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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. nitrate
NO3?
ion pairing
Synthetic condensation polymer (aka a polyamide)
ClO?

2. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Soluble
CO (poisonous)
linear
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)

3. 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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4. permanganate
The Faraday or Faraday's constant.
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?)
MnO4?
Pour liquids using a funnel or down a glass rod

5. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
CnH2n-2
Hg2²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

6. Is a graduated cylinder or beaker more accurate?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
no - they're written undissociated (HAaq)
Graduated cylinder
H2PO4?

7. Which value of R do you use for all energy and kinetics calculations?
ethers
R=8.31 J/mol/K
Tetrahedral
Orange

8. What is the general formula for an ether?
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero
ROR
Insoluble except nitrate and acetate

9. What are isomers?
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?
Iodine and CO2 (dry ice)
Molecules with the same molecular formulas - but different structural formulas

10. How do you dilute an acid?

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11. How are metal oxides and hydrides bonded? are they acidic or basic?
Transition element compounds (except if it has a full or empty d shell)
C4H10
metal oxides and hydrides are ionically bonded and basic
acids

12. Why are i factors (Van't Hoff factors) often less than ideal?
Increases.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ion pairing

13. What is the test for hydrogen?
Pour liquids using a funnel or down a glass rod
strong acids/bases are written as H+ or OH- ions
At half equivalence - pH=pKa
lighted splint (positive result=pop)

14. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CH3COO?
a-IMFs - b-molecular volume
|experimental - accepted|/accepted X 100
Mn²? - Cr³? - Cr³

15. Ca - Sr - Ba
Decant
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
hydroxides (ex: Ba(OH)2)

16. potassium permanganate
NH4?
acid + alcohol
A salt solution.
Purple

17. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K2
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Selective absorption
K1 x K2

18. What part of a liquid do you look at to measure its volume?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Read the bottom of the meniscus
10?8
R=8.31 J/mol/K

19. What shape is ammonia?
Hg²?
Pour liquids using a funnel or down a glass rod
Trigonal pyramidal
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

20. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
allow for the vapor pressure of water and make sure to level levels
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
K2

21. What is the general formula for alkyl halides?
O2 needs 4F/mol H2 needs 2F/mol
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
hydroxides (ex: Ba(OH)2)
RX

22. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
#ligands=charge x2
water and substances with (s) less dense than
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
C4H10

23. Does Benzene react by addition or substitution?
chemically (ex: with carbon)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
it reacts by substitution NOT addition
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

24. What does the solubility of organic compounds depend on?
lighted splint (positive result=pop)
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
H3PO4
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

25. What two types of substances are present in all redox reactions?
At half equivalence - pH=pKa
Salt + water.
Suniverse increases for spontaneous processes
an oxidized and reduced substance

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

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27. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
fruit - fish - bases
The compound with the lowest Ksp value.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

28. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
RCOOR
a-IMFs - b-molecular volume

29. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Hg²?
Increases down group 1 decreases down group 17
Cr2O7²?

30. What do you do to get rid of most of the solution from a precipitate?
S crystal at 0K=0
Insoluble except group 1 and ammonium
bases
Decant

31. What effect does increasing the size/surface area of a voltaic cell have on the cell?
a-IMFs - b-molecular volume
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
K2
Salt and water

32. carbonate
C2O4²?
CO3²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

33. perchlorate
Kc=Kp
ClO4?
Products - reactants (except for BDE when it's reactants - products)
Ksp = 27s4

34. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Soluble
Kc=Kp
bright yellow
ion pairing

35. If Q > Ksp - then system shifts _______ and ppt ______
Pale yellow
left - ppt will form
CO3²?
strong acids/bases are written as H+ or OH- ions

36. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
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.
The dilution effect when the solutions mix. M1V1 = M2V2

37. What is the third law of thermodynamics?
S crystal at 0K=0
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Pour liquids using a funnel or down a glass rod
an oxidized and reduced substance

38. What process do you use to obtain the solute from a solution?
zero
Evaporation
a-IMFs - b-molecular volume
Both electrons come from the same atom (just as good as a regular bond)

39. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
0.10M HCl (more ions)
Ksp = s²
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
Saturated - Substitution (which requires more radical conditions)

40. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
?G=negative - E° must be positive
acids
same KE - but PEice<PEwater

41. What is a dipeptide? polypeptide? protein?
At half equivalence - pH=pKa
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)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
it reacts by substitution NOT addition

42. copper sulfate
atoms
blue
ethers
a-IMFs - b-molecular volume

43. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
T increases exponentially the proportion of molecules with E > Ea
Salt + water
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Anode - oxygen. Cathode - hydrogen

44. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Pale purple - (orange)-yellow - red - blue - green.
Check for air bubbles in the buret and remove the buret funnel from the buret

45. What is the formula for alkynes?
ionic and form hydrogen and hydroxide
CnH2n-2
Unsaturated - addition (ex: decolorize bromine solution)
Saturated - Substitution (which requires more radical conditions)

46. chlorate
Only temperature
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Hg²?
ClO3?

47. If a weak acid is diluted more - what happens to its % dissociation value?
?H-kJ - ?S-J - ?G-kJ
|experimental - accepted|/accepted X 100
Soluble
Increases.

48. What type of compounds do metals/non metals form?
White precipitate
Ionic compounds
Insoluble except nitrate and acetate
Hg²?

49. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
acid + alcohol
Conjugate pair (one must be a weak base or acid)

50. Alcohols and _______ are FG isomers
Selective absorption
ethers
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
White precipitate