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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. C2O4²?
strong bases
oxalate
LE Model
Hybridization

2. C2H3O2¹?
Bronsted-Lowry Base
yellow --> green
wavelength
acetate

3. Universal IMF for nonpolar molecules
London dispersion forces
Q<K
k=Ae^(-Ea/RT)
Net Ionic Equation

4. Ionizes to produce OH- Ions
Balmer Series
LE Model
Arrhenius Base
State Functions

5. Degree of disorder in a system
First-Order Rate Law
entropy (S)
Integrated Zero-Order Rate Law
Law of Conservation of Mass

6. 1 sigma bond - 2 pi bonds
Angular Momentum Quantum Number
Effusion
Bond enthalpy
triple bond

7. r=k
C=(mass)(specific heat)
group
Boltzmann distribution
Zero-Order Rate Law

8. Substance being dissolved in a solution (lower [ ])
Solute
second
are not
Quantum Mechanical Model

9. Type of system in which nothing is transfered (no mass or energy); ideal
Dalton's Law
Normality
London dispersion forces
Isolated System

10. Oxidation # of Polyatomic Ions
AE= AH - RTAn
charge
msAT
Arrhenius equation

11. If anion ends in -ide - acid name ends in
Linear
Open System
hydro-ic acid
Antibonding Molecular Orbital

12. A device in which chemical energy is changed to electrical energy
Galvanic Cell
M = square root (3RT/mm)
anode
Second-Order Half Life

13. 0°C and 1 atm
no precipitate forms
not spontaneous
perchlorate
STP

14. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Ligand
different # of neutrons
1 atm = 760 mmHg = 101.3 kPa
rate

15. Speed per molecule of gas
purple --> pink
v3kT/m
violet
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

16. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Faraday
Equilibrium Expression
# protons + # neutrons
triple point

17. (# of lone pair e-)+1/2(# of shared e-)
AE = q + w
ether
equilibrium
Valence Electrons(assigned)

18. Ability of an atom in a molecule to attract shared electrons to itself
electron affinity
Electronegativity
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
reduction

19. All cations are soluble with sulfate EXCEPT
1.38x10?²³J/K
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Weight
Constant Volume

20. Molarity (M)
Galvanic Cell
p
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
moles of solute/ L of solution

21. CrO4²?
Zero-Order Half Life
chromate
Polar Covalent
H

22. For significant digits - leading zeros ____ significant
are not
entropy (S)
Law of Multiple Proportions
1/2mv²

23. Aldehyde suffix
-al
Trigonal Planar
isothermal
reduction agent

24. Consists of a complex ion - a transition metal with attached ligands - and counterions
Closed System
Lone Pair
sulfate
Coordination Compound

25. Average Kinetic Energy Formula
oxide gas and water
?Hvap
Average KE = 1/2(mass)(average speed of all particles)
are not

26. Half cell in which oxidation occurs
Solution
anode
Sigma Bond
d orbitals

27. AX6
octahedral
nitrate
a precipitate forms
ammonium

28. Absorbs/takes in heat (positive value)
Endothermic
charge
96500
Molarity

29. Mol of solute/kg of solvent
log[H+]
Molality
allotrope
Hess's Law

30. Anything occupying space and with mass
Matter
s orbitals
weak acid strong base rxn
charge

31. Planck's constant - used to calculate energy w/frequency
Coordination Compound
6.63x10?³4Js
pi=(nRT)/v
Dipole-dipole forces

32. MnO4¹?
permanganate
octahedral
Molality
Naming Binary Ionic Compounds

33. Where reduction occurs
blue-green
Cathode
iodide
reduction

34. AX4
methods of increasing rate
excess reactant
complex ions
tetrahedral

35. H?+OH??H2O
excess reactant
M1V1=M2V2
strong acid strong base rxn
melting point

36. Actual Yield/Theoretical Yield*100%
like
Aufbau Principle
Percent Yield
Arrhenius Base

37. If Q>Ksp
paramagnetic
red
-(P)(Change in V)
a precipitate forms

38. 6.022x10^23
activation energy
Molar Mass of Element/ Total Molar Mass %
rate law
mol

39. Color of Li (flame test)
red
Molal BP Elevation Constant
Resonance
Calorimeter

40. Organic reaction in which two functional groups come together - resulting in the release of water
Ligand
d orbitals
salt bridge
condensation

41. Puts OH? into solution
Transition metals
zero
Molar Heat Capacity
Arrhenius base

42. Faraday's constant
96500
allotrope
e-
Surroundings

43. Boiling point elevation formula
linear
?Tb= kb x molality
bent
sublimation

44. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
1 atm = 760 mmHg = 101.3 kPa
increasing
1atm=?Pa

45. The minimum energy that molecules must possess for collisions to be effective - Ea
Bases
activation energy
Zero-Order Half Life
Normality

46. Substance in which something is dissolved in a solution (higher [ ])
Solvent
Monoprotic
Quantum Numbers
condensation

47. Matter can't be created nor destroyed
Entropy (S)
sulfite
strong bases
Law of Conservation of Mass

48. What is defined by you taken from the whole universe
Arrhenius Base
Osmotic Pressure
rate law
System

49. (organics) one carbon
Solute
non-
Anode
meth-

50. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
0.0821 atm L/mol K
insoluble
Radioactivity
Tetrahedral