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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Ionizes to produce H+ ions
Dipole-dipole forces
Hess's Law
Volume Metric Flask & Pipet
Arrhenius Acid

2. ?T=k*m(solute)
-ous acid
permanent gases
Law of Conservation of Mass
Molal FP Depression Constant

3. If Q>Ksp
a precipitate forms
spontaneity
Positive work value; work done on system
0

4. Organic reaction in which two functional groups come together - resulting in the release of water
condensation
Arrhenius base
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
blue

5. To find activation energy use the...
Arrhenius equation
equivalence point
moles solute/kg solvent
system

6. A device used to measure Delta H
s
Calorimeter
Average KE = 1/2(mass)(average speed of all particles)
Hess's Law

7. Hydroxides are soluble or insoluble?
insoluble
trigonal planar
Net Ionic Equation
H

8. NO3¹?
nitrate
Bronsted-Lowry acid
but-
acetate

9. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Solution
Atmospheric Pressure
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
methods of increasing rate

10. Kinetic Energy per molecule
Open System
Adding
+1 - except if bonded to Alkali Metal -1
1/2mv²

11. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
purple --> pink
Formal Charge
cathode
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

12. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
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
endless
Alkali metals

13. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
1 atm
n (first quantum number)
non-

14. Energy needed to vaporize a mole of a liquid
hept-
s (fourth quantum number)
?Hvap
Hess's Law

15. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
AE= AH - RTAn
viscosity
trigonal planar

16. Specific heat of water
Law of Conservation of Mass
4.184
red/orange
t-shape

17. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
triple bond
like
Molecular
-ic acid

18. When ____ significant digits - round answer to least decimal place
Adding
Resonance
Heat
r1/r2

19. 180° - sp
phosphate
hydrocarbons
Linear
Volume Metric Flask & Pipet

20. Elements which have unpaired electrons and highly affected by magnetic fields
paramagnetic
Molarity
Metalliods
Work

21. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Anode
strong acids
STP
Polar Covalent

22. Faraday's constant
Transition metals
Electronegativity
96500
(moles of products that are gasses) - (moles of reactants that are gasses)

23. AX3E2
t-shape
end point
Kinetic Molecular Theory - for ideal gases
methods of increasing rate

24. Entropy in the universe is always...
increasing
Angular Momentum Quantum Number
Buffered Solution
k=Ae^(-Ea/RT)

25. K
Equilibrium constant
endothermic
complex ions
melting

26. r=k[A]^2
Bond enthalpy
Electronegativity
Trigonal Bipyramidal
Second-Order Rate Law

27. Color of Ca (flame test)
isothermal
chlorate
1.38x10?²³J/K
red/orange

28. HF+ OH??H2O
third
methods of increasing rate
indicator
weak acid strong base rxn

29. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
hydrolysis
Solution
Anode
perchlorate

30. q cal = ?
CAT
Acid Dissociation Constant
Antibonding Molecular Orbital
LeChatelier's Principle

31. The rest of the universe (in thermodynamics)
solid CO2
surroundings
s orbitals
square pyramidal

32. Temperature-pressure point after which gas can no longer form liquid
critical point
State Functions
Heat
triple point

33. Ending for alcohols
condensation
work
-ol
Bond Order

34. 0.00°C - 1 atm
Standard Temperature and Pressure
nitrate
soluble
lambda

35. Donates a single H+ Ion (... other prefixes also)
no precipitate forms
Bond Order
Monoprotic
CAT

36. Significant Digits of counted things
Molecular Compounds
endless
cyanide
% yield

37. Forward rxn occurs when
E
system
Q<K
Balmer Series

38. The part of the universe one is focused upon (in thermodynamics)
voltaic cells
Cell Potential (Ecell)
reduction
system

39. Stronger IMF= lower... weaker IMF= higher...
Pressure of H2O must be Subtracted
carbohydrates
vapor pressure
Increase Temperature

40. Solution used in titration
titrant buret
Work
Quantum Model
Zero-Order Rate Law

41. PO4³?
phosphate
Molar Heat Capacity
8.31J/Kmol
square pyramidal

42. SO4²?
sulfate
chloride
yellow --> green
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

43. #NAME?
Normality
E
Pressure
?Hvap

44. Mole Fraction
X of a = moles a/total moles
bond energy
second
sulfite

45. In a given atom no two electrons can have the same set of four quantum numbers
Weight
T-shape
Pauli Exclusion Principle
Law of Multiple Proportions

46. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
T-shape
Heat
Second-Order Half Life

47. Oxidation # of Ions
charge
Weight
carbonate
T-shape

48. Effusion of a gas is inversely proportional to the square root of the molar mass

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49. Like dissolves...
Closed System
Specific Heat Capacity
like
% error

50. (organics) two carbons
eth-
oct-
Specific Heat Capacity
specific heat

Can you answer 50 questions in 15 minutes?

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AP Chemistry

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