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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. Spectrum of light when an electron drops to energy level n=2
eth-
increasing
Balmer Series
Faraday

2. A device used to measure Delta H
k=Ae^(-Ea/RT)
Calorimeter
CAT
AH

3. Isotope
moles of solute/ L of solution
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
k=Ae^(-Ea/RT)
different # of neutrons

4. 90°&120° - dsp^3
paramagnetic
Trigonal Bipyramidal
like
conjugate base

5. Entropy in the universe is always...
high pressure - low temperature
Pressure of H2O must be Subtracted
increasing
msAT

6. High-speed electrons
A Roman numeral
hept-
Beta Particles-
Electronegativity

7. Elements which have unpaired electrons and highly affected by magnetic fields
are not
paramagnetic
s (fourth quantum number)
melting

8. A measure of randomness or disorder
entropy
0.0826Latm/Kmol
condensation
Molality

9. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Increase Temperature
Quantum Model
amine
London dispersion forces

10. Half cell in which oxidation occurs
rate
anode
Adding
Solvent

11. x can be ignored when % ionization is <5%
Transition metals
5% rule
Integrated First-Order Rate Law
hydroxide

12. PV=nRT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Ideal Gas Law
cathode
strong acid strong base rxn

13. Increase Volume
Calorimetry
Increase Temperature
nu
Bond enthalpy

14. When n=3 ->2 - color=
entropy
red
dichromate
Equilibrium Expression

15. Point at which solid?liquid occurs
Molecular Compounds
yellow --> green
melting point
Law of Conservation of Energy

16. Point at which the titrated solution changes color
alkyne
bent
end point
electrolyte

17. The driving force for a spontaneous is an increase in entropy of the universe
rate gas A/rate gas B = square root (mm A/ mm B)
E
Pauli Exclusion Principle
Entropy (S)

18. J/°Cg or J/Kg
complex ions
heat capacity
Effusion
Specific Heat Capacity

19. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Work
moles of solute/ L of solution
Resonance
nitrate

20. A device in which chemical energy is changed to electrical energy
Law of Multiple Proportions
Galvanic Cell
Bond enthalpy
Beta Particles-

21. (organics) six carbons
Cell Potential (Ecell)
London dispersion forces
hex-
Net Ionic Equation

22. Heat needed to change 1 g of substance to 1°C
0 degrees C - 1 atm
specific heat
mol Fraction
Valence Electrons(assigned)

23. The transfer of energy between two objects due to temperature difference
Calorimetry
moles of solute/ L of solution
Heat
-ous acid

24. AX6
vapor pressure
octahedral
end point
van't Hoff Factor

25. NH4¹?
Naming Binary Ionic Compounds
meth-
ammonium
hydro-ic acid

26. Oxidation # of Hydrogen
conjugate base
Magnetic Quantum Number (ml)
specific heat
+1 - except if bonded to Alkali Metal -1

27. q cal = ?
actual yield/theoretical yield x 100%
Beta Particles-
CAT
methods of increasing rate

28. AX3E
trigonal pyramidal
Dalton's Law of Partial Pressures
acid
Matter

29. 90° - d^2sp^3
Second-Order Rate Law
rate gas A/rate gas B = square root (mm A/ mm B)
oxide gas and water
Octahedral

30. Bomb Calorimeter
Constant Volume
endless
Chemical Kinetics
moles solute/kg solvent

31. Unit of electrical potential; J/C
chloride
Volt
electrolyte
X of a = moles a/total moles

32. Degree of disorder in a system
Heat Capacity (C)
4.184
Isolated System
entropy (S)

33. Positive ion
Cation
Van't Hoff factor
3rd law of thermodynamics
Polar Covalent

34. Dirrect Method Formula
hydro-ic acid
r1/r2
Graham's Law
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

35. Chemical composition of dry ice
excess reactant
solid CO2
alkane
State Functions

36. AX5
trigonal bipyramidal
adhesion
0 degrees C - 1 atm
period

37. AX5E
Acid + Base --> Salt + Water
Ideal Gas Law
square pyramidal
+1 - except if bonded to Alkali Metal -1

38. Atoms combine in fixed whole # ratios
Law of Multiple Proportions
Zero-Order Half Life
Hydrogen bonding
Heisenberg Uncertainty Principle

39. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Buffer
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Quantum Numbers
Ligand

40. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
Coordination Compound
Ligand
LeChatelier's Principle
Resonance

41. Different form of same element
Heat Capacity (C)
Enthalpy of Solution
octahedral
allotrope

42. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
Anion
iodide
Entropy (S)

43. CN¹?
chlorite
Heat
N=N.(0.5)^time/time half-life
cyanide

44. A monoatomic cation takes name from...
Hund's Rule
heat of vaporization
Its element
indicator

45. Where oxidation occurs
Endothermic
1 atm
Anode
STP

46. (organics) one carbon
Anion
E
Bronsted-Lowry Base
meth-

47. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals

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48. When n=4 ->2 - color=
catalyst
reduction agent
blue-green
Pi Bond

49. Ecell= E°cell -RT/nF x lnQ
London dispersion forces
Manometer
Nernst Equation
first

50. Oxidation # of Oxygen
condensation
Alkali metals
-2 - with peroxide -1
bent