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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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1. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Law of Conservation of Mass
Covalently w/in themselves - Ionicly bonded w/ each other
Isotopes
hydrolysis

2. The measurement of heat changes
0 degrees C - 1 atm
8.31J/Kmol
8.314 J/K mol
Calorimetry

3. 1/[A]=kt + 1/[A]0
Buffer
Finding Empirical Formulas
Integrated Second-Order Rate Law
Gamma Ray-

4. AX3E
trigonal pyramidal
carbohydrates
eth-
Quantum Model

5. pH=
log[H+]
Weight
Root Mean Square Velocity
Law of Definite Proportion

6. Equation to find Ea from reaction rate constants at two different temperatures
Arrhenius Base
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
3rd law of thermodynamics
1.38x10?²³J/K

7. Significant Digits of counted things
diamagnetic
weak acid strong base rxn
endless
-(P)(Change in V)

8. Solid to gas
blue
sublimation
Standard Temperature and Pressure
reduction agent

9. 96 -485 C/mol e-
Arrhenius Acid
Molarity
Hybridization
Faraday

10. The minimum energy that molecules must possess for collisions to be effective - Ea
anode
4.184
zero
activation energy

11. Molality =
period
Linear
Heat Capacity (C)
moles solute/kg solvent

12. Force per unit area
pi=(nRT)/v
chloride
Pressure
Formal Charge

13. ln[A] vs. time is a ...-order reaction
first
Calorimeter
Net Ionic Equation
amine

14. Mass percent
Principal Quantum Number
Theoretical yield
Amount of atoms present
g solute/g solvent x 100

15. Specific heat of water
Law of Definite Proportion
analyte
4.184
chloride

16. Force that holds atoms together
high pressure - low temperature
X of a = moles a/total moles
Kinetic Molecular Theory - for ideal gases
Chemical Bonds

17. Increase Volume
Increase Temperature
Molarity
bent
t-shape

18. Gain of electrons - decrease in oxidation #
2nd law of thermodynamics
Beta Particles-
reduction
g solute/g solvent x 100

19. AX5E
square pyramidal
purple
Alpha Particles-
Quantum Numbers

20. AX3E2
Constant Pressure
t-shape
critical point
heat of fusion

21. (msubs) Can only be +1/2 or -1/2
-(q of H2O + q of cal)
Boltzmann distribution
Cg=kPg
Electron Spin Quantum Number

22. ?T=k*m(solute)
msAT
Arrhenius acid
l (second quantum number)
Molal BP Elevation Constant

23. Elements which have all electrons paired and relatively unaffected by magnetic fields
Cell Potential (Ecell)
diamagnetic
activation energy
Boltzmann distribution

24. PO4³?
dec-
phosphate
Linear
cathode

25. Wavelength symbol
Constant Volume
geometric isomers
lambda
End Point

26. q H2O = ?
msAT
Volt
e-
Heat Capacity (C)

27. O²?
Reducing Agent
linear
purple --> pink
oxide

28. Isotope
5% rule
different # of neutrons
Molecular Orbitals (MOs)
pent-

29. 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
Decrease Volume and Increase Temperature
Calorimetry
weak acid strong base rxn

30. IMF that occurs with FON
v3kT/m
Strong acid weak base rxn
Hydrogen bonding
analyte

31. H + donor
Bronsted-Lowry Acid
AE= AH - RTAn
Covalently w/in themselves - Ionicly bonded w/ each other
Zero-Order Half Life

32. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
allotrope
Isotopes
boiling point
Colligative properties

33. 109.5° - sp^3
Tetrahedral
Speed of light
Law of Multiple Proportions
Weight

34. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
non-
0.0826Latm/Kmol
Molecular Compounds
moles solute/kg solvent

35. Liquid to solid
trigonal pyramidal
Integrated Rate Law
freezing
Quantum Model

36. Molecules' tendency to stick to one another
rate gas A/rate gas B = square root (mm A/ mm B)
cohesion
permanent gases
log[H+]

37. Amount of gravitational force exerted on an object
force x distance = work done
Weight
violet
1/2mv²

38. AX6
phosphate
Amino-
octahedral
k=Ae^(-Ea/RT)

39. Melting
rate gas A/rate gas B = square root (mm A/ mm B)
0.0826Latm/Kmol
fusion
charge

40. (organics) nine carbons
0.512°C
non-
oct-
deposition

41. Half-life equation
N=N.(0.5)^time/time half-life
Amount of atoms present
End Point
Force = mass x acceleration

42. Boltzmann constant - used in calculating speed of gas per molecule
Atomic Mass Unit
perchlorate
Trigonal Planar
1.38x10?²³J/K

43. Gas to solid
conjugate base
Joule
triple bond
deposition

44. Energy needed to break a bond
bond energy
Alpha Particles-
excess reactant
Calorimeter

45. 0°C and 1 atm
STP
Molecular Orbitals (MOs)
AE = q + w
-1

46. Like dissolves...
like
Constant Pressure
g solute/g solvent x 100
-ol

47. Substance being dissolved in a solution (lower [ ])
Law of Multiple Proportions
Solute
-2 - with peroxide -1
Integrated Zero-Order Rate Law

48. Color of Na (flame test)
alkyne
viscosity
yellow
activated complex (transition state)

49. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Decrease Volume and Increase Temperature
soluble
Matter
0

50. When n=3 ->2 - color=
Van't Hoff factor
red
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
moles solute/kg solvent