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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. Substances that form H+ when dissolved in water; proton donors
octahedral
Chemical Kinetics
Acids
octahedral
2. AX6
Closed System
octahedral
Its element
Increase Temperature
3. CN¹?
zero
hept-
equilibrium
cyanide
4. These orbitals are diagonal
flouride
Lone Pair
d orbitals
Joule
5. Mass reactants= mass products
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
# protons + # neutrons
pent-
Law of Conservation of Mass
6. U(rms)=(3RT/M)^1/2
heat capacity
1atm=?Pa
Root Mean Square Velocity
Constant Pressure
7. E=mc^2
Aufbau Principle
Anion
Theory of Relativity
Multiplying
8. Absorbs/takes in heat (positive value)
k=Ae^(-Ea/RT)
Graham's Law
Endothermic
reduction agent
9. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Equilibrium Expression
boiling point
sulfide
diamagnetic
10. Temperature-pressure point after which gas can no longer form liquid
critical point
not spontaneous
oxidation
Average KE = 1/2(mass)(average speed of all particles)
11. R=
n0
8.31J/Kmol
adiabatic
diamagnetic
12. AX4E2
square planar
Aufbau Principle
% yield
permanganate
13. AX2 - AX2E3
wavelength
linear
boiling point
strong acids
14. Solution used in titration
titrant buret
meth-
Enthalpy of Solution
v3RT/M(in kg)
15. (organics) double-bonded compound
square planar
condensation
sulfate
alkene
16. All _________ compounds are electrolytes
alkene
Law of Definite Proportion
Ionic
Finding Empirical Formulas
17. These orbitals are perpendicular
Cell Potential (Ecell)
ammonium
oxide gas and water
p orbitals
18. Electron (symbol)
e-
s orbitals
condensation
diamagnetic
19. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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20. Molecules' tendency to stick to the container
ether
Constant Volume
iodide
adhesion
21. How to Find an Empirical Formula Given Grams
London Dispersion Forces
Molal FP Depression Constant
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Resonance
22. A molecule having a center of positive charge and a center of negative charge
Bronsted-Lowry Base
activated complex (transition state)
Solution
Dipole Moment
23. Elements on staircase on periodic table
Metalliods
like
eth-
P1= X1P1°
24. These orbitals are spherical
s orbitals
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
p
25. K
Calorimeter
Van't Hoff factor
period
Equilibrium constant
26. Amount of gravitational force exerted on an object
Weight
Hybridization
Solubility Product (Ksp)
London dispersion forces
27. 760mmHg/Torr
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
1atm=?mmHg/Torr
Specific Heat Capacity
hydroxide
28. 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)
Kinetic Molecular Theory - for ideal gases
Exothermic
Integrated Second-Order Rate Law
adhesion
29. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
6.63x10?³4Js
Calorimeter
Atmospheric Pressure
30. Lowers activation energy
flouride
catalyst
phosphate
Ag+ - Pb2+ - Hg2+
31. Only contains ions that change in reaction
linear
C=(mass)(specific heat)
fusion
Net Ionic Equation
32. A single substance that may be an acid or a base (i.e. water)
Alkali metals
blue-violet
oxidizing agent
Amphoteric
33. Boiling point elevation formula
k=Ae^(-Ea/RT)
1.86°C
Cell Potential (Ecell)
?Tb= kb x molality
34. For significant digits - trailing zeros _____ significant
are
Isolated System
Molarity
Amphoteric
35. Group 1 and heavier Group 2 bases
M = square root (3RT/mm)
Second-Order Rate Law
p+
strong bases
36. Work = ?
Arrhenius base
purple --> pink
% yield
-(P)(Change in V)
37. Color of Ca (flame test)
Temperature
(moles of products that are gasses) - (moles of reactants that are gasses)
-ic acid
red/orange
38. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Transition metals
zero
yellow --> green
Chemical Bonds
39. A device in which chemical energy is changed to electrical energy
amine
Delta H or Enthalpy Change
Galvanic Cell
Graham's Law
40. 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
# protons + # neutrons
London Dispersion Forces
Hund's Rule
supercritical fluid
41. BrO3¹?
-oate
bromate
Volume Metric Flask & Pipet
Dipole-dipole forces
42. Ketone suffix
-one
s orbitals
1 atm = 760 mmHg = 101.3 kPa
Pressure
43. Elements which have all electrons paired and relatively unaffected by magnetic fields
Second-Order Rate Law
square planar
-2 - with peroxide -1
diamagnetic
44. AX3E2
First-Order Rate Law
mol
T-shape
conjugate acid
45. A solid or gas that can be formed when 2 or more aqueous reactants come together
effects of IMF
precipitate
?Hvap
Equilibrium constant
46. In a given atom no two electrons can have the same set of four quantum numbers
Increase Temperature
purple
-oic acid
Pauli Exclusion Principle
47. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
sublimation
spontaneous
trigonal planar
analyte
48. When n=5 ->2 - color=
Adding
Cg=kPg
anode
blue-violet
49. Instrument used to measure the pressure of atmospheric gas
Barometer
eth-
M1V1=M2V2
Alkali metals
50. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Root Mean Square Velocity
1atm=?mmHg/Torr
Percent Yield
Manometer
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