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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. SO3²?
group
sulfite
standard solution
yellow

2. Where reduction occurs
0.0826Latm/Kmol
Cathode
?Tb= kb x molality
Endothermic

3. If Q<Ksp
Angular Momentum Quantum Number
hydroxide
no precipitate forms
prop-

4. AX3
trigonal planar
T-shape
melting
1 atm

5. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Covalently w/in themselves - Ionicly bonded w/ each other
Molecular
hept-
LE Model

6. Equation to find Ea from reaction rate constants at two different temperatures
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
-one
see-saw
rate

7. Happens at lines in phase change charts
green/yellow
End Point
equilibrium
phosphate - sulfide - carbonate - sulfate

8. Force per unit area
Pressure
p+
3.0x108m/s
0 degrees C - 1 atm

9. AX5E
square pyramidal
second
Reaction Quotient (Q)
Molecular Compounds

10. When n=6 ->2 - color=
reduction agent
3rd law of thermodynamics
0
violet

11. Unit of electrical potential; J/C
Volt
P of a =(X of a)(total pressure)
spontaneity
Delta H or Enthalpy Change

12. Ptotal=P1+P2+P3+...

13. Energy involved in gaining an electron to become a negative ion
alcohol
chromate
electron affinity
endless

14. Peak of energy diagram
Exothermic
Root Mean Square Velocity
activated complex (transition state)
Bronsted-Lowry acid

15. The total energy of the universe is constant - all systems tend towards minimum energy
1st law of thermodynamics
perchlorate
Diffusion
condensation

16. A single substance that may be an acid or a base (i.e. water)
endless
Naming Binary Ionic Compounds
Amphoteric
Nodes

17. Combined Gas Law Formula
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Volume Metric Flask & Pipet
P1V1/N1T1=P2V2/N2T2
-(P)(Change in V)

18. Heat capacity formula
hydro-ic acid
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Theory of Relativity
C=(mass)(specific heat)

19. Expresses how the concentrations depend on time
perchlorate
Integrated Rate Law
flouride
First-Order Rate Law

20. Moles of solute/volume of soln(L)
Second-Order Rate Law
hydroxide
Molarity
Angular Momentum Quantum Number

21. frequency symbol
bent
Molecular
hept-
nu

22. A molecule having a center of positive charge and a center of negative charge
Ionic
surroundings
-ic acid
Dipole Moment

23. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change

24. Aldehyde suffix
green/yellow
-al
(moles of products that are gasses) - (moles of reactants that are gasses)
melting

25. Point at which the titrated solution changes color
Surroundings
end point
group
are not

26. ?T=k*m(solute)
deposition
f
Molal BP Elevation Constant
p orbitals

27. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
mol
Buffer
Acid + Base --> Salt + Water
heat capacity

28. Elements in groups 3-12
First-Order Half Life
Surroundings
Transition metals
Law of Conservation of Energy

29. Experimental yield/theoretical yieldx100
LE Model
% yield
+1 - except if bonded to Alkali Metal -1
Magnetic Quantum Number (ml)

30. Liquid to solid
Ionic
freezing
g solute/g solvent x 100
seesaw

31. Heat needed to change 1 g of substance to 1°C
specific heat
Octahedral
condensation
Zero-Order Half Life

32. Freezing point depression formula
1 atm = 760 mmHg = 101.3 kPa
f
?Tf= kf x molality
s orbitals

33. The driving force for a spontaneous is an increase in entropy of the universe
work
Entropy (S)
e-
violet

34. q H2O = ?
msAT
Angular Momentum Quantum Number
equilibrium
Hybridization

35. R in instances that pertain to energy
Overall Reaction Order
State Functions
8.314 J/K mol
no precipitate forms

36. q cal = ?
AE = q + w
Aufbau Principle
CAT
nitrite

37. (organics) eight carbons
Calorimetry
Hess's Law
salt bridge
oct-

38. How to Find an Empirical Formula Given Percentages
no precipitate forms
Resonance
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
perchlorate

39. Only contains ions that change in reaction
Naming Binary Ionic Compounds
Net Ionic Equation
London dispersion forces
Hydrogen bonding

40. Loss of electrons - increase in oxidation #
oxidation
0
Dipole-dipole forces
Metalliods

41. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
iodide
End Point
oxide gas and water

42. The part of the universe one is focused upon (in thermodynamics)
actual yield/theoretical yield x 100%
system
alkyne
wavelength

43. Carbon & hydrogen compounds
salt bridge
hydrocarbons
trigonal bipyramidal
voltaic cells

44. r=k[A]^2
Average KE = 1/2(mass)(average speed of all particles)
Second-Order Rate Law
Finding Empirical Formulas
Pauli Exclusion Principle

45. (organics) two carbons
red
dichromate
condensation
eth-

46. When n=4 ->2 - color=
Colligative properties
Theoretical yield
blue-green
Hydrogen bonding

47. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
weak acid strong base rxn
Bronsted-Lowry Base
0

48. Ester suffix
-oate
Barometer
alkene
blue-violet

49. Change in Energy = ? (in terms of constant pressure; for gasses)
van't Hoff Factor
0.512°C
permanganate
AE= AH - RTAn

50. .69/k
3/2RT
First-Order Half Life
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Pauli Exclusion Principle