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Test your basic knowledge |
AP Chemistry
Start Test
Study First
Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.
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. Different form of same element
N=N.(0.5)^time/time half-life
Graham's Law
allotrope
Effusion
2. kb of water
Molar Heat Capacity
Dipole-dipole forces
3rd law of thermodynamics
0.512°C
3. Expresses how the concentrations depend on time
Integrated Rate Law
1.86°C
London dispersion forces
oxidation
4. Oxidation # of Oxygen
-2 - with peroxide -1
Pauli Exclusion Principle
1.38x10?²³J/K
sulfite
5. Speed of light - C
3.0x108m/s
Theoretical yield
State Functions
P of a =(X of a)(total pressure)
6. Formula used when diluting stock solution (to find amount of water or stock needed)
Specific Heat Capacity
M1V1=M2V2
Molar Heat Capacity
Second-Order Rate Law
7. H+ Acceptor
Bronsted-Lowry Base
Temperature
PV=nRT
acetate
8. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
State Functions
Net Ionic Equation
# protons (atom is defined by this)
-2 - with peroxide -1
9. Ptotal=P1+P2+P3+...
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10. (A) - C/s
iodide
Metalliods
Ampere
Constant Pressure
11. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
spontaneous
hydrolysis
msAT
Magnetic Quantum Number (ml)
12. Energy can't be created nor destroyed
v3RT/M(in kg)
Law of Conservation of Energy
Hybridization
tetrahedral
13. Change in Energy (AE) = ? (in terms of work)
AE = q + w
Barometer
adhesion
8.31J/Kmol
14. Heat capacity formula
Ionic Compounds
P1= X1P1°
C=(mass)(specific heat)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
15. Point where acid completely neutralizes base
equivalence point
Chemical Bonds
Graham's Law
Mass
16. Mixing of gases
Diffusion
d
0 degrees C - 1 atm
viscosity
17. We cannot simultaneously determine an atom's exact path or location
Heisenberg Uncertainty Principle
P1= X1P1°
red
Coordination Compound
18. The amount of energy/heat required to raise some substance 1 degree C
Heat Capacity (C)
dec-
Law of Definite Proportion
period
19. Loss of electrons - increase in oxidation #
oxidation
ether
Boltzmann distribution
endothermic
20. Ionizes to produce OH- Ions
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Limiting reactant
l (second quantum number)
Arrhenius Base
21. Symbol for Total Heat absorbed or released
0
mol Fraction
q
Allotrope
22. Polyatomic Ions (bonding)
period
nitrite
hydrocarbons
Covalently w/in themselves - Ionicly bonded w/ each other
23. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Isolated System
Scientific Method
yellow --> green
Electron Spin Quantum Number
24. Nonmetal oxide + H2O ->
Constant Volume
acid
Sigma Bond
isothermal
25. (organics) one carbon
Equivalence Point
meth-
Molecular
Sigma Bond
26. Positive ion
s (fourth quantum number)
Cation
oxalate
Ag+ - Pb2+ - Hg2+
27. Point at which liquid?gas occurs
boiling point
triple bond
red/orange
N=N.(0.5)^time/time half-life
28. 1 sigma bond - 2 pi bonds
ammonium
red
triple bond
hept-
29. MnO4¹?
chloride
1 atm
Ligand
permanganate
30. Group 1 and heavier Group 2 bases
strong bases
System
chlorite
Monoprotic
31. n+m (these are orders of reactants)
Magnetic Quantum Number (ml)
condensation
Acids
Overall Reaction Order
32. Energy involved in gaining an electron to become a negative ion
electron affinity
melting point
Magnetic Quantum Number (ml)
are not
33. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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34. If anion ends in -ate - acid name ends in...
Increase Temperature
lambda
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
-ic acid
35. S²?
catalyst
sulfide
C + 273
Acid + Base --> Salt + Water
36. The line running between the atoms
a precipitate forms
-1
Sigma Bond
0 degrees C - 1 atm
37. IMF that occurs with FON
Percent Yield
Hydrogen bonding
red
ammonium
38. The reactant that is being oxidized - brings about reduction
mol Fraction
reduction agent
End Point
Molarity
39. Ending for alcohols
blue
Entropy (S)
l (second quantum number)
-ol
40. Oxidation # of Polyatomic Ions
0 degrees C - 1 atm
but-
charge
Quantum Model
41. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
methoxy-
Dipole-dipole forces
Root Mean Square Velocity
42. Substances that form H+ when dissolved in water; proton donors
yellow --> green
oxalate
Acids
allotrope
43. Mol of solute/kg of solvent
AH
specific heat
Molality
Equilibrium constant
44. Amount of gravitational force exerted on an object
Weight
Hydrogen bonding
entropy (S)
voltaic cells
45. Force that holds atoms together
vaporization
Chemical Bonds
v3kT/m
p orbitals
46. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
C + 273
green/yellow
5% rule
47. Atoms with the same number of protons but a different number of neutrons
oct-
1.38x10?²³J/K
Isotopes
P1= X1P1°
48. Work = ?
Dalton's Law
-(P)(Change in V)
system
Molar Mass of Element/ Total Molar Mass %
49. Boiling point - melting point - viscosity - vapor pressure - surface tension
Percent Yield
carbohydrates
effects of IMF
hydro-ic acid
50. Atomic #
Q>K
Cation
# protons (atom is defined by this)
vapor pressure