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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.
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1. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
fractional distillation
OH?
atoms

2. What are hybrid orbitals used for?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Making sigma bonds and holding lone pairs
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

3. How are more active metals reduced?
The dilution effect when the solutions mix. M1V1 = M2V2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
O2 needs 4F/mol H2 needs 2F/mol
by electrolysis

4. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Big K=kf/kr
The benzene ring (or more correctly the phenyl group - C6H5)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

5. What are two allotropes of carbon?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
diamond and graphite
benzene has a delocalized pi ring structure
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

6. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
RCOOH
Products - reactants (except for BDE when it's reactants - products)
P2O5
do not change

7. mercury (II) ion
Ppt will NOT form (unsaturated)
Distillation
Hg²?
Clear

8. What are isotopes?
ClO4?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
a-IMFs - b-molecular volume

9. What process do you use to obtain a solvent from a solution?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
OH- and NH3
Only temperature
Distillation

10. chlorine
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Greenish-yellow gas
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
Disulfur dichloride

11. What is an Alkyl group?

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12. What do group I/II metal oxides plus water form?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Ppt will NOT form (unsaturated)
Insoluble except nitrate and acetate
bases

13. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
CN?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CnH2n-2
Current - time and charge on ion (moles of e used in half cell reaction)

14. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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)
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.

15. Name C7H16
They stay the same.
Greenish-yellow gas
Heptane
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

16. What are the formulas for q?
ion pairing
[A?]/[HA] x 100 or [BH?]/[B] x 100
q=mc?T q=mL (or n x ?h)
do not change

17. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
CO3²?
Group 1 hydroxides (ex: NaOH)
boiling without losing volatile solvents/reactants
neutralization: high K - H2O product dissociation: low K - H2O reactant

18. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
ionic and form hydrogen and hydroxide
10?8
redox reaction
Heptane

19. Do anions flow to the cathode or anode?
Hg2²?
ROR
Acidified
Anode

20. How do you find the pH for a dibasic acid? (H2A)?
Pale yellow
Transition element compounds (except if it has a full or empty d shell)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Perform ICE BOX calculation based on K1

21. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Evaporation
The dilution effect when the solutions mix. M1V1 = M2V2
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
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

22. How does the melting point of a mixture compare to the MP of a pure substance?
Perform ICE BOX calculation based on K1
catalyst=conc H2SO4
it is lower and occurs over less sharp a range
No - NH3 and HCl gases are extremely soluble

23. What is the formula for summation?

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24. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
zero
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

25. What is the general formula for an aldehyde?
[A?]/[HA] x 100 or [BH?]/[B] x 100
RCHO (carbonyl at end)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Salt + water

26. Name 2 ways in which you can create a buffer?
CO (poisonous)
ns² electrons (first in-first out)
Exothermic
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)

27. What process do you use to separate two liquids with different boiling points?
fractional distillation
OH?
It ceases - the circuit is broken.
Soluble

28. When the salt bridge is removed what happens to the cell reaction?
Increases.
Anode
It ceases - the circuit is broken.
#ligands=charge x2

29. chromate
acids
q=mc?T q=mL (or n x ?h)
ClO4?
CrO4²?

30. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
S2O3²?
same KE - but PEice<PEwater
different forms of the same element
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

31. 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!
Cu3(PO4)2
Disulfur dichloride
zero

32. thiosulfate
ROR
Transition element compounds (except if it has a full or empty d shell)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
S2O3²?

33. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
a-IMFs - b-molecular volume
Kc=Kp

34. dihydrogen phosphate
H2PO4?
#ligands=charge x2
Pour liquids using a funnel or down a glass rod
Purple

35. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
ClO2?
no - they're written undissociated (HAaq)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Cr2O7²?

36. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
Ksp = 4s³
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.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

37. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
0.10M HCl (more ions)
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
Group 1 hydroxides (ex: NaOH)

38. What type of polymer is nylon?
Perform ICE BOX calculation based on K1
Orange
Synthetic condensation polymer (aka a polyamide)
Filtration

39. Esterification is...
it is lower and occurs over less sharp a range
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Silvery gray solid - brown - purple
acid + alcohol

40. What is the conjugate base of NH3?
catalyst=conc H2SO4
[A?]/[HA] x 100 or [BH?]/[B] x 100
Clear
NH2?

41. What is HCOOCH3?
Acids; HCOOCH3 is an ester
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
?H-kJ - ?S-J - ?G-kJ
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)

42. sulfates
atoms
Soluble except Ag - Pb - Ca - Sr Ba)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Molecules with the same molecular formulas - but different structural formulas

43. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Soluble
?G= -ve - E°= +ve
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

44. What is the slope of the graph of lnk vs. 1/T?
Add acid to water so that the acid doesn't boil and spit
-Ea/R
ROR
Time?¹ - (ex. s?¹ - hr?¹ - etc)

45. chlorite
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ClO2?
non-metal oxides and hydrides are covalently bonded and are acidic.
it reacts by substitution NOT addition

46. What shape is carbon dioxide?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
linear
left - ppt will form
A salt solution.

47. How does the melting point of a mixture compare to the MP of a pure substance?

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48. How are metal oxides and hydrides bonded? are they acidic or basic?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
ethers
voltaic: + electrolytic: -
metal oxides and hydrides are ionically bonded and basic

49. What is the formula for percent error?
Pipette (burette if need repetition)
Soluble
Check for air bubbles in the buret and remove the buret funnel from the buret
|experimental - accepted|/accepted X 100

50. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
OH?
bright yellow
blue (BTB)