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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 for percent yield?
Experimental mass/theoretical mass X 100
No - it depends on the number of ions produced on dissolving.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
#ligands=charge x2

2. What do you use for an acid spill? base spill?
[A?]/[HA] x 100 or [BH?]/[B] x 100
NH4?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
acids

3. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Synthesis - separation and purification of the product and its identification.
Sulfur
The dilution effect when the solutions mix. M1V1 = M2V2
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

4. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Salt and water
acid + alcohol
Group I metals (soft metals) are stored under oil
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

5. Ions are not ______.
red - green - blue
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
atoms
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

6. What value of R do you use for thermo calculations? gas calculations?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
?H formation of an element in standard state=0
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
it is lower and occurs over less sharp a range

7. Color (absorbance) is proportional to ________
zero-th: decreases - first: constant - second: increases
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Concentration
RCOR

8. chromate ion (soln + most solids)
yellow
NH4?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Tetrahedral

9. What do the 'a' and 'b' in Van Der Waal's equation allow for?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
a-IMFs - b-molecular volume
Anode - oxygen. Cathode - hydrogen
Distillation

10. What is the name of S2Cl2? (Know how to name others like this - too)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Disulfur dichloride
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

11. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
water and substances with (s) less dense than
The benzene ring (or more correctly the phenyl group - C6H5)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

12. What shape is methane?
CO3²?
Iodine and CO2 (dry ice)
blue
Tetrahedral

13. silver compounds
Insoluble except for nitrate and acetate
Group 1 hydroxides (ex: NaOH)
The benzene ring (or more correctly the phenyl group - C6H5)
-Ea/R

14. What is the pH of 1.0M HCl? 1M NaOH?
ClO3?
Mono; di; tri; tetra; penta; hexa.
Greenish-yellow gas
0 and 14

15. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Kc=Kp
Ksp = 27s4
Pipette (burette if need repetition)
Current - time and charge on ion (moles of e used in half cell reaction)

16. acetates
K2
An active metal.
#ligands=charge x2
Soluble

17. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
it's lower and occurs over less sharp a range
They stay the same.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

18. What is the test for oxygen?
Glowing splint (positive result=relights)
Cu3(PO4)2
Acidified
linear

19. nitrate
Evaporation
are less dense than water
NO3?
Greenish-yellow gas

20. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Graduated cylinder
HClO4
water and substances with (s) less dense than
Hg2²?

21. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Ksp = 108s5
Time?¹ - (ex. s?¹ - hr?¹ - etc)
A) any range. b) 8-10 c) 4-6
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

22. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
ROR
RNH2
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?)

23. What is the word equation for condensation polymerisation ?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Orange
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

24. thiosulfate
methyl formate
ion pairing
ionic and form hydrogen and hydroxide
S2O3²?

25. What do nonmetal oxides plus water form?
acids
Trigonal pyramidal
NH2?
HClO4

26. What is the formula of copper (II) phosphate?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Cu3(PO4)2
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Acid rain - dissolves marble buildings/statues and kills trees.

27. What do hydrocarbons form when they burn in air (oxygen)?
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.
Both electrons come from the same atom (just as good as a regular bond)
The one with most oxygen atoms (highest oxidation number)

28. primary colors
Mn²? - Cr³? - Cr³
red - green - blue
R=8.31 J/mol/K
Ppt will NOT form (unsaturated)

29. What type of compounds do metals/non metals form?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
atoms
Ionic compounds
CH3COO?

30. 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
The benzene ring (or more correctly the phenyl group - C6H5)
basic
T increases exponentially the proportion of molecules with E > Ea

31. silver iodide
Pale yellow
Sulfur
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Ksp = s²

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

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33. When the salt bridge is removed what happens to the cell reaction?
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.
It ceases - the circuit is broken.
Soluble except Ag - Pb - Ca - Sr Ba)
RNH2

34. Esters smell like _______ and amines smell like _______ and are ______.
Eudiometer
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
brown volatile liquid
fruit - fish - bases

35. What does saturated mean? Unsaturated?
by electrolysis
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Heat a test tube at an angle at the side of the tube (not bottom)
Salts (ex: CaO + SO2 ? CaSO3)

36. What is the formula for summation?

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37. What is the slope of the graph of lnk vs. 1/T?
blue glass - it filters UV
hydroxides (ex: Ba(OH)2)
-Ea/R
How grouped results are

38. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
RCHO (carbonyl at end)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Mn²? - Cr³? - Cr³
Conjugate pair (one must be a weak base or acid)

39. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Pour liquids using a funnel or down a glass rod
water and substances with (s) less dense than
ROR

40. 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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41. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
lighted splint (positive result=pop)
Current - time and charge on ion (moles of e used in half cell reaction)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
No - it depends on the number of ions produced on dissolving.

42. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
brown volatile liquid
blue (BTB)
Glacial acetic acid

43. carbonate
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Soluble
SO4²?
CO3²?

44. Alkanes are _________ and react by _________
CnH2n-2
Saturated - Substitution (which requires more radical conditions)
Read the bottom of the meniscus
Initiation energy (NOT Ea)

45. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Silvery gray solid - brown - purple
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
bent
non-metal oxides and hydrides are covalently bonded and are acidic.

46. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Selective absorption
Salt and water
lighted splint (positive result=pop)

47. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Soluble
voltaic: + electrolytic: -
chemically (ex: with carbon)
P2O5

48. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
allow for the vapor pressure of water and make sure to level levels
Eudiometer
-Ea/R

49. cyanide
Insoluble except for nitrate and acetate
Check for air bubbles in the buret and remove the buret funnel from the buret
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CN?

50. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
fractional distillation
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Salts (ex: CaO + SO2 ? CaSO3)