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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Pipette (burette if need repetition)
Molecules with the same molecular formulas - but different structural formulas
CO (poisonous)
basic

2. What are the signs of ?G and E° for spontaneous reactions?
linear
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)
CnH(2n+2)
?G=negative - E° must be positive

3. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
E=q + w (negative is by system - positive is on system)
Concentration
hydroxides (ex: Ba(OH)2)

4. What element is used to vulcanize rubber?
proton donor base
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Sulfur
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

5. A Bronsted-Lowry acid is...
hydroxides (ex: Ba(OH)2)
atoms
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
proton donor base

6. Why are i factors (Van't Hoff factors) often less than ideal?
do not change
neutralization: high K - H2O product dissociation: low K - H2O reactant
Kc=Kp
ion pairing

7. nitrate
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.
The one with most oxygen atoms (highest oxidation number)
Iodine and CO2 (dry ice)
NO3?

8. What is the formula for alkanes?
Molecules with the same molecular formulas - but different structural formulas
zero
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+2

9. What process do you use to obtain the solute from a solution?
Evaporation
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Salt and water

10. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
zero
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
proton donor base

11. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
[A?]/[HA] x 100 or [BH?]/[B] x 100
No - it depends on the number of ions produced on dissolving.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
More chaotic (ex: gases made)

12. How do you get the equation for a net electrolysis reaction?
ionic and form hydrogen and hydroxide
Combine the equations for the half reactions in the non-spontaneous direction
Salts (ex: CaO + SO2 ? CaSO3)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

13. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
diamond and graphite
Salt + water.
Time?¹ - (ex. s?¹ - hr?¹ - etc)

14. dihydrogen phosphate
K1 x K2
H2PO4?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
0 and 14

15. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
They decrease (or could be the same if the solid has ONLY JUST disappeared)
[A?]/[HA] x 100 or [BH?]/[B] x 100
RCHO (carbonyl at end)

16. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Tetrahedral
Filtration
Evaporation

17. Is the ?H formation of an element in standard state zero?
Pour liquids using a funnel or down a glass rod
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
?H formation of an element in standard state=0
q=mc?T q=mL (or n x ?h)

18. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
ClO2?
The one with most oxygen atoms (highest oxidation number)
Current - time and charge on ion (moles of e used in half cell reaction)

19. What is a dipeptide? polypeptide? protein?
ROR
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
Products - reactants (except for BDE when it's reactants - products)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

20. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Mn²? - Cr³? - Cr³
CO2 and H2O
10?8

21. What is the general formula of an alkane?
Greenish-yellow gas
Trigonal pyramidal
CnH(2n+2)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

22. carbonates
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
brown volatile liquid
10?8
Insoluble except group 1 and ammonium

23. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
Pipette (burette if need repetition)
catalyst=conc H2SO4
Unsaturated - addition (ex: decolorize bromine solution)

24. thiosulfate
At half equivalence - pH=pKa
Q=It (time in seconds)
S2O3²?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

25. ammonium/ammonium compounds
Separating funnel
Soluble
Orange
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

26. Does reactivity increase/decrease going down group 1 and group 17?
RCOOR
NO3?
Hg2²?
Increases down group 1 decreases down group 17

27. Which of the rates changes more when temperature is increased?
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.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
chemically (ex: with carbon)
ROH

28. How are primary alcohols turned into acids?
Cu3(PO4)2
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
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
it is lower and occurs over less sharp a range

29. What is the formula of butane?
voltaic: + electrolytic: -
it reacts by substitution NOT addition
q=mc?T q=mL (or n x ?h)
C4H10

30. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
Mn²? - Cr³? - Cr³
Insoluble
Glowing splint (positive result=relights)

31. How are strong ones written?
Purple
strong acids/bases are written as H+ or OH- ions
allow for the vapor pressure of water and make sure to level levels
Acid rain - dissolves marble buildings/statues and kills trees.

32. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Anode - oxygen. Cathode - hydrogen
An active metal.
yellow

33. What are two allotropes of carbon?
voltaic: + electrolytic: -
diamond and graphite
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
atoms

34. What do you need to make a polymer?
bright yellow
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
The one with most oxygen atoms (highest oxidation number)
ion pairing

35. What type of compounds do metals/non metals form?
chemically (ex: with carbon)
Ionic compounds
diamond and graphite
it reacts by substitution NOT addition

36. carbonate
Distillation
Ionic compounds
Anode - oxygen. Cathode - hydrogen
CO3²?

37. What is the general formula for an alcohol?
same KE - but PEice<PEwater
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
neutralization: high K - H2O product dissociation: low K - H2O reactant
ROH

38. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Iodine and CO2 (dry ice)
H3PO4

39. What type of compounds do Group 14 form?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ROH
Anode
+4-covalent - +2-ionic

40. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
Group I metals (soft metals) are stored under oil
H2PO4?
CrO4²?

41. Why are i factors (Van't Hoff factors) often less than ideal?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ion pairing
proton acceptor.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

42. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
Only temperature
fractional distillation
R=8.31 J/mol/K

43. What shape is ammonia?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
small size and high charge
Acid rain - dissolves marble buildings/statues and kills trees.
Trigonal pyramidal

44. ________ are Lewis bases - because they can donate a lone pair of electrons.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
OH- and NH3
zero

45. What type of metals don't react with water or acids to form H2?

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46. How do you get Ecell for spontaneous reactions?
Salt + water
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
allow for the vapor pressure of water and make sure to level levels
benzene has a delocalized pi ring structure

47. When driving off water from a hydrate - how do you tell you're done?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

48. What do metal oxides plus acids form?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Combine the equations for the half reactions in the non-spontaneous direction
Salt + water
blue glass - it filters UV

49. How do you compute % dissociation?
hydroxides (ex: Ba(OH)2)
CrO4²?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
[A?]/[HA] x 100 or [BH?]/[B] x 100

50. What is the catalyst for this reaction Ester + ?
ethers
non-metal oxides and hydrides are covalently bonded and are acidic.
catalyst=conc H2SO4
Salt and water

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AP Chemistry 2

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