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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.
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 steps do organic labs consist of?
Current - time and charge on ion (moles of e used in half cell reaction)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Synthesis - separation and purification of the product and its identification.

2. How are strong ones written?
CnH(2n+2)
strong acids/bases are written as H+ or OH- ions
Unsaturated - addition (ex: decolorize bromine solution)
small size and high charge

3. What is a dipeptide? polypeptide? protein?
ns² electrons (first in-first out)
Acidified
Q=It (time in seconds)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

4. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
zero
No - NH3 and HCl gases are extremely soluble
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
left - ppt will form

5. Which alkali metals float on water?
All except for lithium
White precipitate
q=mc?T q=mL (or n x ?h)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

6. phosphate
At half equivalence - pH=pKa
SO4²?
CH3COO?
PO4³?

7. BaSO4
voltaic: - electrolytic: +
Insoluble
0 and 14
ROH

8. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
red - green - blue
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.
A) any range. b) 8-10 c) 4-6
Eudiometer

9. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
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.
zero
Soluble

10. A Bronsted-Lowry acid is...
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
proton donor base
neutralization: high K - H2O product dissociation: low K - H2O reactant
CrO4²?

11. Alcohols and _______ are FG isomers
water and substances with (s) less dense than
Ionic compounds
ethers
Heat a test tube at an angle at the side of the tube (not bottom)

12. How do you find the pH for a dibasic acid? (H2A)?
Read the bottom of the meniscus
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?)
Perform ICE BOX calculation based on K1
Disulfur dichloride

13. What is the general formula for alkyl halides?
The compound with the lowest Ksp value.
RX
Suniverse increases for spontaneous processes
water and substances with (s) less dense than

14. What is the general formula of an alkane?
RCOOR
CnH(2n+2)
ion pairing
acid + alcohol

15. 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?
No - it depends on the number of ions produced on dissolving.
The compound with the lowest Ksp value.
Ksp = 108s5
Combine the equations for the half reactions in the non-spontaneous direction

16. How can metals like iron and zinc be reduced?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
E=q + w (negative is by system - positive is on system)
Perform ICE BOX calculation based on K1
chemically (ex: with carbon)

17. What process do you use to obtain the solute from a solution?
The compound with the lowest Ksp value.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Molecules with the same molecular formulas - but different structural formulas
Evaporation

18. What is the formula for alkenes?
Glowing splint (positive result=relights)
Acidified
Insoluble except nitrate and acetate
CnH2n

19. What is the formula for summation?

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20. What type of compounds do Group 14 form?
Suniverse increases for spontaneous processes
+4-covalent - +2-ionic
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?)
basic

21. chromate
same KE - but PEice<PEwater
ClO?
no - they're written undissociated (HAaq)
CrO4²?

22. What do metal oxides plus acids form?
Salt + water
NH2?
C2O4²?
chemically (ex: with carbon)

23. What are hybrid orbitals used for?
Insoluble except group 1 and ammonium
The compound with the lowest Ksp value.
Making sigma bonds and holding lone pairs
A) any range. b) 8-10 c) 4-6

24. 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 -
10?8
Silvery gray solid - brown - purple
atoms

25. What are allotropes?
fruit - fish - bases
zero-th: decreases - first: constant - second: increases
different forms of the same element
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

26. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
CnH2n+2
voltaic: - electrolytic: +
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

27. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Hg2²?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
methyl formate

28. Color is due to ______ _______ of light.
Suniverse increases for spontaneous processes
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
red - green - blue
Selective absorption

29. Is the standard entropy (S°) of an element zero?
neutralization: high K - H2O product dissociation: low K - H2O reactant
no - they're written undissociated (HAaq)
But S° of element is not zero (except at 0K)
non-metal oxides and hydrides are covalently bonded and are acidic.

30. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Most are soluble except Ag - Pb
a-IMFs - b-molecular volume
?H formation of an element in standard state=0
Transition element compounds (except if it has a full or empty d shell)

31. What is the charge on a chlorine atom?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Clear
zero
Only temperature

32. nitrates
diamond and graphite
same KE - but PEice<PEwater
Soluble
Both electrons come from the same atom (just as good as a regular bond)

33. hypochlorite
ClO?
methyl formate
An active metal.
Eudiometer

34. How many ligands attach to a central ion in a complex ion?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Salt + water
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
#ligands=charge x2

35. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
RNH2
Anode - oxygen. Cathode - hydrogen
Synthetic condensation polymer (aka a polyamide)

36. What is the energy you must put into a reaction to make it start called?
Experimental mass/theoretical mass X 100
Initiation energy (NOT Ea)
hydroxides (ex: Ba(OH)2)
O2 needs 4F/mol H2 needs 2F/mol

37. Name six characteristics of transition elements (or their compounds)
ClO2?
are less dense than water
bent
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)

38. What kind of bonding structure does benzene have?
metal oxides and hydrides are ionically bonded and basic
benzene has a delocalized pi ring structure
Q=It (time in seconds)
A) any range. b) 8-10 c) 4-6

39. What complex ion does ammonia form with silver? copper? cadmium? zinc?
?G= -ve - E°= +ve
Pale purple - (orange)-yellow - red - blue - green.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

40. Why are noble gases stable?
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)
Graduated cylinder
Ksp = 108s5
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

41. chlorite
?G= -ve - E°= +ve
ClO2?
atoms
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

42. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
diamond and graphite
ClO2?
T increases exponentially the proportion of molecules with E > Ea

43. What are two allotropes of carbon?
diamond and graphite
0 and 14
SO4²?
zero

44. chlorine
do not change
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)
bent
Greenish-yellow gas

45. dichromate (soln + most solids)
Orange
metal oxides and hydrides are ionically bonded and basic
CnH2n
Anode - oxygen. Cathode - hydrogen

46. halides
H2O + CO2 (it decomposes readily)
Most are soluble except Ag - Pb
ROR
Combine the equations for the half reactions in the non-spontaneous direction

47. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
methyl formate
Unsaturated - addition (ex: decolorize bromine solution)
Ksp = 27s4

48. What causes the dramatic effect of T on rate?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Filtration
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
T increases exponentially the proportion of molecules with E > Ea

49. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
All except for lithium
They decrease (or could be the same if the solid has ONLY JUST disappeared)
bases
ion pairing

50. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Salts (ex: CaO + SO2 ? CaSO3)
non-metal oxides and hydrides are covalently bonded and are acidic.
ClO4?