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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. PV=nRT
Ideal Gas Law
first
red
paramagnetic
2. Only contains ions that change in reaction
Net Ionic Equation
p orbitals
Arrhenius equation
heat of vaporization
3. Increase Pressure
alcohol
Percent Yield
Molar Mass of Element/ Total Molar Mass %
Decrease Volume and Increase Temperature
4. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
k=Ae^(-Ea/RT)
sulfate
supercritical fluid
oct-
5. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
voltaic cells
Ligand
trigonal pyramidal
surroundings
6. Non-Ideal Gas Conditions
complex ions
Average KE = 1/2(mass)(average speed of all particles)
high pressure - low temperature
Scientific Method
7. The amount of energy/heat required to raise some substance 1 degree C
alkane
Heat Capacity (C)
Boltzmann distribution
End Point
8. Half cell in which reduction occurs
solid CO2
trigonal bipyramidal
cathode
second
9. If needed - indicate charge of metal(cation) by...
-ol
experimental yield
A Roman numeral
Normality
10. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Q>K
Covalently w/in themselves - Ionicly bonded w/ each other
First-Order Half Life
soluble
11. (organics) two carbons
are not
eth-
melting point
LeChatelier's Principle
12. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Bond Order
Formal Charge
Closed System
period
13. Weakest IMFs - found in all molecules
-1
H
Bond Order
London dispersion forces
14. Involves quantum numbers
zero
Quantum Mechanical Model
C=(mass)(specific heat)
Trigonal Bipyramidal
15. Temperature-pressure point after which gas can no longer form liquid
meth-
oct-
Formal Charge
critical point
16. Oxidation # of Oxygen
-2 - with peroxide -1
heat of fusion
1atm=?mmHg/Torr
condensation
17. R in ideal gas law
Alkaline earth metals
8.31J/Kmol
see-saw
0.0821 atm L/mol K
18. This MUST be determined experimentally
STP
Arrhenius base
rate law
amine
19. Ptotal=P1+P2+P3+...
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183
20. Symbol for Total Heat absorbed or released
q
Law of Multiple Proportions
viscosity
boiling point
21. Mass #
# protons + # neutrons
Balmer Series
Delta H or Enthalpy Change
Van't Hoff factor
22. AX4E2
but-
H
s orbitals
square planar
23. AX5
(moles of products that are gasses) - (moles of reactants that are gasses)
trigonal bipyramidal
melting
deposition
24. Anything occupying space and with mass
strong acids
first
Matter
strong bases
25. Substances that form H+ when dissolved in water; proton donors
Integrated Rate Law
single bond
yellow
Acids
26. Point at which solid?liquid occurs
melting point
Q>K
Molecular
square planar
27. OIL RIG
Oxidation is Loss Reduction is Gain
Integrated Second-Order Rate Law
hydrocarbons
strong bases
28. Mols A/ total mols - XA
mol Fraction
Hydrogen bonding
Lone Pair
Molecule
29. A measure of resistance of an object to a change in its state of motion
non-
no precipitate forms
Mass
catalyst
30. When n=3 ->2 - color=
red
C + 273
Integrated Zero-Order Rate Law
Entropy (S)
31. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Specific Heat Capacity
no precipitate forms
Volume Metric Flask & Pipet
Acid + Base --> Salt + Water
32. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
hydro-ic acid
Ligand
s orbitals
33. Driving force of the electrons
chlorate
lambda
heat capacity
Cell Potential (Ecell)
34. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
bromate
triple point
soluble
35. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Buffer
freezing
ionic
Barometer
36. HF+ OH??H2O
log[H+]
Graham's Law
0 degrees C - 1 atm
weak acid strong base rxn
37. Molecules' tendency to stick to one another
Ionic Compounds
-oic acid
1 atm = 760 mmHg = 101.3 kPa
cohesion
38. If Q<Ksp
acetate
no precipitate forms
Solubility Product (Ksp)
Quantum Mechanical Model
39. Colors of Reaction when (MnO4 -) --> (Mn2+)
Pauli Exclusion Principle
adhesion
Heisenberg Uncertainty Principle
purple --> pink
40. Proton (symbol)
-oate
Integrated Rate Law
Oxidizing Agent
p+
41. Ionizes to produce OH- Ions
not spontaneous
Arrhenius Base
non-
Hydrogen bonding
42. 180° - sp
-al
ammonium
first
Linear
43. Oxoacid solution (such as HSO4-) forms...
Finding Empirical Formulas
Molarity
oxide gas and water
solid CO2
44. Degree of disorder in a system
surroundings
?Tb= kb x molality
entropy (S)
vaporization
45. E=mc^2
endless
96500
Theory of Relativity
condensation
46. How to Find a Weighted Average
Oxidizing Agent
Matter
Hund's Rule
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
47. Stronger IMF= lower... weaker IMF= higher...
Heat
22.4L
-(q of H2O + q of cal)
vapor pressure
48. (A) - C/s
square pyramidal
experimental yield
Ampere
Sigma Bond
49. Half-life equation
double bond
N=N.(0.5)^time/time half-life
Law of Conservation of Mass
mol
50. Color of Ba (flame test)
catalyst
Amount of atoms present
base and hydrogen gas
green/yellow