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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. Is the standard entropy (S°) of an element zero?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
voltaic: + electrolytic: -
But S° of element is not zero (except at 0K)
benzene is less reactive than alkenes

2. When driving off water from a hydrate - how do you tell you're done?
Both electrons come from the same atom (just as good as a regular bond)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Cu3(PO4)2

3. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
0.10M HCl (more ions)
methyl formate
Increases down group 1 decreases down group 17

4. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
CnH2n+2
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Distillation

5. How are metal oxides and hydrides bonded? are they acidic or basic?
ClO?
metal oxides and hydrides are ionically bonded and basic
How close results are to the accepted value
Ions go through the salt bridge - electrons go through metal wires in the external circuit

6. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
Ppt will NOT form (unsaturated)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
S crystal at 0K=0

7. What is the general formula for an ester?
RCOOR
CN?
blue (BTB)
voltaic: - electrolytic: +

8. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
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
Reduction always takes place at the cathode (RED CAT) In both types of cell!
No - it depends on the number of ions produced on dissolving.
Identity and purity (impure compounds usually have broad & low melting points)

9. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Pale yellow
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
a-IMFs - b-molecular volume

10. What type of solutions do small - highly charged cations tend to form?
R=8.31 J/mol/K
RCOR
White precipitate
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

11. copper sulfate
blue
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
White precipitate
Salt + water

12. What is the formula for summation?

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13. What is the formula of copper (II) phosphate?
Cu3(PO4)2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

14. permanganate
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
How close results are to the accepted value
MnO4?

15. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
At half equivalence - pH=pKa
Sigma bonds are stronger than pi bonds
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
water and substances with (s) less dense than

16. What is the formula of butane?
Greenish-yellow gas
C4H10
RCOOH
ionic and form hydrogen and hydroxide

17. What is the formula for alkanes?
CnH2n+2
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
+4-covalent - +2-ionic
Anode

18. What is the slope of the graph of lnk vs. 1/T?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
-Ea/R
OH?
Heat a test tube at an angle at the side of the tube (not bottom)

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

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20. Alkanes are _________ and react by _________
OH- and NH3
CO (poisonous)
Eudiometer
Saturated - Substitution (which requires more radical conditions)

21. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Acidified
zero
No - NH3 and HCl gases are extremely soluble
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

22. What part of a liquid do you look at to measure its volume?
They stay the same.
Read the bottom of the meniscus
10?8
C2O4²?

23. ammonium/ammonium compounds
Heat a test tube at an angle at the side of the tube (not bottom)
acid + alcohol
Soluble
same KE - but PEice<PEwater

24. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
All except for lithium
boiling without losing volatile solvents/reactants
zero

25. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Sulfur
HClO4
Pale purple - (orange)-yellow - red - blue - green.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

26. Acids + Carbonates (bicarbonates) make?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Disulfur dichloride
Q=It (time in seconds)

27. silver compounds
redox reaction
ion pairing
CnH(2n+2)
Insoluble except for nitrate and acetate

28. group 1 ions/compounds
Pipette (burette if need repetition)
Tetrahedral
Mono; di; tri; tetra; penta; hexa.
Soluble

29. How are non-metal oxides and hydrides bonded? are they acidic or basic?
linear
ion pairing
ClO2?
non-metal oxides and hydrides are covalently bonded and are acidic.

30. What is an Alkyl group?

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31. Neutralization is an ________ reaction.
Graduated cylinder
diamond and graphite
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Exothermic (?H for ANY sa/sb = -57kJ/mol)

32. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
Cu3(PO4)2
SO4²?
catalyst=conc H2SO4

33. primary colors
a-IMFs - b-molecular volume
are less dense than water
red - green - blue
zero-th: decreases - first: constant - second: increases

34. Is a graduated cylinder or beaker more accurate?
Iodine and CO2 (dry ice)
Graduated cylinder
CH3COO?
Ions go through the salt bridge - electrons go through metal wires in the external circuit

35. What is the basic structure of an optical isomer?
O2 needs 4F/mol H2 needs 2F/mol
The one with most oxygen atoms (highest oxidation number)
Ionic compounds
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

36. What apparatus do you use to pour liquids?
zero
OH- and NH3
Pour liquids using a funnel or down a glass rod
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

37. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
RCHO (carbonyl at end)
Ksp = 108s5

38. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
CO (poisonous)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
ns² electrons (first in-first out)

39. What word is a clue for a redox reaction?
Eudiometer
Acidified
Filtration
0 and 14

40. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
CnH2n-2
do not change
'non-active' metals such as Cu - Ag - Au - Pt - etc.

41. Name 2 ways in which you can create a buffer?
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
Molecules with the same molecular formulas - but different structural formulas
neutralization: high K - H2O product dissociation: low K - H2O reactant
Greenish-yellow gas

42. What are isotopes?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
?G= -ve - E°= +ve
Pale yellow

43. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
OH?
Synthesis - separation and purification of the product and its identification.
[A?]/[HA] x 100 or [BH?]/[B] x 100

44. 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 -
Pipette (burette if need repetition)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CrO4²?

45. What shape is carbon dioxide?
Most INsoluble except group 1 and ammonium
T increases exponentially the proportion of molecules with E > Ea
linear
0.10M HCl (more ions)

46. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
S2O3²?
Group 1 hydroxides (ex: NaOH)
H+
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

47. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Sulfur
[A?]/[HA] x 100 or [BH?]/[B] x 100
Insoluble
Current - time and charge on ion (moles of e used in half cell reaction)

48. bromine
brown volatile liquid
do not change
Perform ICE BOX calculation based on K1
C4H10

49. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
|experimental - accepted|/accepted X 100
voltaic: + electrolytic: -
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

50. BaSO4
Decant
Unsaturated - addition (ex: decolorize bromine solution)
allow for the vapor pressure of water and make sure to level levels
Insoluble