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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. The entropy of a pure perfectly formed crystal @0K is 0
Acid + Base --> Salt + Water
3rd law of thermodynamics
heat of fusion
Weight
2. Type of system in which nothing is transfered (no mass or energy); ideal
Temperature
Isolated System
Molecular Compounds
Allotrope
3. If anion ends in -ite - acid name ends in...
Cathode
Osmotic Pressure
-ous acid
excess reactant
4. (organics) four carbons
yellow
Alkali metals
but-
zero
5. Organic w/ -NH2
amine
dichromate
isothermal
chlorate
6. Gas to liquid
condensation
endothermic
0.512°C
Force = mass x acceleration
7. Color of Ba (flame test)
carbonate
strong bases
green/yellow
conjugate base
8. How to Find an Empirical Formula Given Grams
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Beta Particles-
AE= AH - RTAn
geometric isomers
9. Peak of energy diagram
Calorimeter
activated complex (transition state)
s
Mass
10. This MUST be determined experimentally
rate law
red
methods of increasing rate
excess reactant
11. Oxidation # of Oxygen
m (third quantum number)
Sigma Bond
-2 - with peroxide -1
period
12. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
Temperature
Linear
Volt
13. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Calorimeter
strong acids
0 degrees C - 1 atm
Antibonding Molecular Orbital
14. Phase change from gas to solid
M = square root (3RT/mm)
deposition
Van't Hoff factor
chlorite
15. (organics) one carbon
Boltzmann distribution
Molal BP Elevation Constant
Covalently w/in themselves - Ionicly bonded w/ each other
meth-
16. K
Anion
Equilibrium constant
Density
Nernst Equation
17. Ketone suffix
-one
high pressure - low temperature
1/2mv²
22.4L
18. Symbol for Total Heat absorbed or released
square planar
deposition
q
adiabatic
19. frequency symbol
Volt
nu
Effusion
End Point
20. The minimum energy that molecules must possess for collisions to be effective - Ea
6.63x10?³4Js
activation energy
Law of Conservation of Mass
% yield
21. Ecell= E°cell -RT/nF x lnQ
Enthalpy of Solution
Speed of light
eth-
Nernst Equation
22. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
t-shape
PV=nRT
Kinetic Molecular Theory - for ideal gases
freezing
23. (organics) ten carbons
0.0821 atm L/mol K
Entropy (S)
dec-
square planar
24. For significant digits - leading zeros ____ significant
Hybridization
are not
Oxidizing Agent
nitrate
25. Stronger IMF= lower... weaker IMF= higher...
weak acid strong base rxn
Law of Conservation of Mass
cohesion
vapor pressure
26. Forward rxn occurs when
ether
Q<K
precipitate
Arrhenius Acid
27. Phase change from solid to gas
strong acids
Hund's Rule
sublimation
experimental yield
28. Color of Na (flame test)
Molar Mass of Element/ Total Molar Mass %
purple --> pink
yellow
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
29. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Theoretical yield
Colligative properties
% error
Antibonding Molecular Orbital
30. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
specific heat
Acids
not spontaneous
Hund's Rule
31. Composition Formula
red
iodide
0
Molar Mass of Element/ Total Molar Mass %
32. Substance that - when dissolved - is conductive
Hybridization
rate gas A/rate gas B = square root (mm A/ mm B)
-ol
electrolyte
33. Positive enthalpy - heat flows into system
acid
endothermic
reduction
isothermal
34. The reactant that is being oxidized - brings about reduction
Endothermic
reduction agent
Decrease Volume and Increase Temperature
paramagnetic
35. Elements on staircase on periodic table
Metalliods
Solubility Product (Ksp)
Constant Pressure
Integrated Rate Law
36. AX5
London dispersion forces
trigonal bipyramidal
sulfate
chromate
37. Universal IMF for nonpolar molecules
tetrahedral
triple bond
insoluble
London dispersion forces
38. q cal = ?
Percent Yield
complex ions
wavelength
CAT
39. Half cell in which reduction occurs
Hess's Law
cathode
Normality
equivalence point
40. Mass/volume
Density
sublimation
activation energy
vaporization
41. Proton (symbol)
rate law
p+
oxidation
f
42. Coffee Cup Calorimeter
Constant Pressure
Second-Order Rate Law
period
Nodes
43. (organics) nine carbons
blue-green
non-
Hund's Rule
Heisenberg Uncertainty Principle
44. (msubs) Can only be +1/2 or -1/2
Van't Hoff factor
Bronsted-Lowry acid
Electron Spin Quantum Number
work
45. Bomb Calorimeter
Constant Volume
Molality
square pyramidal
melting
46. 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
trigonal bipyramidal
supercritical fluid
Percent Yield
Van't Hoff factor
47. When n=5 ->2 - color=
blue-violet
pi=(nRT)/v
yellow
square pyramidal
48. Has values 1 -2 -3 -...; tells energy levels
v3RT/M(in kg)
0.512°C
Bronsted-Lowry base
Principal Quantum Number
49. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
rate gas A/rate gas B = square root (mm A/ mm B)
Pauli Exclusion Principle
3.0x108m/s
50. n+m (these are orders of reactants)
wavelength
hydrocarbons
Force = mass x acceleration
Overall Reaction Order