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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. What is the pH of 1.0M HCl? 1M NaOH?
Kc=Kp
0 and 14
Q=It (time in seconds)
RNH2

2. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Salt and water
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble except nitrate and acetate

3. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Hg2²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Read the bottom of the meniscus
The dilution effect when the solutions mix. M1V1 = M2V2

4. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
atoms
non-metal oxides and hydrides are covalently bonded and are acidic.

5. What is the conjugate base of NH3?
Hg²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Check for air bubbles in the buret and remove the buret funnel from the buret
NH2?

6. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
neutralization: high K - H2O product dissociation: low K - H2O reactant
basic
Pipette (burette if need repetition)

7. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
lighted splint (positive result=pop)
Soluble except Ag - Pb - Ca - Sr Ba)
Big K=kf/kr
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

8. The definition of acidic basic and neutral aqueous solutions is:
Evaporation
CO3²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

9. acetates
CO (poisonous)
At half equivalence - pH=pKa
Soluble
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

10. dihydrogen phosphate
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
ROH
ionic and form hydrogen and hydroxide
H2PO4?

11. How does half life change for zero-th order - first order - and second order processes?
The dilution effect when the solutions mix. M1V1 = M2V2
zero-th: decreases - first: constant - second: increases
same KE - but PEice<PEwater
Identity and purity (impure compounds usually have broad & low melting points)

12. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Acid rain - dissolves marble buildings/statues and kills trees.
an oxidized and reduced substance

13. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
+4-covalent - +2-ionic
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
H2PO4?
Insoluble except for nitrate and acetate

14. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Clear
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
non-metal oxides and hydrides are covalently bonded and are acidic.
An active metal.

15. acetate
Molecules with the same molecular formulas - but different structural formulas
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CH3COO?
P2O5

16. What apparatus do you use to separate 2 immiscible liquids?
Q=It (time in seconds)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Perform ICE BOX calculation based on K1
Separating funnel

17. What shape is carbon dioxide?
Ksp = s²
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
basic
linear

18. What is the formula for alkynes?
Pipette (burette if need repetition)
Mn²? - Cr³? - Cr³
CnH2n-2
Heat a test tube at an angle at the side of the tube (not bottom)

19. Is the freezing of ice endothermic or exothermic?
CN?
proton donor base
it's lower and occurs over less sharp a range
Exothermic

20. What process do you use to obtain the solute from a solution?
Silvery gray solid - brown - purple
Synthesis - separation and purification of the product and its identification.
Evaporation
Soluble

21. What should you check for before you begin titrating?
Disulfur dichloride
The benzene ring (or more correctly the phenyl group - C6H5)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Check for air bubbles in the buret and remove the buret funnel from the buret

22. What element is used to vulcanize rubber?
same KE - but PEice<PEwater
Sulfur
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero

23. What is the relationship in strength between sigma and pi bonds?
Combine the equations for the half reactions in the non-spontaneous direction
Sigma bonds are stronger than pi bonds
it's lower and occurs over less sharp a range
-Ea/R

24. Why are i factors (Van't Hoff factors) often less than ideal?
Soluble
ROR
Group 1 hydroxides (ex: NaOH)
ion pairing

25. How do you find the pH for a dibasic acid? (H2A)?
K2
Perform ICE BOX calculation based on K1
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
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.

26. lead iodide
lighted splint (positive result=pop)
How close results are to the accepted value
-Ea/R
bright yellow

27. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
SO4²?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Making sigma bonds and holding lone pairs

28. chlorine
Tetrahedral
Acidified
Greenish-yellow gas
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

29. iodine - iodine solution - iodine vapor
Acids; HCOOCH3 is an ester
H2O + CO2 (it decomposes readily)
Salt and water
Silvery gray solid - brown - purple

30. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CrO4²?
An active metal.
no - they're written undissociated (HAaq)
CO (poisonous)

31. A Bronsted-Lowry base is...
bent
Iodine and CO2 (dry ice)
proton acceptor.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

32. What is the formula for summation?

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33. What kind of bonding structure does benzene have?
Only temperature
it is lower and occurs over less sharp a range
benzene has a delocalized pi ring structure
CN?

34. hydroxide
Group 1 hydroxides (ex: NaOH)
CnH2n+2
OH?
CnH2n-2

35. barium sulfate
O2 needs 4F/mol H2 needs 2F/mol
White precipitate
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

36. What is the basic structure of an optical isomer?
OH?
RCOR
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Saturated - Substitution (which requires more radical conditions)

37. Does reactivity increase/decrease going down group 1 and group 17?
ROR
water and substances with (s) less dense than
Salt + water
Increases down group 1 decreases down group 17

38. Buffer capacity must contain decent amounts of a ________ ________
Exothermic (?H for ANY sa/sb = -57kJ/mol)
allow for the vapor pressure of water and make sure to level levels
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Conjugate pair (one must be a weak base or acid)

39. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
H+
blue (BTB)
Making sigma bonds and holding lone pairs

40. What is the word equation for addition polymerisation?
Current - time and charge on ion (moles of e used in half cell reaction)
?G=negative - E° must be positive
SO4²?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

41. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Insoluble
Soluble

42. What changes Keq?
Salt + water
Only temperature
Increases down group 1 decreases down group 17
Both electrons come from the same atom (just as good as a regular bond)

43. What type of metals don't react with water or acids to form H2?

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44. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
Iodine and CO2 (dry ice)
Graduated cylinder
C4H10

45. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Insoluble
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Kc=Kp
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

46. Colorless doesn't mean ______
Clear
RNH2
CrO4²?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

47. bromine
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Insoluble except group 1 and ammonium
brown volatile liquid

48. Esters smell like _______ and amines smell like _______ and are ______.
The one with most oxygen atoms (highest oxidation number)
How grouped results are
PO4³?
fruit - fish - bases

49. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
ROR
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Evaporation

50. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Only temperature
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Identity and purity (impure compounds usually have broad & low melting points)
Ksp = 108s5