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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. I=moles of particles/moles of solute dissolved

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2. (organics) three carbons
prop-
Volt
Arrhenius Base
heat of fusion

3. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
double bond
phosphate
equilibrium
Molecular Compounds

4. Loss of electrons - increase in oxidation #
Octahedral
Equilibrium Expression
carbohydrates
oxidation

5. l=2
d
Molarity
System
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

6. 0°C and 1 atm
sulfite
hex-
STP
Zero-Order Rate Law

7. C2O4²?
Balmer Series
oxalate
r1/r2
experimental yield

8. Puts OH? into solution
Delta H or Enthalpy Change
Buffer
Arrhenius base
Integrated First-Order Rate Law

9. Ptotal=Pa+Pb+Pc....

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10. When n=6 ->2 - color=
violet
Integrated Second-Order Rate Law
Normality
1st law of thermodynamics

11. (organics) triple-bonded compound
viscosity
alkyne
Dipole-dipole forces
mol

12. AX4E2
Law of Multiple Proportions
X of a = moles a/total moles
Lone Pair
square planar

13. Mass reactants= mass products
Law of Conservation of Mass
square pyramidal
tetrahedral
Endothermic

14. A measure of resistance of an object to a change in its state of motion
1/2mv²
trigonal bipyramidal
Mass
sublimation

15. Color of K (flame test)
Amino-
Anion
Electronegativity
purple

16. Specific heat of water
equivalence point
diamagnetic
4.184
STP

17. ?T=k*m(solute)
equivalence point
end point
specific heat
Molal FP Depression Constant

18. Ideal Gas Law Formula
PV=nRT
Colligative properties
square planar
system

19. Ionizes to produce OH- Ions
activated complex (transition state)
Arrhenius Base
wavelength
Kinetic Molecular Theory - for ideal gases

20. Wavelength symbol
lambda
hept-
?Hvap
Molarity

21. To find activation energy use the...
Equilibrium Expression
vapor pressure
Arrhenius equation
Molar Mass of Element/ Total Molar Mass %

22. Electrons in a hydrogen atom move around the nucleus only in circular orbits
log[H+]
not spontaneous
Quantum Model
dec-

23. Isotope
0.0821 atm L/mol K
different # of neutrons
Effusion
Arrhenius Acid

24. Mass/volume
permanganate
endless
Density
conjugate acid

25. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Root Mean Square Velocity
96500
Hund's Rule
soluble

26. r=k[A]^2
AH
Second-Order Rate Law
red
double bond

27. If anion ends in -ite - acid name ends in...
-ous acid
Matter
0
Graham's Law

28. Electron pairs found in the space between the atoms
moles solute/kg solvent
Bonding Pairs
Surroundings
Molarity

29. Speed per molecule of gas
Law of Multiple Proportions
1 atm
v3kT/m
spontaneous

30. Cation first - anion second
Open System
8.31J/Kmol
1/2mv²
Naming Binary Ionic Compounds

31. Oxidation # of Ions
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 degrees C - 1 atm
Equilibrium Expression
charge

32. Mass #
# protons + # neutrons
sublimation
d
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

33. The entropy of a pure perfectly formed crystal @0K is 0
6.63x10?³4Js
cohesion
-1
3rd law of thermodynamics

34. Change in Energy (AE) = ? (in terms of work)
Faraday
AE = q + w
Allotrope
methods of increasing rate

35. The amount of energy/heat required to raise some substance 1 degree C
Heat Capacity (C)
sublimation
condensation
square pyramidal

36. Energy can't be created nor destroyed
Molar Mass of Element/ Total Molar Mass %
Law of Conservation of Energy
p+
T-shape

37. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Mass
Scientific Method
Molarity
Equivalence Point

38. Verticals on the periodic table
Bronsted-Lowry acid
not spontaneous
group
E

39. IMF that exists in polar molecules
Dipole-dipole forces
system
weak acid strong base rxn
Bond enthalpy

40. 109.5° - sp^3
boiling point
Tetrahedral
1st law of thermodynamics
0 degrees C - 1 atm

41. S²?
Constant Pressure
anode
sulfide
Specific Heat Capacity

42. Energy needed to vaporize a mole of a liquid
endless
sulfide
Molality
?Hvap

43. Elements which have unpaired electrons and highly affected by magnetic fields
voltaic cells
geometric isomers
paramagnetic
Alpha Particles-

44. Atomic #
base
% error
msAT
# protons (atom is defined by this)

45. Change in moles (An) =?
Covalently w/in themselves - Ionicly bonded w/ each other
(moles of products that are gasses) - (moles of reactants that are gasses)
0 degrees C - 1 atm
sulfate

46. The transfer of energy between two objects due to temperature difference
Solubility Product (Ksp)
?Tb= kb x molality
Heat
Root Mean Square Velocity

47. Where there are no electrons
bromate
wavelength
e-
Nodes

48. ln[A] vs. time is a ...-order reaction
Naming Binary Ionic Compounds
conjugate acid
deposition
first

49. Point where acid completely neutralizes base
q/moles
-ous acid
equivalence point
triple point

50. Dalton's Law of Partial Pressures (to find partial pressure formula)
Law of Multiple Proportions
P of a =(X of a)(total pressure)
4.184
Arrhenius acid

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Test your basic knowledge |

AP Chemistry

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