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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. AH of formation for a substance in its stablest form (how it is found in nature)
Molal FP Depression Constant
Beta Particles-
-(P)(Change in V)
0
2. Oxidation # of Ions
alcohol
viscosity
charge
Weight
3. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
-1
E
fusion
4. A homogeneous mixture with 1 phase
# protons + # neutrons
PV=nRT
Hydrogen bonding
Solution
5. Elements which have unpaired electrons and highly affected by magnetic fields
P1= X1P1°
blue-green
3rd law of thermodynamics
paramagnetic
6. Substances w/ critical temperatures below 25°C
square pyramidal
Molarity
v3kT/m
permanent gases
7. ClO2¹?
high pressure - low temperature
0.0826Latm/Kmol
single bond
chlorite
8. Variable for type of orbital
oxidizing agent
Angular Momentum Quantum Number
Faraday
l (second quantum number)
9. Solid to liquid
oct-
tetrahedral
Positive work value; work done on system
melting
10. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Alpha Particles-
yellow --> green
Manometer
nitrite
11. A device in which chemical energy is changed to electrical energy
H
System
electrolyte
Galvanic Cell
12. 1 sigma bond
T-shape
melting
single bond
Quantum Model
13. The minimum energy that molecules must possess for collisions to be effective - Ea
moles of solute/ L of solution
freezing
activation energy
Octahedral
14. The line running between the atoms
heat of fusion
Molality
Force = mass x acceleration
Sigma Bond
15. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
Density
entropy (S)
oxalate
16. 2+ charge
chloride
Volume Metric Flask & Pipet
Bond Energy
Alpha Particles-
17. Generally insoluble anions (names)
C=(mass)(specific heat)
Resonance
phosphate - sulfide - carbonate - sulfate
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
18. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
p+
strong acid strong base rxn
Cg=kPg
rate gas A/rate gas B = square root (mm A/ mm B)
19. Combined Gas Law Formula
Nernst Equation
P1V1/N1T1=P2V2/N2T2
high pressure - low temperature
(moles of products that are gasses) - (moles of reactants that are gasses)
20. (msubs) Can only be +1/2 or -1/2
Electron Spin Quantum Number
Constant Pressure
Law of Multiple Proportions
Surroundings
21. Molality =
moles solute/kg solvent
cathode
pi=(nRT)/v
methoxy-
22. Proton donors
Molecule
Equilibrium Expression
weak acid strong base rxn
Bronsted-Lowry acid
23. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
double bond
# protons (atom is defined by this)
q
Ligand
24. Measure of the change in enthalpy
Integrated Zero-Order Rate Law
Kinetic Molecular Theory - for ideal gases
condensation
Delta H or Enthalpy Change
25. Symbol for Enthalpy
nitrate
H
n0
Entropy (S)
26. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
AE= AH - RTAn
C + 273
bromate
27. I=moles of particles/moles of solute dissolved
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28. Force per unit area
Pressure
3rd law of thermodynamics
LE Model
Naming Binary Ionic Compounds
29. Dalton's Law of Partial Pressures (to find partial pressure formula)
Hydrogen bonding
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
P of a =(X of a)(total pressure)
Strong acid weak base rxn
30. Carbon & hydrogen compounds
v3RT/M(in kg)
hydrocarbons
Nernst Equation
chloride
31. These orbitals are perpendicular
condensation
London Dispersion Forces
p orbitals
v3kT/m
32. Half-life equation
Integrated Second-Order Rate Law
M = square root (3RT/mm)
Its root and adding -ide
N=N.(0.5)^time/time half-life
33. SO4²?
P1= X1P1°
Molar Mass of Element/ Total Molar Mass %
sulfate
iodide
34. Within a sublevel - place one e? per orbital before pairing them
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35. A single substance that may be an acid or a base (i.e. water)
Amphoteric
Arrhenius base
chromate
nitrate
36. ClO3²?
mol
lambda
strong acids
chlorate
37. The measurement of heat changes
Integrated First-Order Rate Law
Calorimetry
Transition metals
critical point
38. Forward rxn occurs when
Reducing Agent
purple --> pink
Faraday
Q<K
39. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Colligative properties
Principal Quantum Number
blue
Nodes
40. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
e-
s orbitals
Equivalence Point
Van't Hoff factor
41. Ionizes to produce H+ ions
Arrhenius Acid
spontaneity
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Manometer
42. Point at which liquid?gas occurs
boiling point
First-Order Half Life
viscosity
precipitate
43. CO3²?
experimental yield
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
deposition
carbonate
44. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
London dispersion forces
Boltzmann distribution
Theoretical yield
-ic acid
45. When n=5 ->2 - color=
exothermic
Resonance
-oic acid
blue-violet
46. The reactant in the reduction reaction that forces the oxidation reaction to occur
sulfate
equivalence point
London dispersion forces
Oxidizing Agent
47. Change without heat transfer between the system and its surroundings
Graham's Law
adiabatic
Density
Allotrope
48. 1 sigma bond - 2 pi bonds
trigonal planar
Theoretical yield
triple bond
Its element
49. Heat capacity formula
C=(mass)(specific heat)
trigonal bipyramidal
Le Chatelier's Principle
Dalton's Law
50. l=3
f
Root Mean Square Velocity
single bond
melting