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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. Mass percent
are
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
g solute/g solvent x 100
Balmer Series

2. Variable for spin of electron (+.5 or -.5)
s (fourth quantum number)
p orbitals
l (second quantum number)
chlorate

3. In a given atom no two electrons can have the same set of four quantum numbers
Cg=kPg
electrolyte
Pauli Exclusion Principle
3rd law of thermodynamics

4. Organic w/ -O-
Aufbau Principle
ether
strong acids
Theoretical yield

5. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
dec-
Monoprotic
Arrhenius Acid

6. Solid to liquid
melting
London dispersion forces
but-
phosphate - sulfide - carbonate - sulfate

7. 2+ charge
e-
p
high pressure - low temperature
Alpha Particles-

8. H?+NH3?NH4
22.4L
pi=(nRT)/v
Strong acid weak base rxn
Molal BP Elevation Constant

9. Describe various properties of one orbital
Quantum Numbers
-oate
conjugate acid
specific heat

10. R=
hydrocarbons
8.31J/Kmol
Diffusion
% yield

11. SO3²?
Q>K
Net Ionic Equation
sulfite
# protons (atom is defined by this)

12. Point at which the titrated solution changes color
1atm=?Pa
precipitate
d
end point

13. 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)
Equilibrium constant
bromate
wavelength
Kinetic Molecular Theory - for ideal gases

14. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
van't Hoff Factor
exothermic
0

15. AX5
voltaic cells
trigonal bipyramidal
increasing
p+

16. How to Find a Weighted Average
oxidation
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Second-Order Rate Law
endothermic

17. AX6
Amount of atoms present
Enthalpy of Solution
octahedral
% yield

18. Oxidation # of Halogens
-1
Oxidizing Agent
red
Molarity

19. Group 1 and heavier Group 2 bases
rate law
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
strong bases
Integrated Second-Order Rate Law

20. Polyatomic Ions (bonding)
Hybridization
blue-violet
alkene
Covalently w/in themselves - Ionicly bonded w/ each other

21. Work = ?
red
-(P)(Change in V)
perchlorate
chromate

22. Average speed of gas
London dispersion forces
4.184
v3RT/M(in kg)
Heat Capacity (C)

23. C2O4²?
oxalate
base and hydrogen gas
Formal Charge
Molarity

24. Delta H (AH) = ?
critical point
insoluble
Isolated System
q/moles

25. Ether prefix
Molecular
adhesion
prop-
methoxy-

26. IMF that exists in polar molecules
Dipole-dipole forces
ether
deposition
Solute

27. Puts OH? into solution
Theory of Relativity
hex-
Arrhenius base
t-shape

28. =vM2/M1
System
r1/r2
96500
Isolated System

29. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Alpha Particles-
spontaneous
Boltzmann distribution
Second-Order Half Life

30. Electron pairs found in the space between the atoms
Solution
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Bonding Pairs
a precipitate forms

31. [A] vs. time is a ...-order reaction
zero
red
cathode
Volume Metric Flask & Pipet

32. Molarity (M)
Dipole-dipole forces
moles of solute/ L of solution
double bond
Osmotic Pressure

33. Color of K (flame test)
Law of Multiple Proportions
State Functions
purple
Equivalence Point

34. CN¹?
cyanide
oct-
precipitate
strong acid strong base rxn

35. All cations are soluble with sulfate EXCEPT
Endothermic
Force = mass x acceleration
high pressure - low temperature
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

36. Kinetic Energy is proportional to ______
Temperature
Normality
0
eth-

37. CO3²?
dec-
Percent Yield
carbonate
condensation

38. All _________ compounds are electrolytes
pi=(nRT)/v
mol
oxide
Ionic

39. (organics) triple-bonded compound
2nd law of thermodynamics
Pauli Exclusion Principle
alkyne
Q>K

40. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Metalliods
Cg=kPg
% yield
Cation

41. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
Speed of light
l (second quantum number)
Osmotic Pressure

42. r=k
not spontaneous
Bond Order
Zero-Order Rate Law
red

43. Half cell in which oxidation occurs
Sigma Bond
-ol
Electronegativity
anode

44. Volume of gas @STP
Dalton's Law of Partial Pressures
22.4L
are
not spontaneous

45. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

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46. How to Find an Empirical Formula Given Grams
triple bond
log[H+]
N=N.(0.5)^time/time half-life
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

47. kb of water
0.512°C
Buffer
8.31J/Kmol
3.0x108m/s

48. Liquid to gas
vaporization
8.31J/Kmol
melting point
M = square root (3RT/mm)

49. An element with several different forms - each with different properties (i.e. graphite & diamond)
Positive work value; work done on system
Allotrope
Resonance
phosphate

50. Experimental yield/theoretical yieldx100
square pyramidal
% yield
State Functions
0.0821 atm L/mol K