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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. The likelihood that a rxn will occur "by itself"
Chemical Kinetics
spontaneity
Ionic
weak acid strong base rxn
2. The transfer of energy between two objects due to temperature difference
Zero-Order Half Life
LeChatelier's Principle
Polar Covalent
Heat
3. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Molecular
diamagnetic
p orbitals
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
4. 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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5. ClO2¹?
Molal BP Elevation Constant
chlorite
linear
Calorimetry
6. We cannot simultaneously determine an atom's exact path or location
Heisenberg Uncertainty Principle
Alkaline earth metals
adhesion
Reaction Quotient (Q)
7. I¹?
activation energy
E
iodide
End Point
8. Consists of a complex ion - a transition metal with attached ligands - and counterions
Root Mean Square Velocity
voltaic cells
Coordination Compound
geometric isomers
9. C2O4²?
electron affinity
blue
oxalate
System
10. ClO4¹?
carbonate
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
phosphate - sulfide - carbonate - sulfate
perchlorate
11. Kinetic Energy per mol
diamagnetic
Normality
seesaw
3/2RT
12. R=
8.31J/Kmol
Diffusion
H
Constant Volume
13. Mol/L - concentration of a solution
prop-
Molarity
End Point
Amount of atoms present
14. E=mc^2
Net Ionic Equation
Theory of Relativity
n (first quantum number)
Angular Momentum Quantum Number
15. AX3E2
Electronegativity
Dalton's Law
T-shape
Bronsted-Lowry base
16. (organics) triple-bonded compound
q
Arrhenius Base
Magnetic Quantum Number (ml)
alkyne
17. Point at which solid?liquid occurs
Dipole-dipole forces
Dalton's Law of Partial Pressures
melting point
d orbitals
18. Carbon & hydrogen compounds
insoluble
hydrocarbons
?Tb= kb x molality
Law of Definite Proportion
19. Ability of an atom in a molecule to attract shared electrons to itself
Covalently w/in themselves - Ionicly bonded w/ each other
Faraday
Electronegativity
P1V1/N1T1=P2V2/N2T2
20. Solid to liquid
purple --> pink
Beta Particles-
melting
supercritical fluid
21. Similar to atomic orbitals - except between molecules
Second-Order Half Life
q
Molecular Orbitals (MOs)
double bond
22. The driving force for a spontaneous is an increase in entropy of the universe
Isolated System
Bronsted-Lowry base
Entropy (S)
spontaneous
23. Organic w/ -OH group
Ligand
alcohol
Quantum Model
melting point
24. PO4³?
square pyramidal
phosphate
H
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
25. [A]0/2k
second
-1
Zero-Order Half Life
Magnetic Quantum Number (ml)
26. 6.022x10^23
Quantum Model
different # of neutrons
mol
supercritical fluid
27. l=0
s
experimental yield
carbohydrates
Le Chatelier's Principle
28. Energy required to break a bond
trigonal planar
endless
Bond Energy
log[H+]
29. Anions or cations as needed to produce a compound with non net charge
rate gas A/rate gas B = square root (mm A/ mm B)
salt bridge
Counterions
Decrease Volume and Increase Temperature
30. The amount of energy/heat required to raise some substance 1 degree C
Heat Capacity (C)
f
p
Enthalpy of Solution
31. Increase Volume
Calorimetry
Increase Temperature
AH
Integrated Rate Law
32. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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33. ?Hsoln=?H1+?H2+?H3+...
-2 - with peroxide -1
red
Enthalpy of Solution
M = square root (3RT/mm)
34. r=k
triple point
sulfite
-one
Zero-Order Rate Law
35. Color of Sr (flame test)
Arrhenius Base
red
Quantum Mechanical Model
system
36. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
diamagnetic
critical point
van't Hoff Factor
37. Color of Li (flame test)
Diffusion
yellow
square planar
red
38. Volume of gas @STP
hydrolysis
square pyramidal
Solvent
22.4L
39. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
oxidizing agent
Colligative properties
1 atm
Pauli Exclusion Principle
40. Gas to solid
deposition
Boltzmann distribution
Alkali metals
strong bases
41. Effusion of a gas is inversely proportional to the square root of the molar mass
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42. CO3²?
viscosity
carbonate
Alkaline earth metals
Temperature
43. This MUST be determined experimentally
strong bases
Hess's Law
rate law
Ideal Gas Law
44. A monoatomic cation takes name from...
vaporization
Its element
Positive work value; work done on system
Force = mass x acceleration
45. Kinetic Energy per molecule
Valence Electrons(assigned)
1/2mv²
Hund's Rule
oxidation
46. Temperature-pressure point after which gas can no longer form liquid
Positive work value; work done on system
condensation
linear
critical point
47. Ketone suffix
chloride
p orbitals
alkene
-one
48. Proton acceptors - must have an unshared pair of e?s
adhesion
Lone Pair
cyanide
Bronsted-Lowry base
49. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
p+
Bronsted-Lowry Base
Positive work value; work done on system
50. AX2E - AX2E2
Density
standard solution
bent
0.0821 atm L/mol K