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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
.
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. Happens at lines in phase change charts
equilibrium
yellow
M = square root (3RT/mm)
trigonal bipyramidal
2. Variable for type of orbital
1.38x10?²³J/K
Sigma Bond
base
l (second quantum number)
3. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
Ag+ - Pb2+ - Hg2+
Speed of light
adhesion
4. The minimum energy that molecules must possess for collisions to be effective - Ea
1 atm
-oic acid
activation energy
Ionic
5. Metal oxide + H20 ->
Quantum Mechanical Model
Delta H or Enthalpy Change
base
hydrocarbons
6. Mass reactants= mass products
Volt
Exothermic
2nd law of thermodynamics
Law of Conservation of Mass
7. Substances that form H+ when dissolved in water; proton donors
Acids
l (second quantum number)
Ionic Compounds
blue-violet
8. (organics) ten carbons
Anode
Integrated Rate Law
dec-
single bond
9. Mass #
London dispersion forces
a precipitate forms
# protons + # neutrons
red
10. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
effects of IMF
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
ionic
Ligand
11. 1/[A] vs. time is a ...-order reaction
second
are
Amino-
Heisenberg Uncertainty Principle
12. Tools NEEDED for dilution
d
Overall Reaction Order
Volume Metric Flask & Pipet
p orbitals
13. Average speed of gas
experimental yield
insoluble
Bond Energy
v3RT/M(in kg)
14. Unusually strong dipole forces found when H is bonded to N - O - or F
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Oxidizing Agent
Hydrogen bonding
sublimation
15. Phase change from gas to solid
non-
deposition
moles of solute/ L of solution
methods of increasing rate
16. Pure metal or metal hydride + H20 ->
Acid Dissociation Constant
rate
base and hydrogen gas
Alkali metals
17. Significant Digits of Conversion Factors
Allotrope
1 atm = 760 mmHg = 101.3 kPa
Average KE = 1/2(mass)(average speed of all particles)
endless
18. Calculation from K to C
C + 273
-ol
Van't Hoff factor
Law of Conservation of Mass
19. Point at which the titrated solution changes color
Law of Conservation of Energy
end point
P of a =(X of a)(total pressure)
First-Order Half Life
20. Composition Formula
Sigma Bond
fusion
oxide gas and water
Molar Mass of Element/ Total Molar Mass %
21. Solution in flask being titrated
analyte
hex-
Enthalpy of Solution
electron affinity
22. If anion ends in -ite - acid name ends in...
Thermochemistry
solid CO2
-ous acid
wavelength
23. Boiling point elevation formula
are
increasing
Cg=kPg
?Tb= kb x molality
24. Ester suffix
-oate
2nd law of thermodynamics
Law of Definite Proportion
triple bond
25. Only contains ions that change in reaction
Electronegativity
Molar Mass of Element/ Total Molar Mass %
Net Ionic Equation
Ampere
26. The reactant in the reduction reaction that forces the oxidation reaction to occur
Magnetic Quantum Number (ml)
Theoretical yield
Oxidizing Agent
acid
27. =vM2/M1
Arrhenius Base
Magnetic Quantum Number (ml)
s orbitals
r1/r2
28. I¹?
Dalton's Law of Partial Pressures
iodide
?Hvap
London Dispersion Forces
29. The weighted average of all the isotopes that an atom can have (in g/mol)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Atomic Mass Unit
Amount of atoms present
work
30. (# of lone pair e-)+1/2(# of shared e-)
entropy
Valence Electrons(assigned)
Pressure
(moles of products that are gasses) - (moles of reactants that are gasses)
31. ClO3²?
Law of Conservation of Mass
% yield
linear
chlorate
32. Dalton's Law of Partial Pressures (to find partial pressure formula)
Quantum Model
P of a =(X of a)(total pressure)
insoluble
purple --> pink
33. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Atmospheric Pressure
LE Model
Integrated Zero-Order Rate Law
condensation
34. Specific heat of water
lambda
permanent gases
4.184
Speed of light
35. 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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on line
183
36. The line running between the atoms
Sigma Bond
Pauli Exclusion Principle
LE Model
second
37. l=2
Temperature
Arrhenius Base
Coordination Compound
d
38. SO4²?
A Roman numeral
sulfate
carbohydrates
Ionic Compounds
39. H?+NH3?NH4
Ligand
green/yellow
Strong acid weak base rxn
P of a =(X of a)(total pressure)
40. ?T=k*m(solute)
amine
trigonal bipyramidal
permanent gases
Molal FP Depression Constant
41. Weakest IMFs - found in all molecules
London dispersion forces
Root Mean Square Velocity
a precipitate forms
Dalton's Law of Partial Pressures
42. PO4³?
Boltzmann distribution
standard solution
phosphate
Theory of Relativity
43. Organic reaction in which two functional groups come together - resulting in the release of water
chlorite
Mass
condensation
solid CO2
44. AX3E2
t-shape
chloride
charge
3/2RT
45. Color of Ca (flame test)
State Functions
red/orange
Molecular Orbitals (MOs)
Molality
46. Higher in energy than the atomic orbitals of which it is composed
Thermochemistry
Antibonding Molecular Orbital
tetrahedral
Cg=kPg
47. % yield
solid CO2
Oxidation is Loss Reduction is Gain
0
actual yield/theoretical yield x 100%
48. 1 sigma bond - 2 pi bonds
triple bond
different # of neutrons
Exothermic
but-
49. x can be ignored when % ionization is <5%
5% rule
carbohydrates
Covalently w/in themselves - Ionicly bonded w/ each other
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
50. Colors of Reaction when (MnO4 -) --> (Mn2+)
purple --> pink
alcohol
Reaction Quotient (Q)
titrant buret
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