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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. phosphate
0 and 14
Evaporation
PO4³?
Mn²? - Cr³? - Cr³

2. Which of the rates changes more when temperature is increased?
Ppt will NOT form (unsaturated)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
OH?
?H formation of an element in standard state=0

3. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Anode
fruit - fish - bases

4. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
ROR
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

5. Esterification is...
acid + alcohol
Sulfur
Increases down group 1 decreases down group 17
boiling without losing volatile solvents/reactants

6. How are metal oxides and hydrides bonded? are they acidic or basic?
Acids; HCOOCH3 is an ester
metal oxides and hydrides are ionically bonded and basic
CN?
benzene is less reactive than alkenes

7. thiosulfate
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CrO4²?
Clear
S2O3²?

8. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
Eudiometer
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

9. How are strong ones written?
Saturated - Substitution (which requires more radical conditions)
strong acids/bases are written as H+ or OH- ions
non-metal oxides and hydrides are covalently bonded and are acidic.
acid + alcohol

10. When can supercooling occur? What does it look like on a cooling curve?

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11. How do you identify which is oxidized or otherwise?
|experimental - accepted|/accepted X 100
No - NH3 and HCl gases are extremely soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
look for changes in oxidation # - the one that goes up is oxidized and is the RA

12. What do metal oxides plus acids form?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
H+
proton donor base
Salt + water

13. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
Orange
Most INsoluble except group 1 and ammonium
Evaporation

14. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Anode
K1 x K2
Reduction always takes place at the cathode (RED CAT) In both types of cell!

15. What effect does increasing the size/surface area of a voltaic cell have on the cell?
diamond and graphite
O2 needs 4F/mol H2 needs 2F/mol
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
same KE - but PEice<PEwater

16. Is the freezing of ice endothermic or exothermic?
NH4?
strong acids/bases are written as H+ or OH- ions
Exothermic
an oxidized and reduced substance

17. What are the prefixes for the naming of binary molecular compound formulas (up to six)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Mono; di; tri; tetra; penta; hexa.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
ClO4?

18. How does benzene compare in reactivity to alkenes?
CrO4²?
Cu3(PO4)2
Acids; HCOOCH3 is an ester
benzene is less reactive than alkenes

19. Lattice energy is high for ions with _____ size and _____ charge
Big K=kf/kr
Glowing splint (positive result=relights)
small size and high charge
Decant

20. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Conjugate pair (one must be a weak base or acid)
C2O4²?
O2 needs 4F/mol H2 needs 2F/mol
a-IMFs - b-molecular volume

21. ammonium
NH4?
Concentration
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Q=It (time in seconds)

22. When combining half equations - what do you do to E° values when multiplying coefficients?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Nothing
How close results are to the accepted value
yellow

23. What is the general formula for an acid?
MnO4?
O2 needs 4F/mol H2 needs 2F/mol
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
RCOOH

24. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
proton acceptor.
10?8
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
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)

25. What do group I/II metal oxides and acids form?
A) any range. b) 8-10 c) 4-6
Big K=kf/kr
Salt and water
ion pairing

26. What type of compounds do metals/non metals form?
diamond and graphite
Mono; di; tri; tetra; penta; hexa.
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)
Ionic compounds

27. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
NH2?
Kc=Kp
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

28. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
CnH2n+1 often designated 'R' ex C3H7 is propyl
Hg2²?
voltaic: + electrolytic: -

29. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pipette (burette if need repetition)
Pale purple - (orange)-yellow - red - blue - green.
CnH2n+2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

30. What are the signs for ?G and E° for spontaneous reactions?
ClO2?
H+
benzene has a delocalized pi ring structure
?G= -ve - E°= +ve

31. How do you dilute an acid?

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32. How do you clean a buret/pipette for a titration?
How grouped results are
no - they're written undissociated (HAaq)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
OH?

33. How many ligands attach to a central ion in a complex ion?
Salts (ex: CaO + SO2 ? CaSO3)
#ligands=charge x2
proton donor base
blue glass - it filters UV

34. What steps do organic labs consist of?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
White precipitate
Synthesis - separation and purification of the product and its identification.
T increases exponentially the proportion of molecules with E > Ea

35. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
linear
Products - reactants (except for BDE when it's reactants - products)

36. What process do you use to obtain the precipitate from a solution?
basic
proton acceptor.
Pour liquids using a funnel or down a glass rod
Filtration

37. What do metal oxides plus non- metal oxides form?
Orange
CnH2n+2
#ligands=charge x2
Salts (ex: CaO + SO2 ? CaSO3)

38. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
CnH2n
Soluble except Ag - Pb - Ca - Sr Ba)
Ksp = s²
Pipette (burette if need repetition)

39. Name C7H16
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
ClO3?
Heptane
The benzene ring (or more correctly the phenyl group - C6H5)

40. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
no - they're written undissociated (HAaq)
different forms of the same element
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
basic

41. copper sulfate
blue
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
ion pairing
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

42. Generally - which oxy acid is strongest?
different forms of the same element
The one with most oxygen atoms (highest oxidation number)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
CO2 and H2O

43. What is the energy you must put into a reaction to make it start called?
ClO3?
CnH2n+1 often designated 'R' ex C3H7 is propyl
ROH
Initiation energy (NOT Ea)

44. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
blue
red - green - blue
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.
No - it depends on the number of ions produced on dissolving.

45. iodine - iodine solution - iodine vapor
Most INsoluble except group 1 and ammonium
K1 x K2
MnO4?
Silvery gray solid - brown - purple

46. ________ are Lewis bases - because they can donate a lone pair of electrons.
ClO3?
OH- and NH3
catalyst=conc H2SO4
Saturated - Substitution (which requires more radical conditions)

47. What shape is methane?
Tetrahedral
ns² electrons (first in-first out)
zero-th: decreases - first: constant - second: increases
Experimental mass/theoretical mass X 100

48. chromate ion (soln + most solids)
A) any range. b) 8-10 c) 4-6
?H formation of an element in standard state=0
OH- and NH3
yellow

49. Name some properties of Group 17
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
O2 needs 4F/mol H2 needs 2F/mol
bent

50. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Evaporation
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ns² electrons (first in-first out)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)