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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. An amphiprotic (amphoteric) species is...
Most INsoluble except group 1 and ammonium
acid + alcohol
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

2. phosphates
voltaic: - electrolytic: +
Increases.
Most INsoluble except group 1 and ammonium
ion pairing

3. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
No - it depends on the number of ions produced on dissolving.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

4. lead iodide
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Increases.
bright yellow
O2 needs 4F/mol H2 needs 2F/mol

5. What do hydrocarbons form when they burn in air (oxygen)?
Heat a test tube at an angle at the side of the tube (not bottom)
Salt and water
CO2 and H2O
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

6. chlorate
ROR
ClO3?
C2O4²?
linear

7. Alkanes are _________ and react by _________
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
RNH2
zero-th: decreases - first: constant - second: increases
Saturated - Substitution (which requires more radical conditions)

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

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9. What are isotopes?
ClO?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
H2PO4?
ClO2?

10. What are the products of the reaction between group 1 metals and water?

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11. Esters smell like _______ and amines smell like _______ and are ______.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Greenish-yellow gas
Group 1 hydroxides (ex: NaOH)
fruit - fish - bases

12. 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.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
A) any range. b) 8-10 c) 4-6
red - green - blue
Heat a test tube at an angle at the side of the tube (not bottom)

13. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Nothing
a-IMFs - b-molecular volume
Big K=kf/kr
proton acceptor.

14. carbonate
Anode - oxygen. Cathode - hydrogen
q=mc?T q=mL (or n x ?h)
zero
CO3²?

15. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ClO?
Saturated - Substitution (which requires more radical conditions)
+4-covalent - +2-ionic

16. What are the formulas for q?
MnO4?
a-IMFs - b-molecular volume
q=mc?T q=mL (or n x ?h)
All except for lithium

17. The definition of acidic basic and neutral aqueous solutions is:
same KE - but PEice<PEwater
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Soluble

18. What shape is ammonia?
ClO?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Both electrons come from the same atom (just as good as a regular bond)
Trigonal pyramidal

19. Give an example of a concentrated weak acid.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Glacial acetic acid
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
it is lower and occurs over less sharp a range

20. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Trigonal pyramidal
it's lower and occurs over less sharp a range
CnH(2n+2)
Ksp = s²

21. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Suniverse increases for spontaneous processes
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
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

22. Name 2 ways in which you can create a buffer?
Mono; di; tri; tetra; penta; hexa.
Initiation energy (NOT Ea)
CnH(2n+2)
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)

23. One mole of electrons carries 96500Coulombs - what is this quantity called?

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24. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ksp = 4s³
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

25. What do group I/II metal oxides and acids form?
C2O4²?
Salt and water
Experimental mass/theoretical mass X 100
?G= -ve - E°= +ve

26. chlorine
Greenish-yellow gas
do not change
Purple
Both electrons come from the same atom (just as good as a regular bond)

27. Which alkali metals float on water?
All except for lithium
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
H3PO4
Anode

28. What effect does increasing the size/surface area of a voltaic cell have on the cell?
blue glass - it filters UV
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
NO3?
+4-covalent - +2-ionic

29. What two compounds are great oxidizing agents?

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30. What is the formula for percent error?
Check for air bubbles in the buret and remove the buret funnel from the buret
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
|experimental - accepted|/accepted X 100
red - green - blue

31. What does the solubility of organic compounds depend on?
Ionic compounds
They stay the same.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
-Ea/R

32. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
bent
Ksp = 27s4
q=mc?T q=mL (or n x ?h)
S2O3²?

33. What is the pH of 1.0M HCl? 1M NaOH?
CnH2n+2
?H-kJ - ?S-J - ?G-kJ
non-metal oxides and hydrides are covalently bonded and are acidic.
0 and 14

34. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
look for changes in oxidation # - the one that goes up is oxidized and is the RA
H3PO4
The dilution effect when the solutions mix. M1V1 = M2V2

35. How does group 1 metals' density compare to water's?
Increases.
Acid rain - dissolves marble buildings/statues and kills trees.
are less dense than water
Nothing

36. Color is due to ______ _______ of light.
Tetrahedral
Selective absorption
Saturated - Substitution (which requires more radical conditions)
Filtration

37. What is H2CO3 (carbonate acid) usually written as?
#ligands=charge x2
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
H2O + CO2 (it decomposes readily)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

38. What is HCOOCH3?
chemically (ex: with carbon)
a-IMFs - b-molecular volume
Acids; HCOOCH3 is an ester
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

39. What does saturated mean? Unsaturated?
0 and 14
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Salt + water.
0.10M HCl (more ions)

40. How do you explain trends in atomic properties using Coulomb's Law?
lighted splint (positive result=pop)
No - it depends on the number of ions produced on dissolving.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
look for changes in oxidation # - the one that goes up is oxidized and is the RA

41. barium sulfate
White precipitate
voltaic: - electrolytic: +
Perform ICE BOX calculation based on K1
Both electrons come from the same atom (just as good as a regular bond)

42. How are metal oxides and hydrides bonded? are they acidic or basic?
linear
metal oxides and hydrides are ionically bonded and basic
same KE - but PEice<PEwater
it's lower and occurs over less sharp a range

43. dichromate
Cr2O7²?
Soluble except Ag - Pb - Ca - Sr Ba)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Combine the equations for the half reactions in the non-spontaneous direction

44. sulfates
it reacts by substitution NOT addition
allow for the vapor pressure of water and make sure to level levels
CnH2n+2
Soluble except Ag - Pb - Ca - Sr Ba)

45. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Ppt will NOT form (unsaturated)
diamond and graphite
by electrolysis

46. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
?H-kJ - ?S-J - ?G-kJ
P2O5
Insoluble except for nitrate and acetate
PO4³?

47. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
by electrolysis
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
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
do not change

48. What process do you use to obtain the precipitate from a solution?
Filtration
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
K1 x K2

49. nitrates
MnO4?
Iodine and CO2 (dry ice)
are less dense than water
Soluble

50. How many ligands attach to a central ion in a complex ion?
Orange
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
#ligands=charge x2
H2PO4?