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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 does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Acids; HCOOCH3 is an ester
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?)

2. How do you explain trends in atomic properties using Coulomb's Law?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
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?)
?H-kJ - ?S-J - ?G-kJ

3. What type of polymer is nylon?
blue glass - it filters UV
Synthetic condensation polymer (aka a polyamide)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
H+

4. Metal hydrides are _____ and form _______ and _______ when added to water
Increases down group 1 decreases down group 17
Heat a test tube at an angle at the side of the tube (not bottom)
ionic and form hydrogen and hydroxide
Saturated - Substitution (which requires more radical conditions)

5. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
redox reaction
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
C4H10
zero-th: decreases - first: constant - second: increases

6. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
redox reaction
boiling without losing volatile solvents/reactants
CnH2n
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

7. What is the formula for percent error?
fruit - fish - bases
|experimental - accepted|/accepted X 100
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
non-metal oxides and hydrides are covalently bonded and are acidic.

8. Give an example of a dilute strong acid.
[A?]/[HA] x 100 or [BH?]/[B] x 100
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acidified
HClO4

9. What are the products of the reaction between group 1 metals and water?

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10. What is the formula of copper (II) phosphate?
It ceases - the circuit is broken.
RCOR
Cu3(PO4)2
Insoluble except group 1 and ammonium

11. Acids + Carbonates (bicarbonates) make?
CnH2n+2
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Trigonal pyramidal

12. 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?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
The compound with the lowest Ksp value.
CO (poisonous)
The dilution effect when the solutions mix. M1V1 = M2V2

13. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
It ceases - the circuit is broken.
OH- and NH3
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
[A?]/[HA] x 100 or [BH?]/[B] x 100

14. Neutralization is an ________ reaction.
Only temperature
Most are soluble except Ag - Pb
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Conjugate pair (one must be a weak base or acid)

15. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Identity and purity (impure compounds usually have broad & low melting points)
metal oxides and hydrides are ionically bonded and basic
C2O4²?

16. silver compounds
proton acceptor.
The compound with the lowest Ksp value.
Salt and water
Insoluble except for nitrate and acetate

17. What is the test for oxygen?
Glowing splint (positive result=relights)
A) any range. b) 8-10 c) 4-6
small size and high charge
Experimental mass/theoretical mass X 100

18. What are the formulas for q?
Heptane
q=mc?T q=mL (or n x ?h)
redox reaction
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

19. Are weak acids (and bases) written dissociated?

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20. lead compounds
basic
Insoluble except nitrate and acetate
different forms of the same element
CO2 and H2O

21. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
0.10M HCl (more ions)
voltaic: + electrolytic: -
Heat a test tube at an angle at the side of the tube (not bottom)
water and substances with (s) less dense than

22. Alkanes are _________ and react by _________
Iodine and CO2 (dry ice)
OH- and NH3
Eudiometer
Saturated - Substitution (which requires more radical conditions)

23. barium sulfate
White precipitate
Acids; HCOOCH3 is an ester
Pipette (burette if need repetition)
chemically (ex: with carbon)

24. ammonium/ammonium compounds
do not change
Soluble
No - NH3 and HCl gases are extremely soluble
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

25. During a titration what is present in the beaker at the equivalence point?
Molecules with the same molecular formulas - but different structural formulas
bases
P2O5
A salt solution.

26. What is the relationship in strength between sigma and pi bonds?
ion pairing
Cu3(PO4)2
Sigma bonds are stronger than pi bonds
?H formation of an element in standard state=0

27. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
RCOOH
S2O3²?
Combine the equations for the half reactions in the non-spontaneous direction
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

28. For a dibasic acid (H2A) - [A²?]= ____ ?
Q=It (time in seconds)
Evaporation
K2
An active metal.

29. How do you compute % dissociation?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
S crystal at 0K=0
0 and 14
[A?]/[HA] x 100 or [BH?]/[B] x 100

30. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
How grouped results are
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
It ceases - the circuit is broken.
ionic and form hydrogen and hydroxide

31. chlorate
ClO3?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

32. What are isotopes?
No - it depends on the number of ions produced on dissolving.
zero
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Ions go through the salt bridge - electrons go through metal wires in the external circuit

33. nitrates
PO4³?
Greenish-yellow gas
Soluble
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

34. ammonium
NH4?
ClO2?
it reacts by substitution NOT addition
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

35. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
ion pairing
S2O3²?
Heptane

36. What is the sign of the cathode in voltaic cells? in electrolytic cells?
red - green - blue
voltaic: + electrolytic: -
linear
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

37. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
a-IMFs - b-molecular volume
yellow
basic

38. What element is used to vulcanize rubber?
Pale yellow
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Only temperature
Sulfur

39. How does half life change for zero-th order - first order - and second order processes?
?H-kJ - ?S-J - ?G-kJ
zero-th: decreases - first: constant - second: increases
ethers
Products - reactants (except for BDE when it's reactants - products)

40. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Both electrons come from the same atom (just as good as a regular bond)
But S° of element is not zero (except at 0K)
Soluble except Ag - Pb - Ca - Sr Ba)

41. What are the names and formulas of the 6 strong acids?
neutralization: high K - H2O product dissociation: low K - H2O reactant
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
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

42. How does the melting point of a mixture compare to the MP of a pure substance?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
it is lower and occurs over less sharp a range
acids
Big K=kf/kr

43. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
C4H10
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Sigma bonds are stronger than pi bonds
Mn²? - Cr³? - Cr³

44. Name C7H16
#ligands=charge x2
Heptane
They stay the same.
same KE - but PEice<PEwater

45. What apparatus do you use to pour liquids?
Initiation energy (NOT Ea)
boiling without losing volatile solvents/reactants
same KE - but PEice<PEwater
Pour liquids using a funnel or down a glass rod

46. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Making sigma bonds and holding lone pairs
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
water and substances with (s) less dense than
water and substances with (s) less dense than

47. sulfates
proton donor base
Products - reactants (except for BDE when it's reactants - products)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Soluble except Ag - Pb - Ca - Sr Ba)

48. Alcohols and _______ are FG isomers
They stay the same.
Insoluble except for nitrate and acetate
ethers
Insoluble

49. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ClO3?
Soluble
Exothermic

50. Is the freezing of ice endothermic or exothermic?
At half equivalence - pH=pKa
blue (BTB)
Orange
Exothermic