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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. Variable for spin of electron (+.5 or -.5)
s (fourth quantum number)
strong acid strong base rxn
2nd law of thermodynamics
carbonate

2. Atoms with the same number of protons but a different number of neutrons
spontaneous
Atomic Mass Unit
double bond
Isotopes

3. Lowers activation energy
Boltzmann distribution
viscosity
catalyst
phosphate - sulfide - carbonate - sulfate

4. These orbitals are diagonal
d orbitals
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 agent
Temperature

5. # bonding e- - # antibonding e-/2
trigonal pyramidal
Bond Order
adiabatic
Sigma Bond

6. r=k[A]^2
blue
s orbitals
Second-Order Rate Law
Dalton's Law

7. 90° - d^2sp^3
Octahedral
Beta Particles-
0.0826Latm/Kmol
P1= X1P1°

8. Symbol for Enthalpy
g solute/g solvent x 100
H
E
Heat

9. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
heat capacity
0
experimental yield

10. CO3²?
alkene
Integrated Second-Order Rate Law
carbonate
End Point

11. Point at which the titrated solution changes color
catalyst
condensation
end point
sulfide

12. Energy (definition)
Molarity
force x distance = work done
Covalently w/in themselves - Ionicly bonded w/ each other
oxide

13. Kinetic Energy per molecule
base and hydrogen gas
Buffered Solution
flouride
1/2mv²

14. Work = ?
ammonium
-(P)(Change in V)
lambda
cathode

15. Where there are no electrons
Nodes
Enthalpy of Solution
Anion
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

16. Cl¹?
chloride
triple bond
AE= AH - RTAn
-oic acid

17. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Quantum Numbers
d
Hess's Law
LE Model

18. SO3²?
conjugate acid
sulfite
condensation
(moles of products that are gasses) - (moles of reactants that are gasses)

19. O²?
End Point
oxide
nitrate
-oic acid

20. (organics) three carbons
prop-
-one
Force = mass x acceleration
purple

21. 1 sigma bond - 2 pi bonds
Anion
triple bond
# protons + # neutrons
Polar Covalent

22. Elements on staircase on periodic table
Molarity
Metalliods
endless
deposition

23. J/°Cmol or J/Kmol
msAT
red
Hund's Rule
Molar Heat Capacity

24. Half cell in which reduction occurs
are not
cathode
Enthalpy of Solution
Theoretical yield

25. n+m (these are orders of reactants)
P of a =(X of a)(total pressure)
Manometer
Constant Volume
Overall Reaction Order

26. IMF that occurs with FON
Bases
Hydrogen bonding
-oate
purple

27. Change in Energy (AE) = ? (in terms of work)
Weight
Law of Multiple Proportions
System
AE = q + w

28. How to Balance a Redox Equation
London dispersion forces
E
Van't Hoff factor
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

29. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
oxidation
heat of fusion
AH
Colligative properties

30. Chemical composition of dry ice
Pi Bond
solid CO2
Diffusion
charge

31. [A]=-kt + [A]0
Kinetic Molecular Theory - for ideal gases
Integrated Zero-Order Rate Law
v3kT/m
-oic acid

32. Instrument used to measure the pressure of atmospheric gas
Radioactivity
Van't Hoff factor
Barometer
Hess's Law

33. Puts OH? into solution
oxidizing agent
Arrhenius base
equivalence point
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

34. Group 1 and heavier Group 2 bases
red
Bronsted-Lowry Base
strong bases
Strong acid weak base rxn

35. Amine prefix
eth-
Formal Charge
Acids
Amino-

36. Describe various properties of one orbital
Integrated Rate Law
Quantum Numbers
Arrhenius acid
triple point

37. 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)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
triple bond
vaporization
State Functions

38. Substance that - when dissolved - is conductive
electrolyte
Adding
oxide gas and water
methods of increasing rate

39. HF+ OH??H2O
deposition
Limiting reactant
Finding Empirical Formulas
weak acid strong base rxn

40. Spectrum of light when an electron drops to energy level n=2
oxalate
AE = q + w
Nodes
Balmer Series

41. Kinetic Energy of an individual particle formula
Gamma Ray-
isothermal
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
M = square root (3RT/mm)

42. Ptotal=P1+P2+P3+...

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43. Has values 1 -2 -3 -...; tells energy levels
Calorimetry
Principal Quantum Number
pent-
Linear

44. AX3
force x distance = work done
indicator
trigonal planar
carbonate

45. The mixing of native atomic orbitals to form special orbitals for bonding
Solute
Pressure of H2O must be Subtracted
Coordination Compound
Hybridization

46. Type of system in which the energy may escape - but the mass is conserved
Isolated System
Molarity
AE = q + w
Closed System

47. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
0
1atm=?mmHg/Torr
but-

48. Temperature-pressure combination at which solid - liquid - and gas states appear
e-
triple point
oxalate
3.0x108m/s

49. If Q>Ksp
a precipitate forms
Osmotic Pressure
Metalliods
London Dispersion Forces

50. Color of Na (flame test)
yellow
Valence Electrons(assigned)
-(q of H2O + q of cal)
Acids

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AP Chemistry

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