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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. 0°C and 1 atm
chlorite
first
STP
alkyne
2. Change without heat transfer between the system and its surroundings
not spontaneous
dec-
Molecular
adiabatic
3. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
pent-
LE Model
cohesion
-(P)(Change in V)
4. ?T=k*m(solute)
Hydrogen bonding
Molal BP Elevation Constant
Cation
Law of Multiple Proportions
5. Polyatomic Ions (bonding)
alkene
Covalently w/in themselves - Ionicly bonded w/ each other
Angular Momentum Quantum Number
Molar Mass of Element/ Total Molar Mass %
6. Variable for orientation of orbital (-1 through +1)
eth-
Theory of Relativity
Heat Capacity (C)
m (third quantum number)
7. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Theoretical yield
rate
96500
Pauli Exclusion Principle
8. Forward rxn occurs when
Metalliods
Q<K
f
octahedral
9. 101 -325 Pa
1atm=?Pa
different # of neutrons
Ligand
oct-
10. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Molecular
A Roman numeral
condensation
Equilibrium Expression
11. OIL RIG
Chemical Kinetics
-one
hydrocarbons
Oxidation is Loss Reduction is Gain
12. NO2¹?
Hund's Rule
mol Fraction
Average KE = 1/2(mass)(average speed of all particles)
nitrite
13. Wavelength symbol
bent
lambda
weak acid strong base rxn
cohesion
14. Amount of gravitational force exerted on an object
Law of Conservation of Mass
Dalton's Law of Partial Pressures
Weight
phosphate - sulfide - carbonate - sulfate
15. A molecule having a center of positive charge and a center of negative charge
-1
P1V1/N1T1=P2V2/N2T2
double bond
Dipole Moment
16. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
flouride
q
permanganate
17. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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183
18. Carboxylic acid ending
-oic acid
0.512°C
Colligative properties
spontaneity
19. Carbon & hydrogen compounds
not spontaneous
Oxidizing Agent
red/orange
hydrocarbons
20. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
chromate
Formal Charge
5% rule
chlorate
21. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Molecular Compounds
Law of Definite Proportion
Bonding Pairs
Atmospheric Pressure
22. Mixing of gases
equivalence point
End Point
trigonal planar
Diffusion
23. Larger molecules which have higher mass and therefore electron density have stronger...
London dispersion forces
Sigma Bond
Delta H or Enthalpy Change
Surroundings
24. Passage of gas through tiny orifice
LE Model
Quantum Numbers
Effusion
purple --> pink
25. Weakest IMFs - found in all molecules
-1
second
Linear
London dispersion forces
26. Mass #
PV=nRT
violet
vaporization
# protons + # neutrons
27. Proton (symbol)
Aufbau Principle
p+
Bonding Pairs
0.0821 atm L/mol K
28. H?+OH??H2O
Hybridization
condensation
q
strong acid strong base rxn
29. The rest of the universe (in thermodynamics)
Van't Hoff factor
Work
M1V1=M2V2
surroundings
30. q H2O = ?
3rd law of thermodynamics
purple
C + 273
msAT
31. (N) number of equivalents per liter of solution
Normality
strong acids
1.86°C
weak acid strong base rxn
32. Heat required to raise the system 1°C
London Dispersion Forces
dec-
mol
heat capacity
33. The measurement of heat changes
Quantum Numbers
Calorimetry
critical point
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
34. Color of Cs (flame test)
T-shape
Oxidation is Loss Reduction is Gain
blue
Specific Heat (s)
35. CN¹?
cyanide
Weight
Entropy (S)
oxidizing agent
36. Degree of disorder in a system
Matter
phosphate
entropy (S)
Specific Heat Capacity
37. Non-Ideal Gas Conditions
isothermal
high pressure - low temperature
critical point
Law of Conservation of Energy
38. For significant digits - trailing zeros _____ significant
Electron Spin Quantum Number
are
square pyramidal
Alkali metals
39. AX4E
titrant buret
Closed System
see-saw
% yield
40. A solution that resists a change in pH - contains both a weak acid and its conjugate base
linear
bent
# protons + # neutrons
Buffer
41. Organic w/ -O-
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Hess's Law
ether
effects of IMF
42. If Q>Ksp
a precipitate forms
Enthalpy of Solution
Normality
C=(mass)(specific heat)
43. C2H3O2¹?
acetate
nu
Root Mean Square Velocity
0
44. Oxidation # of Compounds
0
Its element
Q>K
third
45. ?T=k*m(solute)
but-
Molal FP Depression Constant
Molar Mass of Element/ Total Molar Mass %
viscosity
46. The part of the universe one is focused upon (in thermodynamics)
Solubility Product (Ksp)
sulfate
Density
system
47. Energy required for liquid?gas
heat of vaporization
Alkaline earth metals
tetrahedral
# protons + # neutrons
48. 96 -485 C/mol e-
q
Hund's Rule
conjugate base
Faraday
49. (organics) two carbons
green/yellow
eth-
Angular Momentum Quantum Number
second
50. Aldehyde suffix
-al
Zero-Order Rate Law
charge
equilibrium