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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. The part of the universe one is focused upon (in thermodynamics)
system
Pressure of H2O must be Subtracted
LE Model
M1V1=M2V2

2. In a given atom no two electrons can have the same set of four quantum numbers
Transition metals
Speed of light
Pauli Exclusion Principle
Reducing Agent

3. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
1 atm = 760 mmHg = 101.3 kPa
group
voltaic cells
-ous acid

4. AX5
Scientific Method
work
Molar Mass of Element/ Total Molar Mass %
trigonal bipyramidal

5. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
indicator
are
(moles of products that are gasses) - (moles of reactants that are gasses)

6. Point at which vapor pressure=air pressure above
Alpha Particles-
isothermal
boiling point
Nernst Equation

7. Mass #
# protons + # neutrons
Negative work value; work done by system
wavelength
Exothermic

8. R=
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
soluble
8.31J/Kmol
sulfite

9. All _________ compounds are electrolytes
cathode
Integrated Zero-Order Rate Law
Ionic
Equivalence Point

10. Two molecules with identical connectivity but different geometries
Principal Quantum Number
geometric isomers
C + 273
Integrated Second-Order Rate Law

11. 2 or more covalently bonded atoms
Molecule
Surroundings
Anion
C=(mass)(specific heat)

12. x can be ignored when % ionization is <5%
hydrolysis
5% rule
d
Ligand

13. Oxidation # of Oxygen
Molecular Orbitals (MOs)
# protons + # neutrons
-2 - with peroxide -1
Heat Capacity (C)

14. Mol/L - concentration of a solution
Theoretical yield
-1
0.0826Latm/Kmol
Molarity

15. How to Find an Empirical Formula Given Percentages
First-Order Half Life
square planar
-al
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

16. Cation first - anion second
Solute
Naming Binary Ionic Compounds
bent
condensation

17. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps

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18. (organics) triple-bonded compound
nu
alkyne
increasing
strong bases

19. Gas to liquid
System
condensation
sublimation
Q<K

20. Mixing of gases
Diffusion
Anode
Counterions
Polar Covalent

21. Unit of electrical potential; J/C
soluble
end point
Molal BP Elevation Constant
Volt

22. OH¹?
-1
Bond Energy
hydroxide
1 atm = 760 mmHg = 101.3 kPa

23. ClO3²?
3.0x108m/s
Formal Charge
bond energy
chlorate

24. 1/[A] vs. time is a ...-order reaction
Entropy (S)
meth-
Le Chatelier's Principle
second

25. ClO4¹?
perchlorate
Aufbau Principle
m (third quantum number)
Solute

26. Energy required for liquid?gas
hydrocarbons
Chemical Bonds
heat of vaporization
Matter

27. r=k[A]^2
alkane
3.0x108m/s
Second-Order Rate Law
Decrease Volume and Increase Temperature

28. (organics) five carbons
violet
methoxy-
?Tb= kb x molality
pent-

29. Point where acid completely neutralizes base
Principal Quantum Number
equivalence point
Pi Bond
1.38x10?²³J/K

30. CO3²?
-ic acid
carbonate
8.31J/Kmol
bond energy

31. Coffee Cup Calorimeter
Solution
22.4L
Constant Pressure
square pyramidal

32. (msubs) Can only be +1/2 or -1/2
3rd law of thermodynamics
Electron Spin Quantum Number
Acid Dissociation Constant
condensation

33. Color of Sr (flame test)
red
hydrocarbons
# protons (atom is defined by this)
96500

34. Loss of electrons - increase in oxidation #
Closed System
Boltzmann distribution
oxidation
titrant buret

35. ?T=k*m(solute)
Force = mass x acceleration
Sigma Bond
precipitate
Molal FP Depression Constant

36. A monoatomic cation takes name from...
Trigonal Bipyramidal
Its element
square planar
ammonium

37. ClO2¹?
Molecule
chlorite
Formal Charge
carbonate

38. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Pi Bond
insoluble
1st law of thermodynamics
Cell Potential (Ecell)

39. Measure of the average kinetic energy of all the particles in a substance
1/2mv²
Sigma Bond
Temperature
heat of fusion

40. Reactant which doesn't get used up completely in a chemical reaction
Acids
excess reactant
square pyramidal
n (first quantum number)

41. Ionizes to produce H+ ions
Dalton's Law of Partial Pressures
Limiting reactant
Arrhenius Acid
Closed System

42. Resistance to flow
eth-
linear
Radioactivity
viscosity

43. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change

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44. AH of formation for a substance in its stablest form (how it is found in nature)
0
triple point
Adding
nitrite

45. Aldehyde suffix
-al
s (fourth quantum number)
ionic
0

46. Average Kinetic Energy Formula
Alpha Particles-
Joule
force x distance = work done
Average KE = 1/2(mass)(average speed of all particles)

47. Osmotic pressure formula
supercritical fluid
M1V1=M2V2
T-shape
pi=(nRT)/v

48. Dirrect Method Formula
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
reduction agent
?Hvap
+1 - except if bonded to Alkali Metal -1

49. R in ideal gas law
sublimation
0.0821 atm L/mol K
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
8.31J/Kmol

50. q cal = ?
CAT
-ic acid
specific heat
N=N.(0.5)^time/time half-life

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AP Chemistry

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