # of Ions
Solution
charge
end point
anode

39. These orbitals are diagonal
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Pressure
d orbitals
Constant Pressure

40. A given compound always has exactly the same proportion of elements by mass
Boltzmann distribution
Law of Definite Proportion
Pauli Exclusion Principle
Strong acid weak base rxn

41. Moles of solute/volume of soln(L)
rate
Molarity
s
sulfide

42. Reverse rxn occurs when
are
Q>K
Quantum Numbers
q/moles

43. 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)
Arrhenius Base
Negative work value; work done by system
Kinetic Molecular Theory - for ideal gases
chromate

44. Measure of the change in enthalpy
C + 273
Delta H or Enthalpy Change
p orbitals
permanent gases

45. Electron (symbol)
boiling point
1st law of thermodynamics
e-
Heat

46. NO2¹?
Radioactivity
Polar Covalent
adiabatic
nitrite

47. Mass percent
purple
g solute/g solvent x 100
trigonal bipyramidal
specific heat

48. Idea Gas Law (actual rules)
PV=nRT
Metalliods
AH
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

49. Chemical composition of dry ice
Strong acid weak base rxn
Ionic Compounds
Acid Dissociation Constant
solid CO2

50. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
bromate
oxidizing agent
carbohydrates