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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. Boiling point - melting point - viscosity - vapor pressure - surface tension
activation energy
chlorite
van't Hoff Factor
effects of IMF
2. (organics) one carbon
Chemical Kinetics
viscosity
blue-green
meth-
3. R in instances that pertain to energy
Transition metals
8.314 J/K mol
cathode
viscosity
4. Connects the 2 half cells in a voltaic cell
Arrhenius acid
salt bridge
chlorate
s orbitals
5. Universal IMF for nonpolar molecules
Molarity
Pressure
London dispersion forces
Integrated Zero-Order Rate Law
6. The heat changed in a chemical reaction.
Lone Pair
Thermochemistry
Bases
insoluble
7. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
q
Bond enthalpy
Molecular
effects of IMF
8. Oxidation # of Halogens
-1
Bond enthalpy
1 atm = 760 mmHg = 101.3 kPa
London Dispersion Forces
9. Ideal Gas Law Formula
PV=nRT
Equilibrium constant
5% rule
Net Ionic Equation
10. If anion ends in -ide - acid name ends in
Volume Metric Flask & Pipet
deposition
hydro-ic acid
Arrhenius equation
11. Kinetic Energy per molecule
are not
1/2mv²
Delta H or Enthalpy Change
methods of increasing rate
12. (N) number of equivalents per liter of solution
chloride
Molarity
salt bridge
Normality
13. OH¹?
yellow
hydroxide
titrant buret
Amino-
14. Puts H? into solution
yellow
Arrhenius acid
cathode
geometric isomers
15. Increase Volume
Increase Temperature
Bronsted-Lowry acid
Cell Potential (Ecell)
square pyramidal
16. C=2.9979*10^8 m/s
alcohol
Molecule
Ionic
Speed of light
17. The rest of the universe (in thermodynamics)
Dalton's Law of Partial Pressures
Hydrogen bonding
London Dispersion Forces
surroundings
18. AX6
lambda
exothermic
chloride
octahedral
19. Experimental yield/theoretical yieldx100
Equilibrium constant
-(q of H2O + q of cal)
Law of Conservation of Mass
% yield
20. Instrument used to measure the pressure of atmospheric gas
Barometer
standard solution
Le Chatelier's Principle
entropy (S)
21. AX6
octahedral
surroundings
-ous acid
Limiting reactant
22. The driving force for a spontaneous is an increase in entropy of the universe
Entropy (S)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Sigma Bond
square planar
23. We cannot simultaneously determine an atom's exact path or location
Isotopes
Heisenberg Uncertainty Principle
Solubility Product (Ksp)
-al
24. 2+ charge
Specific Heat (s)
Alpha Particles-
Naming Binary Ionic Compounds
Second-Order Rate Law
25. Arrhenius equation
k=Ae^(-Ea/RT)
Limiting reactant
exothermic
Decrease Volume and Increase Temperature
26. Newton's Second Law
Force = mass x acceleration
specific heat
Multiplying
Positive work value; work done on system
27. Mol of solute/kg of solvent
ammonium
Second-Order Rate Law
Molality
Osmotic Pressure
28. Forward rxn occurs when
Q<K
22.4L
conjugate base
Le Chatelier's Principle
29. In a given atom no two electrons can have the same set of four quantum numbers
Pauli Exclusion Principle
0
f
alkyne
30. Metal oxide + H20 ->
base
purple
Balmer Series
Adding
31. Organic reaction in which two functional groups come together - resulting in the release of water
condensation
Second-Order Rate Law
Positive work value; work done on system
strong acid strong base rxn
32. AP doesn't deal with ...-order reaction - don't pick it!
AE= AH - RTAn
permanent gases
third
fusion
33. Elements on staircase on periodic table
v3RT/M(in kg)
Metalliods
Hund's Rule
8.314 J/K mol
34. Point at which the titrated solution changes color
P of a =(X of a)(total pressure)
end point
hex-
Le Chatelier's Principle
35. # bonding e- - # antibonding e-/2
96500
oxide
Bond Order
?Tf= kf x molality
36. NO3¹?
amine
endless
nitrate
E
37. Boltzmann constant - used in calculating speed of gas per molecule
tetrahedral
wavelength
alcohol
1.38x10?²³J/K
38. Consists of a complex ion - a transition metal with attached ligands - and counterions
3.0x108m/s
1atm=?Pa
Coordination Compound
0.0821 atm L/mol K
39. The mixing of native atomic orbitals to form special orbitals for bonding
Hybridization
perchlorate
condensation
Volume Metric Flask & Pipet
40. Equation to find Ea from reaction rate constants at two different temperatures
Zero-Order Half Life
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
triple bond
are not
41. Color of Sr (flame test)
red
Acids
bromate
Aufbau Principle
42. U(rms)=(3RT/M)^1/2
Law of Conservation of Mass
purple --> pink
Theory of Relativity
Root Mean Square Velocity
43. Spontaneous emission of radiation
chlorate
pi=(nRT)/v
are not
Radioactivity
44. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
Molecular
?Hvap
sulfite
45. Higher in energy than the atomic orbitals of which it is composed
are
moles of solute/ L of solution
Heat Capacity (C)
Antibonding Molecular Orbital
46. (organics) single-bonded compound
Solubility Product (Ksp)
alkane
C=(mass)(specific heat)
0
47. J/°Cmol or J/Kmol
Beta Particles-
Law of Multiple Proportions
Q<K
Molar Heat Capacity
48. Dalton's Law of Partial Pressures (to find partial pressure formula)
linear
P of a =(X of a)(total pressure)
second
critical point
49. Ester suffix
Ampere
triple point
cathode
-oate
50. Ending for alcohols
Equilibrium Expression
group
-ol
8.314 J/K mol