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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
bromate
Equilibrium Expression
wavelength
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
2. Dirrect Method Formula
catalyst
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Beta Particles-
4.184
3. To find activation energy use the...
N=N.(0.5)^time/time half-life
isothermal
red
Arrhenius equation
4. Increase Volume
8.314 J/K mol
Molecular Orbitals (MOs)
Increase Temperature
activation energy
5. S²?
like
sulfide
s orbitals
M = square root (3RT/mm)
6. Amount of gravitational force exerted on an object
Heat
n0
Dipole Moment
Weight
7. All forms of energy except for heat
work
Electron Spin Quantum Number
strong bases
bromate
8. Liquid to gas
Law of Conservation of Energy
vaporization
Heisenberg Uncertainty Principle
salt bridge
9. R=
nu
Amino-
8.31J/Kmol
Law of Conservation of Energy
10. A monoatomic anion is named by taking...
violet
Its root and adding -ide
conjugate acid
Net Ionic Equation
11. For significant digits - trailing zeros _____ significant
Standard Temperature and Pressure
Colligative properties
group
are
12. 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)
are not
mol Fraction
Kinetic Molecular Theory - for ideal gases
conjugate base
13. Point where acid completely neutralizes base
actual yield/theoretical yield x 100%
equivalence point
Graham's Law
nu
14. Amount of heat needed to change a system by 1°C
lambda
q
Naming Binary Ionic Compounds
heat capacity
15. (A) - C/s
actual yield/theoretical yield x 100%
Ampere
alkyne
Molality
16. Gain of electrons - decrease in oxidation #
acid
Speed of light
cohesion
reduction
17. Heat capacity formula
C=(mass)(specific heat)
oxidizing agent
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
M1V1=M2V2
18. Forward rxn occurs when
Dipole-dipole forces
Q<K
bromate
Trigonal Planar
19. Mole Fraction
X of a = moles a/total moles
like
# protons + # neutrons
alkane
20. Positive enthalpy - heat flows into system
endless
endothermic
p orbitals
Coordination Compound
21. Theoretical yield-experimental yield/theoretical yieldx100
0
Ideal Gas Law
% error
Thermochemistry
22. Force per unit area
entropy
Bronsted-Lowry base
Pressure
1.38x10?²³J/K
23. CN¹?
fusion
cohesion
log[H+]
cyanide
24. Oxidation # of free elements
Allotrope
P of a =(X of a)(total pressure)
0
PV=nRT
25. NO2¹?
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Trigonal Planar
nitrite
Negative work value; work done by system
26. Where reduction occurs
Cathode
deposition
1 atm
E
27. Organic reaction in which two functional groups come together - resulting in the release of water
iodide
alcohol
are
condensation
28. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
dichromate
Oxidation is Loss Reduction is Gain
Lone Pair
29. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
double bond
Constant Pressure
Quantum Mechanical Model
hydrolysis
30. Ptotal=Pa+Pb+Pc....
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183
31. Solid to gas
perchlorate
Le Chatelier's Principle
Alpha Particles-
sublimation
32. AX5E
voltaic cells
square pyramidal
Net Ionic Equation
Molecule
33. Larger molecules which have higher mass and therefore electron density have stronger...
insoluble
Isolated System
London dispersion forces
P of a =(X of a)(total pressure)
34. Mol/L - concentration of a solution
reduction agent
Decrease Volume and Increase Temperature
are
Molarity
35. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
?Tf= kf x molality
adhesion
Bonding Pairs
36. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Scientific Method
salt bridge
Manometer
ether
37. C=2.9979*10^8 m/s
heat of fusion
Speed of light
adhesion
Root Mean Square Velocity
38. Boltzmann constant - used in calculating speed of gas per molecule
1.38x10?²³J/K
Molecular Orbitals (MOs)
octahedral
geometric isomers
39. negative ion
cohesion
Anion
Thermochemistry
Integrated Zero-Order Rate Law
40. l=0
s
Mass
Pressure of H2O must be Subtracted
deposition
41. SO3²?
adiabatic
sulfite
Atmospheric Pressure
cyanide
42. 2 or more covalently bonded atoms
Molecule
London Dispersion Forces
allotrope
Surroundings
43. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
blue-green
k=Ae^(-Ea/RT)
-(P)(Change in V)
44. Expresses how the concentrations depend on time
8.31J/Kmol
blue
Its root and adding -ide
Integrated Rate Law
45. This MUST be determined experimentally
rate law
carbohydrates
Zero-Order Rate Law
no precipitate forms
46. Only contains ions that change in reaction
actual yield/theoretical yield x 100%
Hund's Rule
p orbitals
Net Ionic Equation
47. Oxidation # of Ions
charge
standard solution
Monoprotic
?Tf= kf x molality
48. Anions or cations as needed to produce a compound with non net charge
spontaneous
first
Force = mass x acceleration
Counterions
49. AX6
octahedral
Galvanic Cell
entropy (S)
blue
50. Substances w/ critical temperatures below 25°C
Negative work value; work done by system
Heisenberg Uncertainty Principle
permanent gases
spontaneous