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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.
If you are not ready to take this test, you can
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. 1 sigma bond
second
E
single bond
complex ions
2. Everything in the universe that is not defined by you as part of the system
Amphoteric
End Point
endothermic
Surroundings
3. Atomic #
third
Strong acid weak base rxn
# protons (atom is defined by this)
Atmospheric Pressure
4. 2+ charge
second
Heat Capacity (C)
Alpha Particles-
0
5. Carbon & hydrogen compounds
sulfide
Sigma Bond
hydrocarbons
hydroxide
6. Metal oxide + H20 ->
base
Equilibrium Expression
96500
End Point
7. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Boltzmann distribution
trigonal planar
State Functions
Equivalence Point
8. .69/k
spontaneous
s (fourth quantum number)
Ionic Compounds
First-Order Half Life
9. Variable for energy of e- - goes from 1 -2 -3 on up
Strong acid weak base rxn
n (first quantum number)
Linear
22.4L
10. AX3E2
T-shape
Allotrope
Second-Order Half Life
log[H+]
11. Substances w/ critical temperatures below 25°C
condensation
Standard Temperature and Pressure
permanent gases
22.4L
12. Color of Li (flame test)
ionic
like
8.31J/Kmol
red
13. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
3/2RT
Zero-Order Rate Law
van't Hoff Factor
14. Mol of solute/kg of solvent
voltaic cells
Delta H or Enthalpy Change
Molality
hept-
15. Dalton's Law of Partial Pressures (to find partial pressure formula)
s
double bond
Average KE = 1/2(mass)(average speed of all particles)
P of a =(X of a)(total pressure)
16. r=k[A]^2
methods of increasing rate
Second-Order Rate Law
State Functions
Theoretical yield
17. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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18. Gas to liquid
adiabatic
Constant Pressure
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
condensation
19. Force per unit area
adhesion
Colligative properties
Pressure
green/yellow
20. The chemical formed when a base accepts a proton
endless
square planar
Bond enthalpy
conjugate acid
21. Average Kinetic Energy Formula
carbohydrates
Average KE = 1/2(mass)(average speed of all particles)
Overall Reaction Order
Second-Order Rate Law
22. Faraday's constant
96500
v3RT/M(in kg)
phosphate - sulfide - carbonate - sulfate
Specific Heat (s)
23. An element with several different forms - each with different properties (i.e. graphite & diamond)
Allotrope
8.314 J/K mol
Anode
Law of Conservation of Mass
24. Oxidation # of Halogens
-1
insoluble
boiling point
Calorimeter
25. (organics) four carbons
triple point
acetate
Work
but-
26. Molecules' tendency to stick to the container
adhesion
alkene
Specific Heat (s)
Hund's Rule
27. Organic w/ -O-
Anion
Trigonal Bipyramidal
ether
0.0821 atm L/mol K
28. Spontaneous emission of radiation
activated complex (transition state)
Bronsted-Lowry Base
see-saw
Radioactivity
29. If heat capacity isn't mentioned - you can assume that q of cal is = ?
0
second
melting
Limiting reactant
30. =vM2/M1
sulfide
Second-Order Half Life
r1/r2
Chemical Kinetics
31. H+ Acceptor
Bronsted-Lowry Base
specific heat
-al
cyanide
32. CO3²?
base
Bases
carbonate
Amino-
33. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
-al
insoluble
trigonal bipyramidal
condensation
34. Oxidation # of Hydrogen
5% rule
s
hex-
+1 - except if bonded to Alkali Metal -1
35. How to Balance a Redox Equation
Trigonal Bipyramidal
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
hydroxide
Ideal Gas Law
36. How to Find a Weighted Average
purple
hydrocarbons
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
London dispersion forces
37. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
phosphate - sulfide - carbonate - sulfate
l (second quantum number)
Polar Covalent
melting
38. Substance that - when dissolved - is conductive
red
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
electrolyte
Cg=kPg
39. A solid or gas that can be formed when 2 or more aqueous reactants come together
Root Mean Square Velocity
precipitate
LeChatelier's Principle
l (second quantum number)
40. AX4E2
Solute
AE= AH - RTAn
square planar
Hund's Rule
41. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
oxide
flouride
Ionic
Kinetic Molecular Theory - for ideal gases
42. Generally insoluble anions (names)
triple bond
Decrease Volume and Increase Temperature
Bronsted-Lowry Acid
phosphate - sulfide - carbonate - sulfate
43. Gas to solid
hydroxide
deposition
phosphate - sulfide - carbonate - sulfate
Force = mass x acceleration
44. Degree of disorder in a system
Le Chatelier's Principle
entropy (S)
heat capacity
moles solute/kg solvent
45. Has values 1 -2 -3 -...; tells energy levels
Ideal Gas Law
Principal Quantum Number
H
E
46. If anion ends in -ide - acid name ends in
hydro-ic acid
AE= AH - RTAn
Cation
work
47. Work = ?
3rd law of thermodynamics
-(P)(Change in V)
ammonium
AE= AH - RTAn
48. R in instances that pertain to energy
8.314 J/K mol
n0
22.4L
P1V1/N1T1=P2V2/N2T2
49. Connects the 2 half cells in a voltaic cell
CAT
salt bridge
indicator
van't Hoff Factor
50. HF+ OH??H2O
1st law of thermodynamics
weak acid strong base rxn
blue
Atmospheric Pressure