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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. What is the formula of butane?
a-IMFs - b-molecular volume
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
No - it depends on the number of ions produced on dissolving.
C4H10

2. What shape is carbon dioxide?
linear
do not change
Exothermic (?H for ANY sa/sb = -57kJ/mol)
atoms

3. Does Benzene react by addition or substitution?
linear
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
it reacts by substitution NOT addition
Nothing

4. How do you get Ecell for spontaneous reactions?
?H-kJ - ?S-J - ?G-kJ
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Making sigma bonds and holding lone pairs
Heptane

5. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
|experimental - accepted|/accepted X 100
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Ksp = s²

6. What electrons are lost/gained first in transition element ions?
CH3COO?
Anode - oxygen. Cathode - hydrogen
ns² electrons (first in-first out)
-Ea/R

7. How are metal oxides and hydrides bonded? are they acidic or basic?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
metal oxides and hydrides are ionically bonded and basic
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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

8. 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?
Ksp = 27s4
Disulfur dichloride
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
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

9. What is the general formula for an ether?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
ROR
R=8.31 J/mol/K
A salt solution.

10. What is the charge on a chlorine atom?
zero
Pipette (burette if need repetition)
Ksp = 4s³
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

11. oxalate
-Ea/R
Perform ICE BOX calculation based on K1
C2O4²?
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?)

12. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Ksp = 27s4
strong acids/bases are written as H+ or OH- ions
Pale yellow

13. What are the common strong bases?
S2O3²?
bent
Group 1 hydroxides (ex: NaOH)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

14. What do group I/II metal oxides plus water form?
Q=It (time in seconds)
bases
R=8.31 J/mol/K
NH2?

15. carbonate
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
CO3²?
bright yellow

16. Which of the rates changes more when temperature is increased?
K2
no - they're written undissociated (HAaq)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
allow for the vapor pressure of water and make sure to level levels

17. phosphates
Most INsoluble except group 1 and ammonium
How close results are to the accepted value
Distillation
Glacial acetic acid

18. Does Kw increase or decrease with T? Why?
non-metal oxides and hydrides are covalently bonded and are acidic.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Concentration

19. What do metal oxides plus acids form?
Eudiometer
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
The dilution effect when the solutions mix. M1V1 = M2V2
Salt + water

20. mercury (II) ion
Combine the equations for the half reactions in the non-spontaneous direction
Hg²?
q=mc?T q=mL (or n x ?h)
ionic and form hydrogen and hydroxide

21. potassium permanganate
CO2 and H2O
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Purple
ionic and form hydrogen and hydroxide

22. chlorine
Greenish-yellow gas
Increases down group 1 decreases down group 17
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)
ClO4?

23. dichromate (soln + most solids)
Orange
basic
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

24. What are the signs for ?G and E° for spontaneous reactions?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
C4H10
?G= -ve - E°= +ve
How close results are to the accepted value

25. What is the conjugate base of NH3?
NH2?
allow for the vapor pressure of water and make sure to level levels
Saturated - Substitution (which requires more radical conditions)
CN?

26. What things should you remember to do when collecting gas over water?
Salts (ex: CaO + SO2 ? CaSO3)
allow for the vapor pressure of water and make sure to level levels
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
0.10M HCl (more ions)

27. Name 2 ways in which you can create a buffer?
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)
linear
Insoluble except group 1 and ammonium
Decant

28. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Ksp = s²
But S° of element is not zero (except at 0K)
Insoluble except for nitrate and acetate

29. group 1 ions/compounds
Soluble
Purple
10?8
Concentration

30. Neutralization is an ________ reaction.
MnO4?
blue glass - it filters UV
E=q + w (negative is by system - positive is on system)
Exothermic (?H for ANY sa/sb = -57kJ/mol)

31. What do you need to make a polymer?
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)
SO4²?
blue

32. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
White precipitate
same KE - but PEice<PEwater
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
CnH(2n+2)

33. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
proton acceptor.
How close results are to the accepted value
do not change

34. What type of solutions do small - highly charged cations tend to form?
CnH2n-2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Exothermic

35. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Acids; HCOOCH3 is an ester
Synthetic condensation polymer (aka a polyamide)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

36. Lattice energy is high for ions with _____ size and _____ charge
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
small size and high charge
Glowing splint (positive result=relights)
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?)

37. Where are group I metals stored?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Unsaturated - addition (ex: decolorize bromine solution)
Group I metals (soft metals) are stored under oil
The Faraday or Faraday's constant.

38. What shape is ammonia?
K1 x K2
Hg²?
Heat a test tube at an angle at the side of the tube (not bottom)
Trigonal pyramidal

39. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
An active metal.
ROH
RX

40. What are isomers?
Purple
ionic and form hydrogen and hydroxide
water and substances with (s) less dense than
Molecules with the same molecular formulas - but different structural formulas

41. What word is a clue for a redox reaction?
Insoluble except for nitrate and acetate
O2 needs 4F/mol H2 needs 2F/mol
Acidified
+4-covalent - +2-ionic

42. hypochlorite
K2
ClO?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
blue glass - it filters UV

43. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
blue (BTB)
Eudiometer
Ksp = s²
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

44. What are the formulas for q?
CnH2n
H2PO4?
q=mc?T q=mL (or n x ?h)
chemically (ex: with carbon)

45. How do you compute % dissociation?
0.10M HCl (more ions)
CnH2n+2
Initiation energy (NOT Ea)
[A?]/[HA] x 100 or [BH?]/[B] x 100

46. What kind of bonding structure does benzene have?
benzene is less reactive than alkenes
benzene has a delocalized pi ring structure
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
H2PO4?

47. Metal hydrides are _____ and form _______ and _______ when added to water
The benzene ring (or more correctly the phenyl group - C6H5)
allow for the vapor pressure of water and make sure to level levels
Add acid to water so that the acid doesn't boil and spit
ionic and form hydrogen and hydroxide

48. What effect does increasing the size/surface area of a voltaic cell have on the cell?
diamond and graphite
yellow
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
|experimental - accepted|/accepted X 100

49. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Tetrahedral
q=mc?T q=mL (or n x ?h)
methyl formate

50. What are hybrid orbitals used for?
CO2 and H2O
Making sigma bonds and holding lone pairs
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)