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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.
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study here
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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. Significant Digits of counted things
Isotopes
endless
alkene
Cell Potential (Ecell)
2. l=3
r1/r2
trigonal bipyramidal
Integrated Second-Order Rate Law
f
3. Stronger IMF= lower... weaker IMF= higher...
vapor pressure
lambda
AH
C + 273
4. (organics) six carbons
sublimation
rate law
1atm=?Pa
hex-
5. Solid to gas
0.0821 atm L/mol K
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
spontaneous
sublimation
6. Substances w/ critical temperatures below 25°C
third
permanent gases
Beta Particles-
Limiting reactant
7. Cr2O7²?
phosphate - sulfide - carbonate - sulfate
boiling point
dichromate
Heat
8. Mol/L - concentration of a solution
endless
Transition metals
increasing
Molarity
9. A given compound always has exactly the same proportion of elements by mass
Dalton's Law
eth-
Law of Definite Proportion
Hess's Law
10. Color of Li (flame test)
red
Radioactivity
8.314 J/K mol
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
11. Type of system in which the energy may escape - but the mass is conserved
Closed System
different # of neutrons
1 atm
3/2RT
12. A monoatomic cation takes name from...
Reaction Quotient (Q)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
% error
Its element
13. ClO4¹?
activated complex (transition state)
soluble
green/yellow
perchlorate
14. K
Equilibrium constant
Buffer
bond energy
LE Model
15. When n=5 ->2 - color=
sulfide
blue-violet
spontaneity
Aufbau Principle
16. IMF that exists in polar molecules
phosphate - sulfide - carbonate - sulfate
strong acids
m (third quantum number)
Dipole-dipole forces
17. Change that occurs at constant temperature
Calorimeter
3.0x108m/s
?Tf= kf x molality
isothermal
18. Passage of gas through tiny orifice
reduction agent
s orbitals
Effusion
pi=(nRT)/v
19. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
phosphate - sulfide - carbonate - sulfate
London Dispersion Forces
Alkaline earth metals
triple point
20. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
increasing
-2 - with peroxide -1
oxidation
21. A solid or gas that can be formed when 2 or more aqueous reactants come together
work
8.31J/Kmol
insoluble
precipitate
22. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
adhesion
Colligative properties
Finding Empirical Formulas
Quantum Mechanical Model
23. Oxidation # of Compounds
surroundings
condensation
0
LeChatelier's Principle
24. Calculation from K to C
-oate
Equilibrium Expression
C + 273
-2 - with peroxide -1
25. Tools NEEDED for dilution
see-saw
Volume Metric Flask & Pipet
nu
P of a =(X of a)(total pressure)
26. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
1atm=?Pa
permanent gases
amine
27. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
spontaneity
Law of Conservation of Mass
Negative work value; work done by system
28. Polyatomic Ions (bonding)
meth-
Adding
Acids
Covalently w/in themselves - Ionicly bonded w/ each other
29. Molecules' tendency to stick to one another
Arrhenius equation
cohesion
increasing
T-shape
30. Puts OH? into solution
Osmotic Pressure
charge
Arrhenius base
Theory of Relativity
31. Symbol for Total Heat absorbed or released
Principal Quantum Number
q
Ideal Gas Law
0
32. AH of formation for a substance in its stablest form (how it is found in nature)
alcohol
work
0
deposition
33. ?T=k*m(solute)
Molal FP Depression Constant
Counterions
condensation
Second-Order Rate Law
34. Within a sublevel - place one e? per orbital before pairing them
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183
35. Cation first - anion second
third
triple bond
Naming Binary Ionic Compounds
weak acid strong base rxn
36. Occupies the space above and below a sigma bond
adhesion
London dispersion forces
0
Pi Bond
37. NO3¹?
Zero-Order Rate Law
nitrate
Counterions
Effusion
38. Amine prefix
Amino-
Ligand
hydroxide
condensation
39. AX3E2
t-shape
Buffered Solution
end point
Hess's Law
40. A measure of randomness or disorder
entropy
Oxidation is Loss Reduction is Gain
reduction
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
41. C2H3O2¹?
acetate
q
sulfide
like
42. Heat capacity formula
endothermic
C=(mass)(specific heat)
oxalate
Speed of light
43. A device used to measure Delta H
Calorimeter
activated complex (transition state)
M = square root (3RT/mm)
Exothermic
44. J/°Cg or J/Kg
First-Order Rate Law
Manometer
Specific Heat Capacity
condensation
45. Ester suffix
strong bases
diamagnetic
precipitate
-oate
46. Describe various properties of one orbital
Density
msAT
Trigonal Bipyramidal
Quantum Numbers
47. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
first
pent-
Finding Empirical Formulas
endless
48. Bomb Calorimeter
iodide
Constant Volume
N=N.(0.5)^time/time half-life
Percent Yield
49. (msubs) Can only be +1/2 or -1/2
alkane
0.0826Latm/Kmol
Electron Spin Quantum Number
Bonding Pairs
50. All forms of energy except for heat
Law of Conservation of Mass
H
work
e-
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