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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. Ideal Gas Law Formula
linear
PV=nRT
8.31J/Kmol
N=N.(0.5)^time/time half-life

2. Pressure Units/Conversions
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
Heat Capacity (C)
supercritical fluid
1 atm = 760 mmHg = 101.3 kPa

3. 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)
catalyst
Ionic Compounds
moles of solute/ L of solution
titrant buret

4. Change in Energy = ? (in terms of constant pressure; for gasses)
Faraday
AE= AH - RTAn
heat of fusion
Mass

5. AX6
octahedral
Molecular Orbitals (MOs)
n (first quantum number)
P of a =(X of a)(total pressure)

6. (# of lone pair e-)+1/2(# of shared e-)
hydro-ic acid
t-shape
Mass
Valence Electrons(assigned)

7. Amount of gravitational force exerted on an object
Weight
Equilibrium constant
insoluble
anode

8. Substances that form H+ when dissolved in water; proton donors
Van't Hoff factor
triple point
Acids
melting

9. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
Dalton's Law
-ous acid
bent

10. Mass #
specific heat
Volt
catalyst
# protons + # neutrons

11. Aldehyde suffix
Graham's Law
1.38x10?²³J/K
-al
rate

12. Ester suffix
specific heat
hept-
-oate
Arrhenius base

13. H+ Acceptor
Bronsted-Lowry Base
Formal Charge
1atm=?mmHg/Torr
green/yellow

14. Nonmetal oxide + H2O ->
rate gas A/rate gas B = square root (mm A/ mm B)
acid
Electron Spin Quantum Number
Resonance

15. C2O4²?
Finding Empirical Formulas
oxalate
bent
Allotrope

16. The mixing of native atomic orbitals to form special orbitals for bonding
Galvanic Cell
non-
Hybridization
Alkali metals

17. AX5
# protons (atom is defined by this)
sulfite
trigonal bipyramidal
Cathode

18. (msubs) Can only be +1/2 or -1/2
Electron Spin Quantum Number
5% rule
AH
viscosity

19. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
conjugate base
Molecular
third
Hydrogen bonding

20. Force acting over distance
Work
entropy
red
0

21. Symbol for the heat absorbed or lost molecularly (PER MOLE)
third
AH
Law of Definite Proportion
purple --> pink

22. Driving force of the electrons
-ol
bent
Cell Potential (Ecell)
8.31J/Kmol

23. Heat capacity formula
Bond Order
Integrated First-Order Rate Law
Ampere
C=(mass)(specific heat)

24. Matter can't be created nor destroyed
Heisenberg Uncertainty Principle
Nodes
Law of Conservation of Mass
charge

25. Degree of disorder in a system
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
v3RT/M(in kg)
entropy (S)
Surroundings

26. Point at which solid?liquid occurs
red
Molal FP Depression Constant
melting point
Isotopes

27. OH¹?
hydroxide
0
System
+1 - except if bonded to Alkali Metal -1

28. Combined Gas Law Formula
Boltzmann distribution
Multiplying
paramagnetic
P1V1/N1T1=P2V2/N2T2

29. A solution used in titrations whose concentration is known
standard solution
phosphate - sulfide - carbonate - sulfate
dichromate
freezing

30. What is defined by you taken from the whole universe
System
chlorate
Lone Pair
nitrite

31. O²?
alkyne
oxide
salt bridge
sulfate

32. [A]0/2k
Zero-Order Half Life
Matter
Atmospheric Pressure
effects of IMF

33. Ether prefix
Cation
methoxy-
phosphate
analyte

34. l=1
ammonium
p
Pressure
Hydrogen bonding

35. A device used to measure Delta H
C + 273
spontaneity
Calorimeter
London Dispersion Forces

36. (organics) nine carbons
oct-
mol
non-
endothermic

37. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Balmer Series
Alpha Particles-
Formal Charge
Temperature

38. STP
0 degrees C - 1 atm
Standard Temperature and Pressure
activated complex (transition state)
bond energy

39. AX3E2
Matter
chromate
T-shape
Galvanic Cell

40. #NAME?
oxidizing agent
Nernst Equation
rate law
E

41. F¹?
flouride
22.4L
Q>K
Ag+ - Pb2+ - Hg2+

42. Isotope
Molecular Orbitals (MOs)
octahedral
condensation
different # of neutrons

43. A single substance that may be an acid or a base (i.e. water)
but-
indicator
octahedral
Amphoteric

44. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
permanganate
End Point
Solute

45. When n=5 ->2 - color=
triple point
viscosity
blue-violet
3/2RT

46. When n=4 ->2 - color=
surroundings
blue-green
electron affinity
Pi Bond

47. If Q>Ksp
Heisenberg Uncertainty Principle
a precipitate forms
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Integrated Zero-Order Rate Law

48. Organic w/ -NH2
Linear
amine
critical point
square pyramidal

49. Wavelength symbol
-(P)(Change in V)
lambda
entropy (S)
activated complex (transition state)

50. Proton (symbol)
Hund's Rule
p+
3.0x108m/s
salt bridge

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AP Chemistry

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