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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. Energy required for melting to occur
heat of fusion
Gamma Ray-
anode
Allotrope
2. AX5
trigonal bipyramidal
acid
like
Pi Bond
3. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
Covalently w/in themselves - Ionicly bonded w/ each other
viscosity
End Point
bond energy
4. Amount of gravitational force exerted on an object
oxide gas and water
1.86°C
Weight
equivalence point
5. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
End Point
Chemical Kinetics
3rd law of thermodynamics
excess reactant
6. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
rate
group
Graham's Law
7. (organics) nine carbons
non-
Arrhenius equation
Hund's Rule
dichromate
8. Driving force of the electrons
Cell Potential (Ecell)
Antibonding Molecular Orbital
22.4L
Galvanic Cell
9. Elements which have all electrons paired and relatively unaffected by magnetic fields
LeChatelier's Principle
End Point
activation energy
diamagnetic
10. Significant Digits of counted things
dichromate
endless
Pi Bond
Dipole Moment
11. Idea Gas Law (actual rules)
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
second
LeChatelier's Principle
Negative work value; work done by system
12. Molecules' tendency to stick to the container
Increase Temperature
r1/r2
adhesion
Law of Multiple Proportions
13. How to Balance a Redox Equation
strong acids
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
Nernst Equation
Theoretical yield
14. A homogeneous mixture with 1 phase
nitrate
% error
Solution
-ic acid
15. Melting
work
fusion
Multiplying
0.0826Latm/Kmol
16. The reactant in the reduction reaction that forces the oxidation reaction to occur
square planar
Oxidizing Agent
Scientific Method
purple
17. Instrument used to measure the pressure of atmospheric gas
Cation
-ol
q/moles
Barometer
18. NH4¹?
ammonium
Molecular Orbitals (MOs)
Colligative properties
-ol
19. Energy required for liquid?gas
?Tf= kf x molality
heat of vaporization
adiabatic
Law of Multiple Proportions
20. ClO2¹?
v3kT/m
moles solute/kg solvent
chlorite
yellow
21. kb of water
-(P)(Change in V)
0.512°C
Electronegativity
triple point
22. Color of Cs (flame test)
Scientific Method
P of a =(X of a)(total pressure)
blue
reduction agent
23. 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)
Kinetic Molecular Theory - for ideal gases
3rd law of thermodynamics
Gamma Ray-
96500
24. Puts H? into solution
Principal Quantum Number
system
Molar Heat Capacity
Arrhenius acid
25. Boiling point elevation formula
Alkaline earth metals
?Tb= kb x molality
hept-
-oate
26. Oxidation # of Ions
charge
3/2RT
-ol
square pyramidal
27. Point at which the titrated solution changes color
end point
trigonal planar
Ideal Gas Law
amine
28. Ester suffix
condensation
State Functions
-oate
Trigonal Planar
29. Mass #
oxidation
# protons + # neutrons
condensation
Pressure
30. The driving force for a spontaneous is an increase in entropy of the universe
Entropy (S)
dec-
Aufbau Principle
Sigma Bond
31. Volume of gas @STP
22.4L
1.86°C
AE= AH - RTAn
Hund's Rule
32. A measure of resistance of an object to a change in its state of motion
Mass
AE= AH - RTAn
1atm=?Pa
Law of Multiple Proportions
33. E=mc^2
Arrhenius base
% yield
Theory of Relativity
Amino-
34. Oxidation # of Compounds
0
Osmotic Pressure
red/orange
-oic acid
35. The part of the universe one is focused upon (in thermodynamics)
system
salt bridge
acetate
Bond Order
36. Color of Na (flame test)
Molality
permanent gases
conjugate base
yellow
37. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Theoretical yield
alkyne
Equivalence Point
triple bond
38. C2O4²?
Tetrahedral
s orbitals
oxalate
period
39. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Arrhenius acid
trigonal planar
red/orange
Molecular Compounds
40. Carbon - hydrogen - oxygen compounds
Beta Particles-
Specific Heat (s)
carbohydrates
are not
41. Different form of same element
equilibrium
allotrope
amine
viscosity
42. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
wavelength
Increase Temperature
insoluble
43. Temperature-pressure combination at which solid - liquid - and gas states appear
triple point
# protons + # neutrons
melting point
8.31J/Kmol
44. For significant digits - trailing zeros _____ significant
effects of IMF
are
Magnetic Quantum Number (ml)
dec-
45. Negative enthalpy - heat flows into surroundings
non-
boiling point
exothermic
mol Fraction
46. Gas to liquid
condensation
blue-green
chloride
Polar Covalent
47. Where oxidation occurs
l (second quantum number)
Anode
trigonal pyramidal
AE = q + w
48. If needed - indicate charge of metal(cation) by...
seesaw
Bronsted-Lowry Acid
square pyramidal
A Roman numeral
49. A solid or gas that can be formed when 2 or more aqueous reactants come together
exothermic
Theory of Relativity
precipitate
0
50. All _________ compounds are electrolytes
1/2mv²
ether
Nernst Equation
Ionic