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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 is reflux?
benzene has a delocalized pi ring structure
CnH2n
boiling without losing volatile solvents/reactants
10?8

2. How are primary alcohols turned into acids?
voltaic: + electrolytic: -
The one with most oxygen atoms (highest oxidation number)
Initiation energy (NOT Ea)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

3. Is a graduated cylinder or beaker more accurate?
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)
linear
Insoluble
Graduated cylinder

4. perchlorate
strong acids/bases are written as H+ or OH- ions
ClO4?
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.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

5. Give an example of a dilute strong acid.
bases
Soluble except Ag - Pb - Ca - Sr Ba)
HClO4
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

6. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
The dilution effect when the solutions mix. M1V1 = M2V2
CnH2n+1 often designated 'R' ex C3H7 is propyl
water and substances with (s) less dense than
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

7. During a titration what is present in the beaker at the equivalence point?
ion pairing
10?8
A salt solution.
Insoluble (except group 1 ammonium and Ba)

8. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Graduated cylinder
K1 x K2
do not change
water and substances with (s) less dense than

9. What causes the dramatic effect of T on rate?
it is lower and occurs over less sharp a range
ethers
T increases exponentially the proportion of molecules with E > Ea
?G=negative - E° must be positive

10. When can supercooling occur? What does it look like on a cooling curve?

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11. What effect does increasing the size/surface area of a voltaic cell have on the cell?
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.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Initiation energy (NOT Ea)
are less dense than water

12. hydroxide
OH?
NO3?
ClO4?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

13. What is accuracy?
How close results are to the accepted value
Identity and purity (impure compounds usually have broad & low melting points)
Cr2O7²?
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

14. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
HClO4
Pour liquids using a funnel or down a glass rod
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Soluble

15. What do you use to look at burning magnesium? why?
blue glass - it filters UV
boiling without losing volatile solvents/reactants
strong acids/bases are written as H+ or OH- ions
Salt + water.

16. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
NO3?
10?8
Conjugate pair (one must be a weak base or acid)
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)

17. How are metal oxides and hydrides bonded? are they acidic or basic?
All except for lithium
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
metal oxides and hydrides are ionically bonded and basic
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

18. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Concentration
A) any range. b) 8-10 c) 4-6
Ksp = s²
Suniverse increases for spontaneous processes

19. What is the formula for alkynes?
water and substances with (s) less dense than
ClO3?
CnH2n-2
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

20. What is the third law of thermodynamics?
S crystal at 0K=0
H2PO4?
Initiation energy (NOT Ea)
No - NH3 and HCl gases are extremely soluble

21. What type of polymer is nylon?
NO3?
Synthetic condensation polymer (aka a polyamide)
q=mc?T q=mL (or n x ?h)
Orange

22. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Identity and purity (impure compounds usually have broad & low melting points)
H+
Read the bottom of the meniscus
Ppt will NOT form (unsaturated)

23. If a weak acid is diluted more - what happens to its % dissociation value?
Ionic compounds
ns² electrons (first in-first out)
Increases.
Decant

24. What do nonmetal oxides plus water form?
acids
allow for the vapor pressure of water and make sure to level levels
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Add acid to water so that the acid doesn't boil and spit

25. Does Benzene react by addition or substitution?
Concentration
methyl formate
Q=It (time in seconds)
it reacts by substitution NOT addition

26. What is the general formula for alkyl halides?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
A salt solution.
#ligands=charge x2
RX

27. What are isomers?
Experimental mass/theoretical mass X 100
Soluble
S2O3²?
Molecules with the same molecular formulas - but different structural formulas

28. What do you use for an acid spill? base spill?
allow for the vapor pressure of water and make sure to level levels
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Pale purple - (orange)-yellow - red - blue - green.
water and substances with (s) less dense than

29. carbonates
Insoluble except group 1 and ammonium
q=mc?T q=mL (or n x ?h)
same KE - but PEice<PEwater
All except for lithium

30. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Salt and water
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Heat a test tube at an angle at the side of the tube (not bottom)

31. One mole of electrons carries 96500Coulombs - what is this quantity called?

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32. Name six characteristics of transition elements (or their compounds)
H3PO4
zero
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)
CO2 and H2O

33. Is the standard entropy (S°) of an element zero?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Separating funnel
ClO3?
But S° of element is not zero (except at 0K)

34. 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
Both electrons come from the same atom (just as good as a regular bond)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
diamond and graphite

35. hydroxides
lighted splint (positive result=pop)
Insoluble (except group 1 ammonium and Ba)
by electrolysis
K2

36. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Decant
Anode - oxygen. Cathode - hydrogen
blue glass - it filters UV
same KE - but PEice<PEwater

37. What is the catalyst for this reaction Ester + ?
Hg²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
catalyst=conc H2SO4
Nothing

38. What does a short - sharp melting point indicate?
Glowing splint (positive result=relights)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero
Identity and purity (impure compounds usually have broad & low melting points)

39. Ions are not ______.
atoms
Mn²? - Cr³? - Cr³
CO2 and H2O
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

40. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Hg2²?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Big K=kf/kr
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

41. Which of the rates changes more when temperature is increased?
diamond and graphite
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
The compound with the lowest Ksp value.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

42. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Q=It (time in seconds)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Clear

43. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Unsaturated - addition (ex: decolorize bromine solution)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

44. cyanide
Acids; HCOOCH3 is an ester
CN?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Salts (ex: CaO + SO2 ? CaSO3)

45. What are the common strong bases?
Eudiometer
Mn²? - Cr³? - Cr³
Group 1 hydroxides (ex: NaOH)
diamond and graphite

46. How are more active metals reduced?
0.10M HCl (more ions)
by electrolysis
Exothermic
How grouped results are

47. How does benzene compare in reactivity to alkenes?
Eudiometer
Acids; HCOOCH3 is an ester
benzene is less reactive than alkenes
non-metal oxides and hydrides are covalently bonded and are acidic.

48. Nonmetals are good _____ agents. Metals are good _______ agents.
bent
methyl formate
Greenish-yellow gas
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

49. How are strong ones written?
Insoluble except group 1 and ammonium
S2O3²?
RCHO (carbonyl at end)
strong acids/bases are written as H+ or OH- ions

50. What are allotropes?
do not change
allow for the vapor pressure of water and make sure to level levels
different forms of the same element
CH3COO?