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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. 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
Suniverse increases for spontaneous processes
Making sigma bonds and holding lone pairs
[A?]/[HA] x 100 or [BH?]/[B] x 100

2. What is the second law of thermodynamics?
Soluble except Ag - Pb - Ca - Sr Ba)
PO4³?
Suniverse increases for spontaneous processes
Initiation energy (NOT Ea)

3. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
Ksp = 4s³
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

4. If ?S is positive - are the products more or less chaotic than the reactants?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
More chaotic (ex: gases made)
They stay the same.
it's lower and occurs over less sharp a range

5. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
fruit - fish - bases
it's lower and occurs over less sharp a range
neutralization: high K - H2O product dissociation: low K - H2O reactant
K1 x K2

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

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7. What process do you use to obtain a solvent from a solution?
Orange
Distillation
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Salt + water.

8. Can you collect soluble gases over water?
diamond and graphite
a-IMFs - b-molecular volume
No - NH3 and HCl gases are extremely soluble
Decant

9. What is precision?
ClO3?
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)
Mono; di; tri; tetra; penta; hexa.
How grouped results are

10. What is H2CO3 (carbonate acid) usually written as?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
H2PO4?
H2O + CO2 (it decomposes readily)
Disulfur dichloride

11. Does Benzene react by addition or substitution?
Both electrons come from the same atom (just as good as a regular bond)
it reacts by substitution NOT addition
Salt + water
Molecules with the same molecular formulas - but different structural formulas

12. What is reflux?
CN?
Soluble except Ag - Pb - Ca - Sr Ba)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
boiling without losing volatile solvents/reactants

13. nitrate
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
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.
proton acceptor.
NO3?

14. What type of polymer is nylon?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Synthetic condensation polymer (aka a polyamide)
basic
non-metal oxides and hydrides are covalently bonded and are acidic.

15. What type of solutions do small - highly charged cations tend to form?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Decant
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

16. What is the formula for summation?

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17. What are the common strong bases?
strong acids/bases are written as H+ or OH- ions
How grouped results are
Group 1 hydroxides (ex: NaOH)
Most are soluble except Ag - Pb

18. Why are noble gases stable?
-Ea/R
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

19. What are hybrid orbitals used for?
hydroxides (ex: Ba(OH)2)
The compound with the lowest Ksp value.
Making sigma bonds and holding lone pairs
Synthetic condensation polymer (aka a polyamide)

20. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Eudiometer
non-metal oxides and hydrides are covalently bonded and are acidic.
The compound with the lowest Ksp value.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

21. What is the conjugate acid of H2PO4?
q=mc?T q=mL (or n x ?h)
H3PO4
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Selective absorption

22. What do group I/II metal oxides plus water form?
Experimental mass/theoretical mass X 100
How grouped results are
bases
Greenish-yellow gas

23. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
CnH(2n+2)
Clear
But S° of element is not zero (except at 0K)

24. chlorate
ClO3?
An active metal.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
blue (BTB)

25. What is a coordinate covalent bond?
non-metal oxides and hydrides are covalently bonded and are acidic.
Insoluble except for nitrate and acetate
Transition element compounds (except if it has a full or empty d shell)
Both electrons come from the same atom (just as good as a regular bond)

26. Name 2 ways in which you can create a buffer?
R=8.31 J/mol/K
H+
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)
red - green - blue

27. What equipment do you need for a titration?
ROH
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Perform ICE BOX calculation based on K1
NH2?

28. What shape is ammonia?
boiling without losing volatile solvents/reactants
blue (BTB)
by electrolysis
Trigonal pyramidal

29. 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?
Perform ICE BOX calculation based on K1
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH2n-2
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

30. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Graduated cylinder
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
do not change
Identity and purity (impure compounds usually have broad & low melting points)

31. oxalate
C2O4²?
Synthesis - separation and purification of the product and its identification.
Filtration
Sulfur

32. What is the general formula for alkyl halides?
?G= -ve - E°= +ve
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
RX
linear

33. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
left - ppt will form
different forms of the same element
fractional distillation

34. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Most are soluble except Ag - Pb
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
No - it depends on the number of ions produced on dissolving.
The Faraday or Faraday's constant.

35. halides
CnH2n
Most are soluble except Ag - Pb
S crystal at 0K=0
Ksp = s²

36. What are the units of the first order rate constant?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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

37. primary colors
ClO2?
red - green - blue
+4-covalent - +2-ionic
Pour liquids using a funnel or down a glass rod

38. Alkenes are ________ and react by __________
a-IMFs - b-molecular volume
T increases exponentially the proportion of molecules with E > Ea
Kc=Kp
Unsaturated - addition (ex: decolorize bromine solution)

39. If a free element is involved - what type of reaction must be involved?
Greenish-yellow gas
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Insoluble except for nitrate and acetate
redox reaction

40. What is the word equation for addition polymerisation?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
An active metal.
Pale yellow

41. Which alkali metals float on water?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
All except for lithium
Purple
strong acids/bases are written as H+ or OH- ions

42. bromine
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
S crystal at 0K=0
brown volatile liquid
S2O3²?

43. When is ?G zero?
?G=negative - E° must be positive
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
NO3?

44. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
NH2?
Unsaturated - addition (ex: decolorize bromine solution)
linear
zero

45. mercury (I) ion
Hg2²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Synthesis - separation and purification of the product and its identification.

46. What electrons are lost/gained first in transition element ions?
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.
Most INsoluble except group 1 and ammonium
ns² electrons (first in-first out)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

47. ammonium
ClO?
The one with most oxygen atoms (highest oxidation number)
An active metal.
NH4?

48. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Current - time and charge on ion (moles of e used in half cell reaction)
Insoluble (except group 1 ammonium and Ba)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

49. What type of compounds do metals/non metals form?
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.
CO3²?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ionic compounds

50. What do group I/II metal oxides and acids form?
H2O + CO2 (it decomposes readily)
OH?
fractional distillation
Salt and water