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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. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
zero
chemically (ex: with carbon)
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)
P2O5

2. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
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.
10?8
Check for air bubbles in the buret and remove the buret funnel from the buret
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

3. What do you do to get rid of most of the solution from a precipitate?
Perform ICE BOX calculation based on K1
Decant
0.10M HCl (more ions)
Identity and purity (impure compounds usually have broad & low melting points)

4. phosphates
Greenish-yellow gas
Most INsoluble except group 1 and ammonium
ClO2?
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

5. Acid plus base make?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
At half equivalence - pH=pKa
Acidified
Salt + water.

6. bromine
ionic and form hydrogen and hydroxide
Sigma bonds are stronger than pi bonds
Clear
brown volatile liquid

7. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
RNH2
proton acceptor.

8. What do ions and electrons travel through in a voltaic/electrolytic cell?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
redox reaction

9. Does Benzene react by addition or substitution?
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
ROR
Iodine and CO2 (dry ice)
it reacts by substitution NOT addition

10. What is the general formula for an acid?
CH3COO?
RCOOH
Evaporation
Most INsoluble except group 1 and ammonium

11. ________ are Lewis bases - because they can donate a lone pair of electrons.
SO4²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
redox reaction
OH- and NH3

12. A geometric (or cis-trans) isomer exists due to.....
Check for air bubbles in the buret and remove the buret funnel from the buret
Soluble
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
The dilution effect when the solutions mix. M1V1 = M2V2

13. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
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)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Greenish-yellow gas
neutralization: high K - H2O product dissociation: low K - H2O reactant

14. dichromate (soln + most solids)
Acids; HCOOCH3 is an ester
All except for lithium
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
Orange

15. When a cell is 'flat' What is its voltage?
More chaotic (ex: gases made)
blue (BTB)
R=8.31 J/mol/K
zero

16. What are the formulas for q?
zero
Monomer + monomer = polymer product + a simple molecule such as water or HCl
q=mc?T q=mL (or n x ?h)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

17. perchlorate
ClO4?
same KE - but PEice<PEwater
Add acid to water so that the acid doesn't boil and spit
Soluble

18. How many normal boiling points and boiling points are there?

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19. Name 2 ways in which you can create a buffer?
Greenish-yellow gas
atoms
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)
fractional distillation

20. sulfates
It ceases - the circuit is broken.
Soluble except Ag - Pb - Ca - Sr Ba)
H+
RX

21. What do you use for an acid spill? base spill?
They stay the same.
MnO4?
Disulfur dichloride
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

22. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
A salt solution.
Trigonal pyramidal

23. 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.
atoms
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

24. dihydrogen phosphate
Soluble
Glowing splint (positive result=relights)
ClO2?
H2PO4?

25. Do anions flow to the cathode or anode?
acids
Anode
are less dense than water
q=mc?T q=mL (or n x ?h)

26. How are strong ones written?
+4-covalent - +2-ionic
Insoluble except nitrate and acetate
strong acids/bases are written as H+ or OH- ions
Heat a test tube at an angle at the side of the tube (not bottom)

27. A Bronsted-Lowry base is...
a-IMFs - b-molecular volume
proton acceptor.
-Ea/R
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)

28. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
How grouped results are
strong acids/bases are written as H+ or OH- 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

29. Do you use J or kJ for ?H - ?S - and ?G?
White precipitate
How close results are to the accepted value
?H-kJ - ?S-J - ?G-kJ
?G=negative - E° must be positive

30. BaSO4
ethers
Insoluble except for nitrate and acetate
CrO4²?
Insoluble

31. What are allotropes?
Anode
diamond and graphite
Soluble
different forms of the same element

32. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
same KE - but PEice<PEwater
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
RCOOH

33. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Glowing splint (positive result=relights)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
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
Pour liquids using a funnel or down a glass rod

34. What are amphoteric oxides?
Making sigma bonds and holding lone pairs
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
bases

35. phosphate
Soluble
PO4³?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
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

36. What is the formula for alkynes?
basic
Acid rain - dissolves marble buildings/statues and kills trees.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
CnH2n-2

37. For a dibasic acid (H2A) - [A²?]= ____ ?
Silvery gray solid - brown - purple
Insoluble except for nitrate and acetate
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)
K2

38. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
CH3COO?
Insoluble (except group 1 ammonium and Ba)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

39. Metal hydrides are _____ and form _______ and _______ when added to water
The Faraday or Faraday's constant.
ionic and form hydrogen and hydroxide
Pipette (burette if need repetition)
Group 1 hydroxides (ex: NaOH)

40. 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)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Concentration
Reduction always takes place at the cathode (RED CAT) In both types of cell!

41. The oxidation # for acid base reactions...
zero
They decrease (or could be the same if the solid has ONLY JUST disappeared)
How close results are to the accepted value
do not change

42. How do you identify which is oxidized or otherwise?
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
look for changes in oxidation # - the one that goes up is oxidized and is the RA
diamond and graphite
Anode - oxygen. Cathode - hydrogen

43. lead iodide
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Anode
bright yellow
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

44. What part of a liquid do you look at to measure its volume?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Read the bottom of the meniscus
But S° of element is not zero (except at 0K)
The compound with the lowest Ksp value.

45. What apparatus do you use to pour liquids?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Pour liquids using a funnel or down a glass rod
The Faraday or Faraday's constant.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

46. Is the freezing of ice endothermic or exothermic?
Exothermic
metal oxides and hydrides are ionically bonded and basic
Synthesis - separation and purification of the product and its identification.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

47. How are more active metals reduced?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
by electrolysis
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
+4-covalent - +2-ionic

48. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
CO3²?
zero
Soluble

49. thiosulfate
S2O3²?
Clear
ion pairing
P2O5

50. Where are group I metals stored?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Group I metals (soft metals) are stored under oil
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Glacial acetic acid