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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. kf of water
q
p
1.86°C
Decrease Volume and Increase Temperature
2. Spectrum of light when an electron drops to energy level n=2
Second-Order Rate Law
van't Hoff Factor
Balmer Series
Antibonding Molecular Orbital
3. SO3²?
sulfite
Arrhenius equation
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
3rd law of thermodynamics
4. Kinetic Energy per molecule
oxide
1/2mv²
1.86°C
AE = q + w
5. Variable for type of orbital
-1
voltaic cells
l (second quantum number)
Hess's Law
6. The amount of energy/heat required to raise some substance 1 degree C
third
strong bases
Heat Capacity (C)
pi=(nRT)/v
7. Amine prefix
-1
Calorimeter
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Amino-
8. Moles of solute/volume of soln(L)
msAT
Molarity
Integrated Second-Order Rate Law
hydro-ic acid
9. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
iodide
melting
Metalliods
Boltzmann distribution
10. Diatomic Molecules
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Surroundings
boiling point
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
11. Ptotal=P1+P2+P3+...
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12. Boltzmann constant - used in calculating speed of gas per molecule
Scientific Method
Monoprotic
1.38x10?²³J/K
Nernst Equation
13. SO4²?
hept-
f
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
sulfate
14. Positive ion
X of a = moles a/total moles
Cation
Cathode
Speed of light
15. Planck's constant - used to calculate energy w/frequency
6.63x10?³4Js
Calorimeter
Limiting reactant
LeChatelier's Principle
16. Weakest IMFs - found in all molecules
Cg=kPg
London dispersion forces
violet
8.31J/Kmol
17. Electron pairs found in the space between the atoms
P1= X1P1°
Diffusion
0
Bonding Pairs
18. Substances that form OH- when dissolved in water; proton acceptors
Solution
hydrolysis
Bases
8.31J/Kmol
19. AX2 - AX2E3
Integrated First-Order Rate Law
Pi Bond
linear
Chemical Bonds
20. Mol/kg of solvent - used in calculating colligative properties
8.314 J/K mol
melting point
Molality
entropy (S)
21. Universal IMF for nonpolar molecules
heat capacity
q/moles
endothermic
London dispersion forces
22. Oxidation # of Oxygen
endless
-2 - with peroxide -1
geometric isomers
Positive work value; work done on system
23. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
prop-
Limiting reactant
0.0826Latm/Kmol
24. Mols A/ total mols - XA
Molar Mass of Element/ Total Molar Mass %
heat of vaporization
mol Fraction
Dalton's Law of Partial Pressures
25. How to Find an Empirical Formula Given Percentages
Standard Temperature and Pressure
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
nitrite
sulfite
26. Aldehyde suffix
Its element
?Tf= kf x molality
# protons + # neutrons
-al
27. Ending for alcohols
blue-green
Metalliods
-ol
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
28. Half cell in which oxidation occurs
anode
Integrated Rate Law
phosphate - sulfide - carbonate - sulfate
Van't Hoff factor
29. Point at which liquid?gas occurs
Gamma Ray-
boiling point
Molecule
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
30. % yield
experimental yield
Boltzmann distribution
Surroundings
actual yield/theoretical yield x 100%
31. A device used to measure Delta H
Hydrogen bonding
Calorimeter
octahedral
3/2RT
32. Point where acid completely neutralizes base
Theory of Relativity
endless
equivalence point
Ag+ - Pb2+ - Hg2+
33. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Arrhenius base
complex ions
salt bridge
Second-Order Rate Law
34. Change in Energy (AE) = ? (in terms of work)
cyanide
AE = q + w
pi=(nRT)/v
chlorite
35. How to Find an Empirical Formula Given Grams
l (second quantum number)
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Quantum Mechanical Model
geometric isomers
36. C2O4²?
Molal BP Elevation Constant
oxalate
isothermal
q
37. Everything in the universe that is not defined by you as part of the system
standard solution
are
Pauli Exclusion Principle
Surroundings
38. Half-life equation
moles of solute/ L of solution
0
N=N.(0.5)^time/time half-life
Finding Empirical Formulas
39. A measure of resistance of an object to a change in its state of motion
-2 - with peroxide -1
Acids
Mass
Chemical Kinetics
40. C=2.9979*10^8 m/s
1/2mv²
melting point
Speed of light
entropy
41. If anion ends in -ide - acid name ends in
Hydrogen bonding
hydro-ic acid
Net Ionic Equation
Ionic
42. Reactant which doesn't get used up completely in a chemical reaction
moles of solute/ L of solution
Hydrogen bonding
excess reactant
insoluble
43. Ptotal=Pa+Pb+Pc....
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44. Oxidation # of Ions
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Octahedral
charge
Calorimeter
45. Donates a single H+ Ion (... other prefixes also)
0
mol
Monoprotic
nitrate
46. AX4E
flouride
Solute
see-saw
96500
47. SI unit of energy; Kg*m^2/s^2
Acid Dissociation Constant
Graham's Law
actual yield/theoretical yield x 100%
Joule
48. Where there are no electrons
blue-violet
ionic
Force = mass x acceleration
Nodes
49. NO2¹?
specific heat
nitrite
deposition
Manometer
50. Change in Energy = ? (in terms of constant pressure; for gasses)
geometric isomers
soluble
AE= AH - RTAn
Nodes