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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 a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
The benzene ring (or more correctly the phenyl group - C6H5)
H+
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.
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.

2. Does Kw increase or decrease with T? Why?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
zero
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
O2 needs 4F/mol H2 needs 2F/mol

3. What do metal oxides plus acids form?
Salt + water
methyl formate
E=q + w (negative is by system - positive is on system)
Cu3(PO4)2

4. If Q < Ksp a ppt ______
same KE - but PEice<PEwater
Ksp = 27s4
ClO4?
Ppt will NOT form (unsaturated)

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

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6. What shape is water?
Making sigma bonds and holding lone pairs
Most INsoluble except group 1 and ammonium
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
bent

7. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Saturated - Substitution (which requires more radical conditions)
Synthesis - separation and purification of the product and its identification.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

8. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Sulfur
water and substances with (s) less dense than
Orange

9. sulfates
Ksp = s²
Soluble except Ag - Pb - Ca - Sr Ba)
Read the bottom of the meniscus
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

10. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
Acidified
ethers
Cu3(PO4)2

11. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
H2O + CO2 (it decomposes readily)
P2O5
Evaporation
Salt + water

12. What is the formula of butane?
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)
C4H10
CN?
The one with most oxygen atoms (highest oxidation number)

13. dichromate (soln + most solids)
q=mc?T q=mL (or n x ?h)
fractional distillation
NH2?
Orange

14. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
same KE - but PEice<PEwater
Salt and water
Ksp = s²

15. What are isomers?
Purple
Molecules with the same molecular formulas - but different structural formulas
Time?¹ - (ex. s?¹ - hr?¹ - etc)
zero-th: decreases - first: constant - second: increases

16. How are primary alcohols turned into acids?
redox reaction
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
basic
Glacial acetic acid

17. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
10?8
Ionic compounds
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

18. When a cell is 'flat' What is its voltage?
Salt + water
Sigma bonds are stronger than pi bonds
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
zero

19. barium sulfate
Tetrahedral
it's lower and occurs over less sharp a range
White precipitate
a-IMFs - b-molecular volume

20. mercury (II) ion
Decant
H3PO4
Heptane
Hg²?

21. What are the signs of ?G and E° for spontaneous reactions?
A) any range. b) 8-10 c) 4-6
Soluble
?G=negative - E° must be positive
CnH2n

22. How do you identify which is oxidized or otherwise?
Pour liquids using a funnel or down a glass rod
look for changes in oxidation # - the one that goes up is oxidized and is the RA
T increases exponentially the proportion of molecules with E > Ea
H3PO4

23. What do metal oxides plus non- metal oxides form?
Transition element compounds (except if it has a full or empty d shell)
At half equivalence - pH=pKa
Most INsoluble except group 1 and ammonium
Salts (ex: CaO + SO2 ? CaSO3)

24. What effect does increasing the size/surface area of a voltaic cell have on the cell?
[A?]/[HA] x 100 or [BH?]/[B] x 100
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
P2O5
Acid rain - dissolves marble buildings/statues and kills trees.

25. How does the melting point of a mixture compare to the MP of a pure substance?
Perform ICE BOX calculation based on K1
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
voltaic: - electrolytic: +
it is lower and occurs over less sharp a range

26. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Anode
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Filtration

27. Give an example of a concentrated weak acid.
?G= -ve - E°= +ve
catalyst=conc H2SO4
Cu3(PO4)2
Glacial acetic acid

28. What is HCOOCH3?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Both electrons come from the same atom (just as good as a regular bond)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Acids; HCOOCH3 is an ester

29. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
OH- and NH3
H2O + CO2 (it decomposes readily)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
The compound with the lowest Ksp value.

30. How can metals like iron and zinc be reduced?
Experimental mass/theoretical mass X 100
RCOOH
chemically (ex: with carbon)
Read the bottom of the meniscus

31. How are more active metals reduced?
RCOR
by electrolysis
Heat a test tube at an angle at the side of the tube (not bottom)
No - it depends on the number of ions produced on dissolving.

32. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H2O + CO2 (it decomposes readily)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
NO3?

33. Is the standard entropy (S°) of an element zero?
Iodine and CO2 (dry ice)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
0 and 14
But S° of element is not zero (except at 0K)

34. What do you need to make a polymer?
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)
CN?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
water and substances with (s) less dense than

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

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36. 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 -
H2PO4?
Soluble
bases

37. Both Acetic acid and ____________ are also functional isomers.
H3PO4
methyl formate
fruit - fish - bases
hydroxides (ex: Ba(OH)2)

38. Lattice energy is high for ions with _____ size and _____ charge
bent
Tetrahedral
small size and high charge
At half equivalence - pH=pKa

39. How do you explain trends in atomic properties using Coulomb's Law?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
atoms

40. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Ksp = 4s³
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
T increases exponentially the proportion of molecules with E > Ea
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

41. What should you check for before you begin titrating?
Tetrahedral
voltaic: - electrolytic: +
RCOR
Check for air bubbles in the buret and remove the buret funnel from the buret

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

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43. Can you collect soluble gases over water?
Products - reactants (except for BDE when it's reactants - products)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Cr2O7²?
No - NH3 and HCl gases are extremely soluble

44. Generally - which oxy acid is strongest?
blue (BTB)
The one with most oxygen atoms (highest oxidation number)
Mn²? - Cr³? - Cr³
?H-kJ - ?S-J - ?G-kJ

45. If a free element is involved - what type of reaction must be involved?
redox reaction
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
a-IMFs - b-molecular volume
Insoluble except nitrate and acetate

46. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CnH2n-2
ClO4?
are less dense than water
a-IMFs - b-molecular volume

47. What is precision?
How grouped results are
An active metal.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Current - time and charge on ion (moles of e used in half cell reaction)

48. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CO (poisonous)
metal oxides and hydrides are ionically bonded and basic

49. What is a dipeptide? polypeptide? protein?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Anode
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Perform ICE BOX calculation based on K1

50. chlorite
ClO2?
Filtration
Orange
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)