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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. Mass percent
Acid + Base --> Salt + Water
oct-
Average KE = 1/2(mass)(average speed of all particles)
g solute/g solvent x 100

2. Like dissolves...
like
solid CO2
Le Chatelier's Principle
reduction

3. (organics) ten carbons
Volume Metric Flask & Pipet
Negative work value; work done by system
Equilibrium constant
dec-

4. Solution in flask being titrated
analyte
Cation
Volt
State Functions

5. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Second-Order Half Life
Colligative properties
Antibonding Molecular Orbital
Buffer

6. l=0
voltaic cells
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
s
-al

7. A monoatomic anion is named by taking...
base and hydrogen gas
P of a =(X of a)(total pressure)
Its root and adding -ide
Antibonding Molecular Orbital

8. The entropy of a pure perfectly formed crystal @0K is 0
Diffusion
Trigonal Bipyramidal
3rd law of thermodynamics
0

9. CrO4²?
chromate
Ionic
prop-
trigonal bipyramidal

10. Oxidation # of Halogens
Its root and adding -ide
Transition metals
Electronegativity
-1

11. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Zero-Order Half Life
Molal BP Elevation Constant
octahedral

12. # bonding e- - # antibonding e-/2
Bond Order
Osmotic Pressure
s
1st law of thermodynamics

13. The reactant that is being reduced - brings about oxidation
oxidizing agent
Hess's Law
non-
Equilibrium constant

14. Type of system in which the energy and mass may leave or enter
Open System
Hund's Rule
oxide gas and water
specific heat

15. Actual Yield/Theoretical Yield*100%
Percent Yield
flouride
purple --> pink
Bronsted-Lowry Acid

16. Half-life equation
excess reactant
Oxidation is Loss Reduction is Gain
First-Order Rate Law
N=N.(0.5)^time/time half-life

17. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Ionic Compounds
reduction agent
M1V1=M2V2
96500

18. A single substance that may be an acid or a base (i.e. water)
Amphoteric
Molarity
ionic
second

19. Degree of disorder in a system
entropy (S)
linear
Ideal Gas Law
amine

20. The measurement of heat changes
Calorimetry
Bronsted-Lowry acid
hex-
Naming Binary Ionic Compounds

21. Where there are no electrons
-one
prop-
oxidizing agent
Nodes

22. An equilibrium expression
electrolyte
Solubility Product (Ksp)
n (first quantum number)
3rd law of thermodynamics

23. CO3²?
carbonate
Temperature
M = square root (3RT/mm)
alkene

24. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Kinetic Molecular Theory - for ideal gases
Electronegativity
Quantum Mechanical Model
% error

25. The mixing of native atomic orbitals to form special orbitals for bonding
hydrocarbons
Hybridization
Dipole-dipole forces
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

26. R in ideal gas law
Constant Pressure
N=N.(0.5)^time/time half-life
0.0821 atm L/mol K
alkyne

27. All _________ compounds are electrolytes
Ionic
Constant Pressure
activated complex (transition state)
methods of increasing rate

28. Ionizes to produce H+ ions
cyanide
Alpha Particles-
Effusion
Arrhenius Acid

29. 760 mmHg - 760 torr
sulfate
Graham's Law
1 atm
Normality

30. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
condensation
Bronsted-Lowry Acid
oxidizing agent
Acid + Base --> Salt + Water

31. The reactant in the reduction reaction that forces the oxidation reaction to occur
meth-
Oxidizing Agent
Cg=kPg
freezing

32. Mole Fraction
X of a = moles a/total moles
viscosity
0
Ligand

33. 90°&120° - dsp^3
Trigonal Bipyramidal
Negative work value; work done by system
Bond Energy
Zero-Order Rate Law

34. AX3E
analyte
trigonal pyramidal
hydro-ic acid
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

35. 1 sigma bond - 2 pi bonds
triple bond
Molecular Orbitals (MOs)
work
complex ions

36. Organic w/ -OH group
group
alcohol
Radioactivity
1/2mv²

37. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Amino-
Equilibrium Expression
Finding Empirical Formulas
strong acids

38. IMF that occurs with FON
E
hydrolysis
Hydrogen bonding
isothermal

39. ClO3²?
Its element
3rd law of thermodynamics
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
chlorate

40. Isotope
Calorimetry
Quantum Mechanical Model
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
different # of neutrons

41. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
Arrhenius acid
Zero-Order Half Life
Counterions

42. The weighted average of all the isotopes that an atom can have (in g/mol)
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
boiling point
s
Atomic Mass Unit

43. As protons are added to the nucleus - electrons are similarly added
adiabatic
lambda
Aufbau Principle
Specific Heat (s)

44. n+m (these are orders of reactants)
zero
Van't Hoff factor
Overall Reaction Order
Q<K

45. Half cell in which oxidation occurs
t-shape
anode
Constant Volume
Amount of atoms present

46. Kinetic Energy per mol
octahedral
Law of Conservation of Mass
3/2RT
Volt

47. Anions or cations as needed to produce a compound with non net charge
melting
Counterions
Hess's Law
Alpha Particles-

48. Force per unit area
dec-
adhesion
Pressure
triple point

49. Calculation from K to C
titrant buret
Amount of atoms present
C + 273
% yield

50. Kinetic Energy per molecule
catalyst
Specific Heat Capacity
1/2mv²
Pressure