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Test your basic knowledge |
AP Chemistry
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Study First
Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
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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 likelihood that a rxn will occur "by itself"
adhesion
1.86°C
1/2mv²
spontaneity
2. Significant Digits of Conversion Factors
Closed System
C=(mass)(specific heat)
trigonal planar
endless
3. (organics) nine carbons
blue-violet
non-
Hess's Law
Ionic Compounds
4. Osmotic pressure=MRT
Solution
8.314 J/K mol
Osmotic Pressure
Second-Order Half Life
5. .69/k
Bronsted-Lowry acid
Chemical Kinetics
Principal Quantum Number
First-Order Half Life
6. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Bronsted-Lowry Base
Decrease Volume and Increase Temperature
Molecular Compounds
not spontaneous
7. Kinetic Energy is proportional to ______
Temperature
Entropy (S)
moles of solute/ L of solution
Pressure
8. 0.00°C - 1 atm
Standard Temperature and Pressure
Ionic Compounds
Octahedral
heat of vaporization
9. Atomic #
# protons (atom is defined by this)
vapor pressure
Diffusion
Amount of atoms present
10. AX3E
trigonal pyramidal
oxidizing agent
double bond
Principal Quantum Number
11. A monoatomic anion is named by taking...
0 degrees C - 1 atm
Manometer
strong acid strong base rxn
Its root and adding -ide
12. Diatomic Molecules
q/moles
excess reactant
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
London dispersion forces
13. All cations are soluble with sulfate EXCEPT
Boltzmann distribution
a precipitate forms
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Matter
14. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
work
Adding
rate
Increase Temperature
15. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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16. Mol/L - concentration of a solution
Molarity
p orbitals
LeChatelier's Principle
Cathode
17. Pure metal or metal hydride + H20 ->
base and hydrogen gas
iodide
P1V1/N1T1=P2V2/N2T2
Integrated Rate Law
18. Nonmetal oxide + H2O ->
triple bond
acid
oxidizing agent
0
19. Elements on staircase on periodic table
Dipole-dipole forces
Metalliods
Chemical Bonds
carbohydrates
20. l=3
Coordination Compound
8.314 J/K mol
f
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
21. Wavelength symbol
M1V1=M2V2
methods of increasing rate
Arrhenius Base
lambda
22. ln[A] vs. time is a ...-order reaction
Transition metals
Reaction Quotient (Q)
first
Atmospheric Pressure
23. A single substance that may be an acid or a base (i.e. water)
Amphoteric
oxide gas and water
insoluble
Effusion
24. Substance being dissolved in a solution (lower [ ])
Solute
sublimation
reduction agent
tetrahedral
25. Kinetic Energy per molecule
Specific Heat Capacity
1/2mv²
Cell Potential (Ecell)
reduction
26. Ketone suffix
Thermochemistry
Second-Order Half Life
-one
Molarity
27. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Percent Yield
Colligative properties
Zero-Order Rate Law
Enthalpy of Solution
28. Heat required to raise the system 1°C
heat capacity
hydrolysis
heat of fusion
seesaw
29. Amount of heat needed to change a system by 1°C
heat capacity
iodide
Multiplying
Q<K
30. Like dissolves...
oct-
msAT
Volume Metric Flask & Pipet
like
31. Ionizes to produce OH- Ions
entropy
Arrhenius Base
adhesion
no precipitate forms
32. 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
q/moles
Average KE = 1/2(mass)(average speed of all particles)
-oate
33. Measure of the average kinetic energy of all the particles in a substance
Lone Pair
Temperature
ether
activation energy
34. 120° - sp^2
rate law
mol
Hess's Law
Trigonal Planar
35. J/°Cmol or J/Kmol
1/2mv²
Molar Heat Capacity
tetrahedral
First-Order Rate Law
36. Different form of same element
Principal Quantum Number
Coordination Compound
allotrope
Bronsted-Lowry base
37. kf of water
-oic acid
hydrocarbons
adiabatic
1.86°C
38. Change in moles (An) =?
q
hydroxide
0
(moles of products that are gasses) - (moles of reactants that are gasses)
39. Delta H (AH) = ?
blue-violet
Isolated System
q/moles
?Tf= kf x molality
40. Ionizes to produce H+ ions
square planar
Density
Arrhenius Acid
base and hydrogen gas
41. #NAME?
Strong acid weak base rxn
E
Beta Particles-
bond energy
42. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
spontaneous
Integrated Rate Law
boiling point
-one
43. Oxidation # of Ions
Atmospheric Pressure
fusion
charge
hex-
44. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
t-shape
d orbitals
Open System
Equilibrium Expression
45. I¹?
heat of fusion
Covalently w/in themselves - Ionicly bonded w/ each other
iodide
boiling point
46. Ecell= E°cell -RT/nF x lnQ
Nernst Equation
Heisenberg Uncertainty Principle
heat capacity
group
47. IMF that occurs with FON
Surroundings
M = square root (3RT/mm)
Hydrogen bonding
condensation
48. H + donor
Dalton's Law
Bronsted-Lowry Acid
Work
Bond enthalpy
49. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
Pressure
1 atm = 760 mmHg = 101.3 kPa
alcohol
50. Arrhenius equation
Cathode
k=Ae^(-Ea/RT)
Molecular Compounds
mol
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