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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. (A) - C/s
-2 - with peroxide -1
Ampere
Counterions
E

2. AX6
octahedral
Angular Momentum Quantum Number
heat capacity
Ionic

3. Expresses how the concentrations depend on time
Antibonding Molecular Orbital
n (first quantum number)
Integrated Rate Law
1/2mv²

4. Solid to liquid
8.314 J/K mol
3/2RT
melting
Integrated Rate Law

5. Weakest IMFs - found in all molecules
standard solution
+1 - except if bonded to Alkali Metal -1
London dispersion forces
carbonate

6. Ptotal=P1+P2+P3+...

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7. 2 or more covalently bonded atoms
System
oct-
Molecule
Linear

8. Passage of gas through tiny orifice
Effusion
-2 - with peroxide -1
N=N.(0.5)^time/time half-life
trigonal planar

9. 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)
State Functions
Multiplying
square planar
Constant Pressure

10. r=k
M = square root (3RT/mm)
bond energy
Zero-Order Rate Law
Constant Pressure

11. Substance that - when dissolved - is conductive
Exothermic
electrolyte
Polar Covalent
oxide gas and water

12. How to Find a Weighted Average
Acids
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Reaction Quotient (Q)
Metalliods

13. If Q>Ksp
8.31J/Kmol
Arrhenius equation
Dalton's Law of Partial Pressures
a precipitate forms

14. Atoms combine in fixed whole # ratios
# protons + # neutrons
Le Chatelier's Principle
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Law of Multiple Proportions

15. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
supercritical fluid
% error
Hydrogen bonding
d orbitals

16. Connects the 2 half cells in a voltaic cell
salt bridge
second
Arrhenius equation
Bases

17. Ionizes to produce OH- Ions
moles of solute/ L of solution
chlorite
Specific Heat (s)
Arrhenius Base

18. 2+ charge
Alpha Particles-
are
AE= AH - RTAn
meth-

19. Substances w/ critical temperatures below 25°C
Amount of atoms present
Acid Dissociation Constant
permanent gases
nu

20. H?+OH??H2O
1/2mv²
increasing
strong acid strong base rxn
Solute

21. (organics) three carbons
prop-
trigonal planar
1 atm
Formal Charge

22. Combined Gas Law Formula
First-Order Rate Law
A Roman numeral
e-
P1V1/N1T1=P2V2/N2T2

23. Ester suffix
LE Model
Reaction Quotient (Q)
-oate
exothermic

24. kf of water
1.86°C
titrant buret
8.314 J/K mol
Molecular

25. Determined by the formula h/m(in kg)v - (v=velocity)
heat of vaporization
acid
wavelength
-oic acid

26. .69/k
d orbitals
Delta H or Enthalpy Change
First-Order Half Life
Specific Heat (s)

27. A device used to measure Delta H
Calorimeter
Open System
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
electron affinity

28. Color of Na (flame test)
yellow
amine
Gamma Ray-
square planar

29. Negative enthalpy - heat flows into surroundings
Overall Reaction Order
linear
condensation
exothermic

30. Ecell= E°cell -RT/nF x lnQ
s (fourth quantum number)
Integrated Zero-Order Rate Law
Nernst Equation
methoxy-

31. The heat changed in a chemical reaction.
Molal FP Depression Constant
1.86°C
Reaction Quotient (Q)
Thermochemistry

32. Type of system in which nothing is transfered (no mass or energy); ideal
vapor pressure
London dispersion forces
Isolated System
no precipitate forms

33. AX6
octahedral
6.63x10?³4Js
Ideal Gas Law
Angular Momentum Quantum Number

34. How to Find an Empirical Formula Given Percentages
voltaic cells
base and hydrogen gas
Theoretical yield
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

35. The actual amount of product produced in an experiment
actual yield/theoretical yield x 100%
Colligative properties
Manometer
experimental yield

36. Substances that form H+ when dissolved in water; proton donors
mol
endless
Constant Pressure
Acids

37. Measure of the average kinetic energy of all the particles in a substance
Temperature
q
Joule
Dipole Moment

38. Where reduction occurs
Ampere
Cathode
hept-
square pyramidal

39. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Its root and adding -ide
Amount of atoms present
Integrated Zero-Order Rate Law
yellow --> green

40. Point at which the titrated solution changes color
Law of Conservation of Mass
-ol
end point
Covalently w/in themselves - Ionicly bonded w/ each other

41. Like dissolves...
like
blue-violet
Quantum Numbers
system

42. Change without heat transfer between the system and its surroundings
Joule
Solution
adiabatic
Bronsted-Lowry Base

43. When n=5 ->2 - color=
blue-violet
bromate
eth-
Bronsted-Lowry Base

44. Two molecules with identical connectivity but different geometries
Law of Multiple Proportions
increasing
chromate
geometric isomers

45. Mass #
Atmospheric Pressure
Pi Bond
% error
# protons + # neutrons

46. Kinetic Energy per mol
solid CO2
entropy
3/2RT
Work

47. Change in moles (An) =?
London dispersion forces
(moles of products that are gasses) - (moles of reactants that are gasses)
London Dispersion Forces
Formal Charge

48. For significant digits - trailing zeros _____ significant
seesaw
are
acid
Beta Particles-

49. Reactant that's completely used up in a chemical reaction
Limiting reactant
Hund's Rule
not spontaneous
Effusion

50. Point where acid completely neutralizes base
Open System
equivalence point
Oxidation is Loss Reduction is Gain
f