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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. For a dibasic acid (H2A) - [A²?]= ____ ?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Greenish-yellow gas
Glacial acetic acid
K2

2. If Q < Ksp a ppt ______
bent
Ppt will NOT form (unsaturated)
methyl formate
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

3. What do metal oxides plus acids form?
Ksp = 108s5
Salt + water
voltaic: - electrolytic: +
Current - time and charge on ion (moles of e used in half cell reaction)

4. 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
Graduated cylinder
Mn²? - Cr³? - Cr³
non-metal oxides and hydrides are covalently bonded and are acidic.

5. During a titration what is present in the beaker at the equivalence point?
A salt solution.
ethers
look for changes in oxidation # - the one that goes up is oxidized and is the RA
MnO4?

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

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7. What process do you use to obtain the solute from a solution?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Current - time and charge on ion (moles of e used in half cell reaction)
Evaporation
basic

8. What do nonmetal oxides plus water form?
acids
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Time?¹ - (ex. s?¹ - hr?¹ - etc)

9. mercury (I) ion
Hg2²?
ns² electrons (first in-first out)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

10. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
They stay the same.
Mn²? - Cr³? - Cr³
Ppt will NOT form (unsaturated)

11. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
?G=negative - E° must be positive
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
q=mc?T q=mL (or n x ?h)

12. How are non-metal oxides and hydrides bonded? are they acidic or basic?
lighted splint (positive result=pop)
non-metal oxides and hydrides are covalently bonded and are acidic.
Eudiometer
Big K=kf/kr

13. Does reactivity increase/decrease going down group 1 and group 17?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Exothermic
Ppt will NOT form (unsaturated)
Increases down group 1 decreases down group 17

14. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Big K=kf/kr
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
a-IMFs - b-molecular volume
Molecules with the same molecular formulas - but different structural formulas

15. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
benzene has a delocalized pi ring structure
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
same KE - but PEice<PEwater
Time?¹ - (ex. s?¹ - hr?¹ - etc)

16. What is the test for oxygen?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
no - they're written undissociated (HAaq)
Glowing splint (positive result=relights)
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)

17. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
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
Silvery gray solid - brown - purple
Ionic compounds

18. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
acid + alcohol
O2 needs 4F/mol H2 needs 2F/mol
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

19. What are the prefixes for the naming of binary molecular compound formulas (up to six)
|experimental - accepted|/accepted X 100
How close results are to the accepted value
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
Mono; di; tri; tetra; penta; hexa.

20. What are the common strong bases?
But S° of element is not zero (except at 0K)
strong acids/bases are written as H+ or OH- ions
Mono; di; tri; tetra; penta; hexa.
Group 1 hydroxides (ex: NaOH)

21. What type of compounds do Group 14 form?
Soluble
+4-covalent - +2-ionic
ClO3?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

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

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23. permanganate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
T increases exponentially the proportion of molecules with E > Ea
MnO4?
Soluble

24. A Bronsted-Lowry acid is...
proton donor base
The dilution effect when the solutions mix. M1V1 = M2V2
NH2?
RCOOR

25. Give an example of a concentrated weak acid.
Glacial acetic acid
Trigonal pyramidal
?H-kJ - ?S-J - ?G-kJ
methyl formate

26. What are two allotropes of carbon?
yellow
diamond and graphite
boiling without losing volatile solvents/reactants
Exothermic

27. Lattice energy is high for ions with _____ size and _____ charge
The dilution effect when the solutions mix. M1V1 = M2V2
Mn²? - Cr³? - Cr³
small size and high charge
fractional distillation

28. What is the pH of 1.0M HCl? 1M NaOH?
0.10M HCl (more ions)
a-IMFs - b-molecular volume
Concentration
0 and 14

29. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Purple
ethers
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Salts (ex: CaO + SO2 ? CaSO3)

30. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Anode - oxygen. Cathode - hydrogen
Combine the equations for the half reactions in the non-spontaneous direction
MnO4?

31. What things should you remember to do when collecting gas over water?
Add acid to water so that the acid doesn't boil and spit
allow for the vapor pressure of water and make sure to level levels
How close results are to the accepted value
RCOR

32. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
CH3COO?
non-metal oxides and hydrides are covalently bonded and are acidic.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

33. dichromate
A salt solution.
non-metal oxides and hydrides are covalently bonded and are acidic.
?G=negative - E° must be positive
Cr2O7²?

34. 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?)
Tetrahedral
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Insoluble

35. What is the relationship in strength between sigma and pi bonds?
ROR
Current - time and charge on ion (moles of e used in half cell reaction)
Sigma bonds are stronger than pi bonds
Pipette (burette if need repetition)

36. Color (absorbance) is proportional to ________
CnH2n+2
Unsaturated - addition (ex: decolorize bromine solution)
Concentration
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

37. What do metal oxides plus non- metal oxides form?
Identity and purity (impure compounds usually have broad & low melting points)
T increases exponentially the proportion of molecules with E > Ea
Salts (ex: CaO + SO2 ? CaSO3)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

38. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
redox reaction
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?)
Ksp = 4s³
zero

39. What is the test for hydrogen?
lighted splint (positive result=pop)
Insoluble
acids
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

40. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
hydroxides (ex: Ba(OH)2)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

41. How do you compute % dissociation?
HClO4
[A?]/[HA] x 100 or [BH?]/[B] x 100
?G= -ve - E°= +ve
zero

42. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Identity and purity (impure compounds usually have broad & low melting points)
RCHO (carbonyl at end)
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
NH4?

43. What word is a clue for a redox reaction?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acidified
strong acids/bases are written as H+ or OH- ions
Distillation

44. If a weak acid is diluted more - what happens to its % dissociation value?
atoms
Increases.
Most are soluble except Ag - Pb
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

45. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
SO4²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
it reacts by substitution NOT addition
[A?]/[HA] x 100 or [BH?]/[B] x 100

46. halides
H+
Most are soluble except Ag - Pb
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)
H3PO4

47. What are the names and formulas of the 6 strong acids?
ClO?
|experimental - accepted|/accepted X 100
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
?G= -ve - E°= +ve

48. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
ClO2?
Kc=Kp
CO2 and H2O
ionic and form hydrogen and hydroxide

49. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
K1 x K2
Conjugate pair (one must be a weak base or acid)
NO3?

50. Which of the rates changes more when temperature is increased?
The one with most oxygen atoms (highest oxidation number)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Iodine and CO2 (dry ice)
a-IMFs - b-molecular volume

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AP Chemistry 2

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