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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. Organic w/ -O-
Enthalpy of Solution
ether
soluble
e-
2. Molecules' tendency to stick to one another
cohesion
insoluble
iodide
Average KE = 1/2(mass)(average speed of all particles)
3. AX6
octahedral
van't Hoff Factor
Ligand
Law of Conservation of Mass
4. A solid or gas that can be formed when 2 or more aqueous reactants come together
specific heat
n0
strong bases
precipitate
5. Heat capacity formula
2nd law of thermodynamics
Molality
Joule
C=(mass)(specific heat)
6. ?H when 1 mol of bonds is broken in the gaseous state
Ligand
STP
Bond enthalpy
Increase Temperature
7. 1/([A]0*k)
Second-Order Half Life
Electron Spin Quantum Number
Formal Charge
permanganate
8. Formula used when diluting stock solution (to find amount of water or stock needed)
Speed of light
M1V1=M2V2
Constant Volume
square planar
9. Type of system in which the energy and mass may leave or enter
heat capacity
-ol
First-Order Half Life
Open System
10. Carbon & hydrogen compounds
purple
hydrocarbons
insoluble
endothermic
11. Ketone suffix
AE= AH - RTAn
-oate
-one
endless
12. In a given atom no two electrons can have the same set of four quantum numbers
cathode
Specific Heat Capacity
tetrahedral
Pauli Exclusion Principle
13. Degree of disorder in a system
Root Mean Square Velocity
cyanide
Colligative properties
entropy (S)
14. Ionizes to produce OH- Ions
Arrhenius Base
Percent Yield
different # of neutrons
hydrocarbons
15. 1/[A]=kt + 1/[A]0
Lone Pair
charge
system
Integrated Second-Order Rate Law
16. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
triple point
Manometer
1.86°C
permanent gases
17. Dalton's Law of Partial Pressures (to find partial pressure formula)
Barometer
Calorimetry
allotrope
P of a =(X of a)(total pressure)
18. ?Hsoln=?H1+?H2+?H3+...
Magnetic Quantum Number (ml)
adhesion
Enthalpy of Solution
condensation
19. Speed per molecule of gas
AH
v3kT/m
Acid + Base --> Salt + Water
geometric isomers
20. Positive ion
Cation
trigonal pyramidal
freezing
Oxidizing Agent
21. Like dissolves...
like
Its element
Angular Momentum Quantum Number
hydroxide
22. Energy needed to break a bond
Ampere
strong acids
Heisenberg Uncertainty Principle
bond energy
23. 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)
96500
Theoretical yield
square planar
Kinetic Molecular Theory - for ideal gases
24. R=
Law of Definite Proportion
0.0826Latm/Kmol
Law of Conservation of Energy
Principal Quantum Number
25. Isotope
Endothermic
different # of neutrons
Molal FP Depression Constant
Linear
26. Variable for energy of e- - goes from 1 -2 -3 on up
charge
n (first quantum number)
prop-
lambda
27. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Formal Charge
-oic acid
0.0826Latm/Kmol
0 degrees C - 1 atm
28. The reactant in the oxidizing reaction that forces the reduction reaction to occur
precipitate
trigonal planar
Reducing Agent
strong acids
29. Mols A/ total mols - XA
Le Chatelier's Principle
Its element
mol Fraction
wavelength
30. Ability of an atom in a molecule to attract shared electrons to itself
Electronegativity
bromate
-ous acid
Tetrahedral
31. A solution that resists a change in its pH
Acids
perchlorate
Buffered Solution
Limiting reactant
32. An equilibrium expression
Solubility Product (Ksp)
Ionic
Linear
Bronsted-Lowry Base
33. PO4³?
d orbitals
Joule
phosphate
Law of Multiple Proportions
34. Force acting over distance
deposition
Kinetic Molecular Theory - for ideal gases
octahedral
Work
35. Resistance to flow
Strong acid weak base rxn
effects of IMF
viscosity
Molecular Compounds
36. Within a sublevel - place one e? per orbital before pairing them
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37. AX5E
condensation
Positive work value; work done on system
square pyramidal
M = square root (3RT/mm)
38. Speed of Diffusion/Effusion formula
0
v3RT/M(in kg)
sulfite
rate gas A/rate gas B = square root (mm A/ mm B)
39. A homogeneous mixture with 1 phase
Solution
msAT
nu
Angular Momentum Quantum Number
40. Describe various properties of one orbital
Quantum Numbers
e-
Boltzmann distribution
T-shape
41. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Heat Capacity (C)
Finding Empirical Formulas
electron affinity
Buffer
42. Symbol for Total Heat absorbed or released
triple bond
q
alkane
hept-
43. How to Balance a Redox Equation
CAT
electrolyte
Arrhenius base
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
44. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
?Tb= kb x molality
rate
Heisenberg Uncertainty Principle
activated complex (transition state)
45. Type of system in which the energy may escape - but the mass is conserved
Enthalpy of Solution
Acid + Base --> Salt + Water
Closed System
iodide
46. Elements which have unpaired electrons and highly affected by magnetic fields
Acids
# protons (atom is defined by this)
paramagnetic
m (third quantum number)
47. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Galvanic Cell
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
p
not spontaneous
48. Theoretical yield-experimental yield/theoretical yieldx100
% error
LeChatelier's Principle
r1/r2
1 atm = 760 mmHg = 101.3 kPa
49. Gas to solid
AE= AH - RTAn
Reducing Agent
deposition
activated complex (transition state)
50. (organics) one carbon
Ionic
wavelength
meth-
Density