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AP Chemistry 2

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. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
White precipitate
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
fractional distillation
Big K=kf/kr

2. permanganate
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
bent
A) any range. b) 8-10 c) 4-6
MnO4?

3. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
H2O + CO2 (it decomposes readily)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)

4. What do you do to get rid of most of the solution from a precipitate?
The compound with the lowest Ksp value.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Ksp = s
Decant

5. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
non-metal oxides and hydrides are covalently bonded and are acidic.

6. What type of metals don't react with water or acids to form H2?
K2
HClO4
bent
'non-active' metals such as Cu - Ag - Au - Pt - etc.

7. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
All single: sp - one double: sp - two doubles: sp - one triple: sp - two single and two lone pairs: sp - three single and one lone pair: sp
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
strong acids/bases are written as H+ or OH- ions
No - it depends on the number of ions produced on dissolving.

8. What process do you use to obtain the solute from a solution?
Evaporation
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
water and substances with (s) less dense than
CrO4?

9. chromate
blue glass - it filters UV
neutralization: high K - H2O product dissociation: low K - H2O reactant
CrO4?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)

10. potassium permanganate
Sulfur
NH2?
same KE - but PEice<PEwater
Purple

11. Name six characteristics of transition elements (or their compounds)
Good catalysts - form multiple oxidation states - often paramagnetic - good structural metals - form a host of alloys (similar sized atoms) - have similar I energies (inner filling)
Synthesis - separation and purification of the product and its identification.
bent
[Ag(NH3)2]? - [Cu(NH3)4]? - [Cd(NH3)4]? - [Zn(NH3)4]?

12. How do you get the equation for a net electrolysis reaction?
ion pairing
yellow
voltaic: + electrolytic: -
Combine the equations for the half reactions in the non-spontaneous direction

13. What shape is carbon dioxide?
CO3?
CH3COO?
linear
Ions go through the salt bridge - electrons go through metal wires in the external circuit

14. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
R=8.31 J/mol/K
Mn? - Cr? - Cr
bases
The compound with the lowest Ksp value.

15. What two types of substances are present in all redox reactions?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
an oxidized and reduced substance
Iodine and CO2 (dry ice)
The Faraday or Faraday's constant.

16. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
R=8.31 J/mol/K
Cr2O7?
acid + alcohol

17. How does group 1 metals' density compare to water's?
Q=It (time in seconds)
Clear
Glacial acetic acid
are less dense than water

18. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
They stay the same.
Q=It (time in seconds)
it's lower and occurs over less sharp a range

19. What is the conjugate acid of H2PO4?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Silvery gray solid - brown - purple
H3PO4
H2O + CO2 (it decomposes readily)

20. When the salt bridge is removed what happens to the cell reaction?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Insoluble
?H formation of an element in standard state=0
It ceases - the circuit is broken.

21. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
ion pairing
ClO2?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

22. Aromatic compounds contain what?
NO3?
Salts (ex: CaO + SO2 ? CaSO3)
NH2?
The benzene ring (or more correctly the phenyl group - C6H5)

23. How does the KE and PE of ice at 0C compare to the KE and PE of water at 0C?
same KE - but PEice<PEwater
Current - time and charge on ion (moles of e used in half cell reaction)
NO3?
atoms

24. hydroxides
Insoluble (except group 1 ammonium and Ba)
Orange
Anode
Soluble

25. What is the formula for percent error?
Perform ICE BOX calculation based on K1
an oxidized and reduced substance
|experimental - accepted|/accepted X 100
Hydrogen (active metals are metals with more negative reduction potentials in E chart)

26. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Saturated - Substitution (which requires more radical conditions)
Kc=Kp
Eudiometer
metal oxides and hydrides are ionically bonded and basic

27. Acids + Carbonates (bicarbonates) make?
Pipette (burette if need repetition)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Acid rain - dissolves marble buildings/statues and kills trees.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

28. What is reflux?
boiling without losing volatile solvents/reactants
S2O3?
Distillation
Ksp = 4s

29. Is the standard entropy (S) of an element zero?
zero
Glowing splint (positive result=relights)
Soluble except Ag - Pb - Ca - Sr Ba)
But S of element is not zero (except at 0K)

30. What do you need to make a polymer?
Suniverse increases for spontaneous processes
+4-covalent - +2-ionic
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
Increases down group 1 decreases down group 17

31. What are allotropes?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
zero
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
different forms of the same element

32. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Soluble
Ksp = 4s
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

33. What does a short - sharp melting point indicate?
?H formation of an element in standard state=0
Identity and purity (impure compounds usually have broad & low melting points)
Making sigma bonds and holding lone pairs
Mono; di; tri; tetra; penta; hexa.

34. Name 2 ways in which you can create a buffer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
boiling without losing volatile solvents/reactants
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
Ksp = 108s5

35. chlorite
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Pour liquids using a funnel or down a glass rod
ClO2?
Ksp = 27s4

36. sulfate
SO4?
R=8.31 J/mol/K
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the
Read the bottom of the meniscus

37. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
Both electrons come from the same atom (just as good as a regular bond)
Reverse most negative E and add voltages to get Ecell (or take absolute difference between Ered values)
OH?

38. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
?G=negative - E must be positive
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Graduated cylinder
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

39. primary colors
red - green - blue
Big K=kf/kr
water and substances with (s) less dense than
Pour liquids using a funnel or down a glass rod

40. What type of solutions do small - highly charged cations tend to form?
q=mc?T q=mL (or n x ?h)
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Transition element compounds (except if it has a full or empty d shell)
C2O4?

41. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
chemically (ex: with carbon)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Glacial acetic acid

42. Is the ?H formation of an element in standard state zero?
hydroxides (ex: Ba(OH)2)
?H formation of an element in standard state=0
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
An active metal.

43. What should you check for before you begin titrating?
Purple
Check for air bubbles in the buret and remove the buret funnel from the buret
An active metal.
allow for the vapor pressure of water and make sure to level levels

44. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Salt and water
Salt + water
NH2?

45. At what point during titration do you have the perfect buffer - and what is the pH at this point?
?G= -ve - E= +ve
Pale purple - (orange)-yellow - red - blue - green.
At half equivalence - pH=pKa
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

46. What do metal oxides plus acids form?
Salt + water
The Faraday or Faraday's constant.
PO4?
basic

47. What is the general formula for an acid?
RCOOH
ion pairing
Q=It (time in seconds)
CnH(2n+2)

48. How many normal boiling points and boiling points are there?
-Ea/R
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Supercooling can occur when cooling a solvent or solution. It occurs when there's a dip and then a rise back up to the melting point on a cooling curve.

49. What is precision?
Time? - (ex. s? - hr? - etc)
Salt + water
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
How grouped results are

50. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Evaporation
Pipette (burette if need repetition)
10?8
Combine the equations for the half reactions in the non-spontaneous direction

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