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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. Melting
System
square planar
fusion
Specific Heat Capacity

2. Composition Formula
Molar Mass of Element/ Total Molar Mass %
alkyne
Positive work value; work done on system
increasing

3. Point at which vapor pressure=air pressure above
5% rule
boiling point
purple
Galvanic Cell

4. Color of Cs (flame test)
blue
bromate
d orbitals
excess reactant

5. Amine prefix
oct-
Amino-
square pyramidal
diamagnetic

6. Puts OH? into solution
deposition
Acid Dissociation Constant
Arrhenius base
Kinetic Molecular Theory - for ideal gases

7. Solution in flask being titrated
freezing
Transition metals
Enthalpy of Solution
analyte

8. Carbon - hydrogen - oxygen compounds
standard solution
s orbitals
carbohydrates
n0

9. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
Theory of Relativity
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Volt

10. Peak of energy diagram
Van't Hoff factor
1.38x10?²³J/K
equivalence point
activated complex (transition state)

11. 101 -325 Pa
square planar
Q<K
1atm=?Pa
Buffer

12. This MUST be determined experimentally
Closed System
rate law
blue-violet
Calorimetry

13. An equilibrium expression
spontaneity
trigonal planar
Endothermic
Solubility Product (Ksp)

14. NO3¹?
tetrahedral
equilibrium
nitrate
perchlorate

15. NO2¹?
Ideal Gas Law
Gamma Ray-
pi=(nRT)/v
nitrite

16. Color of Ba (flame test)
end point
green/yellow
Kinetic Molecular Theory - for ideal gases
activation energy

17. 1 sigma bond - 1 pi bond
Cg=kPg
activation energy
Joule
double bond

18. Average Kinetic Energy Formula
Zero-Order Rate Law
seesaw
Average KE = 1/2(mass)(average speed of all particles)
complex ions

19. (organics) one carbon
conjugate base
meth-
oxidizing agent
specific heat

20. BrO3¹?
Net Ionic Equation
bromate
vapor pressure
Integrated First-Order Rate Law

21. ?T=k*m(solute)
nitrite
melting point
pi=(nRT)/v
Molal FP Depression Constant

22. OH¹?
hydroxide
hex-
n0
permanganate

23. These orbitals are diagonal
Second-Order Half Life
d orbitals
iodide
Dalton's Law

24. C2H3O2¹?
acetate
electron affinity
Equivalence Point
red

25. Ecell= E°cell -RT/nF x lnQ
8.31J/Kmol
Octahedral
Monoprotic
Nernst Equation

26. R in instances that pertain to energy
Ideal Gas Law
8.314 J/K mol
alkyne
-oate

27. ClO4¹?
8.31J/Kmol
Electron Spin Quantum Number
perchlorate
but-

28. J/°Cmol or J/Kmol
voltaic cells
Molar Heat Capacity
reduction
l (second quantum number)

29. l=3
f
solid CO2
Alpha Particles-
Law of Conservation of Mass

30. A method of investigation involving observation and theory to test scientific hypotheses
Bases
Scientific Method
Heat Capacity (C)
zero

31. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
iodide
Finding Empirical Formulas
Lone Pair
Acids

32. Matter can't be created nor destroyed
purple
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
strong acids
Law of Conservation of Mass

33. =vM2/M1
viscosity
d
r1/r2
Hund's Rule

34. H+ Acceptor
Solution
dichromate
Bronsted-Lowry Base
flouride

35. Dirrect Method Formula
catalyst
Molality
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Equilibrium constant

36. ClO3²?
chlorate
endothermic
cathode
sulfate

37. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Equilibrium Expression
Quantum Model
blue-violet
1.86°C

38. Symbol for the heat absorbed or lost molecularly (PER MOLE)
Integrated Rate Law
AH
Polar Covalent
soluble

39. 1/[A] vs. time is a ...-order reaction
AE= AH - RTAn
second
Strong acid weak base rxn
London dispersion forces

40. When ____ significant digits - round answer to least decimal place
Sigma Bond
Adding
?Tb= kb x molality
PV=nRT

41. Variable for orientation of orbital (-1 through +1)
m (third quantum number)
r1/r2
Ag+ - Pb2+ - Hg2+
Q<K

42. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Dalton's Law
Magnetic Quantum Number (ml)
Le Chatelier's Principle
-(P)(Change in V)

43. Instrument used to measure the pressure of atmospheric gas
Barometer
bent
n0
Pauli Exclusion Principle

44. Amount of heat needed to change a system by 1°C
hex-
red/orange
-(P)(Change in V)
heat capacity

45. Atomic #
Positive work value; work done on system
Principal Quantum Number
chlorate
# protons (atom is defined by this)

46. Pure metal or metal hydride + H20 ->
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
base and hydrogen gas
Positive work value; work done on system
Amino-

47. E?s fill the lowest energy orbital first - then work their way up
Work
linear
Aufbau Principle
Exothermic

48. A monoatomic anion is named by taking...
Root Mean Square Velocity
Its root and adding -ide
dichromate
Cell Potential (Ecell)

49. Has values 1 -2 -3 -...; tells energy levels
Theoretical yield
Second-Order Half Life
Principal Quantum Number
Amphoteric

50. A weak acid that changes color at or near the equivalence point
Buffered Solution
heat of fusion
indicator
Reducing Agent