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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.
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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. Spectrum of light when an electron drops to energy level n=2
mol
T-shape
Balmer Series
Overall Reaction Order
2. Color of Ca (flame test)
eth-
pent-
red/orange
Arrhenius equation
3. Osmotic pressure=MRT
Pressure
Root Mean Square Velocity
Volt
Osmotic Pressure
4. neutron (symbol)
yellow
experimental yield
n0
Weight
5. Expresses how the concentrations depend on time
Integrated Rate Law
equivalence point
force x distance = work done
?Tf= kf x molality
6. Puts OH? into solution
reduction agent
Arrhenius base
Constant Pressure
octahedral
7. Reactant that's completely used up in a chemical reaction
Limiting reactant
octahedral
Angular Momentum Quantum Number
d
8. Gas to liquid
base
condensation
single bond
phosphate - sulfide - carbonate - sulfate
9. Where oxidation occurs
-oate
+1 - except if bonded to Alkali Metal -1
Naming Binary Ionic Compounds
Anode
10. H?+NH3?NH4
Strong acid weak base rxn
strong bases
Molar Mass of Element/ Total Molar Mass %
Matter
11. Increase Pressure
Decrease Volume and Increase Temperature
Bond Energy
vapor pressure
Cathode
12. #NAME?
Oxidizing Agent
E
Hess's Law
carbonate
13. As protons are added to the nucleus - electrons are similarly added
Its root and adding -ide
Aufbau Principle
Allotrope
M = square root (3RT/mm)
14. Each orbital can hold two e?s each w/ opposite spins
Dalton's Law of Partial Pressures
Pauli Exclusion Principle
First-Order Rate Law
rate law
15. Change in Energy = ? (in terms of constant pressure; for gasses)
Weight
isothermal
salt bridge
AE= AH - RTAn
16. Significant Digits of Conversion Factors
endless
seesaw
Alkaline earth metals
exothermic
17. Point at which solid?liquid occurs
melting point
Bronsted-Lowry Acid
Hess's Law
# protons + # neutrons
18. 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
LE Model
specific heat
exothermic
moles solute/kg solvent
19. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
First-Order Rate Law
g solute/g solvent x 100
Overall Reaction Order
hydrolysis
20. The reactant in the oxidizing reaction that forces the reduction reaction to occur
-one
Oxidizing Agent
Reducing Agent
octahedral
21. Resistance to flow
strong acids
viscosity
Mass
weak acid strong base rxn
22. (organics) nine carbons
octahedral
Atmospheric Pressure
non-
Law of Multiple Proportions
23. Mass #
perchlorate
# protons + # neutrons
Trigonal Planar
Matter
24. Positive enthalpy - heat flows into system
End Point
chloride
STP
endothermic
25. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
-one
cyanide
Cg=kPg
Thermochemistry
26. Kinetic Energy per mol
Increase Temperature
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
3/2RT
Arrhenius acid
27. Variable for spin of electron (+.5 or -.5)
s (fourth quantum number)
tetrahedral
sublimation
Ampere
28. Color of Ba (flame test)
zero
e-
Heat
green/yellow
29. Absorbs/takes in heat (positive value)
group
Endothermic
heat capacity
cathode
30. Liquid to gas
specific heat
vaporization
group
equivalence point
31. If Q<Ksp
0 degrees C - 1 atm
no precipitate forms
-(q of H2O + q of cal)
Pressure
32. E?s fill the lowest energy orbital first - then work their way up
allotrope
red
-al
Aufbau Principle
33. A single substance that may be an acid or a base (i.e. water)
Amphoteric
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
boiling point
Colligative properties
34. Molarity (M)
moles of solute/ L of solution
allotrope
indicator
P1V1/N1T1=P2V2/N2T2
35. Energy needed to vaporize a mole of a liquid
Solute
?Hvap
Pi Bond
Integrated Rate Law
36. x can be ignored when % ionization is <5%
5% rule
f
condensation
Solvent
37. E=mc^2
Antibonding Molecular Orbital
Theory of Relativity
Constant Volume
Surroundings
38. The minimum energy that molecules must possess for collisions to be effective - Ea
activation energy
Joule
tetrahedral
chloride
39. Variable for energy of e- - goes from 1 -2 -3 on up
increasing
catalyst
Chemical Bonds
n (first quantum number)
40. AX6
Monoprotic
base
octahedral
Arrhenius Acid
41. Actual Yield/Theoretical Yield*100%
cyanide
rate gas A/rate gas B = square root (mm A/ mm B)
Percent Yield
Decrease Volume and Increase Temperature
42. To find activation energy use the...
Beta Particles-
Buffer
Arrhenius equation
electron affinity
43. Pressure Units/Conversions
E
1 atm = 760 mmHg = 101.3 kPa
Ideal Gas Law
oct-
44. AX4
p
Law of Definite Proportion
tetrahedral
Bronsted-Lowry acid
45. Liquid to solid
freezing
-one
purple --> pink
square pyramidal
46. Spontaneous emission of radiation
Solvent
condensation
Radioactivity
-ous acid
47. Planck's constant - used to calculate energy w/frequency
Equilibrium constant
endless
6.63x10?³4Js
surroundings
48. AX3E
hydrocarbons
amine
carbonate
trigonal pyramidal
49. Raoult's Law - relations between vapor pressure and concentrations
Manometer
period
prop-
P1= X1P1°
50. Matter can't be created nor destroyed
Oxidation is Loss Reduction is Gain
4.184
Amino-
Law of Conservation of Mass
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