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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. Mol/kg of solvent - used in calculating colligative properties
Lone Pair
?Tb= kb x molality
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Molality

2. (organics) triple-bonded compound
Naming Binary Ionic Compounds
alkyne
base
boiling point

3. A homogeneous mixture with 1 phase
period
Solution
condensation
sulfate

4. 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)
Molality
1.38x10?²³J/K
Kinetic Molecular Theory - for ideal gases
0

5. R=
Bronsted-Lowry acid
Barometer
LE Model
8.31J/Kmol

6. q rxn = ?
-(q of H2O + q of cal)
g solute/g solvent x 100
London Dispersion Forces
C=(mass)(specific heat)

7. Ionizes to produce OH- Ions
Percent Yield
Arrhenius Base
Theory of Relativity
Standard Temperature and Pressure

8. Mass/volume
Solvent
Ionic
Density
bent

9. High-energy light
Normality
hept-
Gamma Ray-
eth-

10. Variable for orientation of orbital (-1 through +1)
triple bond
Integrated Zero-Order Rate Law
m (third quantum number)
iodide

11. A method of investigation involving observation and theory to test scientific hypotheses
Scientific Method
Acid Dissociation Constant
base
entropy

12. Electrons in a hydrogen atom move around the nucleus only in circular orbits
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
isothermal
Monoprotic
Quantum Model

13. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Q>K
Strong acid weak base rxn
melting
Chemical Kinetics

14. PV=nRT
chlorate
Ideal Gas Law
Hydrogen bonding
3rd law of thermodynamics

15. (organics) one carbon
acetate
meth-
Net Ionic Equation
Constant Volume

16. Point at which vapor pressure=air pressure above
deposition
boiling point
methods of increasing rate
freezing

17. K
Equilibrium constant
Arrhenius equation
Magnetic Quantum Number (ml)
Temperature

18. The amount of energy/heat required to raise some substance 1 degree C
# protons + # neutrons
Beta Particles-
s
Heat Capacity (C)

19. Molecules' tendency to stick to one another
bromate
phosphate - sulfide - carbonate - sulfate
cohesion
Ampere

20. Mass percent
Normality
Molal FP Depression Constant
g solute/g solvent x 100
double bond

21. Proton donors
precipitate
purple
Bronsted-Lowry acid
square planar

22. kb of water
viscosity
Its root and adding -ide
0.512°C
but-

23. Significant Digits of Conversion Factors
6.63x10?³4Js
endless
trigonal pyramidal
high pressure - low temperature

24. Substance that - when dissolved - is conductive
electrolyte
0.0821 atm L/mol K
LE Model
precipitate

25. 1 sigma bond
Theoretical yield
Ionic
Law of Conservation of Mass
single bond

26. Kinetic Energy of an individual particle formula
Q<K
Trigonal Bipyramidal
purple --> pink
M = square root (3RT/mm)

27. 109.5° - sp^3
base
Tetrahedral
0
prop-

28. If anion ends in -ite - acid name ends in...
P of a =(X of a)(total pressure)
-ous acid
0
isothermal

29. neutron (symbol)
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
n0
end point
Net Ionic Equation

30. ClO4¹?
perchlorate
violet
yellow --> green
Hybridization

31. Significant Digits of counted things
endless
Cation
trigonal bipyramidal
octahedral

32. CN¹?
oxidation
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
cyanide
Molal FP Depression Constant

33. Proton (symbol)
chlorate
Bonding Pairs
p+
Boltzmann distribution

34. When n=4 ->2 - color=
oct-
work
blue-green
Effusion

35. Symbol for the heat absorbed or lost molecularly (PER MOLE)
8.314 J/K mol
P1= X1P1°
Equivalence Point
AH

36. IMF that exists in polar molecules
end point
Bond enthalpy
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Dipole-dipole forces

37. Positive enthalpy - heat flows into system
0.512°C
e-
endothermic
Osmotic Pressure

38. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
1 atm
soluble
Alkali metals
3/2RT

39. For significant digits - trailing zeros _____ significant
melting
are
Isotopes
0 degrees C - 1 atm

40. AX3E
Temperature
Alpha Particles-
condensation
trigonal pyramidal

41. Symbol for Total Heat absorbed or released
q
voltaic cells
bent
p+

42. A device used to measure Delta H
endothermic
Coordination Compound
Calorimeter
Ampere

43. AP doesn't deal with ...-order reaction - don't pick it!
-1
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
third
square planar

44. Isotope
Ionic
Volume Metric Flask & Pipet
different # of neutrons
m (third quantum number)

45. (organics) four carbons
1st law of thermodynamics
but-
Anion
Ag+ - Pb2+ - Hg2+

46. Change in Energy (AE) = ? (in terms of work)
work
chlorate
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
AE = q + w

47. Loss of electrons - increase in oxidation #
oxidation
precipitate
d orbitals
Alkali metals

48. Work = ?
spontaneous
oxide gas and water
-(P)(Change in V)
charge

49. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
bromate
condensation
hydrolysis
Theory of Relativity

50. (organics) double-bonded compound
0
heat capacity
alkene
Aufbau Principle