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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. Two molecules with identical connectivity but different geometries
P of a =(X of a)(total pressure)
0.0826Latm/Kmol
STP
geometric isomers

2. For significant digits - leading zeros ____ significant
chromate
Temperature
are not
Its root and adding -ide

3. Universal IMF for nonpolar molecules
Hydrogen bonding
+1 - except if bonded to Alkali Metal -1
eth-
London dispersion forces

4. Cl¹?
q/moles
Bonding Pairs
Atomic Mass Unit
chloride

5. HF+ OH??H2O
octahedral
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
weak acid strong base rxn
different # of neutrons

6. 109.5° - sp^3
# protons + # neutrons
Thermochemistry
Equilibrium constant
Tetrahedral

7. l=1
p
insoluble
Temperature
Trigonal Planar

8. Ester suffix
triple bond
van't Hoff Factor
Covalently w/in themselves - Ionicly bonded w/ each other
-oate

9. Carboxylic acid ending
heat of vaporization
v3RT/M(in kg)
-oic acid
base

10. (organics) eight carbons
1 atm = 760 mmHg = 101.3 kPa
weak acid strong base rxn
oct-
X of a = moles a/total moles

11. Reactant that's completely used up in a chemical reaction
Naming Binary Ionic Compounds
Barometer
8.31J/Kmol
Limiting reactant

12. The likelihood that a rxn will occur "by itself"
exothermic
spontaneity
Colligative properties
q

13. Ideal Gas Law Formula
London dispersion forces
End Point
PV=nRT
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

14. Gas to liquid
mol Fraction
1/2mv²
condensation
Cathode

15. Point at which liquid?gas occurs
seesaw
boiling point
Cathode
Constant Volume

16. Point at which solid?liquid occurs
Molecular
LeChatelier's Principle
melting point
red

17. The reactant that is being reduced - brings about oxidation
oxidizing agent
Polar Covalent
Angular Momentum Quantum Number
paramagnetic

18. Formula used when diluting stock solution (to find amount of water or stock needed)
Specific Heat (s)
high pressure - low temperature
Kinetic Molecular Theory - for ideal gases
M1V1=M2V2

19. Isotope
allotrope
different # of neutrons
H
Anode

20. Substance being dissolved in a solution (lower [ ])
Solute
Molarity
Bronsted-Lowry acid
square pyramidal

21. Boiling point - melting point - viscosity - vapor pressure - surface tension
Temperature
C + 273
effects of IMF
oct-

22. AX5
isothermal
titrant buret
trigonal bipyramidal
End Point

23. Oxidation # of free elements
1.86°C
0
Buffer
Volume Metric Flask & Pipet

24. Bomb Calorimeter
Manometer
Bronsted-Lowry Acid
Constant Volume
Quantum Numbers

25. Raoult's Law - relations between vapor pressure and concentrations
chloride
0
P1= X1P1°
1.86°C

26. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Law of Conservation of Mass
p
Speed of light

27. Horizontals on the periodic table
Solvent
Sigma Bond
trigonal bipyramidal
period

28. The mixing of native atomic orbitals to form special orbitals for bonding
Hybridization
Molecular Orbitals (MOs)
carbonate
8.314 J/K mol

29. Increase Volume
Increase Temperature
8.314 J/K mol
nitrate
heat capacity

30. 1/[A] vs. time is a ...-order reaction
second
Atmospheric Pressure
ionic
M1V1=M2V2

31. Gain of electrons - decrease in oxidation #
red
square pyramidal
Average KE = 1/2(mass)(average speed of all particles)
reduction

32. ?T=k*m(solute)
m (third quantum number)
sublimation
-ous acid
Molal FP Depression Constant

33. 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
Density
Positive work value; work done on system
Le Chatelier's Principle
supercritical fluid

34. Atomic #
# protons (atom is defined by this)
0
Cell Potential (Ecell)
m (third quantum number)

35. A measure of resistance of an object to a change in its state of motion
Mass
rate gas A/rate gas B = square root (mm A/ mm B)
base and hydrogen gas
Acids

36. Composition Formula
Atomic Mass Unit
indicator
Molar Mass of Element/ Total Molar Mass %
Molality

37. MnO4¹?
Force = mass x acceleration
sulfite
permanganate
base

38. Ending for alcohols
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
end point
Law of Multiple Proportions
-ol

39. A solution that resists a change in its pH
Buffered Solution
5% rule
C=(mass)(specific heat)
Integrated Second-Order Rate Law

40. Osmotic pressure=MRT
Hess's Law
1/2mv²
Osmotic Pressure
% yield

41. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
adhesion
0
London Dispersion Forces
Theoretical yield

42. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Equivalence Point
Boltzmann distribution
Counterions
vaporization

43. Ionizes to produce OH- Ions
Theoretical yield
96500
Arrhenius Base
vaporization

44. Speed of light - C
standard solution
flouride
endothermic
3.0x108m/s

45. Color of K (flame test)
critical point
purple
Molal FP Depression Constant
yellow --> green

46. SO3²?
sulfite
are not
p orbitals
London dispersion forces

47. Phase change from gas to solid
linear
deposition
Standard Temperature and Pressure
but-

48. (organics) seven carbons
Temperature
chloride
Bonding Pairs
hept-

49. Variable for energy of e- - goes from 1 -2 -3 on up
boiling point
Ag+ - Pb2+ - Hg2+
n (first quantum number)
Equilibrium Expression

50. Mol of solute/kg of solvent
allotrope
Cg=kPg
acid
Molality

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Test your basic knowledge |

AP Chemistry

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