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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. Oxidation # of Hydrogen
Adding
seesaw
Pauli Exclusion Principle
+1 - except if bonded to Alkali Metal -1

2. Molecules' tendency to stick to one another
P1= X1P1°
cohesion
Matter
entropy (S)

3. AX5
Pauli Exclusion Principle
trigonal bipyramidal
First-Order Rate Law
permanganate

4. Composition Formula
Tetrahedral
Dipole Moment
Molar Mass of Element/ Total Molar Mass %
Pressure

5. A measure of resistance of an object to a change in its state of motion
Mass
Chemical Kinetics
hydroxide
X of a = moles a/total moles

6. Pure metal or metal hydride + H20 ->
base and hydrogen gas
sublimation
hept-
m (third quantum number)

7. Substance that - when dissolved - is conductive
electrolyte
heat capacity
allotrope
Isotopes

8. Half cell in which reduction occurs
Cation
charge
oct-
cathode

9. Elements which have unpaired electrons and highly affected by magnetic fields
Finding Empirical Formulas
Atmospheric Pressure
solid CO2
paramagnetic

10. Spectrum of light when an electron drops to energy level n=2
complex ions
Balmer Series
Aufbau Principle
Cell Potential (Ecell)

11. E=mc^2
catalyst
Theory of Relativity
standard solution
Covalently w/in themselves - Ionicly bonded w/ each other

12. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

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13. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
?Tb= kb x molality
effects of IMF
Cg=kPg

14. l=0
carbonate
Gamma Ray-
viscosity
s

15. Instrument used to measure the pressure of atmospheric gas
Ionic Compounds
Enthalpy of Solution
Ampere
Barometer

16. Kinetic Energy is proportional to ______
PV=nRT
?Tf= kf x molality
Temperature
Electronegativity

17. Peak of energy diagram
oxide
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
increasing
activated complex (transition state)

18. Consists of a complex ion - a transition metal with attached ligands - and counterions
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Q>K
Coordination Compound
Manometer

19. Planck's constant - used to calculate energy w/frequency
Standard Temperature and Pressure
6.63x10?³4Js
blue-green
4.184

20. 109.5° - sp^3
1atm=?Pa
PV=nRT
Tetrahedral
-ic acid

21. Energy required for liquid?gas
Ampere
heat of vaporization
Counterions
q

22. Symbol for Total Heat absorbed or released
Molar Heat Capacity
Ionic Compounds
adhesion
q

23. Faraday's constant
moles solute/kg solvent
Law of Conservation of Energy
96500
weak acid strong base rxn

24. Force acting over distance
?Tf= kf x molality
Work
Galvanic Cell
ether

25. 101 -325 Pa
1atm=?Pa
First-Order Rate Law
Diffusion
base

26. Variable for orientation of orbital (-1 through +1)
AE= AH - RTAn
Work
Le Chatelier's Principle
m (third quantum number)

27. Mass percent
Bronsted-Lowry Base
g solute/g solvent x 100
Integrated Second-Order Rate Law
Positive work value; work done on system

28. The likelihood that a rxn will occur "by itself"
spontaneity
PV=nRT
Heat
Average KE = 1/2(mass)(average speed of all particles)

29. Molecules' tendency to stick to the container
endless
Graham's Law
oxide gas and water
adhesion

30. Idea Gas Law (actual rules)
End Point
spontaneity
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
Bond Energy

31. Atoms with the same number of protons but a different number of neutrons
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Quantum Model
rate law
Isotopes

32. If anion ends in -ate - acid name ends in...
-ic acid
non-
% error
STP

33. K
Equilibrium constant
ammonium
Weight
trigonal pyramidal

34. Similar to atomic orbitals - except between molecules
yellow
Molecular
hept-
Molecular Orbitals (MOs)

35. Rate of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
blue-green
Allotrope
conjugate base

36. Lowers activation energy
Its root and adding -ide
Multiplying
no precipitate forms
catalyst

37. Variable for type of orbital
Trigonal Bipyramidal
l (second quantum number)
solid CO2
red/orange

38. (organics) single-bonded compound
hydrocarbons
alkane
Molality
supercritical fluid

39. Ability of an atom in a molecule to attract shared electrons to itself
Ionic
Electronegativity
Percent Yield
rate gas A/rate gas B = square root (mm A/ mm B)

40. Absorbs/takes in heat (positive value)
Nernst Equation
Endothermic
Scientific Method
Weight

41. Ideal Gas Law Formula
Amphoteric
lambda
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
PV=nRT

42. Pairs of electrons localized on an atom
8.314 J/K mol
Law of Multiple Proportions
3/2RT
Lone Pair

43. AX4E
see-saw
4.184
+1 - except if bonded to Alkali Metal -1
Quantum Mechanical Model

44. IMF that exists in polar molecules
yellow --> green
Dipole-dipole forces
hex-
acetate

45. Carbon - hydrogen - oxygen compounds
geometric isomers
Surroundings
-ic acid
carbohydrates

46. Polyatomic Ions (bonding)
Covalently w/in themselves - Ionicly bonded w/ each other
C=(mass)(specific heat)
End Point
X of a = moles a/total moles

47. Weakest IMFs - found in all molecules
Arrhenius Acid
dichromate
London dispersion forces
Calorimeter

48. Melting
1st law of thermodynamics
fusion
?Tb= kb x molality
rate

49. Reverse rxn occurs when
Integrated First-Order Rate Law
Q>K
Percent Yield
isothermal

50. Type of system in which the energy may escape - but the mass is conserved
Closed System
Open System
eth-
period