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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. Mol/kg of solvent - used in calculating colligative properties
Principal Quantum Number
Molality
Ampere
group
2. Releases/gives off heat (negative value)
s (fourth quantum number)
Exothermic
heat capacity
Heat
3. Heat capacity formula
Endothermic
boiling point
C=(mass)(specific heat)
London Dispersion Forces
4. 96 -485 C/mol e-
flouride
Faraday
wavelength
octahedral
5. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Manometer
Anion
Reducing Agent
electrolyte
6. Liquid to solid
0.0821 atm L/mol K
freezing
rate
Molar Heat Capacity
7. R=
8.31J/Kmol
Alpha Particles-
Increase Temperature
Effusion
8. Osmotic pressure formula
Ideal Gas Law
indicator
pi=(nRT)/v
2nd law of thermodynamics
9. CN¹?
Le Chatelier's Principle
cyanide
condensation
endless
10. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
sublimation
complex ions
methods of increasing rate
0
11. A solution that resists a change in its pH
work
d
?Tf= kf x molality
Buffered Solution
12. Boltzmann constant - used in calculating speed of gas per molecule
-oate
pent-
reduction agent
1.38x10?²³J/K
13. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
LE Model
sulfite
melting point
14. Where reduction occurs
Nernst Equation
Cathode
Ligand
entropy
15. neutron (symbol)
sulfide
n0
force x distance = work done
p orbitals
16. PO4³?
deposition
critical point
but-
phosphate
17. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
eth-
sublimation
5% rule
18. l=2
Trigonal Planar
5% rule
Sigma Bond
d
19. Arrhenius equation
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
k=Ae^(-Ea/RT)
isothermal
Constant Volume
20. 1/[A]=kt + 1/[A]0
Osmotic Pressure
group
double bond
Integrated Second-Order Rate Law
21. Loss of electrons - increase in oxidation #
ionic
oxidation
viscosity
spontaneous
22. Heat needed to change 1 g of substance to 1°C
Acid Dissociation Constant
E
Molecular
specific heat
23. Spontaneous emission of radiation
Radioactivity
M1V1=M2V2
reduction agent
trigonal planar
24. AP doesn't deal with ...-order reaction - don't pick it!
geometric isomers
third
square pyramidal
Heat
25. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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26. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Molecular
Molarity
Diffusion
Magnetic Quantum Number (ml)
27. [A]0/2k
methoxy-
Zero-Order Half Life
viscosity
yellow --> green
28. Elements in groups 3-12
Transition metals
n (first quantum number)
Oxidizing Agent
Effusion
29. AX4E2
carbonate
Quantum Model
square planar
dec-
30. E?s fill the lowest energy orbital first - then work their way up
cathode
?Tb= kb x molality
violet
Aufbau Principle
31. Color of Sr (flame test)
Dipole-dipole forces
Antibonding Molecular Orbital
red
boiling point
32. Determined by the formula h/m(in kg)v - (v=velocity)
hex-
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
endless
wavelength
33. CrO4²?
d
sulfite
Delta H or Enthalpy Change
chromate
34. Ionizes to produce OH- Ions
paramagnetic
Arrhenius Base
p+
State Functions
35. Diatomic Molecules
carbohydrates
oxide gas and water
strong bases
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
36. Phase change from gas to solid
Beta Particles-
Enthalpy of Solution
deposition
Root Mean Square Velocity
37. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
CAT
0
nitrate
38. Forward rxn occurs when
yellow
Molality
Q<K
rate gas A/rate gas B = square root (mm A/ mm B)
39. The heat changed in a chemical reaction.
Thermochemistry
Negative work value; work done by system
Bronsted-Lowry acid
q
40. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Ionic Compounds
k=Ae^(-Ea/RT)
end point
Manometer
41. Significant Digits of Conversion Factors
red
1atm=?mmHg/Torr
endless
Integrated Zero-Order Rate Law
42. (organics) one carbon
Arrhenius acid
Specific Heat (s)
meth-
AE= AH - RTAn
43. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
C + 273
soluble
specific heat
alcohol
44. 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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45. AX2E - AX2E2
Kinetic Molecular Theory - for ideal gases
E
sublimation
bent
46. Specific heat of water
4.184
(moles of products that are gasses) - (moles of reactants that are gasses)
permanganate
entropy (S)
47. Equation to find Ea from reaction rate constants at two different temperatures
t-shape
C=(mass)(specific heat)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Graham's Law
48. AH of formation for a substance in its stablest form (how it is found in nature)
Valence Electrons(assigned)
r1/r2
Dalton's Law
0
49. Each orbital can hold two e?s each w/ opposite spins
Magnetic Quantum Number (ml)
Integrated Zero-Order Rate Law
AH
Pauli Exclusion Principle
50. Group 1 metals
viscosity
Alkali metals
Law of Definite Proportion
Amount of atoms present
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