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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. The driving force for a spontaneous is an increase in entropy of the universe
Entropy (S)
end point
Density
Dalton's Law of Partial Pressures

2. Raising heat - adding catalyst - heighten concentration - bigger surface area
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
e-
Reducing Agent
methods of increasing rate

3. C2H3O2¹?
-1
Decrease Volume and Increase Temperature
not spontaneous
acetate

4. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
heat of vaporization
hydrolysis
Ionic
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

5. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
Root Mean Square Velocity
State Functions
insoluble
Bronsted-Lowry Acid

6. Involves quantum numbers
different # of neutrons
End Point
Hund's Rule
Quantum Mechanical Model

7. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Speed of light
Polar Covalent
Integrated Second-Order Rate Law
Molal FP Depression Constant

8. 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
Sigma Bond
supercritical fluid
Calorimeter
endothermic

9. Universal IMF for nonpolar molecules
P1V1/N1T1=P2V2/N2T2
Positive work value; work done on system
London dispersion forces
not spontaneous

10. Ester suffix
Calorimeter
-oate
Open System
Finding Empirical Formulas

11. (organics) eight carbons
Acid Dissociation Constant
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
oct-
-one

12. ClO4¹?
bent
vapor pressure
perchlorate
# protons + # neutrons

13. Forward rxn occurs when
3/2RT
Hydrogen bonding
Q<K
heat capacity

14. The line running between the atoms
allotrope
Transition metals
blue
Sigma Bond

15. Symbol for Total Heat absorbed or released
permanganate
Molar Mass of Element/ Total Molar Mass %
Specific Heat (s)
q

16. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
0
0.0821 atm L/mol K
3rd law of thermodynamics

17. CO3²?
second
carbonate
-(q of H2O + q of cal)
Molecule

18. Group 2 metals
Diffusion
Alkaline earth metals
electron affinity
Osmotic Pressure

19. AX6
trigonal planar
Monoprotic
octahedral
Cg=kPg

20. Cr2O7²?
double bond
yellow
phosphate
dichromate

21. Increase Volume
Increase Temperature
trigonal bipyramidal
octahedral
Osmotic Pressure

22. Formula used when diluting stock solution (to find amount of water or stock needed)
Molal FP Depression Constant
analyte
M1V1=M2V2
effects of IMF

23. Ending for alcohols
deposition
Delta H or Enthalpy Change
-ol
acid

24. Osmotic pressure formula
iodide
pi=(nRT)/v
Law of Multiple Proportions
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

25. x can be ignored when % ionization is <5%
Solubility Product (Ksp)
Solvent
Open System
5% rule

26. A measure of resistance of an object to a change in its state of motion
Mass
Pressure
Molecular Compounds
flouride

27. F¹?
oct-
flouride
conjugate acid
chloride

28. If Q>Ksp
-(q of H2O + q of cal)
methoxy-
a precipitate forms
dec-

29. (A) - C/s
T-shape
d
Ampere
P of a =(X of a)(total pressure)

30. Oxidation # of Ions
charge
Theory of Relativity
STP
boiling point

31. When n=5 ->2 - color=
endless
Kinetic Molecular Theory - for ideal gases
blue-violet
Diffusion

32. Where oxidation occurs
system
tetrahedral
Anode
work

33. When gas compresses ...
rate law
sublimation
Positive work value; work done on system
M = square root (3RT/mm)

34. Half-life equation
0.512°C
Ionic
N=N.(0.5)^time/time half-life
solid CO2

35. Verticals on the periodic table
3.0x108m/s
Entropy (S)
group
e-

36. 0.00°C - 1 atm
d orbitals
Dipole Moment
Integrated First-Order Rate Law
Standard Temperature and Pressure

37. AX4E2
square planar
Nodes
rate
Aufbau Principle

38. Substances that form H+ when dissolved in water; proton donors
Acids
Positive work value; work done on system
perchlorate
voltaic cells

39. Specific heat of water
4.184
catalyst
Density
N=N.(0.5)^time/time half-life

40. ClO3²?
Hybridization
Trigonal Planar
chlorate
Zero-Order Rate Law

41. ?T=k*m(solute)
reduction
-ous acid
heat capacity
Molal BP Elevation Constant

42. Occupies the space above and below a sigma bond
Polar Covalent
Boltzmann distribution
Pi Bond
Its element

43. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
iodide
Diffusion
Graham's Law
Chemical Kinetics

44. (organics) nine carbons
nitrate
3.0x108m/s
non-
freezing

45. [A] vs. time is a ...-order reaction
Reducing Agent
Q>K
zero
flouride

46. Proton donors
pi=(nRT)/v
Bronsted-Lowry acid
Balmer Series
exothermic

47. Pressure Units/Conversions
-(P)(Change in V)
1 atm = 760 mmHg = 101.3 kPa
Constant Volume
alkyne

48. Spontaneous emission of radiation
flouride
adhesion
d
Radioactivity

49. Oxidation # of Halogens
d orbitals
-1
triple bond
Polar Covalent

50. Hydroxides are soluble or insoluble?
solid CO2
1 atm
insoluble
Quantum Model

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AP Chemistry

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