Test your basic knowledge |

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 shape is ammonia?
Trigonal pyramidal
boiling without losing volatile solvents/reactants
Soluble except Ag - Pb - Ca - Sr Ba)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

2. What is the pH of 1.0M HCl? 1M NaOH?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Insoluble
0 and 14
-Ea/R

3. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Synthetic condensation polymer (aka a polyamide)
CH3COO?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
do not change

4. What is the word equation for condensation polymerisation ?
Acid rain - dissolves marble buildings/statues and kills trees.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Soluble
All except for lithium

5. chromate ion (soln + most solids)
do not change
yellow
Group I metals (soft metals) are stored under oil
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

6. chlorate
ClO3?
Synthesis - separation and purification of the product and its identification.
?G= -ve - E= +ve
The compound with the lowest Ksp value.

7. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]? - [Cd(NH3)4]? - [Zn(NH3)4]?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

8. What is the test for oxygen?
The dilution effect when the solutions mix. M1V1 = M2V2
NO3?
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2
Glowing splint (positive result=relights)

9. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
proton acceptor.
Hg2?
Conjugate pair (one must be a weak base or acid)

10. What is the basic structure of an optical isomer?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Perform ICE BOX calculation based on K1
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

11. What is a dipeptide? polypeptide? protein?
Filtration
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
allow for the vapor pressure of water and make sure to level levels
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

12. What is the sign of the cathode in voltaic cells? in electrolytic cells?
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
CO (poisonous)
O2 needs 4F/mol H2 needs 2F/mol
voltaic: + electrolytic: -

13. primary colors
chemically (ex: with carbon)
different forms of the same element
red - green - blue
RCOOR

14. A geometric (or cis-trans) isomer exists due to.....
Ksp = s
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
?H formation of an element in standard state=0
RCOOR

15. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Ksp = 27s4
Ksp = 4s
ion pairing

16. What is HCOOCH3?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Filtration
Acids; HCOOCH3 is an ester
H+

17. Give an example of a dilute strong acid.
O2 needs 4F/mol H2 needs 2F/mol
bent
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
HClO4

18. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
diamond and graphite
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
blue (BTB)

19. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
Soluble
Soluble
Add acid to water so that the acid doesn't boil and spit

20. Alkanes are _________ and react by _________
NO3?
10?8
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Saturated - Substitution (which requires more radical conditions)

21. When can supercooling occur? What does it look like on a cooling curve?
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.
Sigma bonds are stronger than pi bonds
E=q + w (negative is by system - positive is on system)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

22. Do anions flow to the cathode or anode?
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Ksp = 108s5
Anode
Hydrogen (active metals are metals with more negative reduction potentials in E chart)

23. bromine
proton donor base
brown volatile liquid
Pale purple - (orange)-yellow - red - blue - green.
White precipitate

24. What is the conjugate acid of H2PO4?
H3PO4
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Ksp = 108s5

25. If a weak acid is diluted more - what happens to its % dissociation value?
H2O + CO2 (it decomposes readily)
Hg?
Increases.
4 sigma bonds-109 - sp - one double bond-120 - sp two double bonds-180 - sp one triple bond-180 - sp

26. What shape is carbon dioxide?
RCHO (carbonyl at end)
10?8
Hg2?
linear

27. How do you explain trends in atomic properties using Coulomb's Law?
Soluble
-Ea/R
fruit - fish - bases
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

28. lead iodide
same KE - but PEice<PEwater
bright yellow
linear
Pale purple - (orange)-yellow - red - blue - green.

29. At what point during titration do you have the perfect buffer - and what is the pH at this point?
NH4?
water and substances with (s) less dense than
At half equivalence - pH=pKa
Sulfur

30. What are the units of the first order rate constant?
Acid rain - dissolves marble buildings/statues and kills trees.
No - it depends on the number of ions produced on dissolving.
strong acids/bases are written as H+ or OH- ions
Time? - (ex. s? - hr? - etc)

31. What process do you use to obtain the solute from a solution?
Soluble
do not change
Evaporation
They stay the same.

32. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
a-IMFs - b-molecular volume
small size and high charge
Products - reactants (except for BDE when it's reactants - products)

33. permanganate
ethers
More chaotic (ex: gases made)
MnO4?
allow for the vapor pressure of water and make sure to level levels

34. For a dibasic acid (H2A) - [A?]= ____ ?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Synthetic condensation polymer (aka a polyamide)
K2

35. What is the general formula for an acid?
Anode
S crystal at 0K=0
RCOOH
Products - reactants (except for BDE when it's reactants - products)

36. What are the products for these common oxidizing agents? MnO4? - CrO4? - Cr2O7?
Suniverse increases for spontaneous processes
Mn? - Cr? - Cr
Perform ICE BOX calculation based on K1
C4H10

37. What are the products of the reaction between group 1 metals and water?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
How close results are to the accepted value
Mono; di; tri; tetra; penta; hexa.
The dilution effect when the solutions mix. M1V1 = M2V2

38. Why are i factors (Van't Hoff factors) often less than ideal?
#ligands=charge x2
Salt and water
ion pairing
PO4?

39. What process do you use to obtain a solvent from a solution?
RCHO (carbonyl at end)
They stay the same.
Distillation
Soluble

40. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
small size and high charge
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)
Current - time and charge on ion (moles of e used in half cell reaction)

41. What equipment do you need for a titration?
same KE - but PEice<PEwater
OH?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

42. What are the signs of ?G and E for spontaneous reactions?
More chaotic (ex: gases made)
?G=negative - E must be positive
chemically (ex: with carbon)
The one with most oxygen atoms (highest oxidation number)

43. Is the standard entropy (S) of an element zero?
But S of element is not zero (except at 0K)
CnH2n
CrO4?
Anode

44. What reacts with an acid to create hydrogen gas?
fruit - fish - bases
Ions go through the salt bridge - electrons go through metal wires in the external circuit
An active metal.
catalyst=conc H2SO4

45. The oxidation # for acid base reactions...
S crystal at 0K=0
do not change
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
A salt solution.

46. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Clear
water and substances with (s) less dense than
a-IMFs - b-molecular volume
Molecules with the same molecular formulas - but different structural formulas

47. Esters smell like _______ and amines smell like _______ and are ______.
Sigma bonds are stronger than pi bonds
a-IMFs - b-molecular volume
Cu3(PO4)2
fruit - fish - bases

48. copper sulfate
blue
it's lower and occurs over less sharp a range
ClO4?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

49. What two compounds are great oxidizing agents?
voltaic: + electrolytic: -
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Glowing splint (positive result=relights)

50. Name C7H16
Heptane
The Faraday or Faraday's constant.
Acid rain - dissolves marble buildings/statues and kills trees.
E=q + w (negative is by system - positive is on system)

Test your basic knowledge |

AP Chemistry 2

Link to This Test

Related Subjects