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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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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. Measure of the average kinetic energy of all the particles in a substance
Oxidizing Agent
Bond Order
Temperature
geometric isomers

2. The reactant that is being reduced - brings about oxidation
Cathode
weak acid strong base rxn
oxidizing agent
activation energy

3. A method of investigation involving observation and theory to test scientific hypotheses
m (third quantum number)
Scientific Method
6.63x10?³4Js
strong acids

4. Puts H? into solution
Bonding Pairs
Arrhenius acid
Colligative properties
-one

5. Delta H (AH) = ?
Magnetic Quantum Number (ml)
heat of fusion
q/moles
Mass

6. If needed - indicate charge of metal(cation) by...
permanganate
A Roman numeral
conjugate base
0.512°C

7. 1 sigma bond
perchlorate
single bond
0.0821 atm L/mol K
endless

8. =vM2/M1
cathode
Amphoteric
s orbitals
r1/r2

9. Entropy in the universe is always...
Bronsted-Lowry Acid
Ionic
increasing
3rd law of thermodynamics

10. What is defined by you taken from the whole universe
linear
Decrease Volume and Increase Temperature
System
bond energy

11. STP
green/yellow
0 degrees C - 1 atm
Faraday
Normality

12. If anion ends in -ide - acid name ends in
Equilibrium constant
Cell Potential (Ecell)
hydro-ic acid
P1= X1P1°

13. Melting
fusion
Law of Conservation of Mass
like
exothermic

14. NH4¹?
Solvent
Hess's Law
soluble
ammonium

15. The minimum energy that molecules must possess for collisions to be effective - Ea
activation energy
deposition
Positive work value; work done on system
Temperature

16. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Average KE = 1/2(mass)(average speed of all particles)
complex ions
Hybridization
Solvent

17. n+m (these are orders of reactants)
Decrease Volume and Increase Temperature
Overall Reaction Order
Closed System
0

18. 0.00°C - 1 atm
0.512°C
Nernst Equation
2nd law of thermodynamics
Standard Temperature and Pressure

19. H + donor
Bronsted-Lowry Acid
+1 - except if bonded to Alkali Metal -1
hex-
bent

20. (organics) eight carbons
-oic acid
oct-
lambda
n (first quantum number)

21. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
voltaic cells
hydrolysis
Its root and adding -ide
Molecule

22. As protons are added to the nucleus - electrons are similarly added
Joule
Aufbau Principle
diamagnetic
AE = q + w

23. [A]=-kt + [A]0
endothermic
boiling point
Integrated Zero-Order Rate Law
a precipitate forms

24. AX6
Bases
yellow
octahedral
8.314 J/K mol

25. Variable for type of orbital
see-saw
Law of Conservation of Energy
l (second quantum number)
Octahedral

26. The line running between the atoms
msAT
1.38x10?²³J/K
mol
Sigma Bond

27. PO4³?
phosphate
standard solution
Surroundings
surroundings

28. Idea Gas Law (actual rules)
Heat
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
rate
Boltzmann distribution

29. Color of Sr (flame test)
1.38x10?²³J/K
Hydrogen bonding
v3RT/M(in kg)
red

30. (organics) three carbons
Zero-Order Half Life
prop-
Law of Conservation of Energy
Dipole Moment

31. Universal IMF for nonpolar molecules
sublimation
London dispersion forces
p orbitals
green/yellow

32. Degree of disorder in a system
Calorimetry
First-Order Rate Law
entropy (S)
vapor pressure

33. IMF that occurs with FON
strong acids
equilibrium
Hydrogen bonding
Electron Spin Quantum Number

34. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Limiting reactant
Integrated First-Order Rate Law
f

35. Polyatomic Ions (bonding)
Buffer
dichromate
Linear
Covalently w/in themselves - Ionicly bonded w/ each other

36. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
Lone Pair
Equilibrium constant
Equilibrium Expression

37. 2+ charge
Alpha Particles-
salt bridge
entropy (S)
oxalate

38. SO4²?
pent-
melting point
carbonate
sulfate

39. Ka=[products]^m/[reactants]^n
Molal BP Elevation Constant
Acid Dissociation Constant
Cathode
Arrhenius equation

40. Combined Gas Law Formula
alkene
Manometer
Pauli Exclusion Principle
P1V1/N1T1=P2V2/N2T2

41. Involves quantum numbers
increasing
Quantum Mechanical Model
trigonal planar
Constant Volume

42. frequency symbol
Balmer Series
linear
nu
Sigma Bond

43. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
ether
chlorate
Ionic Compounds
Oxidizing Agent

44. Oxidation # of Polyatomic Ions
Atmospheric Pressure
adiabatic
?Tb= kb x molality
charge

45. How to Find a Weighted Average
96500
nu
viscosity
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

46. Solution used in titration
Hund's Rule
titrant buret
trigonal planar
Cell Potential (Ecell)

47. Like dissolves...
solid CO2
like
PV=nRT
E

48. Elements in groups 3-12
phosphate - sulfide - carbonate - sulfate
Bronsted-Lowry base
t-shape
Transition metals

49. Ptotal=Pa+Pb+Pc....

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50. Ecell= E°cell -RT/nF x lnQ
Nernst Equation
rate
chloride
Beta Particles-