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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 things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
proton donor base
CnH(2n+2)
White precipitate

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

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3. What electrons are lost/gained first in transition element ions?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ns² electrons (first in-first out)
Salt + water.
Soluble

4. Can you collect soluble gases over water?
fruit - fish - bases
R=8.31 J/mol/K
Glowing splint (positive result=relights)
No - NH3 and HCl gases are extremely soluble

5. What device would you use to measure a volume of gas?
K1 x K2
NO3?
Eudiometer
ethers

6. Metal hydrides are _____ and form _______ and _______ when added to water
it is lower and occurs over less sharp a range
Graduated cylinder
The dilution effect when the solutions mix. M1V1 = M2V2
ionic and form hydrogen and hydroxide

7. What do nonmetal oxides plus water form?
More chaotic (ex: gases made)
Distillation
acids
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

8. bromine
benzene is less reactive than alkenes
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Distillation
brown volatile liquid

9. Neutralization is an ________ reaction.
Purple
Pipette (burette if need repetition)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
-Ea/R

10. If Q < Ksp a ppt ______
S crystal at 0K=0
Ppt will NOT form (unsaturated)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Eudiometer

11. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
catalyst=conc H2SO4
Reduction always takes place at the cathode (RED CAT) In both types of cell!
HClO4

12. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Mn²? - Cr³? - Cr³
?H formation of an element in standard state=0
a-IMFs - b-molecular volume
Insoluble except for nitrate and acetate

13. What do acids plus active metals form?
lighted splint (positive result=pop)
voltaic: + electrolytic: -
Hg²?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

14. What do group I/II metal oxides plus water form?
bases
?H formation of an element in standard state=0
+4-covalent - +2-ionic
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

15. hydroxides
Insoluble (except group 1 ammonium and Ba)
RNH2
?G=negative - E° must be positive
It ceases - the circuit is broken.

16. What type of compounds are almost always colored?
Ionic compounds
bases
ns² electrons (first in-first out)
Transition element compounds (except if it has a full or empty d shell)

17. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Ksp = s²
Anode - oxygen. Cathode - hydrogen
Pale purple - (orange)-yellow - red - blue - green.
Glowing splint (positive result=relights)

18. hydroxide
Ionic compounds
ClO2?
brown volatile liquid
OH?

19. How does group 1 metals' density compare to water's?
are less dense than water
voltaic: - electrolytic: +
Both electrons come from the same atom (just as good as a regular bond)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

20. How are strong ones written?
Mn²? - Cr³? - Cr³
SO4²?
Group 1 hydroxides (ex: NaOH)
strong acids/bases are written as H+ or OH- ions

21. What is Big K in terms of kf and kr?
same KE - but PEice<PEwater
Eudiometer
K2
Big K=kf/kr

22. What is HCOOCH3?
Acid rain - dissolves marble buildings/statues and kills trees.
Acids; HCOOCH3 is an ester
fractional distillation
K1 x K2

23. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
zero
NH2?
'non-active' metals such as Cu - Ag - Au - Pt - etc.

24. Color (absorbance) is proportional to ________
Concentration
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
small size and high charge

25. What are allotropes?
A salt solution.
different forms of the same element
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
q=mc?T q=mL (or n x ?h)

26. chromate
CrO4²?
RX
RCOOH
Separating funnel

27. What are isomers?
strong acids/bases are written as H+ or OH- ions
White precipitate
Insoluble except group 1 and ammonium
Molecules with the same molecular formulas - but different structural formulas

28. Do anions flow to the cathode or anode?
OH?
The compound with the lowest Ksp value.
zero
Anode

29. How do you dilute an acid?

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30. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
How grouped results are
Making sigma bonds and holding lone pairs

31. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
#ligands=charge x2
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
benzene has a delocalized pi ring structure
Exothermic (?H for ANY sa/sb = -57kJ/mol)

32. If a weak acid is diluted more - what happens to its % dissociation value?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Increases.
P2O5
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

33. 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?
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
by electrolysis
brown volatile liquid
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

34. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Most are soluble except Ag - Pb
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

35. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Glacial acetic acid

36. What process do you use to obtain a solvent from a solution?
Distillation
Concentration
They stay the same.
Filtration

37. Alkanes are _________ and react by _________
brown volatile liquid
Saturated - Substitution (which requires more radical conditions)
RCOR
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?)

38. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Exothermic (?H for ANY sa/sb = -57kJ/mol)
are less dense than water
by electrolysis

39. Give an example of a concentrated weak acid.
Glacial acetic acid
?G= -ve - E°= +ve
CnH2n-2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

40. permanganate
CN?
MnO4?
?G= -ve - E°= +ve
allow for the vapor pressure of water and make sure to level levels

41. Generally - which oxy acid is strongest?
Salt + water
it is lower and occurs over less sharp a range
The one with most oxygen atoms (highest oxidation number)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

42. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
voltaic: - electrolytic: +
Mono; di; tri; tetra; penta; hexa.
Cu3(PO4)2

43. What shape is water?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Increases.
Suniverse increases for spontaneous processes
bent

44. What is a coordinate covalent bond?
Exothermic
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Both electrons come from the same atom (just as good as a regular bond)
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?)

45. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
They stay the same.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Synthesis - separation and purification of the product and its identification.
O2 needs 4F/mol H2 needs 2F/mol

46. What is the charge on a chlorine atom?
Pale yellow
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
zero
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

47. lead compounds
Greenish-yellow gas
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Experimental mass/theoretical mass X 100
Insoluble except nitrate and acetate

48. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
it reacts by substitution NOT addition
RCOOR
redox reaction
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

49. How does the melting point of a mixture compare to the MP of a pure substance?

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50. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Silvery gray solid - brown - purple
Synthetic condensation polymer (aka a polyamide)
redox reaction