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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. STP
Van't Hoff factor
0 degrees C - 1 atm
p+
Integrated Zero-Order Rate Law
2. Ability of an atom in a molecule to attract shared electrons to itself
Law of Conservation of Energy
Electronegativity
analyte
P of a =(X of a)(total pressure)
3. Weakest IMFs - found in all molecules
spontaneous
insoluble
base and hydrogen gas
London dispersion forces
4. PO4³?
H
Endothermic
phosphate
6.63x10?³4Js
5. How to Find an Empirical Formula Given Percentages
Arrhenius Acid
excess reactant
8.314 J/K mol
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
6. Idea Gas Law (actual rules)
ionic
Allotrope
nu
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
7. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Integrated Zero-Order Rate Law
hydrolysis
Oxidation is Loss Reduction is Gain
3/2RT
8. Kinetic Energy per mol
3/2RT
sulfate
-ic acid
oxidizing agent
9. Combined Gas Law Formula
Dipole-dipole forces
hydrocarbons
heat of fusion
P1V1/N1T1=P2V2/N2T2
10. (organics) three carbons
green/yellow
prop-
d orbitals
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
11. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
London Dispersion Forces
Isolated System
Nernst Equation
not spontaneous
12. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Heat
Quantum Model
Molarity
condensation
13. Equation to find Ea from reaction rate constants at two different temperatures
Graham's Law
strong acids
Its root and adding -ide
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
14. When gas expands ...
trigonal bipyramidal
tetrahedral
Enthalpy of Solution
Negative work value; work done by system
15. Measure of the average kinetic energy of all the particles in a substance
a precipitate forms
like
Thermochemistry
Temperature
16. If Q>Ksp
log[H+]
a precipitate forms
permanganate
Manometer
17. The chemical formed when a base accepts a proton
deposition
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
r1/r2
conjugate acid
18. AX3E2
t-shape
Amino-
base and hydrogen gas
period
19. Variable for type of orbital
l (second quantum number)
Ionic Compounds
Adding
Bond enthalpy
20. How to Find a Weighted Average
Law of Multiple Proportions
critical point
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Atomic Mass Unit
21. % yield
96500
Molecular
Calorimeter
actual yield/theoretical yield x 100%
22. Significant Digits of Conversion Factors
endless
base and hydrogen gas
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
yellow
23. Melting
22.4L
Aufbau Principle
fusion
Pressure of H2O must be Subtracted
24. Anions or cations as needed to produce a compound with non net charge
electrolyte
96500
Counterions
Scientific Method
25. Specific heat of water
s (fourth quantum number)
4.184
amine
% yield
26. For significant digits - trailing zeros _____ significant
Colligative properties
3.0x108m/s
are
oxalate
27. AX5
critical point
carbohydrates
conjugate base
trigonal bipyramidal
28. Matter can't be created nor destroyed
Law of Conservation of Mass
oxalate
ether
acid
29. Group 1 metals
Exothermic
v3RT/M(in kg)
Alkali metals
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
30. J/°Cmol or J/Kmol
Molar Heat Capacity
activation energy
activated complex (transition state)
hydrolysis
31. Substances that form OH- when dissolved in water; proton acceptors
Isotopes
Bond enthalpy
Bases
ionic
32. 1/[A]=kt + 1/[A]0
carbohydrates
hept-
square pyramidal
Integrated Second-Order Rate Law
33. A measure of resistance of an object to a change in its state of motion
third
deposition
Mass
Osmotic Pressure
34. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Molecule
hept-
equivalence point
complex ions
35. Reactant that's completely used up in a chemical reaction
Limiting reactant
Adding
r1/r2
iodide
36. PV=nRT
Ideal Gas Law
Multiplying
Volume Metric Flask & Pipet
linear
37. A method of investigation involving observation and theory to test scientific hypotheses
Zero-Order Rate Law
+1 - except if bonded to Alkali Metal -1
p+
Scientific Method
38. The entropy of a pure perfectly formed crystal @0K is 0
zero
Boltzmann distribution
but-
3rd law of thermodynamics
39. The driving force for a spontaneous is an increase in entropy of the universe
-ol
Entropy (S)
specific heat
freezing
40. (organics) five carbons
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
pent-
Theory of Relativity
Ag+ - Pb2+ - Hg2+
41. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
1.38x10?²³J/K
Heat Capacity (C)
Atmospheric Pressure
State Functions
42. The rest of the universe (in thermodynamics)
sulfate
surroundings
msAT
Equilibrium Expression
43. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Theoretical yield
Law of Definite Proportion
red/orange
Equivalence Point
44. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
First-Order Half Life
hydro-ic acid
Tetrahedral
yellow --> green
45. Degree of disorder in a system
0.512°C
entropy (S)
E
Solubility Product (Ksp)
46. Change that occurs at constant temperature
increasing
isothermal
moles of solute/ L of solution
AE= AH - RTAn
47. AX5E
square pyramidal
Force = mass x acceleration
are
Anode
48. Newton's Second Law
Anion
Bond Energy
Dipole Moment
Force = mass x acceleration
49. Expresses how the concentrations depend on time
solid CO2
not spontaneous
Integrated Rate Law
geometric isomers
50. Point at which vapor pressure=air pressure above
Ideal Gas Law
tetrahedral
boiling point
Force = mass x acceleration