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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. The total energy of the universe is constant - all systems tend towards minimum energy
oxidation
Its root and adding -ide
1st law of thermodynamics
s

2. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
3/2RT
X of a = moles a/total moles
spontaneous
0

3. Point at which the titrated solution changes color
end point
Molecular Compounds
adhesion
Metalliods

4. The rest of the universe (in thermodynamics)
trigonal bipyramidal
surroundings
1.38x10?²³J/K
equivalence point

5. How to Find an Empirical Formula Given Percentages
hydroxide
standard solution
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
-(P)(Change in V)

6. Delta H (AH) = ?
first
q/moles
Dalton's Law
Molar Mass of Element/ Total Molar Mass %

7. Carboxylic acid ending
rate law
Cg=kPg
Amount of atoms present
-oic acid

8. Different form of same element
?Tf= kf x molality
nitrite
allotrope
Bases

9. To find activation energy use the...
Arrhenius equation
moles of solute/ L of solution
Trigonal Bipyramidal
Strong acid weak base rxn

10. Like dissolves...
like
ammonium
wavelength
Temperature

11. Measure of the average kinetic energy of all the particles in a substance
Bonding Pairs
Ligand
Temperature
Acid + Base --> Salt + Water

12. CN¹?
charge
Hybridization
cyanide
Bronsted-Lowry Base

13. kf of water
-oic acid
Polar Covalent
1.86°C
freezing

14. 1 sigma bond - 1 pi bond
double bond
nitrate
vapor pressure
charge

15. Phase change from gas to solid
excess reactant
Dalton's Law
deposition
strong acid strong base rxn

16. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Reducing Agent
tetrahedral
Chemical Kinetics
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

17. The entropy of a pure perfectly formed crystal @0K is 0
-2 - with peroxide -1
C + 273
3rd law of thermodynamics
1 atm = 760 mmHg = 101.3 kPa

18. r=k[A]
condensation
Graham's Law
First-Order Rate Law
Manometer

19. How to Find a Weighted Average
Pressure
purple --> pink
Ionic Compounds
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

20. Oxidation # of Ions
iodide
Heisenberg Uncertainty Principle
charge
Cation

21. IMF that exists in polar molecules
heat capacity
Solute
Dipole-dipole forces
Molarity

22. OIL RIG
high pressure - low temperature
London dispersion forces
Oxidation is Loss Reduction is Gain
Surroundings

23. Ending for alcohols
Heat Capacity (C)
violet
-ol
M1V1=M2V2

24. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
charge
endless
Equilibrium Expression
standard solution

25. Mol/kg of solvent - used in calculating colligative properties
Molality
-al
% error
s (fourth quantum number)

26. Substances w/ critical temperatures below 25°C
Anode
charge
permanent gases
alkene

27. AH of formation for a substance in its stablest form (how it is found in nature)
oct-
0
Closed System
Law of Definite Proportion

28. Mass/volume
Density
hept-
Adding
Tetrahedral

29. Happens at lines in phase change charts
CAT
Positive work value; work done on system
equilibrium
blue-violet

30. negative ion
Anion
?Hvap
Entropy (S)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

31. 180° - sp
deposition
End Point
Linear
1st law of thermodynamics

32. frequency symbol
moles solute/kg solvent
nu
reduction agent
equivalence point

33. A measure of resistance of an object to a change in its state of motion
Multiplying
Mass
p orbitals
Reaction Quotient (Q)

34. Point at which liquid?gas occurs
% error
surroundings
boiling point
3rd law of thermodynamics

35. Amount of heat needed to change a system by 1°C
heat capacity
Temperature
STP
Q<K

36. PO4³?
phosphate
insoluble
Law of Multiple Proportions
s (fourth quantum number)

37. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
square pyramidal
adhesion
hydroxide

38. A solid or gas that can be formed when 2 or more aqueous reactants come together
1/2mv²
spontaneous
purple
precipitate

39. (organics) triple-bonded compound
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
charge
alkyne
moles of solute/ L of solution

40. Formula used when diluting stock solution (to find amount of water or stock needed)
AH
Pauli Exclusion Principle
1atm=?Pa
M1V1=M2V2

41. Kinetic Energy per mol
anode
3/2RT
1 atm
oxidation

42. AX3E2
indicator
t-shape
sublimation
seesaw

43. AX4E2
deposition
n (first quantum number)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
square planar

44. Similar to atomic orbitals - except between molecules
geometric isomers
Molecular Orbitals (MOs)
Integrated Rate Law
Open System

45. Kinetic Energy of an individual particle formula
Exothermic
M = square root (3RT/mm)
5% rule
Polar Covalent

46. (organics) single-bonded compound
Exothermic
Atmospheric Pressure
First-Order Rate Law
alkane

47. Entropy in the universe is always...
Antibonding Molecular Orbital
increasing
not spontaneous
non-

48. Symbol for Total Heat absorbed or released
q
excess reactant
Solution
Antibonding Molecular Orbital

49. Change in Energy (AE) = ? (in terms of work)
sulfide
AE = q + w
Second-Order Rate Law
cyanide

50. Color of Na (flame test)
blue-green
Law of Definite Proportion
0
yellow