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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. Only contains ions that change in reaction
Net Ionic Equation
Balmer Series
cyanide
Linear

2. Energy can't be created nor destroyed
spontaneity
Trigonal Bipyramidal
Hybridization
Law of Conservation of Energy

3. Molecules' tendency to stick to one another
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
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
Heat
cohesion

4. Proton (symbol)
p+
hydrolysis
0 degrees C - 1 atm
Volt

5. (A) - C/s
Ampere
deposition
meth-
Bronsted-Lowry base

6. The reactant in the reduction reaction that forces the oxidation reaction to occur
p
Barometer
Oxidizing Agent
Weight

7. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
increasing
analyte
rate law

8. Dirrect Method Formula
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
LeChatelier's Principle
Cell Potential (Ecell)
Manometer

9. Kinetic Energy of an individual particle formula
Bases
Hydrogen bonding
M = square root (3RT/mm)
First-Order Half Life

10. Type of system in which the energy and mass may leave or enter
actual yield/theoretical yield x 100%
end point
Open System
soluble

11. q cal = ?
boiling point
Volt
CAT
red/orange

12. Oxidation # of Hydrogen
period
base and hydrogen gas
+1 - except if bonded to Alkali Metal -1
freezing

13. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Equilibrium Expression
acetate
First-Order Rate Law
octahedral

14. Gas to solid
a precipitate forms
P of a =(X of a)(total pressure)
deposition
-ic acid

15. When gas expands ...
Molecule
Increase Temperature
Negative work value; work done by system
Bond enthalpy

16. If anion ends in -ite - acid name ends in...
oxalate
-ous acid
reduction
Trigonal Planar

17. Coffee Cup Calorimeter
Surroundings
Constant Pressure
chlorate
AE = q + w

18. Type of system in which the energy may escape - but the mass is conserved
Delta H or Enthalpy Change
Closed System
Integrated Rate Law
carbohydrates

19. Amount of heat needed to change a system by 1°C
oxalate
# protons (atom is defined by this)
Pauli Exclusion Principle
heat capacity

20. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
Finding Empirical Formulas
equivalence point
Buffered Solution

21. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
Root Mean Square Velocity
violet
Bronsted-Lowry base

22. U(rms)=(3RT/M)^1/2
Decrease Volume and Increase Temperature
Solution
tetrahedral
Root Mean Square Velocity

23. AX4E
paramagnetic
ionic
see-saw
activated complex (transition state)

24. Raoult's Law - relations between vapor pressure and concentrations
fusion
Aufbau Principle
P1= X1P1°
Reducing Agent

25. Osmotic pressure=MRT
Weight
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
strong bases
Osmotic Pressure

26. A measure of randomness or disorder
entropy
3rd law of thermodynamics
viscosity
high pressure - low temperature

27. A molecule having a center of positive charge and a center of negative charge
Arrhenius base
n0
carbohydrates
Dipole Moment

28. If needed - indicate charge of metal(cation) by...
Integrated Rate Law
T-shape
A Roman numeral
pent-

29. Describe various properties of one orbital
Quantum Numbers
actual yield/theoretical yield x 100%
cyanide
Bond enthalpy

30. (organics) one carbon
Atmospheric Pressure
Quantum Numbers
Ag+ - Pb2+ - Hg2+
meth-

31. Occupies the space above and below a sigma bond
charge
strong acids
Pi Bond
Kinetic Molecular Theory - for ideal gases

32. Half cell in which reduction occurs
Adding
cathode
sulfide
single bond

33. E?s fill the lowest energy orbital first - then work their way up
hydro-ic acid
analyte
1st law of thermodynamics
Aufbau Principle

34. 96 -485 C/mol e-
Naming Binary Ionic Compounds
H
Faraday
Calorimeter

35. For significant digits - leading zeros ____ significant
are not
log[H+]
Hydrogen bonding
increasing

36. # bonding e- - # antibonding e-/2
1 atm
0
Manometer
Bond Order

37. Metal oxide + H20 ->
Lone Pair
moles solute/kg solvent
base
permanent gases

38. AX4
single bond
-2 - with peroxide -1
tetrahedral
Bonding Pairs

39. Solid to liquid
1 atm
methods of increasing rate
melting
Open System

40. Newton's Second Law
Force = mass x acceleration
Molality
Adding
3/2RT

41. When n=5 ->2 - color=
activation energy
1 atm = 760 mmHg = 101.3 kPa
Hess's Law
blue-violet

42. The line running between the atoms
specific heat
Molecular Compounds
Sigma Bond
heat of fusion

43. All cations are soluble with bromide - chloride and iodide EXCEPT
electron affinity
methoxy-
electrolyte
Ag+ - Pb2+ - Hg2+

44. Two molecules with identical connectivity but different geometries
specific heat
heat of vaporization
Pauli Exclusion Principle
geometric isomers

45. Pure metal or metal hydride + H20 ->
base and hydrogen gas
blue-green
paramagnetic
Pi Bond

46. Polyatomic Ions (bonding)
Covalently w/in themselves - Ionicly bonded w/ each other
rate
Kinetic Molecular Theory - for ideal gases
pent-

47. pH=
log[H+]
Bronsted-Lowry acid
Speed of light
lambda

48. AX5
Arrhenius acid
heat of vaporization
Amino-
trigonal bipyramidal

49. 1/([A]0*k)
Pi Bond
sublimation
Second-Order Half Life
endothermic

50. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
standard solution
Pi Bond
Ligand
London Dispersion Forces