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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 the catalyst for this reaction Ester + ?
proton acceptor.
q=mc?T q=mL (or n x ?h)
Products - reactants (except for BDE when it's reactants - products)
catalyst=conc H2SO4

2. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
CO2 and H2O
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.
lighted splint (positive result=pop)

3. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
Insoluble
White precipitate
How close results are to the accepted value

4. What are the formulas for q?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
left - ppt will form
q=mc?T q=mL (or n x ?h)
fractional distillation

5. What is the word equation for addition polymerisation?
ionic and form hydrogen and hydroxide
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The one with most oxygen atoms (highest oxidation number)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

6. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
red - green - blue
Heptane
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?)

7. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acid rain - dissolves marble buildings/statues and kills trees.
Cu3(PO4)2

8. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
acid + alcohol
CO (poisonous)
Selective absorption
?G=negative - E° must be positive

9. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
More chaotic (ex: gases made)
Ksp = 4s³
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
|experimental - accepted|/accepted X 100

10. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
An active metal.
Pale purple - (orange)-yellow - red - blue - green.
?H-kJ - ?S-J - ?G-kJ
No - it depends on the number of ions produced on dissolving.

11. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Group I metals (soft metals) are stored under oil
P2O5
[A?]/[HA] x 100 or [BH?]/[B] x 100
Molecules with the same molecular formulas - but different structural formulas

12. Can you collect soluble gases over water?
Heptane
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
No - NH3 and HCl gases are extremely soluble
Pour liquids using a funnel or down a glass rod

13. Why are noble gases stable?
0.10M HCl (more ions)
How grouped results are
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
blue glass - it filters UV

14. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Check for air bubbles in the buret and remove the buret funnel from the buret
H+
Increases.
water and substances with (s) less dense than

15. hydroxide
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
A) any range. b) 8-10 c) 4-6
OH?

16. nitrate
Products - reactants (except for BDE when it's reactants - products)
NO3?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Increases down group 1 decreases down group 17

17. Nonmetals are good _____ agents. Metals are good _______ agents.
bases
Acids; HCOOCH3 is an ester
Ksp = 108s5
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

18. Why are i factors (Van't Hoff factors) often less than ideal?
water and substances with (s) less dense than
Unsaturated - addition (ex: decolorize bromine solution)
ion pairing
Soluble

19. What is precision?
How grouped results are
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Soluble
Exothermic

20. How do you get Ecell for spontaneous reactions?
H3PO4
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
NH4?

21. What is the formula for alkenes?
CnH2n
Insoluble except group 1 and ammonium
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
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

22. thiosulfate
do not change
An active metal.
S2O3²?
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)

23. acetate
Orange
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CH3COO?
methyl formate

24. What do group I/II metal oxides and acids form?
The one with most oxygen atoms (highest oxidation number)
Salt and water
ns² electrons (first in-first out)
Kc=Kp

25. What do you need to make a polymer?
An active metal.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
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)
Insoluble except group 1 and ammonium

26. Alkenes are ________ and react by __________
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
O2 needs 4F/mol H2 needs 2F/mol
Unsaturated - addition (ex: decolorize bromine solution)
same KE - but PEice<PEwater

27. silver iodide
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Pale yellow
Hg2²?

28. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Synthetic condensation polymer (aka a polyamide)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
atoms
Synthesis - separation and purification of the product and its identification.

29. 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
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Salt + water

30. An amphiprotic (amphoteric) species is...
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
Hg²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Ppt will NOT form (unsaturated)

31. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Sigma bonds are stronger than pi bonds
Trigonal pyramidal

32. What shape is ammonia?
Trigonal pyramidal
Orange
Transition element compounds (except if it has a full or empty d shell)
CO (poisonous)

33. silver compounds
Insoluble except for nitrate and acetate
an oxidized and reduced substance
An active metal.
At half equivalence - pH=pKa

34. mercury (II) ion
bent
Ksp = s²
Graduated cylinder
Hg²?

35. What is the conjugate acid of H2PO4?
H3PO4
HClO4
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Both electrons come from the same atom (just as good as a regular bond)

36. What is the word equation for condensation polymerisation ?
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)
Big K=kf/kr
Monomer + monomer = polymer product + a simple molecule such as water or HCl
PO4³?

37. During a titration what is present in the beaker at the equivalence point?
ClO?
A salt solution.
NH4?
Glowing splint (positive result=relights)

38. How many faradays of electric charge do you need to produce one mole of O2? H2?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
O2 needs 4F/mol H2 needs 2F/mol
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Conjugate pair (one must be a weak base or acid)

39. What are two substances that sublime at 1 atm when heated?
The one with most oxygen atoms (highest oxidation number)
It ceases - the circuit is broken.
CO2 and H2O
Iodine and CO2 (dry ice)

40. What is a dipeptide? polypeptide? protein?
strong acids/bases are written as H+ or OH- ions
Distillation
But S° of element is not zero (except at 0K)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

41. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
q=mc?T q=mL (or n x ?h)
Acid rain - dissolves marble buildings/statues and kills trees.
|experimental - accepted|/accepted X 100

42. What is the name of S2Cl2? (Know how to name others like this - too)
0 and 14
acids
Disulfur dichloride
same KE - but PEice<PEwater

43. Give an example of a dilute strong acid.
HClO4
Trigonal pyramidal
An active metal.
Exothermic

44. What do you use to look at burning magnesium? why?
blue glass - it filters UV
Exothermic
catalyst=conc H2SO4
brown volatile liquid

45. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
proton donor base
Insoluble (except group 1 ammonium and Ba)
Check for air bubbles in the buret and remove the buret funnel from the buret

46. How does group 1 metals' density compare to water's?
Cu3(PO4)2
Salt + water.
are less dense than water
Ions go through the salt bridge - electrons go through metal wires in the external circuit

47. What is a coordinate covalent bond?
atoms
a-IMFs - b-molecular volume
ns² electrons (first in-first out)
Both electrons come from the same atom (just as good as a regular bond)

48. Is the freezing of ice endothermic or exothermic?
zero
Conjugate pair (one must be a weak base or acid)
RNH2
Exothermic

49. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
Ksp = 4s³
It ceases - the circuit is broken.
S2O3²?

50. chromate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ppt will NOT form (unsaturated)
basic
CrO4²?