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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. chlorate
bent
ClO3?
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
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

2. If Q > Ksp - then system shifts _______ and ppt ______
Clear
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Nothing
left - ppt will form

3. When can supercooling occur? What does it look like on a cooling curve?

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4. When is ?G zero?
Cu3(PO4)2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
At half equivalence - pH=pKa
it is lower and occurs over less sharp a range

5. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
A salt solution.
Heat a test tube at an angle at the side of the tube (not bottom)
same KE - but PEice<PEwater

6. What type of compounds do metals/non metals form?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
blue glass - it filters UV
Ionic compounds

7. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
H2O + CO2 (it decomposes readily)
CnH2n

8. bromothymol
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Group 1 hydroxides (ex: NaOH)
blue (BTB)

9. What are two substances that sublime at 1 atm when heated?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
O2 needs 4F/mol H2 needs 2F/mol
Iodine and CO2 (dry ice)
OH- and NH3

10. Metal hydrides are _____ and form _______ and _______ when added to water
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Glowing splint (positive result=relights)
ionic and form hydrogen and hydroxide
are less dense than water

11. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
non-metal oxides and hydrides are covalently bonded and are acidic.
ion pairing
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

12. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
blue (BTB)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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)

13. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
ClO?
Evaporation
Synthesis - separation and purification of the product and its identification.

14. Name six characteristics of transition elements (or their compounds)
RCOOR
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
yellow
Good catalysts - form multiple oxidation states - often paramagnetic - good structural metals - form a host of alloys (similar sized atoms) - have similar I energies (inner filling)

15. For a dibasic acid (H2A) - [A²?]= ____ ?
linear
Heat a test tube at an angle at the side of the tube (not bottom)
K2
bases

16. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
PO4³?
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
E=q + w (negative is by system - positive is on system)

17. dihydrogen phosphate
Suniverse increases for spontaneous processes
10?8
Initiation energy (NOT Ea)
H2PO4?

18. ammonium
NH4?
Ksp = 4s³
Glowing splint (positive result=relights)
Mono; di; tri; tetra; penta; hexa.

19. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
H2PO4?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Products - reactants (except for BDE when it's reactants - products)

20. What are isomers?
?H formation of an element in standard state=0
Molecules with the same molecular formulas - but different structural formulas
CN?
Mono; di; tri; tetra; penta; hexa.

21. primary colors
Hg²?
red - green - blue
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Molecules with the same molecular formulas - but different structural formulas

22. Give an example of a concentrated weak acid.
Glacial acetic acid
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Insoluble except for nitrate and acetate
Ksp = s²

23. lead compounds
CO (poisonous)
zero
Read the bottom of the meniscus
Insoluble except nitrate and acetate

24. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Soluble
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Add acid to water so that the acid doesn't boil and spit
zero

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

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26. group 1 ions/compounds
CnH2n
Soluble
Pour liquids using a funnel or down a glass rod
RCHO (carbonyl at end)

27. Where are group I metals stored?
Ksp = 108s5
Group I metals (soft metals) are stored under oil
Insoluble except nitrate and acetate
The compound with the lowest Ksp value.

28. What element is used to vulcanize rubber?
Sulfur
Transition element compounds (except if it has a full or empty d shell)
zero-th: decreases - first: constant - second: increases
Group I metals (soft metals) are stored under oil

29. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
R=8.31 J/mol/K
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
More chaotic (ex: gases made)
Group 1 hydroxides (ex: NaOH)

30. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Insoluble except for nitrate and acetate
CnH2n+1 often designated 'R' ex C3H7 is propyl
a-IMFs - b-molecular volume
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

31. What do group I/II metal oxides and acids form?
Identity and purity (impure compounds usually have broad & low melting points)
Salt and water
Mono; di; tri; tetra; penta; hexa.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

32. copper sulfate
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Hg²?
blue
acid + alcohol

33. What is the sign of the anode in voltaic cells? in electrolytic cells?
The benzene ring (or more correctly the phenyl group - C6H5)
voltaic: - electrolytic: +
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
bent

34. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Anode
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Hg²?

35. nitrate
NO3?
Pale yellow
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
basic

36. Ions are not ______.
atoms
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
voltaic: + electrolytic: -

37. What is the formula for alkenes?
Suniverse increases for spontaneous processes
Good catalysts - form multiple oxidation states - often paramagnetic - good structural metals - form a host of alloys (similar sized atoms) - have similar I energies (inner filling)
CnH2n
PO4³?

38. What word is a clue for a redox reaction?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Glowing splint (positive result=relights)
Acidified
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

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

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40. permanganate
But S° of element is not zero (except at 0K)
different forms of the same element
Insoluble except nitrate and acetate
MnO4?

41. What kind of bonding structure does benzene have?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
do not change
benzene has a delocalized pi ring structure
RCOOR

42. What is the test for hydrogen?
lighted splint (positive result=pop)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
OH- and NH3

43. What is the catalyst for this reaction Ester + ?
?G=negative - E° must be positive
Soluble
S crystal at 0K=0
catalyst=conc H2SO4

44. acetates
Perform ICE BOX calculation based on K1
Synthesis - separation and purification of the product and its identification.
Soluble
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)

45. How are metal oxides and hydrides bonded? are they acidic or basic?
How grouped results are
metal oxides and hydrides are ionically bonded and basic
E=q + w (negative is by system - positive is on system)
Synthetic condensation polymer (aka a polyamide)

46. acetate
Ksp = 27s4
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
water and substances with (s) less dense than
CH3COO?

47. What is the general formula for a ketone?
Anode
RCOR
Ksp = 4s³
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

48. What is the general formula for an ester?
Sigma bonds are stronger than pi bonds
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RCOOR
O2 needs 4F/mol H2 needs 2F/mol

49. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
a-IMFs - b-molecular volume
Ksp = s²
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

50. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Purple
Ksp = 4s³
Evaporation
proton donor base

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AP Chemistry 2

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