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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. (organics) triple-bonded compound
alkyne
acid
Allotrope
# protons (atom is defined by this)

2. Metal oxide + H20 ->
Hund's Rule
base
# protons + # neutrons
dichromate

3. Boiling point elevation formula
supercritical fluid
Buffer
Pauli Exclusion Principle
?Tb= kb x molality

4. If Q<Ksp
H
3rd law of thermodynamics
heat capacity
no precipitate forms

5. Molarity (M)
trigonal bipyramidal
double bond
moles of solute/ L of solution
prop-

6. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
hydrolysis
Integrated Rate Law
anode
State Functions

7. NO3¹?
Amount of atoms present
e-
charge
nitrate

8. Nonmetal oxide + H2O ->
-al
Molecular Compounds
acid
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

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)
cohesion
State Functions
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Atomic Mass Unit

10. Work = ?
Bronsted-Lowry base
-(q of H2O + q of cal)
Naming Binary Ionic Compounds
-(P)(Change in V)

11. Negative enthalpy - heat flows into surroundings
exothermic
Chemical Kinetics
Molarity
London Dispersion Forces

12. CN¹?
Heat Capacity (C)
Finding Empirical Formulas
viscosity
cyanide

13. Composition Formula
Molar Mass of Element/ Total Molar Mass %
Bronsted-Lowry base
-ol
van't Hoff Factor

14. Anything occupying space and with mass
Quantum Mechanical Model
Coordination Compound
Matter
Chemical Bonds

15. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
Lone Pair
square planar
voltaic cells
red/orange

16. AX6
pent-
Molal BP Elevation Constant
octahedral
System

17. Consists of a complex ion - a transition metal with attached ligands - and counterions
chlorate
Diffusion
Coordination Compound
Density

18. E=mc^2
Theory of Relativity
flouride
Reaction Quotient (Q)
Cathode

19. 1/[A] vs. time is a ...-order reaction
Entropy (S)
second
double bond
melting point

20. H?+NH3?NH4
Strong acid weak base rxn
Bond Energy
cyanide
octahedral

21. Oxoacid solution (such as HSO4-) forms...
oxide gas and water
Valence Electrons(assigned)
Root Mean Square Velocity
yellow --> green

22. Osmotic pressure=MRT
Osmotic Pressure
Exothermic
red
Chemical Bonds

23. A monoatomic anion is named by taking...
Its root and adding -ide
8.314 J/K mol
chromate
conjugate base

24. O²?
oxide
alkane
mol
critical point

25. Temperature-pressure point after which gas can no longer form liquid
Molar Heat Capacity
soluble
critical point
yellow

26. Oxidation # of free elements
red/orange
0
viscosity
complex ions

27. Newton's Second Law
Bases
First-Order Rate Law
hept-
Force = mass x acceleration

28. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium

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29. Atoms combine in fixed whole # ratios
heat capacity
Law of Multiple Proportions
nu
electrolyte

30. Elements on staircase on periodic table
Zero-Order Half Life
0 degrees C - 1 atm
Metalliods
AH

31. Substances that form H+ when dissolved in water; proton donors
Boltzmann distribution
-(q of H2O + q of cal)
Acids
Molecular Compounds

32. OIL RIG
group
M1V1=M2V2
Oxidation is Loss Reduction is Gain
activation energy

33. Ending for alcohols
Alkali metals
Trigonal Bipyramidal
-ol
Alkaline earth metals

34. Amount of product produced when limiting reactant is used up
analyte
Constant Volume
Quantum Model
Theoretical yield

35. Group 1 metals
exothermic
Cg=kPg
Molecular
Alkali metals

36. Aldehyde suffix
lambda
Dipole-dipole forces
-al
electron affinity

37. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
Balmer Series
viscosity
2nd law of thermodynamics

38. The chemical formed when an acid donates a proton
Zero-Order Half Life
conjugate base
titrant buret
hydrolysis

39. r=k
iodide
Molecule
Zero-Order Rate Law
equilibrium

40. Phase change from gas to solid
conjugate base
deposition
Bonding Pairs
-one

41. Oxidation # of Ions
salt bridge
Law of Conservation of Energy
charge
isothermal

42. Cr2O7²?
P of a =(X of a)(total pressure)
Solution
dichromate
dec-

43. Actual Yield/Theoretical Yield*100%
Equilibrium constant
q
Percent Yield
Its root and adding -ide

44. Mass reactants= mass products
Nernst Equation
Law of Conservation of Mass
square pyramidal
Quantum Numbers

45. Universal IMF for nonpolar molecules
London dispersion forces
Cg=kPg
viscosity
like

46. Gain of electrons - decrease in oxidation #
reduction
96500
critical point
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

47. Donates a single H+ Ion (... other prefixes also)
Diffusion
Monoprotic
Quantum Mechanical Model
% yield

48. Degree of disorder in a system
increasing
entropy (S)
Molar Heat Capacity
Molal BP Elevation Constant

49. Liquid to gas
adhesion
Alkaline earth metals
Colligative properties
vaporization

50. Reactant that's completely used up in a chemical reaction
Limiting reactant
work
Boltzmann distribution
Constant Pressure

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AP Chemistry

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