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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. C2O4²?
heat of vaporization
-al
oxalate
no precipitate forms

2. l=3
22.4L
oxidation
f
E

3. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Law of Multiple Proportions
5% rule
1atm=?mmHg/Torr
Acid + Base --> Salt + Water

4. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
blue-green
Molecular Compounds
First-Order Half Life

5. Does the same as equilibrium expression - except it uses initial concentrations
Reaction Quotient (Q)
Weight
reduction
Standard Temperature and Pressure

6. ClO3²?
3/2RT
chlorate
?Tf= kf x molality
-(P)(Change in V)

7. ClO2¹?
Closed System
Hybridization
activation energy
chlorite

8. The chemical formed when an acid donates a proton
nitrate
M1V1=M2V2
Theory of Relativity
conjugate base

9. Happens at lines in phase change charts
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
equilibrium
group
Delta H or Enthalpy Change

10. Kinetic Energy of an individual particle formula
M = square root (3RT/mm)
First-Order Rate Law
Arrhenius base
third

11. H?+OH??H2O
strong acid strong base rxn
Temperature
Trigonal Planar
melting

12. q H2O = ?
sulfite
msAT
0
permanent gases

13. How to Find an Empirical Formula Given Percentages
AH
Average KE = 1/2(mass)(average speed of all particles)
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
P1V1/N1T1=P2V2/N2T2

14. The likelihood that a rxn will occur "by itself"
ammonium
not spontaneous
spontaneity
hydrolysis

15. ClO4¹?
d
perchlorate
Bronsted-Lowry Base
Trigonal Planar

16. Color of Na (flame test)
Trigonal Planar
Oxidizing Agent
Aufbau Principle
yellow

17. Oxoacid solution (such as HSO4-) forms...
oxide gas and water
iodide
E
mol

18. Change in Energy (AE) = ? (in terms of work)
AE = q + w
Molality
Solvent
Temperature

19. ?T=k*m(solute)
+1 - except if bonded to Alkali Metal -1
Dalton's Law of Partial Pressures
nitrate
Molal BP Elevation Constant

20. The rest of the universe (in thermodynamics)
surroundings
phosphate - sulfide - carbonate - sulfate
Isolated System
carbohydrates

21. Ability of an atom in a molecule to attract shared electrons to itself
exothermic
Dipole-dipole forces
Principal Quantum Number
Electronegativity

22. J/°Cmol or J/Kmol
strong bases
Molar Heat Capacity
oxidizing agent
entropy (S)

23. If Q>Ksp
bromate
Pi Bond
a precipitate forms
Strong acid weak base rxn

24. Increase Volume
2nd law of thermodynamics
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Increase Temperature
activated complex (transition state)

25. Energy needed to break a bond
endless
chromate
bond energy
Cathode

26. 1 sigma bond - 2 pi bonds
hydro-ic acid
London dispersion forces
triple bond
f

27. (organics) one carbon
Volt
meth-
d
sulfite

28. Molality =
q
3rd law of thermodynamics
moles solute/kg solvent
adhesion

29. AX5E
square pyramidal
t-shape
second
-(q of H2O + q of cal)

30. Force per unit area
ionic
log[H+]
Second-Order Half Life
Pressure

31. 2+ charge
Speed of light
hex-
Alpha Particles-
equilibrium

32. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
pi=(nRT)/v
q
Ligand
nitrite

33. Oxidation # of Compounds
acid
0
analyte
square planar

34. (organics) seven carbons
effects of IMF
Ampere
Molarity
hept-

35. n+m (these are orders of reactants)
Sigma Bond
Overall Reaction Order
solid CO2
triple bond

36. Amount of gravitational force exerted on an object
Weight
Surroundings
Solubility Product (Ksp)
green/yellow

37. Releases/gives off heat (negative value)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
reduction
Exothermic
hydro-ic acid

38. An element with several different forms - each with different properties (i.e. graphite & diamond)
perchlorate
Allotrope
end point
acetate

39. Elements in groups 3-12
first
Transition metals
like
Valence Electrons(assigned)

40. Raising heat - adding catalyst - heighten concentration - bigger surface area
sulfate
methods of increasing rate
Specific Heat (s)
Solvent

41. Average speed of gas
v3RT/M(in kg)
Percent Yield
deposition
Integrated Zero-Order Rate Law

42. Change in Energy = ? (in terms of constant pressure; for gasses)
moles of solute/ L of solution
AE= AH - RTAn
hept-
Galvanic Cell

43. High-energy light
Chemical Bonds
Molecular Orbitals (MOs)
Gamma Ray-
pi=(nRT)/v

44. Puts OH? into solution
Acids
Arrhenius base
Temperature
X of a = moles a/total moles

45. The energy required to raise 1 g of substance 1 degree C
oxidation
Specific Heat (s)
heat capacity
0

46. Coffee Cup Calorimeter
Exothermic
Constant Pressure
red
Osmotic Pressure

47. Driving force of the electrons
Molecular Orbitals (MOs)
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
Its element
Cell Potential (Ecell)

48. Substances that form H+ when dissolved in water; proton donors
square planar
Acids
Solute
P1= X1P1°

49. Osmotic pressure=MRT
Osmotic Pressure
dec-
0
sulfide

50. Type of system in which the energy may escape - but the mass is conserved
Closed System
purple --> pink
reduction
P1V1/N1T1=P2V2/N2T2

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AP Chemistry

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