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Test your basic knowledge |
AP Chemistry
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Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
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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. Change in Energy (AE) = ? (in terms of work)
melting
are
1st law of thermodynamics
AE = q + w
2. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
high pressure - low temperature
Ionic Compounds
Net Ionic Equation
Amount of atoms present
3. (organics) five carbons
insoluble
pent-
trigonal planar
first
4. H + donor
Barometer
0.512°C
Equilibrium Expression
Bronsted-Lowry Acid
5. SO4²?
Specific Heat Capacity
-1
T-shape
sulfate
6. The actual amount of product produced in an experiment
salt bridge
strong acid strong base rxn
experimental yield
dec-
7. Force that holds atoms together
Cathode
Chemical Bonds
Faraday
Ag+ - Pb2+ - Hg2+
8. NH4¹?
activated complex (transition state)
ammonium
period
seesaw
9. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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10. kb of water
v3RT/M(in kg)
% yield
0.512°C
Equilibrium constant
11. When n=5 ->2 - color=
viscosity
blue-violet
1/2mv²
Enthalpy of Solution
12. neutron (symbol)
n0
First-Order Half Life
insoluble
anode
13. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
+1 - except if bonded to Alkali Metal -1
reduction
Ligand
14. Liquid to gas
vaporization
Integrated First-Order Rate Law
0
Work
15. Color of Ca (flame test)
Oxidation is Loss Reduction is Gain
pent-
Zero-Order Half Life
red/orange
16. Loss of electrons - increase in oxidation #
Resonance
oxidation
zero
STP
17. Change that occurs at constant temperature
no precipitate forms
isothermal
Kinetic Molecular Theory - for ideal gases
trigonal planar
18. Cl¹?
experimental yield
chloride
paramagnetic
22.4L
19. The total energy of the universe is constant - all systems tend towards minimum energy
3rd law of thermodynamics
cathode
Octahedral
1st law of thermodynamics
20. Molecules' tendency to stick to one another
g solute/g solvent x 100
oxide gas and water
phosphate
cohesion
21. In ideal gas law problem - when it says "atmospheric" ...
activated complex (transition state)
are
Pressure of H2O must be Subtracted
square pyramidal
22. MnO4¹?
?Tb= kb x molality
are not
Nodes
permanganate
23. Oxidation # of Oxygen
Second-Order Half Life
N=N.(0.5)^time/time half-life
Isolated System
-2 - with peroxide -1
24. Speed of light - C
Diffusion
3.0x108m/s
Alkaline earth metals
1st law of thermodynamics
25. ClO3²?
Acids
chlorate
prop-
Bronsted-Lowry Base
26. Mole Fraction
k=Ae^(-Ea/RT)
X of a = moles a/total moles
Quantum Mechanical Model
sulfate
27. Bomb Calorimeter
Integrated Rate Law
Hess's Law
Constant Volume
(moles of products that are gasses) - (moles of reactants that are gasses)
28. Larger molecules which have higher mass and therefore electron density have stronger...
nu
Naming Binary Ionic Compounds
London dispersion forces
Molar Mass of Element/ Total Molar Mass %
29. Generally insoluble anions (names)
oxide
Second-Order Rate Law
phosphate - sulfide - carbonate - sulfate
Decrease Volume and Increase Temperature
30. Liquid to solid
freezing
LeChatelier's Principle
r1/r2
Delta H or Enthalpy Change
31. Ether prefix
methoxy-
5% rule
nu
0
32. An equilibrium expression
Solubility Product (Ksp)
8.31J/Kmol
Molarity
Linear
33. Puts OH? into solution
Arrhenius base
supercritical fluid
Specific Heat (s)
Net Ionic Equation
34. R=
8.31J/Kmol
mol Fraction
First-Order Rate Law
titrant buret
35. Entropy in the universe is always...
experimental yield
nu
increasing
Barometer
36. Cr2O7²?
Buffer
hydrocarbons
5% rule
dichromate
37. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
no precipitate forms
Molal FP Depression Constant
Open System
38. Oxidation # of free elements
Specific Heat (s)
Molecular
0
96500
39. When n=4 ->2 - color=
v3kT/m
square pyramidal
blue-green
voltaic cells
40. Dirrect Method Formula
Electronegativity
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
single bond
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
41. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
activated complex (transition state)
Bases
-ous acid
supercritical fluid
42. AX4E
green/yellow
boiling point
Trigonal Bipyramidal
see-saw
43. IMF that exists in polar molecules
Entropy (S)
Dipole-dipole forces
Oxidizing Agent
are
44. How to Balance a Redox Equation
Reducing Agent
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
0
s orbitals
45. Driving force of the electrons
Principal Quantum Number
alkane
Cell Potential (Ecell)
nitrate
46. Solid to liquid
q
Linear
Heat
melting
47. Has values from 0 to (n-1); tells shape of atomic orbitals
Chemical Bonds
electrolyte
Specific Heat Capacity
Angular Momentum Quantum Number
48. Polyatomic Ions (bonding)
eth-
Covalently w/in themselves - Ionicly bonded w/ each other
d orbitals
actual yield/theoretical yield x 100%
49. Energy needed to vaporize a mole of a liquid
square planar
Cell Potential (Ecell)
?Hvap
Manometer
50. J/°Cg or J/Kg
Cell Potential (Ecell)
Specific Heat Capacity
endless
Net Ionic Equation
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