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

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2. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Heat a test tube at an angle at the side of the tube (not bottom)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Synthesis - separation and purification of the product and its identification.

3. What do you use for an acid spill? base spill?
zero
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Big K=kf/kr
q=mc?T q=mL (or n x ?h)

4. Alkenes are ________ and react by __________
OH?
ROH
Unsaturated - addition (ex: decolorize bromine solution)
CnH2n-2

5. What is the test for oxygen?
Anode - oxygen. Cathode - hydrogen
Glowing splint (positive result=relights)
metal oxides and hydrides are ionically bonded and basic
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

6. What is the formula for alkenes?
CnH2n
Increases.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
benzene has a delocalized pi ring structure

7. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
+4-covalent - +2-ionic
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

8. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
Graduated cylinder
acids
linear

9. What is the general formula of an alkane?
Increases.
left - ppt will form
Synthesis - separation and purification of the product and its identification.
CnH(2n+2)

10. Both Acetic acid and ____________ are also functional isomers.
Sigma bonds are stronger than pi bonds
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
It ceases - the circuit is broken.
methyl formate

11. For a dibasic acid (H2A) - [A²?]= ____ ?
CnH2n+1 often designated 'R' ex C3H7 is propyl
K2
same KE - but PEice<PEwater
brown volatile liquid

12. bromothymol
Acid rain - dissolves marble buildings/statues and kills trees.
?G=negative - E° must be positive
Saturated - Substitution (which requires more radical conditions)
blue (BTB)

13. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
bent
Transition element compounds (except if it has a full or empty d shell)

14. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Suniverse increases for spontaneous processes
Molecules with the same molecular formulas - but different structural formulas
red - green - blue
neutralization: high K - H2O product dissociation: low K - H2O reactant

15. What shape is ammonia?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Trigonal pyramidal
CnH2n

16. mercury (I) ion
Hg2²?
blue glass - it filters UV
SO4²?
?H-kJ - ?S-J - ?G-kJ

17. What is the first law of thermodynamics?
C4H10
E=q + w (negative is by system - positive is on system)
linear
ROH

18. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
water and substances with (s) less dense than
Initiation energy (NOT Ea)
ROH

19. What complex ion does ammonia form with silver? copper? cadmium? zinc?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Clear
Pale purple - (orange)-yellow - red - blue - green.

20. Metal hydrides are _____ and form _______ and _______ when added to water
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ionic and form hydrogen and hydroxide
water and substances with (s) less dense than
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

21. If Q > Ksp - then system shifts _______ and ppt ______
it's lower and occurs over less sharp a range
left - ppt will form
Synthetic condensation polymer (aka a polyamide)
?H-kJ - ?S-J - ?G-kJ

22. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
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
CnH2n+1 often designated 'R' ex C3H7 is propyl
Identity and purity (impure compounds usually have broad & low melting points)

23. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
-Ea/R
Purple
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

24. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
ns² electrons (first in-first out)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Making sigma bonds and holding lone pairs

25. hydroxide
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Exothermic
OH?

26. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Trigonal pyramidal
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
CO (poisonous)
More chaotic (ex: gases made)

27. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
allow for the vapor pressure of water and make sure to level levels
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
NO3?
Ksp = 108s5

28. What causes the dramatic effect of T on rate?
A) any range. b) 8-10 c) 4-6
T increases exponentially the proportion of molecules with E > Ea
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.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

29. Name 2 ways in which you can create a buffer?
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)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Ions go through the salt bridge - electrons go through metal wires in the external circuit

30. Which would cause the bulb in a conductivity apparatus to be brightest?
More chaotic (ex: gases made)
Synthetic condensation polymer (aka a polyamide)
0.10M HCl (more ions)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

31. When combining half equations - what do you do to E° values when multiplying coefficients?
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
RCOR
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Nothing

32. lead iodide
bright yellow
CH3COO?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
#ligands=charge x2

33. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Purple
Insoluble except group 1 and ammonium
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

34. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
Anode
chemically (ex: with carbon)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

35. Color (absorbance) is proportional to ________
ionic and form hydrogen and hydroxide
non-metal oxides and hydrides are covalently bonded and are acidic.
Concentration
Insoluble except nitrate and acetate

36. Ions are not ______.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
But S° of element is not zero (except at 0K)
atoms
ionic and form hydrogen and hydroxide

37. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
T increases exponentially the proportion of molecules with E > Ea
Evaporation
Exothermic
10?8

38. During a titration what is present in the beaker at the equivalence point?
RCHO (carbonyl at end)
water and substances with (s) less dense than
A salt solution.
0 and 14

39. Why are i factors (Van't Hoff factors) often less than ideal?
RX
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Disulfur dichloride
ion pairing

40. Nonmetals are good _____ agents. Metals are good _______ agents.
Increases down group 1 decreases down group 17
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
0.10M HCl (more ions)
K2

41. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Conjugate pair (one must be a weak base or acid)
Acid rain - dissolves marble buildings/statues and kills trees.
Mono; di; tri; tetra; penta; hexa.
CrO4²?

42. Buffer capacity must contain decent amounts of a ________ ________
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Conjugate pair (one must be a weak base or acid)
All except for lithium
Exothermic

43. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
Pour liquids using a funnel or down a glass rod
The compound with the lowest Ksp value.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Unsaturated - addition (ex: decolorize bromine solution)

44. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Initiation energy (NOT Ea)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Acid rain - dissolves marble buildings/statues and kills trees.
More chaotic (ex: gases made)

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

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46. What do you do to get rid of most of the solution from a precipitate?
atoms
voltaic: - electrolytic: +
Decant
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

47. chromate
CrO4²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
NH2?
White precipitate

48. If a weak acid is diluted more - what happens to its % dissociation value?
neutralization: high K - H2O product dissociation: low K - H2O reactant
CO2 and H2O
Acidified
Increases.

49. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
acid + alcohol
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Greenish-yellow gas

50. iodine - iodine solution - iodine vapor
The benzene ring (or more correctly the phenyl group - C6H5)
Silvery gray solid - brown - purple
CnH2n
Insoluble except nitrate and acetate