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AP Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Solution in flask being titrated
m (third quantum number)
ionic
6.63x10?³4Js
analyte

2. Mixing of gases
Diffusion
1st law of thermodynamics
Quantum Numbers
Law of Conservation of Energy

3. AX5E
titrant buret
square pyramidal
methoxy-
-1

4. Metal oxide + H20 ->
reduction
base
hept-
Root Mean Square Velocity

5. Composition Formula
Molar Mass of Element/ Total Molar Mass %
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Isolated System
AE = q + w

6. AX5E
Angular Momentum Quantum Number
violet
Osmotic Pressure
square pyramidal

7. r=k[A]^2
Second-Order Rate Law
Quantum Numbers
Beta Particles-
1atm=?Pa

8. l=2
State Functions
d
phosphate - sulfide - carbonate - sulfate
Graham's Law

9. AX6
salt bridge
0
effects of IMF
octahedral

10. [A]=-kt + [A]0
nitrate
Integrated Zero-Order Rate Law
supercritical fluid
1/2mv²

11. Substance in which something is dissolved in a solution (higher [ ])
Solvent
oxide gas and water
Polar Covalent
not spontaneous

12. 96 -485 C/mol e-
perchlorate
electrolyte
Faraday
3/2RT

13. A device used to measure Delta H
rate gas A/rate gas B = square root (mm A/ mm B)
Law of Conservation of Mass
Anion
Calorimeter

14. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Acids
Acid + Base --> Salt + Water
Atmospheric Pressure
purple --> pink

15. A device in which chemical energy is changed to electrical energy
isothermal
titrant buret
Amphoteric
Galvanic Cell

16. AX5
Force = mass x acceleration
Temperature
Temperature
trigonal bipyramidal

17. Oxidation # of Oxygen
green/yellow
Amphoteric
-2 - with peroxide -1
Kinetic Molecular Theory - for ideal gases

18. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Isolated System
q
oxide gas and water
Resonance

19. R=
0.0826Latm/Kmol
Law of Definite Proportion
exothermic
red

20. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
AE= AH - RTAn
Ag+ - Pb2+ - Hg2+
Joule

21. (# of lone pair e-)+1/2(# of shared e-)
-(P)(Change in V)
van't Hoff Factor
Reducing Agent
Valence Electrons(assigned)

22. Volume of gas @STP
Strong acid weak base rxn
Arrhenius equation
sulfide
22.4L

23. Temperature-pressure combination at which solid - liquid - and gas states appear
hydroxide
sulfite
hydrocarbons
triple point

24. Energy (definition)
isothermal
State Functions
C + 273
force x distance = work done

25. Arrhenius equation
sulfate
Allotrope
Anion
k=Ae^(-Ea/RT)

26. Reverse rxn occurs when
cathode
Q>K
catalyst
Oxidation is Loss Reduction is Gain

27. Force acting over distance
Integrated Zero-Order Rate Law
Work
Solution
Molecular Orbitals (MOs)

28. Elements in groups 3-12
Q>K
96500
Kinetic Molecular Theory - for ideal gases
Transition metals

29. Horizontals on the periodic table
Electron Spin Quantum Number
k=Ae^(-Ea/RT)
period
Acid + Base --> Salt + Water

30. O²?
octahedral
1 atm
oxidation
oxide

31. A solution that resists a change in its pH
Buffered Solution
Solvent
van't Hoff Factor
red

32. Spontaneous emission of radiation
increasing
Radioactivity
hex-
ionic

33. Hydroxides are soluble or insoluble?
insoluble
Temperature
Radioactivity
alkyne

34. Oxidation # of Hydrogen
Average KE = 1/2(mass)(average speed of all particles)
+1 - except if bonded to Alkali Metal -1
Aufbau Principle
Bond enthalpy

35. MnO4¹?
van't Hoff Factor
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
permanganate
force x distance = work done

36. Non-Ideal Gas Conditions
high pressure - low temperature
insoluble
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
viscosity

37. NH4¹?
-al
Quantum Numbers
ammonium
Theory of Relativity

38. r=k
wavelength
oxidation
standard solution
Zero-Order Rate Law

39. Phase change from gas to solid
deposition
n (first quantum number)
Le Chatelier's Principle
endless

40. A solution used in titrations whose concentration is known
1.38x10?²³J/K
% yield
standard solution
Arrhenius base

41. Energy required for liquid?gas
spontaneous
heat of vaporization
precipitate
Molal BP Elevation Constant

42. Ending for alcohols
Molality
-ol
Arrhenius base
Acids

43. Mol/kg of solvent - used in calculating colligative properties
Molality
ether
critical point
Standard Temperature and Pressure

44. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
viscosity
blue-violet
Molal BP Elevation Constant

45. Raising heat - adding catalyst - heighten concentration - bigger surface area
Quantum Numbers
Alpha Particles-
methods of increasing rate
Colligative properties

46. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
anode
Finding Empirical Formulas
precipitate
Its root and adding -ide

47. Substances w/ critical temperatures below 25°C
hept-
permanent gases
Law of Conservation of Mass
Integrated Zero-Order Rate Law

48. negative ion
Anion
s orbitals
k=Ae^(-Ea/RT)
like

49. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
sulfite
phosphate - sulfide - carbonate - sulfate
Atomic Mass Unit

50. Two molecules with identical connectivity but different geometries
van't Hoff Factor
0.0826Latm/Kmol
Le Chatelier's Principle
geometric isomers

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AP Chemistry

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