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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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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. l=3
dec-
f
Ag+ - Pb2+ - Hg2+
Metalliods

2. Metal oxide + H20 ->
base
Alkaline earth metals
Barometer
red

3. Energy required for melting to occur
heat of fusion
Enthalpy of Solution
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
not spontaneous

4. l=0
s
London dispersion forces
Aufbau Principle
cyanide

5. When gas expands ...
Negative work value; work done by system
Atmospheric Pressure
p orbitals
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

6. Similar to atomic orbitals - except between molecules
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
bent
Molecular Orbitals (MOs)
Entropy (S)

7. Change without heat transfer between the system and its surroundings
Speed of light
boiling point
lambda
adiabatic

8. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
specific heat
blue
Graham's Law

9. The reactant that is being reduced - brings about oxidation
X of a = moles a/total moles
log[H+]
Molecule
oxidizing agent

10. Group 1 metals
Monoprotic
methods of increasing rate
Alkali metals
0.0826Latm/Kmol

11. Molality =
moles solute/kg solvent
Hybridization
Molecular Orbitals (MOs)
Integrated Second-Order Rate Law

12. Oxidation # of Ions
heat capacity
equilibrium
charge
insoluble

13. Spectrum of light when an electron drops to energy level n=2
Law of Conservation of Mass
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Balmer Series
electron affinity

14. J/°Cmol or J/Kmol
Manometer
boiling point
sulfate
Molar Heat Capacity

15. frequency symbol
Law of Definite Proportion
viscosity
nu
vapor pressure

16. Theoretical yield-experimental yield/theoretical yieldx100
% error
Molecule
Dalton's Law of Partial Pressures
1 atm = 760 mmHg = 101.3 kPa

17. E?s fill the lowest energy orbital first - then work their way up
fusion
group
trigonal planar
Aufbau Principle

18. Boiling point - melting point - viscosity - vapor pressure - surface tension
prop-
effects of IMF
Pauli Exclusion Principle
zero

19. Ester suffix
Delta H or Enthalpy Change
Temperature
r1/r2
-oate

20. negative ion
perchlorate
Chemical Kinetics
Anion
like

21. neutron (symbol)
n0
Exothermic
LE Model
work

22. Occupies the space above and below a sigma bond
London Dispersion Forces
red
Trigonal Planar
Pi Bond

23. Group 2 metals
red
Work
Law of Definite Proportion
Alkaline earth metals

24. A monoatomic cation takes name from...
seesaw
acetate
Open System
Its element

25. Amount of gravitational force exerted on an object
spontaneity
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
oxidation
Weight

26. Group 1 and heavier Group 2 bases
M = square root (3RT/mm)
-ous acid
Bonding Pairs
strong bases

27. Planck's constant - used to calculate energy w/frequency
Finding Empirical Formulas
Law of Conservation of Mass
purple --> pink
6.63x10?³4Js

28. Electron (symbol)
Dipole-dipole forces
critical point
-(P)(Change in V)
e-

29. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
work
Arrhenius base
zero
Boltzmann distribution

30. Amount of product produced when limiting reactant is used up
Matter
Allotrope
Theoretical yield
alcohol

31. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Metalliods
Specific Heat (s)
3rd law of thermodynamics
Equilibrium Expression

32. kf of water
Bronsted-Lowry Base
hydroxide
Bonding Pairs
1.86°C

33. ?T=k*m(solute)
Molal BP Elevation Constant
Adding
paramagnetic
deposition

34. The chemical formed when a base accepts a proton
conjugate acid
Molecular Orbitals (MOs)
p
Quantum Model

35. Ionizes to produce H+ ions
Radioactivity
electrolyte
Arrhenius Acid
d orbitals

36. AX4E2
Pauli Exclusion Principle
red
Oxidizing Agent
square planar

37. AX4
CAT
Mass
tetrahedral
voltaic cells

38. Where reduction occurs
Molal BP Elevation Constant
vapor pressure
Hybridization
Cathode

39. 90° - d^2sp^3
Octahedral
Isotopes
green/yellow
Entropy (S)

40. Proton acceptors - must have an unshared pair of e?s
hydrolysis
g solute/g solvent x 100
Bronsted-Lowry base
Zero-Order Half Life

41. Change in moles (An) =?
trigonal planar
Cation
(moles of products that are gasses) - (moles of reactants that are gasses)
Solution

42. Substances that form H+ when dissolved in water; proton donors
Acids
n (first quantum number)
Strong acid weak base rxn
prop-

43. Oxidation # of Compounds
0
Solubility Product (Ksp)
-oate
adhesion

44. The transfer of energy between two objects due to temperature difference
Ionic Compounds
alcohol
Arrhenius base
Heat

45. Newton's Second Law
Octahedral
Force = mass x acceleration
Covalently w/in themselves - Ionicly bonded w/ each other
heat capacity

46. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Matter
% error
LE Model
Molar Mass of Element/ Total Molar Mass %

47. Melting
fusion
-oic acid
Integrated Rate Law
Buffer

48. Degree of disorder in a system
geometric isomers
ammonium
entropy (S)
0

49. Where there are no electrons
Calorimetry
System
Nodes
t-shape

50. Organic w/ -O-
Negative work value; work done by system
ether
see-saw
Quantum Mechanical Model