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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 transfer of energy between two objects due to temperature difference
Heat
Q<K
heat of fusion
period
2. 180° - sp
salt bridge
Linear
3/2RT
% yield
3. Different form of same element
0.0826Latm/Kmol
London dispersion forces
allotrope
nu
4. Electron pairs found in the space between the atoms
Ideal Gas Law
square pyramidal
Bonding Pairs
Zero-Order Half Life
5. Speed per molecule of gas
v3kT/m
equilibrium
f
Polar Covalent
6. The line running between the atoms
methoxy-
Sigma Bond
Atomic Mass Unit
Hess's Law
7. The minimum energy that molecules must possess for collisions to be effective - Ea
diamagnetic
activation energy
rate gas A/rate gas B = square root (mm A/ mm B)
dec-
8. (organics) nine carbons
Closed System
non-
bent
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
9. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
actual yield/theoretical yield x 100%
Hund's Rule
geometric isomers
Colligative properties
10. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
endless
standard solution
pent-
11. Electron (symbol)
non-
Molecular Orbitals (MOs)
e-
Polar Covalent
12. Heat required to raise the system 1°C
heat capacity
Strong acid weak base rxn
Law of Multiple Proportions
wavelength
13. All _________ compounds are electrolytes
Diffusion
Anode
equilibrium
Ionic
14. Substance that - when dissolved - is conductive
Its element
electrolyte
sulfide
1.86°C
15. Mass reactants= mass products
Molecular Compounds
-oate
Law of Conservation of Mass
-oic acid
16. How to Find an Empirical Formula Given Grams
2nd law of thermodynamics
C + 273
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Integrated Rate Law
17. Passage of gas through tiny orifice
soluble
Effusion
Buffered Solution
Electron Spin Quantum Number
18. Chemical composition of dry ice
solid CO2
electron affinity
anode
p+
19. Planck's constant - used to calculate energy w/frequency
6.63x10?³4Js
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Endothermic
reduction
20. The likelihood that a rxn will occur "by itself"
Constant Volume
trigonal pyramidal
spontaneity
precipitate
21. Pressure Units/Conversions
1 atm = 760 mmHg = 101.3 kPa
Hybridization
electrolyte
Linear
22. (organics) five carbons
actual yield/theoretical yield x 100%
pent-
Buffer
permanent gases
23. % yield
actual yield/theoretical yield x 100%
purple
Joule
Molarity
24. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Molecular
Average KE = 1/2(mass)(average speed of all particles)
ether
Q>K
25. These orbitals are perpendicular
v3kT/m
p orbitals
Quantum Model
Gamma Ray-
26. Amine prefix
Amino-
charge
non-
Second-Order Rate Law
27. Proton donors
pi=(nRT)/v
square pyramidal
Bronsted-Lowry acid
London dispersion forces
28. Gain of electrons - decrease in oxidation #
Trigonal Bipyramidal
reduction
Balmer Series
are not
29. Theoretical yield-experimental yield/theoretical yieldx100
Mass
% error
yellow
sulfide
30. Ptotal=P1+P2+P3+...
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31. Half cell in which reduction occurs
s (fourth quantum number)
Arrhenius Base
-2 - with peroxide -1
cathode
32. A solution that resists a change in its pH
Multiplying
Barometer
adiabatic
Buffered Solution
33. The total entropy is always increasing - all systems tend towards maximum entropy
0
Standard Temperature and Pressure
2nd law of thermodynamics
square pyramidal
34. Color of Na (flame test)
period
yellow
bromate
moles of solute/ L of solution
35. Elements which have unpaired electrons and highly affected by magnetic fields
Arrhenius equation
Osmotic Pressure
paramagnetic
Acid + Base --> Salt + Water
36. Average Kinetic Energy Formula
Heat
single bond
Boltzmann distribution
Average KE = 1/2(mass)(average speed of all particles)
37. Within a sublevel - place one e? per orbital before pairing them
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38. Force that holds atoms together
precipitate
Chemical Bonds
charge
Second-Order Rate Law
39. Color of Li (flame test)
Amphoteric
Pressure of H2O must be Subtracted
red
Cation
40. Aldehyde suffix
-al
Surroundings
Hydrogen bonding
d orbitals
41. In a given atom no two electrons can have the same set of four quantum numbers
Specific Heat Capacity
standard solution
Pauli Exclusion Principle
solid CO2
42. F¹?
Molarity
cohesion
Density
flouride
43. Dalton's Law of Partial Pressures (to find partial pressure formula)
insoluble
pi=(nRT)/v
P of a =(X of a)(total pressure)
Equivalence Point
44. Mols A/ total mols - XA
mol Fraction
bent
Root Mean Square Velocity
Barometer
45. (organics) two carbons
1/2mv²
high pressure - low temperature
?Tb= kb x molality
eth-
46. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
adhesion
hydroxide
violet
London Dispersion Forces
47. Unusually strong dipole forces found when H is bonded to N - O - or F
Cell Potential (Ecell)
Hydrogen bonding
blue-green
LeChatelier's Principle
48. Measure of the average kinetic energy of all the particles in a substance
-oate
conjugate base
Temperature
base
49. Matter can't be created nor destroyed
Law of Conservation of Mass
Specific Heat (s)
first
surroundings
50. What is defined by you taken from the whole universe
Bond Order
e-
Hydrogen bonding
System