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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. Nonmetals are good _____ agents. Metals are good _______ agents.
linear
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
different forms of the same element
E=q + w (negative is by system - positive is on system)

2. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Salt + water.
Soluble

3. chlorite
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH2n
ClO2?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

4. What element is used to vulcanize rubber?
C4H10
ROR
Sulfur
Only temperature

5. A Bronsted-Lowry acid is...
The compound with the lowest Ksp value.
linear
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
proton donor base

6. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
linear
Molecules with the same molecular formulas - but different structural formulas
Group I metals (soft metals) are stored under oil

7. What is accuracy?
Acids; HCOOCH3 is an ester
Clear
How close results are to the accepted value
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

8. What is reflux?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Acidified
boiling without losing volatile solvents/reactants
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

9. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Trigonal pyramidal
All except for lithium
10?8

10. What is the charge on a chlorine atom?
zero
q=mc?T q=mL (or n x ?h)
ClO3?
#ligands=charge x2

11. What is the word equation for condensation polymerisation ?
OH?
non-metal oxides and hydrides are covalently bonded and are acidic.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
[A?]/[HA] x 100 or [BH?]/[B] x 100

12. What process do you use to obtain the solute from a solution?
by electrolysis
Evaporation
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

13. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Suniverse increases for spontaneous processes
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

14. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
hydroxides (ex: Ba(OH)2)
water and substances with (s) less dense than
RCOOH

15. What do nonmetal oxides plus water form?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Eudiometer
acids
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

16. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
non-metal oxides and hydrides are covalently bonded and are acidic.

17. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
The dilution effect when the solutions mix. M1V1 = M2V2
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Insoluble except nitrate and acetate

18. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
RCHO (carbonyl at end)
Most are soluble except Ag - Pb
water and substances with (s) less dense than
Glacial acetic acid

19. How do you explain trends in atomic properties using Coulomb's Law?
Filtration
Most INsoluble except group 1 and ammonium
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
fractional distillation

20. Does Kw increase or decrease with T? Why?
yellow
[A?]/[HA] x 100 or [BH?]/[B] x 100
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Perform ICE BOX calculation based on K1

21. What is the name of S2Cl2? (Know how to name others like this - too)
CrO4²?
Disulfur dichloride
zero
A) any range. b) 8-10 c) 4-6

22. chlorate
Sigma bonds are stronger than pi bonds
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ClO3?
Iodine and CO2 (dry ice)

23. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Unsaturated - addition (ex: decolorize bromine solution)
Synthetic condensation polymer (aka a polyamide)
ClO?

24. An amphiprotic (amphoteric) species is...
But S° of element is not zero (except at 0K)
P2O5
Mn²? - Cr³? - Cr³
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

25. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Purple
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Pipette (burette if need repetition)

26. potassium permanganate
Purple
basic
do not change
Graduated cylinder

27. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Pour liquids using a funnel or down a glass rod
T increases exponentially the proportion of molecules with E > Ea
O2 needs 4F/mol H2 needs 2F/mol
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

28. Esters smell like _______ and amines smell like _______ and are ______.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Suniverse increases for spontaneous processes
Group 1 hydroxides (ex: NaOH)
fruit - fish - bases

29. ammonium/ammonium compounds
bent
Soluble
basic
C2O4²?

30. What process do you use to separate two liquids with different boiling points?
Sigma bonds are stronger than pi bonds
Eudiometer
fractional distillation
ClO2?

31. What is the slope of the graph of lnk vs. 1/T?
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
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
ns² electrons (first in-first out)
-Ea/R

32. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
The compound with the lowest Ksp value.
Kc=Kp
White precipitate
Salts (ex: CaO + SO2 ? CaSO3)

33. What do metal oxides plus non- metal oxides form?
catalyst=conc H2SO4
CO2 and H2O
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Salts (ex: CaO + SO2 ? CaSO3)

34. ________ are Lewis bases - because they can donate a lone pair of electrons.
zero
Glacial acetic acid
Salts (ex: CaO + SO2 ? CaSO3)
OH- and NH3

35. What is HCOOCH3?
red - green - blue
Disulfur dichloride
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Acids; HCOOCH3 is an ester

36. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Greenish-yellow gas
basic
Insoluble
They decrease (or could be the same if the solid has ONLY JUST disappeared)

37. Color (absorbance) is proportional to ________
Ksp = 4s³
Concentration
boiling without losing volatile solvents/reactants
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

38. What measuring device would you use for very small volumes of liquids?
Iodine and CO2 (dry ice)
Pipette (burette if need repetition)
it's lower and occurs over less sharp a range
Clear

39. What equipment do you need for a titration?
blue (BTB)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
ClO4?
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³

40. acetates
Nothing
redox reaction
Soluble
A salt solution.

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)
ionic and form hydrogen and hydroxide
Check for air bubbles in the buret and remove the buret funnel from the buret
Saturated - Substitution (which requires more radical conditions)

42. dihydrogen phosphate
ClO?
H2PO4?
small size and high charge
Ksp = s²

43. What apparatus do you use to separate 2 immiscible liquids?
benzene has a delocalized pi ring structure
Separating funnel
Suniverse increases for spontaneous processes
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

44. What changes Keq?
zero
Only temperature
But S° of element is not zero (except at 0K)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

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

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46. halides
Disulfur dichloride
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Most are soluble except Ag - Pb
RCOOH

47. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
same KE - but PEice<PEwater
do not change
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
benzene has a delocalized pi ring structure

48. If ?S is positive - are the products more or less chaotic than the reactants?
Molecules with the same molecular formulas - but different structural formulas
More chaotic (ex: gases made)
RNH2
Trigonal pyramidal

49. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Q=It (time in seconds)
Ksp = s²
How close results are to the accepted value
chemically (ex: with carbon)

50. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
catalyst=conc H2SO4
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Greenish-yellow gas
They decrease (or could be the same if the solid has ONLY JUST disappeared)