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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
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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. Variable for energy of e- - goes from 1 -2 -3 on up
Molal BP Elevation Constant
Volume Metric Flask & Pipet
n (first quantum number)
Oxidation is Loss Reduction is Gain
2. Mass percent
g solute/g solvent x 100
Van't Hoff factor
Molar Heat Capacity
Quantum Model
3. The mixing of native atomic orbitals to form special orbitals for bonding
Transition metals
Hybridization
Equivalence Point
complex ions
4. l=3
q
green/yellow
f
p orbitals
5. The transfer of energy between two objects due to temperature difference
acetate
Heat
octahedral
carbonate
6. Ability of an atom in a molecule to attract shared electrons to itself
Electronegativity
iodide
increasing
0
7. Composition Formula
Ampere
Molar Mass of Element/ Total Molar Mass %
Balmer Series
Integrated Zero-Order Rate Law
8. Rate of Diffusion/Effusion formula
ammonium
N=N.(0.5)^time/time half-life
hex-
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
9. Proton donors
Transition metals
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Joule
Bronsted-Lowry acid
10. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Specific Heat Capacity
force x distance = work done
Acid + Base --> Salt + Water
Bond Order
11. Diatomic Molecules
square pyramidal
amine
0.0821 atm L/mol K
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
12. Measure of the change in enthalpy
Delta H or Enthalpy Change
Hydrogen bonding
reduction agent
Ideal Gas Law
13. Elements on staircase on periodic table
Metalliods
mol
viscosity
k=Ae^(-Ea/RT)
14. AX3E2
1 atm
t-shape
Molality
perchlorate
15. Substances that form H+ when dissolved in water; proton donors
square planar
Arrhenius base
P of a =(X of a)(total pressure)
Acids
16. Actual Yield/Theoretical Yield*100%
# protons (atom is defined by this)
Percent Yield
effects of IMF
AE = q + w
17. Oxidation # of Polyatomic Ions
charge
3.0x108m/s
Specific Heat (s)
0.512°C
18. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
Heat Capacity (C)
Amino-
red/orange
19. What is defined by you taken from the whole universe
Magnetic Quantum Number (ml)
bent
H
System
20. When gas expands ...
Negative work value; work done by system
0
6.63x10?³4Js
system
21. The amount of energy/heat required to raise some substance 1 degree C
red/orange
Covalently w/in themselves - Ionicly bonded w/ each other
Heat Capacity (C)
Molal FP Depression Constant
22. SO3²?
Zero-Order Half Life
high pressure - low temperature
sulfite
increasing
23. AX2E - AX2E2
bent
insoluble
E
0
24. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
moles of solute/ L of solution
Ag+ - Pb2+ - Hg2+
Amphoteric
Formal Charge
25. #NAME?
Theory of Relativity
E
Heisenberg Uncertainty Principle
P1V1/N1T1=P2V2/N2T2
26. 180° - sp
Hydrogen bonding
Linear
Constant Pressure
sulfite
27. 0.00°C - 1 atm
Molality
Trigonal Bipyramidal
rate gas A/rate gas B = square root (mm A/ mm B)
Standard Temperature and Pressure
28. OH¹?
condensation
Heat
hydroxide
AE = q + w
29. F¹?
flouride
work
lambda
Metalliods
30. Connects the 2 half cells in a voltaic cell
salt bridge
deposition
seesaw
linear
31. These orbitals are spherical
linear
P of a =(X of a)(total pressure)
s orbitals
Ideal Gas Law
32. O²?
Pressure of H2O must be Subtracted
solid CO2
Trigonal Bipyramidal
oxide
33. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
voltaic cells
cathode
Bronsted-Lowry acid
deposition
34. ClO4¹?
perchlorate
alcohol
Colligative properties
M = square root (3RT/mm)
35. r=k[A]
bent
?Tf= kf x molality
second
First-Order Rate Law
36. Molality =
moles solute/kg solvent
Tetrahedral
-(q of H2O + q of cal)
Cg=kPg
37. AX5E
Electronegativity
square pyramidal
Ideal Gas Law
Joule
38. Atomic #
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
+1 - except if bonded to Alkali Metal -1
force x distance = work done
# protons (atom is defined by this)
39. 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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40. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Hybridization
e-
41. A monoatomic cation takes name from...
Its element
Pauli Exclusion Principle
1 atm
-al
42. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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43. Reverse rxn occurs when
Q>K
Weight
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Sigma Bond
44. I¹?
Effusion
Ampere
iodide
Principal Quantum Number
45. Faraday's constant
96500
solid CO2
v3kT/m
acid
46. Loss of electrons - increase in oxidation #
oxidation
Diffusion
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Molality
47. A given compound always has exactly the same proportion of elements by mass
T-shape
Hess's Law
Law of Multiple Proportions
Law of Definite Proportion
48. IMF that occurs with FON
base and hydrogen gas
alkene
Hydrogen bonding
charge
49. Positive enthalpy - heat flows into system
-(P)(Change in V)
third
square pyramidal
endothermic
50. If anion ends in -ate - acid name ends in...
Aufbau Principle
sulfide
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
-ic acid
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