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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. How do you get Ecell for spontaneous reactions?
same KE - but PEice<PEwater
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CO (poisonous)
White precipitate

2. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Insoluble except group 1 and ammonium
Pipette (burette if need repetition)
H3PO4
Mn²? - Cr³? - Cr³

3. acetate
Ksp = s²
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
HClO4
CH3COO?

4. cyanide
S crystal at 0K=0
CnH2n+2
Combine the equations for the half reactions in the non-spontaneous direction
CN?

5. What are the formulas for q?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
q=mc?T q=mL (or n x ?h)
Disulfur dichloride
CnH2n

6. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
A) any range. b) 8-10 c) 4-6
Salt + water.
same KE - but PEice<PEwater

7. What process do you use to obtain the solute from a solution?
brown volatile liquid
Heptane
Evaporation
[A?]/[HA] x 100 or [BH?]/[B] x 100

8. What type of compounds do Group 14 form?
proton donor base
Acid rain - dissolves marble buildings/statues and kills trees.
Separating funnel
+4-covalent - +2-ionic

9. Alcohols and _______ are FG isomers
allow for the vapor pressure of water and make sure to level levels
left - ppt will form
Initiation energy (NOT Ea)
ethers

10. What is the general formula for an acid?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Iodine and CO2 (dry ice)
|experimental - accepted|/accepted X 100
RCOOH

11. What is the formula for summation?

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12. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ROH
non-metal oxides and hydrides are covalently bonded and are acidic.
CO (poisonous)

13. Is a graduated cylinder or beaker more accurate?
|experimental - accepted|/accepted X 100
Mono; di; tri; tetra; penta; hexa.
Salts (ex: CaO + SO2 ? CaSO3)
Graduated cylinder

14. Which value of R do you use for all energy and kinetics calculations?
it reacts by substitution NOT addition
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
R=8.31 J/mol/K
Salt + water.

15. The definition of acidic basic and neutral aqueous solutions is:
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
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
The Faraday or Faraday's constant.
P2O5

16. What do you use to look at burning magnesium? why?
Insoluble except nitrate and acetate
T increases exponentially the proportion of molecules with E > Ea
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
blue glass - it filters UV

17. Why are noble gases stable?
Mono; di; tri; tetra; penta; hexa.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Hg²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

18. permanganate
CrO4²?
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
zero-th: decreases - first: constant - second: increases
MnO4?

19. How do you clean a buret/pipette for a titration?
CO2 and H2O
do not change
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
q=mc?T q=mL (or n x ?h)

20. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
0.10M HCl (more ions)
Acids; HCOOCH3 is an ester
P2O5

21. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
blue glass - it filters UV
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?)
They stay the same.
Increases down group 1 decreases down group 17

22. What is a coordinate covalent bond?
Exothermic
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Both electrons come from the same atom (just as good as a regular bond)
Hg²?

23. What is accuracy?
Soluble
small size and high charge
How close results are to the accepted value
Only temperature

24. What is the word equation for addition polymerisation?
Ksp = 4s³
Pipette (burette if need repetition)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
#ligands=charge x2

25. perchlorate
ClO4?
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
Read the bottom of the meniscus
Exothermic

26. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
ClO?
?G= -ve - E°= +ve
CO (poisonous)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

27. What things should you remember to do when collecting gas over water?
ethers
allow for the vapor pressure of water and make sure to level levels
Ions go through the salt bridge - electrons go through metal wires in the external circuit
No - it depends on the number of ions produced on dissolving.

28. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
CnH2n+1 often designated 'R' ex C3H7 is propyl
CH3COO?
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

29. potassium permanganate
Purple
Acid rain - dissolves marble buildings/statues and kills trees.
CnH2n+1 often designated 'R' ex C3H7 is propyl
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

30. When a cell is 'flat' What is its voltage?
an oxidized and reduced substance
RNH2
by electrolysis
zero

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

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32. Neutralization is an ________ reaction.
10?8
Exothermic (?H for ANY sa/sb = -57kJ/mol)
C2O4²?
Soluble

33. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Clear
Sigma bonds are stronger than pi bonds
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
A salt solution.

34. What word is a clue for a redox reaction?
zero-th: decreases - first: constant - second: increases
A) any range. b) 8-10 c) 4-6
#ligands=charge x2
Acidified

35. If a free element is involved - what type of reaction must be involved?
redox reaction
Big K=kf/kr
Insoluble (except group 1 ammonium and Ba)
OH?

36. An amphiprotic (amphoteric) species is...
basic
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Evaporation
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

37. What type of polymer is nylon?
do not change
Iodine and CO2 (dry ice)
Synthetic condensation polymer (aka a polyamide)
?G= -ve - E°= +ve

38. What steps do organic labs consist of?
Mono; di; tri; tetra; penta; hexa.
Insoluble except nitrate and acetate
Synthesis - separation and purification of the product and its identification.
Ksp = s²

39. Is the standard entropy (S°) of an element zero?
NH2?
Anode - oxygen. Cathode - hydrogen
benzene is less reactive than alkenes
But S° of element is not zero (except at 0K)

40. Generally - which oxy acid is strongest?
zero
Both electrons come from the same atom (just as good as a regular bond)
The one with most oxygen atoms (highest oxidation number)
T increases exponentially the proportion of molecules with E > Ea

41. What do group I/II metal oxides and acids form?
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)
Salt and water
They stay the same.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

42. lead compounds
Insoluble except nitrate and acetate
Soluble
They stay the same.
neutralization: high K - H2O product dissociation: low K - H2O reactant

43. If a weak acid is diluted more - what happens to its % dissociation value?
Big K=kf/kr
Soluble
Hg²?
Increases.

44. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Pale purple - (orange)-yellow - red - blue - green.
K1 x K2
Most are soluble except Ag - Pb
CN?

45. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Pour liquids using a funnel or down a glass rod
CnH2n-2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

46. What shape is water?
E=q + w (negative is by system - positive is on system)
same KE - but PEice<PEwater
bent
fractional distillation

47. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
ns² electrons (first in-first out)
proton donor base
Add acid to water so that the acid doesn't boil and spit
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

48. hydroxides
Insoluble (except group 1 ammonium and Ba)
+4-covalent - +2-ionic
S2O3²?
Anode

49. How are metal oxides and hydrides bonded? are they acidic or basic?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
metal oxides and hydrides are ionically bonded and basic
Initiation energy (NOT Ea)
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?)

50. dihydrogen phosphate
They stay the same.
H2PO4?
fruit - fish - bases
Initiation energy (NOT Ea)