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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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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. Which alkali metals float on water?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
?G= -ve - E°= +ve
All except for lithium
SO4²?

2. How are metal oxides and hydrides bonded? are they acidic or basic?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
metal oxides and hydrides are ionically bonded and basic
Exothermic (?H for ANY sa/sb = -57kJ/mol)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

3. How can metals like iron and zinc be reduced?
no - they're written undissociated (HAaq)
chemically (ex: with carbon)
bright yellow
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

4. What are the names and formulas of the 6 strong acids?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
?G=negative - E° must be positive
Graduated cylinder

5. What does a short - sharp melting point indicate?
OH?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Identity and purity (impure compounds usually have broad & low melting points)
0.10M HCl (more ions)

6. cyanide
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
atoms
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
CN?

7. What type of compounds do metals/non metals form?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
C4H10
Soluble except Ag - Pb - Ca - Sr Ba)
Ionic compounds

8. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Ksp = 108s5
Ionic compounds
K1 x K2
NH4?

9. What is the conjugate acid of H2PO4?
H3PO4
?H-kJ - ?S-J - ?G-kJ
acid + alcohol
SO4²?

10. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
CnH2n
acids
zero
Evaporation

11. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
a-IMFs - b-molecular volume
q=mc?T q=mL (or n x ?h)
PO4³?

12. How are primary alcohols turned into acids?
ClO4?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
10?8
water and substances with (s) less dense than

13. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Tetrahedral
?G= -ve - E°= +ve
HClO4
same KE - but PEice<PEwater

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

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15. Name 2 ways in which you can create a buffer?
MnO4?
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)
same KE - but PEice<PEwater
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

16. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
chemically (ex: with carbon)
H+
ClO3?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

17. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
hydroxides (ex: Ba(OH)2)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
An active metal.

18. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Add acid to water so that the acid doesn't boil and spit
redox reaction
Current - time and charge on ion (moles of e used in half cell reaction)

19. What apparatus do you use to separate 2 immiscible liquids?
zero
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Separating funnel
bright yellow

20. What is the charge on a chlorine atom?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
zero
Most are soluble except Ag - Pb
Unsaturated - addition (ex: decolorize bromine solution)

21. bromothymol
NO3?
benzene is less reactive than alkenes
blue (BTB)
blue glass - it filters UV

22. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
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)
strong acids/bases are written as H+ or OH- ions
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
Sulfur

23. What shape is ammonia?
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
Insoluble except group 1 and ammonium
Trigonal pyramidal
Cu3(PO4)2

24. What is an Alkyl group?

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25. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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

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27. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ClO?
linear

28. 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.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Both electrons come from the same atom (just as good as a regular bond)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

29. Which would cause the bulb in a conductivity apparatus to be brightest?
ClO2?
0.10M HCl (more ions)
bases
H+

30. What is the formula for alkanes?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
CnH2n+2
left - ppt will form

31. What is the name of S2Cl2? (Know how to name others like this - too)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
linear
RCHO (carbonyl at end)
Disulfur dichloride

32. 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)
basic
diamond and graphite
Sigma bonds are stronger than pi bonds

33. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
boiling without losing volatile solvents/reactants
Distillation
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
water and substances with (s) less dense than

34. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
redox reaction
Purple
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

35. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
+4-covalent - +2-ionic
Kc=Kp
Salt + water
CH3COO?

36. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
ion pairing
CN?
methyl formate

37. What is precision?
#ligands=charge x2
P2O5
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
How grouped results are

38. What is accuracy?
Cu3(PO4)2
10?8
#ligands=charge x2
How close results are to the accepted value

39. What causes the dramatic effect of T on rate?
10?8
Ksp = 4s³
T increases exponentially the proportion of molecules with E > Ea
ROR

40. What kind of bonding structure does benzene have?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Monomer + monomer = polymer product + a simple molecule such as water or HCl
benzene has a delocalized pi ring structure
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)

41. What are two substances that sublime at 1 atm when heated?
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.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Iodine and CO2 (dry ice)
CO3²?

42. BaSO4
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
CrO4²?
Insoluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

43. Both Acetic acid and ____________ are also functional isomers.
0.10M HCl (more ions)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
A) any range. b) 8-10 c) 4-6
methyl formate

44. When is ?G zero?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Check for air bubbles in the buret and remove the buret funnel from the buret
brown volatile liquid

45. Acidic gases like SO2 in the atmosphere cause what environmental problems?
catalyst=conc H2SO4
Acid rain - dissolves marble buildings/statues and kills trees.
Salt + water.
atoms

46. sulfate
Salts (ex: CaO + SO2 ? CaSO3)
SO4²?
Q=It (time in seconds)
Saturated - Substitution (which requires more radical conditions)

47. Is the ?H formation of an element in standard state zero?
Eudiometer
Purple
?H formation of an element in standard state=0
Cu3(PO4)2

48. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
ionic and form hydrogen and hydroxide
Ionic compounds
Salt and water
Reduction always takes place at the cathode (RED CAT) In both types of cell!

49. What are the signs of ?G and E° for spontaneous reactions?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Experimental mass/theoretical mass X 100
?G=negative - E° must be positive

50. Does reactivity increase/decrease going down group 1 and group 17?
A) any range. b) 8-10 c) 4-6
acids
CN?
Increases down group 1 decreases down group 17