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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. Ionizes to produce OH- Ions
Lone Pair
fusion
Arrhenius Base
are not

2. These orbitals are spherical
acetate
Oxidation is Loss Reduction is Gain
s orbitals
Bronsted-Lowry Base

3. HF+ OH??H2O
weak acid strong base rxn
+1 - except if bonded to Alkali Metal -1
permanent gases
Molecular

4. Symbol for Enthalpy
Theoretical yield
H
0.512°C
X of a = moles a/total moles

5. Freezing point depression formula
?Tf= kf x molality
Amount of atoms present
charge
Molal FP Depression Constant

6. (organics) seven carbons
Buffered Solution
Quantum Model
Angular Momentum Quantum Number
hept-

7. For significant digits - leading zeros ____ significant
p+
C=(mass)(specific heat)
are not
Its element

8. Ideal Gas Law Formula
phosphate
PV=nRT
Molal FP Depression Constant
vaporization

9. Organic w/ -O-
Average KE = 1/2(mass)(average speed of all particles)
C=(mass)(specific heat)
STP
ether

10. F¹?
# protons + # neutrons
Ampere
flouride
n (first quantum number)

11. Experimental yield/theoretical yieldx100
seesaw
Tetrahedral
Amino-
% yield

12. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Colligative properties
meth-
Cell Potential (Ecell)
oct-

13. Point at which vapor pressure=air pressure above
First-Order Half Life
boiling point
Ideal Gas Law
London Dispersion Forces

14. CrO4²?
Closed System
Transition metals
Hund's Rule
chromate

15. 2 or more covalently bonded atoms
third
ammonium
Molecule
Reducing Agent

16. High-speed electrons
STP
Increase Temperature
alcohol
Beta Particles-

17. Solution used in titration
square pyramidal
titrant buret
v3kT/m
carbonate

18. (organics) six carbons
hex-
equilibrium
freezing
Reducing Agent

19. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

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20. These orbitals are perpendicular
Molar Mass of Element/ Total Molar Mass %
prop-
Entropy (S)
p orbitals

21. How to Find an Empirical Formula Given Percentages
trigonal pyramidal
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
charge
Quantum Numbers

22. Group 1 and heavier Group 2 bases
Nernst Equation
activation energy
strong bases
Le Chatelier's Principle

23. ClO3²?
chlorate
C + 273
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Positive work value; work done on system

24. The energy required to raise 1 g of substance 1 degree C
equilibrium
Specific Heat (s)
Bond Energy
chloride

25. NO2¹?
nitrite
equivalence point
phosphate - sulfide - carbonate - sulfate
vapor pressure

26. As protons are added to the nucleus - electrons are similarly added
H
Increase Temperature
Aufbau Principle
Quantum Model

27. Actual Yield/Theoretical Yield*100%
are not
Graham's Law
boiling point
Percent Yield

28. H?+NH3?NH4
red
Allotrope
ammonium
Strong acid weak base rxn

29. Instrument used to measure the pressure of atmospheric gas
Pi Bond
Molar Mass of Element/ Total Molar Mass %
+1 - except if bonded to Alkali Metal -1
Barometer

30. If anion ends in -ite - acid name ends in...
Ag+ - Pb2+ - Hg2+
sulfite
Pi Bond
-ous acid

31. r=k
Zero-Order Rate Law
heat of vaporization
period
96500

32. OH¹?
Alkali metals
Linear
Joule
hydroxide

33. Ester suffix
Equilibrium constant
Positive work value; work done on system
Sigma Bond
-oate

34. Where oxidation occurs
96500
cathode
q/moles
Anode

35. (organics) five carbons
iodide
8.31J/Kmol
analyte
pent-

36. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
yellow --> green
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
hex-

37. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Resonance
Ag+ - Pb2+ - Hg2+
v3kT/m
London dispersion forces

38. Molality =
moles solute/kg solvent
6.63x10?³4Js
msAT
Chemical Bonds

39. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
Cg=kPg
Counterions
carbonate

40. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
E
Aufbau Principle
Scientific Method
Magnetic Quantum Number (ml)

41. J/°Cmol or J/Kmol
amine
Molar Heat Capacity
heat capacity
X of a = moles a/total moles

42. Cation first - anion second
# protons + # neutrons
Diffusion
Naming Binary Ionic Compounds
Galvanic Cell

43. Organic w/ -NH2
amine
second
-ic acid
hydrocarbons

44. Composition Formula
-ol
Molar Mass of Element/ Total Molar Mass %
Principal Quantum Number
heat capacity

45. J/°Cg or J/Kg
Acid + Base --> Salt + Water
square planar
green/yellow
Specific Heat Capacity

46. The reactant in the reduction reaction that forces the oxidation reaction to occur
second
mol Fraction
viscosity
Oxidizing Agent

47. Oxidation # of Polyatomic Ions
strong bases
Pi Bond
Counterions
charge

48. Faraday's constant
Electron Spin Quantum Number
Cation
96500
flouride

49. Mol of solute/kg of solvent
Arrhenius Acid
Molality
blue
8.314 J/K mol

50. Energy involved in gaining an electron to become a negative ion
% yield
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
electron affinity
4.184