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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. permanganate
blue glass - it filters UV
MnO4?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
different forms of the same element

2. If a weak acid is diluted more - what happens to its % dissociation value?
proton acceptor.
Increases down group 1 decreases down group 17
Increases.
Reduction always takes place at the cathode (RED CAT) In both types of cell!

3. How are strong ones written?
Salt + water
red - green - blue
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
strong acids/bases are written as H+ or OH- ions

4. If a free element is involved - what type of reaction must be involved?
redox reaction
blue glass - it filters UV
K2
Hg²?

5. Is a graduated cylinder or beaker more accurate?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
CnH2n+1 often designated 'R' ex C3H7 is propyl
CnH2n+2
Graduated cylinder

6. perchlorate
ClO4?
fruit - fish - bases
Unsaturated - addition (ex: decolorize bromine solution)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

7. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
S2O3²?
Current - time and charge on ion (moles of e used in half cell reaction)
Insoluble (except group 1 ammonium and Ba)

8. phosphate
different forms of the same element
The Faraday or Faraday's constant.
PO4³?
Ksp = s²

9. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
They stay the same.
redox reaction
allow for the vapor pressure of water and make sure to level levels

10. What is the basic structure of an optical isomer?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
bases
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

11. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
chemically (ex: with carbon)
The compound with the lowest Ksp value.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
H+

12. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
water and substances with (s) less dense than
methyl formate
voltaic: + electrolytic: -

13. Where are group I metals stored?
Add acid to water so that the acid doesn't boil and spit
T increases exponentially the proportion of molecules with E > Ea
Hg2²?
Group I metals (soft metals) are stored under oil

14. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Insoluble except group 1 and ammonium
0 and 14

15. potassium permanganate
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ns² electrons (first in-first out)
Purple

16. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
water and substances with (s) less dense than
zero
Heptane

17. What is the difference between equivalence point and end point of a titration.
Insoluble (except group 1 ammonium and Ba)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Heat a test tube at an angle at the side of the tube (not bottom)
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the

18. 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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19. phosphates
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Most INsoluble except group 1 and ammonium
Most are soluble except Ag - Pb
0 and 14

20. What is the word equation for addition polymerisation?
Glacial acetic acid
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
benzene is less reactive than alkenes
CN?

21. cyanide
CnH2n+1 often designated 'R' ex C3H7 is propyl
Heat a test tube at an angle at the side of the tube (not bottom)
CN?
Ksp = 108s5

22. What two compounds are great oxidizing agents?

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23. chlorine
RCHO (carbonyl at end)
Iodine and CO2 (dry ice)
Greenish-yellow gas
0 and 14

24. What do metal oxides plus non- metal oxides form?
-Ea/R
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Suniverse increases for spontaneous processes
Salts (ex: CaO + SO2 ? CaSO3)

25. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
yellow
CO (poisonous)
Glacial acetic acid
RCOOH

26. BaSO4
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
ClO4?
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.
Insoluble

27. chlorate
fractional distillation
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
ClO3?

28. lead iodide
bright yellow
Pour liquids using a funnel or down a glass rod
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Synthetic condensation polymer (aka a polyamide)

29. What shape is water?
S2O3²?
Synthetic condensation polymer (aka a polyamide)
OH- and NH3
bent

30. What are the units of the first order rate constant?
Soluble
Both electrons come from the same atom (just as good as a regular bond)
Ksp = 4s³
Time?¹ - (ex. s?¹ - hr?¹ - etc)

31. What do you use to look at burning magnesium? why?
water and substances with (s) less dense than
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.
CnH2n
blue glass - it filters UV

32. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
Ksp = 27s4
acid + alcohol
methyl formate

33. acetate
E=q + w (negative is by system - positive is on system)
CH3COO?
benzene is less reactive than alkenes
Selective absorption

34. How do you dilute an acid?

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35. chlorite
ClO2?
CnH2n+2
it reacts by substitution NOT addition
voltaic: + electrolytic: -

36. How do you get the equation for a net electrolysis reaction?
Trigonal pyramidal
A) any range. b) 8-10 c) 4-6
Combine the equations for the half reactions in the non-spontaneous direction
RNH2

37. What is the sign of the cathode in voltaic cells? in electrolytic cells?
hydroxides (ex: Ba(OH)2)
zero
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
voltaic: + electrolytic: -

38. What is the conjugate base of NH3?
NO3?
NH2?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Group I metals (soft metals) are stored under oil

39. What measuring device would you use for very small volumes of liquids?
Saturated - Substitution (which requires more radical conditions)
Pipette (burette if need repetition)
linear
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

40. Name some properties of Group 17
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Identity and purity (impure compounds usually have broad & low melting points)
Nothing

41. What does saturated mean? Unsaturated?
brown volatile liquid
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Sulfur
Mn²? - Cr³? - Cr³

42. What is the general formula for a ketone?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
RCOR
Pale yellow

43. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
ion pairing
Sigma bonds are stronger than pi bonds
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

44. What does a short - sharp melting point indicate?
CnH2n-2
bent
C2O4²?
Identity and purity (impure compounds usually have broad & low melting points)

45. Ions are not ______.
Heat a test tube at an angle at the side of the tube (not bottom)
Salt + water
atoms
RX

46. What are the prefixes for the naming of binary molecular compound formulas (up to six)
?G= -ve - E°= +ve
CH3COO?
Mono; di; tri; tetra; penta; hexa.
metal oxides and hydrides are ionically bonded and basic

47. Give an example of a dilute strong acid.
HClO4
hydroxides (ex: Ba(OH)2)
A salt solution.
Selective absorption

48. primary colors
Insoluble
RCHO (carbonyl at end)
red - green - blue
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

49. Acidic gases like SO2 in the atmosphere cause what environmental problems?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Acid rain - dissolves marble buildings/statues and kills trees.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

50. bromine
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Insoluble except group 1 and ammonium
Current - time and charge on ion (moles of e used in half cell reaction)
brown volatile liquid