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AP Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
electron affinity
Molecular
square pyramidal
-oate

2. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Octahedral
Law of Multiple Proportions
vapor pressure
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

3. Within a sublevel - place one e? per orbital before pairing them

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4. Diatomic Molecules
E
Law of Multiple Proportions
tetrahedral
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

5. r=k[A]
msAT
First-Order Rate Law
Arrhenius Acid
Root Mean Square Velocity

6. Arrhenius equation
Lone Pair
Alkaline earth metals
k=Ae^(-Ea/RT)
-one

7. Puts OH? into solution
Integrated Rate Law
Faraday
Arrhenius base
1st law of thermodynamics

8. Ketone suffix
Molality
-one
third
period

9. Energy needed to vaporize a mole of a liquid
P of a =(X of a)(total pressure)
-ol
?Hvap
Angular Momentum Quantum Number

10. If Q<Ksp
no precipitate forms
AE = q + w
Principal Quantum Number
Multiplying

11. Carboxylic acid ending
ether
amine
-oic acid
-ol

12. Color of Ca (flame test)
red/orange
Constant Volume
paramagnetic
-ic acid

13. #NAME?
Surroundings
?Tf= kf x molality
E
Weight

14. Color of Na (flame test)
methods of increasing rate
Theoretical yield
London Dispersion Forces
yellow

15. 2 or more covalently bonded atoms
State Functions
CAT
Speed of light
Molecule

16. H+ Acceptor
Bronsted-Lowry Base
alkene
mol Fraction
Its element

17. Passage of gas through tiny orifice
ammonium
Van't Hoff factor
Effusion
bond energy

18. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals

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19. Average Kinetic Energy Formula
heat capacity
Anion
Average KE = 1/2(mass)(average speed of all particles)
anode

20. Variable for energy of e- - goes from 1 -2 -3 on up
activated complex (transition state)
# protons (atom is defined by this)
endothermic
n (first quantum number)

21. kb of water
0.512°C
Open System
phosphate
rate law

22. (msubs) Can only be +1/2 or -1/2
oxidizing agent
Percent Yield
Dalton's Law of Partial Pressures
Electron Spin Quantum Number

23. 90°&120° - dsp^3
Bronsted-Lowry Acid
p+
Trigonal Bipyramidal
no precipitate forms

24. Phase change from gas to solid
# protons + # neutrons
deposition
meth-
rate

25. Absorbs/takes in heat (positive value)
Bronsted-Lowry Acid
not spontaneous
Endothermic
Electron Spin Quantum Number

26. Dirrect Method Formula
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Ionic Compounds
Molarity
purple --> pink

27. Each orbital can hold two e?s each w/ opposite spins
Law of Definite Proportion
conjugate base
Pauli Exclusion Principle
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

28. C=2.9979*10^8 m/s
Weight
Speed of light
melting point
red

29. Change that occurs at constant temperature
isothermal
sulfide
System
Dalton's Law

30. High-energy light
indicator
Gamma Ray-
system
3.0x108m/s

31. AX4E
Its root and adding -ide
are
sublimation
see-saw

32. Change in Energy (AE) = ? (in terms of work)
AE = q + w
sublimation
P of a =(X of a)(total pressure)
N=N.(0.5)^time/time half-life

33. U(rms)=(3RT/M)^1/2
Root Mean Square Velocity
Metalliods
Positive work value; work done on system
sulfite

34. STP
Mass
0 degrees C - 1 atm
Amino-
amine

35. 0°C and 1 atm
# protons (atom is defined by this)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
STP
Endothermic

36. Half-life equation
surroundings
N=N.(0.5)^time/time half-life
X of a = moles a/total moles
Counterions

37. Isotope
different # of neutrons
Specific Heat Capacity
Bronsted-Lowry Base
spontaneous

38. 0.00°C - 1 atm
Standard Temperature and Pressure
Net Ionic Equation
effects of IMF
Hydrogen bonding

39. When n=6 ->2 - color=
diamagnetic
excess reactant
violet
hydroxide

40. Rate of Diffusion/Effusion formula
trigonal pyramidal
sulfate
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Bond Energy

41. 6.022x10^23
deposition
mol
r1/r2
Normality

42. Universal IMF for nonpolar molecules
Specific Heat Capacity
-2 - with peroxide -1
red
London dispersion forces

43. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
1.38x10?²³J/K
3rd law of thermodynamics
voltaic cells
ether

44. % yield
actual yield/theoretical yield x 100%
exothermic
Hess's Law
Alkaline earth metals

45. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
% error
acid
period

46. Force acting over distance
indicator
Work
Diffusion
-oate

47. Type of system in which the energy and mass may leave or enter
sublimation
Limiting reactant
E
Open System

48. Amount of gravitational force exerted on an object
Weight
charge
carbohydrates
3/2RT

49. Mol/kg of solvent - used in calculating colligative properties
0.0821 atm L/mol K
trigonal planar
single bond
Molality

50. Point at which the titrated solution changes color
m (third quantum number)
Arrhenius equation
end point
M1V1=M2V2