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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. Where oxidation occurs
Anode
exothermic
Root Mean Square Velocity
Equivalence Point
2. Pure metal or metal hydride + H20 ->
fusion
base and hydrogen gas
oxidizing agent
d
3. Ester suffix
s (fourth quantum number)
Scientific Method
London dispersion forces
-oate
4. Ether prefix
methoxy-
complex ions
carbohydrates
supercritical fluid
5. Heat needed to change 1 g of substance to 1°C
nitrite
M = square root (3RT/mm)
specific heat
Transition metals
6. The heat changed in a chemical reaction.
strong bases
actual yield/theoretical yield x 100%
Thermochemistry
Law of Conservation of Energy
7. A molecule having a center of positive charge and a center of negative charge
are
Galvanic Cell
violet
Dipole Moment
8. A monoatomic cation takes name from...
alkene
equivalence point
Its element
Aufbau Principle
9. Generally insoluble anions (names)
Allotrope
phosphate - sulfide - carbonate - sulfate
Strong acid weak base rxn
activation energy
10. Ka=[products]^m/[reactants]^n
-oate
eth-
4.184
Acid Dissociation Constant
11. High-speed electrons
Second-Order Rate Law
Beta Particles-
Bond Order
?Tf= kf x molality
12. Measure of the change in enthalpy
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
methods of increasing rate
Antibonding Molecular Orbital
Delta H or Enthalpy Change
13. Electron (symbol)
prop-
e-
AE= AH - RTAn
-1
14. AP doesn't deal with ...-order reaction - don't pick it!
third
titrant buret
base
excess reactant
15. Positive ion
geometric isomers
First-Order Rate Law
Cation
salt bridge
16. 1 sigma bond
Bronsted-Lowry base
3/2RT
single bond
log[H+]
17. Color of Cs (flame test)
blue
yellow --> green
Quantum Mechanical Model
third
18. Does the same as equilibrium expression - except it uses initial concentrations
trigonal pyramidal
force x distance = work done
Molecule
Reaction Quotient (Q)
19. q H2O = ?
conjugate base
Naming Binary Ionic Compounds
Positive work value; work done on system
msAT
20. Occupies the space above and below a sigma bond
-al
Q<K
acid
Pi Bond
21. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
voltaic cells
Magnetic Quantum Number (ml)
eth-
Dalton's Law of Partial Pressures
22. Solution used in titration
moles of solute/ L of solution
g solute/g solvent x 100
titrant buret
different # of neutrons
23. Variable for orientation of orbital (-1 through +1)
Polar Covalent
m (third quantum number)
Van't Hoff factor
Overall Reaction Order
24. ClO3²?
charge
Reaction Quotient (Q)
chlorate
First-Order Rate Law
25. Elements which have unpaired electrons and highly affected by magnetic fields
geometric isomers
Electron Spin Quantum Number
base and hydrogen gas
paramagnetic
26. A solution that resists a change in its pH
-2 - with peroxide -1
Matter
isothermal
Buffered Solution
27. A measure of resistance of an object to a change in its state of motion
Limiting reactant
ether
Mass
spontaneous
28. The driving force for a spontaneous is an increase in entropy of the universe
1.38x10?²³J/K
Entropy (S)
Strong acid weak base rxn
% error
29. Ending for alcohols
Boltzmann distribution
-ol
X of a = moles a/total moles
effects of IMF
30. Polyatomic Ions (bonding)
pent-
Bond Order
Covalently w/in themselves - Ionicly bonded w/ each other
heat of fusion
31. Energy needed to vaporize a mole of a liquid
CAT
v3RT/M(in kg)
?Hvap
Naming Binary Ionic Compounds
32. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
Bond Order
Weight
condensation
33. Type of system in which the energy and mass may leave or enter
Open System
Acid + Base --> Salt + Water
0 degrees C - 1 atm
Law of Conservation of Mass
34. ClO2¹?
Molecular Compounds
C + 273
chlorite
Pressure
35. ClO4¹?
-(P)(Change in V)
Scientific Method
not spontaneous
perchlorate
36. Universal IMF for nonpolar molecules
geometric isomers
Finding Empirical Formulas
London dispersion forces
moles solute/kg solvent
37. Atoms with the same number of protons but a different number of neutrons
Amount of atoms present
Ag+ - Pb2+ - Hg2+
Isotopes
chloride
38. AX3
Integrated First-Order Rate Law
Law of Multiple Proportions
phosphate - sulfide - carbonate - sulfate
trigonal planar
39. Weakest IMFs - found in all molecules
0
London dispersion forces
a precipitate forms
E
40. Carboxylic acid ending
-oic acid
Its element
standard solution
Bronsted-Lowry acid
41. Delta H (AH) = ?
Nernst Equation
q/moles
electron affinity
adiabatic
42. Organic w/ -O-
allotrope
ether
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
43. Color of Sr (flame test)
Normality
linear
Bonding Pairs
red
44. Symbol for Total Heat absorbed or released
see-saw
q
trigonal pyramidal
a precipitate forms
45. (organics) two carbons
Theory of Relativity
Q>K
eth-
-(P)(Change in V)
46. Actual Yield/Theoretical Yield*100%
Acid Dissociation Constant
Negative work value; work done by system
pent-
Percent Yield
47. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
not spontaneous
-ic acid
octahedral
48. 2+ charge
Alpha Particles-
l (second quantum number)
Electron Spin Quantum Number
Trigonal Bipyramidal
49. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
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
Pressure of H2O must be Subtracted
Resonance
conjugate acid
50. AX5E
n0
square pyramidal
iodide
Metalliods