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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. Solution used in titration
Bond Energy
Molecule
Aufbau Principle
titrant buret

2. Rate of Diffusion/Effusion formula
trigonal pyramidal
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
double bond
conjugate base

3. Average Kinetic Energy Formula
N=N.(0.5)^time/time half-life
Average KE = 1/2(mass)(average speed of all particles)
octahedral
Net Ionic Equation

4. CO3²?
Oxidizing Agent
carbonate
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
8.31J/Kmol

5. Color of K (flame test)
Scientific Method
Dalton's Law
Atomic Mass Unit
purple

6. The driving force for a spontaneous is an increase in entropy of the universe
t-shape
Entropy (S)
-ous acid
alcohol

7. r=k
AE = q + w
Zero-Order Rate Law
Positive work value; work done on system
oct-

8. The energy required to raise 1 g of substance 1 degree C
are
Ideal Gas Law
Specific Heat (s)
chloride

9. (organics) one carbon
charge
Hess's Law
Valence Electrons(assigned)
meth-

10. Entropy in the universe is always...
-al
Theory of Relativity
hydrocarbons
increasing

11. 0.00°C - 1 atm
deposition
Endothermic
Standard Temperature and Pressure
catalyst

12. If Q<Ksp
Molecular
adiabatic
condensation
no precipitate forms

13. Average speed of gas
Ionic
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
-(P)(Change in V)
v3RT/M(in kg)

14. Consists of a complex ion - a transition metal with attached ligands - and counterions
Linear
hydrolysis
acetate
Coordination Compound

15. Half cell in which reduction occurs
Molarity
square planar
cathode
% yield

16. The weighted average of all the isotopes that an atom can have (in g/mol)
London dispersion forces
Isolated System
Atomic Mass Unit
Integrated Zero-Order Rate Law

17. 2 or more covalently bonded atoms
anode
Standard Temperature and Pressure
Molecule
a precipitate forms

18. Substance that - when dissolved - is conductive
electrolyte
Cell Potential (Ecell)
Diffusion
phosphate

19. AX4E2
Volume Metric Flask & Pipet
carbohydrates
square planar
?Tf= kf x molality

20. When gas expands ...
oxide gas and water
Ionic Compounds
system
Negative work value; work done by system

21. Energy can't be created nor destroyed
Law of Conservation of Energy
Law of Definite Proportion
d
Molecule

22. A device in which chemical energy is changed to electrical energy
oxidizing agent
Galvanic Cell
cyanide
electrolyte

23. In covalent bonds - prefixes are used to tell...
Amount of atoms present
Oxidation is Loss Reduction is Gain
Solute
+1 - except if bonded to Alkali Metal -1

24. l=3
Dipole Moment
Effusion
cohesion
f

25. All forms of energy except for heat
-one
3.0x108m/s
work
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

26. Dalton's Law of Partial Pressures (to find partial pressure formula)
moles solute/kg solvent
Constant Pressure
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
P of a =(X of a)(total pressure)

27. Kinetic Energy per molecule
conjugate acid
1/2mv²
moles solute/kg solvent
chromate

28. Has values 1 -2 -3 -...; tells energy levels
Pi Bond
Delta H or Enthalpy Change
Tetrahedral
Principal Quantum Number

29. Isotope
sublimation
Arrhenius base
different # of neutrons
Temperature

30. Wavelength symbol
endless
Exothermic
Anode
lambda

31. Oxidation # of Compounds
0
heat capacity
condensation
Ideal Gas Law

32. x can be ignored when % ionization is <5%
Integrated Second-Order Rate Law
5% rule
chlorite
Metalliods

33. Energy needed to vaporize a mole of a liquid
Anode
heat capacity
?Hvap
Negative work value; work done by system

34. Two molecules with identical connectivity but different geometries
chromate
Molecule
a precipitate forms
geometric isomers

35. SO4²?
excess reactant
sulfate
Beta Particles-
nitrite

36. When n=5 ->2 - color=
blue-violet
Ampere
double bond
Arrhenius Base

37. Ionizes to produce H+ ions
1atm=?Pa
?Hvap
Arrhenius Acid
red

38. Atoms with the same number of protons but a different number of neutrons
Isotopes
charge
H
A Roman numeral

39. A single substance that may be an acid or a base (i.e. water)
1.38x10?²³J/K
Amphoteric
PV=nRT
activated complex (transition state)

40. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
Pressure
+1 - except if bonded to Alkali Metal -1
Equilibrium Expression
End Point

41. Heat capacity formula
Hybridization
Cg=kPg
C=(mass)(specific heat)
condensation

42. These orbitals are spherical
s orbitals
Arrhenius Acid
sublimation
Open System

43. Loss of electrons - increase in oxidation #
oxidation
charge
phosphate - sulfide - carbonate - sulfate
Speed of light

44. An element with several different forms - each with different properties (i.e. graphite & diamond)
Law of Multiple Proportions
e-
g solute/g solvent x 100
Allotrope

45. H + donor
methods of increasing rate
base
Bronsted-Lowry Acid
-al

46. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
p
electron affinity
carbonate

47. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Second-Order Half Life
8.31J/Kmol
Equilibrium Expression
Cation

48. # bonding e- - # antibonding e-/2
Bond Order
Quantum Mechanical Model
Molecular Compounds
Antibonding Molecular Orbital

49. A method of investigation involving observation and theory to test scientific hypotheses
hept-
-2 - with peroxide -1
Scientific Method
Solute

50. AX4E
Specific Heat Capacity
Chemical Kinetics
surroundings
see-saw