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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. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Law of Multiple Proportions
base and hydrogen gas
Equilibrium Expression
nitrite
2. Rate of Diffusion/Effusion formula
experimental yield
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
viscosity
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
3. Point at which vapor pressure=air pressure above
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
boiling point
Molecular Compounds
Law of Conservation of Mass
4. Energy required to break a bond
Law of Conservation of Mass
Closed System
Bond Energy
methoxy-
5. Temperature-pressure point after which gas can no longer form liquid
Pi Bond
critical point
square pyramidal
n (first quantum number)
6. Metal oxide + H20 ->
base
chromate
Law of Multiple Proportions
bromate
7. 1 sigma bond - 2 pi bonds
Pi Bond
triple bond
Coordination Compound
van't Hoff Factor
8. AX3E2
Law of Multiple Proportions
Ionic
charge
T-shape
9. Dirrect Method Formula
Root Mean Square Velocity
sulfate
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
octahedral
10. (organics) two carbons
eth-
Anode
triple point
carbonate
11. Change without heat transfer between the system and its surroundings
chromate
adiabatic
square pyramidal
blue-green
12. R=
Molecule
Ideal Gas Law
8.31J/Kmol
critical point
13. Point at which the titrated solution changes color
Scientific Method
condensation
end point
96500
14. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
yellow --> green
seesaw
Naming Binary Ionic Compounds
(moles of products that are gasses) - (moles of reactants that are gasses)
15. Force acting over distance
trigonal planar
Work
analyte
second
16. OH¹?
entropy
Standard Temperature and Pressure
hydroxide
hydrocarbons
17. Atoms with the same number of protons but a different number of neutrons
deposition
Isotopes
Coordination Compound
q
18. Gas to solid
-(q of H2O + q of cal)
8.31J/Kmol
deposition
Osmotic Pressure
19. Expresses how the concentrations depend on time
Integrated Rate Law
hydrolysis
oxidation
Pressure of H2O must be Subtracted
20. S²?
Hybridization
electron affinity
increasing
sulfide
21. STP
0.0821 atm L/mol K
London dispersion forces
Principal Quantum Number
0 degrees C - 1 atm
22. 90°&120° - dsp^3
Isolated System
Trigonal Bipyramidal
Endothermic
fusion
23. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Finding Empirical Formulas
Nodes
freezing
deposition
24. Driving force of the electrons
Cathode
Bronsted-Lowry Acid
dec-
Cell Potential (Ecell)
25. q cal = ?
CAT
purple
Arrhenius base
Open System
26. 90° - d^2sp^3
X of a = moles a/total moles
Octahedral
oxide
Antibonding Molecular Orbital
27. 109.5° - sp^3
surroundings
Equilibrium Expression
Tetrahedral
high pressure - low temperature
28. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Enthalpy of Solution
Aufbau Principle
third
London Dispersion Forces
29. Mole Fraction
London dispersion forces
X of a = moles a/total moles
Bond Energy
t-shape
30. A measure of randomness or disorder
AE= AH - RTAn
sulfite
entropy
second
31. For significant digits - trailing zeros _____ significant
nitrite
are
bent
condensation
32. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
alkane
Chemical Bonds
meth-
33. .69/k
First-Order Half Life
specific heat
-al
melting point
34. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
single bond
T-shape
soluble
Specific Heat (s)
35. These orbitals are spherical
s orbitals
0.512°C
Adding
permanent gases
36. Unit of electrical potential; J/C
adiabatic
Volt
deposition
Heat Capacity (C)
37. 101 -325 Pa
Gamma Ray-
1atm=?Pa
Coordination Compound
Van't Hoff factor
38. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
moles of solute/ L of solution
strong bases
Decrease Volume and Increase Temperature
spontaneous
39. (organics) four carbons
Molecular
strong acid strong base rxn
bent
but-
40. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
1atm=?Pa
Equivalence Point
heat of vaporization
Angular Momentum Quantum Number
41. (organics) one carbon
hept-
Magnetic Quantum Number (ml)
meth-
Arrhenius base
42. Reactant that's completely used up in a chemical reaction
alcohol
n (first quantum number)
Limiting reactant
Manometer
43. ln[A]=-kt + ln[A]0
Ligand
see-saw
Limiting reactant
Integrated First-Order Rate Law
44. Boiling point elevation formula
Cathode
1/2mv²
?Tb= kb x molality
Nernst Equation
45. A monoatomic cation takes name from...
Its element
soluble
Cell Potential (Ecell)
Arrhenius equation
46. If Q>Ksp
adiabatic
a precipitate forms
P1= X1P1°
square pyramidal
47. SI unit of energy; Kg*m^2/s^2
Bronsted-Lowry acid
first
0.512°C
Joule
48. Proton donors
viscosity
Bronsted-Lowry acid
Kinetic Molecular Theory - for ideal gases
H
49. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Graham's Law
trigonal pyramidal
Molecular
base and hydrogen gas
50. Molarity (M)
(moles of products that are gasses) - (moles of reactants that are gasses)
moles of solute/ L of solution
Dalton's Law of Partial Pressures
Molecule