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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. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
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
Transition element compounds (except if it has a full or empty d shell)
Salt + water.

2. What do you use for an acid spill? base spill?
The compound with the lowest Ksp value.
Anode - oxygen. Cathode - hydrogen
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
[A?]/[HA] x 100 or [BH?]/[B] x 100

3. Esters smell like _______ and amines smell like _______ and are ______.
PO4³?
redox reaction
fruit - fish - bases
0.10M HCl (more ions)

4. What measuring device would you use for very small volumes of liquids?
Insoluble (except group 1 ammonium and Ba)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
?H-kJ - ?S-J - ?G-kJ
Pipette (burette if need repetition)

5. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
ionic and form hydrogen and hydroxide
Ionic compounds
linear

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

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7. What is the formula for summation?

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8. How does group 1 metals' density compare to water's?
But S° of element is not zero (except at 0K)
CO2 and H2O
are less dense than water
by electrolysis

9. What is the energy you must put into a reaction to make it start called?
CrO4²?
Initiation energy (NOT Ea)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
by electrolysis

10. Name 2 ways in which you can create a buffer?
OH- and NH3
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)
Suniverse increases for spontaneous processes
Increases down group 1 decreases down group 17

11. What shape is methane?
Perform ICE BOX calculation based on K1
Check for air bubbles in the buret and remove the buret funnel from the buret
ROH
Tetrahedral

12. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
RCOOH
linear
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
lighted splint (positive result=pop)

13. What is the formula of copper (II) phosphate?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
But S° of element is not zero (except at 0K)
Ksp = 108s5
Cu3(PO4)2

14. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
H2O + CO2 (it decomposes readily)
Glowing splint (positive result=relights)
brown volatile liquid

15. What process do you use to obtain the solute from a solution?
blue (BTB)
Iodine and CO2 (dry ice)
Evaporation
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

16. How does half life change for zero-th order - first order - and second order processes?
Q=It (time in seconds)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
An active metal.
zero-th: decreases - first: constant - second: increases

17. 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?
an oxidized and reduced substance
The compound with the lowest Ksp value.
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)
Clear

18. What are amphoteric oxides?
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?)
basic
Most INsoluble except group 1 and ammonium
look for changes in oxidation # - the one that goes up is oxidized and is the RA

19. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
T increases exponentially the proportion of molecules with E > Ea

20. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
different forms of the same element
proton donor base
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

21. What do group I/II metal oxides plus water form?
bases
Ksp = 4s³
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Q=It (time in seconds)

22. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Unsaturated - addition (ex: decolorize bromine solution)
H3PO4
C4H10

23. A geometric (or cis-trans) isomer exists due to.....
metal oxides and hydrides are ionically bonded and basic
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Soluble
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?)

24. Why are i factors (Van't Hoff factors) often less than ideal?
H3PO4
?H-kJ - ?S-J - ?G-kJ
Anode - oxygen. Cathode - hydrogen
ion pairing

25. How are non-metal oxides and hydrides bonded? are they acidic or basic?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
non-metal oxides and hydrides are covalently bonded and are acidic.
Current - time and charge on ion (moles of e used in half cell reaction)
no - they're written undissociated (HAaq)

26. silver compounds
Soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Insoluble except for nitrate and acetate

27. Esterification is...
acid + alcohol
Insoluble
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Cr2O7²?

28. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
But S° of element is not zero (except at 0K)
an oxidized and reduced substance

29. Color (absorbance) is proportional to ________
Concentration
do not change
Selective absorption
zero

30. What things should you remember to do when collecting gas over water?
benzene has a delocalized pi ring structure
allow for the vapor pressure of water and make sure to level levels
bent
No - it depends on the number of ions produced on dissolving.

31. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
K1 x K2
chemically (ex: with carbon)
No - it depends on the number of ions produced on dissolving.
it's lower and occurs over less sharp a range

32. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
bent
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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.

33. What shape is water?
Perform ICE BOX calculation based on K1
Most INsoluble except group 1 and ammonium
ClO3?
bent

34. cyanide
Identity and purity (impure compounds usually have broad & low melting points)
NH4?
CN?
NH2?

35. What part of a liquid do you look at to measure its volume?
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.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Read the bottom of the meniscus
CO3²?

36. What is HCOOCH3?
Insoluble except for nitrate and acetate
K1 x K2
Acids; HCOOCH3 is an ester
blue

37. What is the second law of thermodynamics?
ClO?
Synthesis - separation and purification of the product and its identification.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Suniverse increases for spontaneous processes

38. Alcohols and _______ are FG isomers
basic
ethers
Hg2²?
0.10M HCl (more ions)

39. What do you use to look at burning magnesium? why?
blue glass - it filters UV
ion pairing
CnH2n+1 often designated 'R' ex C3H7 is propyl
boiling without losing volatile solvents/reactants

40. What is the conjugate base of NH3?
NH2?
CnH(2n+2)
do not change
Exothermic

41. What type of solutions do small - highly charged cations tend to form?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
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
Kc=Kp

42. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
?H-kJ - ?S-J - ?G-kJ
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Soluble

43. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
water and substances with (s) less dense than
ROR

44. Alkenes are ________ and react by __________
RCOR
Ksp = 108s5
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Unsaturated - addition (ex: decolorize bromine solution)

45. bromothymol
blue (BTB)
Exothermic
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Only temperature

46. hypochlorite
ClO?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
voltaic: - electrolytic: +
same KE - but PEice<PEwater

47. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
ROH
NH4?
allow for the vapor pressure of water and make sure to level levels
H+

48. What is the third law of thermodynamics?
How close results are to the accepted value
Increases down group 1 decreases down group 17
HClO4
S crystal at 0K=0

49. What is an Alkyl group?

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50. The definition of acidic basic and neutral aqueous solutions is:
C2O4²?
RX
Big K=kf/kr
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]