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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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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 does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
Group I metals (soft metals) are stored under oil
linear
ClO4?

2. How are primary alcohols turned into acids?
Acid rain - dissolves marble buildings/statues and kills trees.
ion pairing
How grouped results are
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

3. At what point during titration do you have the perfect buffer - and what is the pH at this point?
More chaotic (ex: gases made)
At half equivalence - pH=pKa
Glowing splint (positive result=relights)
Soluble

4. What shape is methane?
C4H10
Tetrahedral
it's lower and occurs over less sharp a range
are less dense than water

5. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Cu3(PO4)2
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Eudiometer

6. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
zero
ClO?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

7. lead compounds
Clear
Greenish-yellow gas
methyl formate
Insoluble except nitrate and acetate

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

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9. How many faradays of electric charge do you need to produce one mole of O2? H2?
atoms
CO (poisonous)
O2 needs 4F/mol H2 needs 2F/mol
same KE - but PEice<PEwater

10. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Ksp = 4s³
No - it depends on the number of ions produced on dissolving.
Glowing splint (positive result=relights)
OH?

11. A Bronsted-Lowry acid is...
0 and 14
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
basic
proton donor base

12. What is the general formula for an amine?
How grouped results are
Concentration
Orange
RNH2

13. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
CrO4²?
?H formation of an element in standard state=0
fractional distillation

14. What two compounds are great oxidizing agents?

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15. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
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)
ROH
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

16. Acids + Carbonates (bicarbonates) make?
But S° of element is not zero (except at 0K)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
CnH2n

17. What complex ion does ammonia form with silver? copper? cadmium? zinc?
water and substances with (s) less dense than
CnH2n
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
benzene has a delocalized pi ring structure

18. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Heptane
proton donor base

19. What is reflux?
strong acids/bases are written as H+ or OH- ions
boiling without losing volatile solvents/reactants
+4-covalent - +2-ionic
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

20. hydroxide
OH?
Anode
Most INsoluble except group 1 and ammonium
Increases.

21. Nonmetals are good _____ agents. Metals are good _______ agents.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
They decrease (or could be the same if the solid has ONLY JUST disappeared)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
it reacts by substitution NOT addition

22. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Anode
Reduction always takes place at the cathode (RED CAT) In both types of cell!
redox reaction
RCOOH

23. What is the formula for alkynes?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CnH2n-2
voltaic: + electrolytic: -
No - NH3 and HCl gases are extremely soluble

24. What is the test for hydrogen?
chemically (ex: with carbon)
lighted splint (positive result=pop)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
ion pairing

25. What do ions and electrons travel through in a voltaic/electrolytic cell?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Making sigma bonds and holding lone pairs
Ions go through the salt bridge - electrons go through metal wires in the external circuit

26. Do anions flow to the cathode or anode?
acids
Insoluble except for nitrate and acetate
They stay the same.
Anode

27. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
'non-active' metals such as Cu - Ag - Au - Pt - etc.

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

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29. What changes Keq?
Add acid to water so that the acid doesn't boil and spit
ClO2?
Only temperature
+4-covalent - +2-ionic

30. What shape is ammonia?
bases
a-IMFs - b-molecular volume
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Trigonal pyramidal

31. phosphates
fruit - fish - bases
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
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?)
Most INsoluble except group 1 and ammonium

32. How do you clean a buret/pipette for a titration?
?G=negative - E° must be positive
Exothermic
Increases.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

33. nitrate
NO3?
ion pairing
C4H10
Molecules with the same molecular formulas - but different structural formulas

34. How do you identify which is oxidized or otherwise?
RX
diamond and graphite
ClO4?
look for changes in oxidation # - the one that goes up is oxidized and is the RA

35. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
The compound with the lowest Ksp value.
H3PO4
Mn²? - Cr³? - Cr³

36. How are strong ones written?
proton donor base
bases
strong acids/bases are written as H+ or OH- ions
E=q + w (negative is by system - positive is on system)

37. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Most are soluble except Ag - Pb
Insoluble

38. Does Kw increase or decrease with T? Why?
Pale yellow
Hg2²?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
But S° of element is not zero (except at 0K)

39. permanganate
different forms of the same element
Molecules with the same molecular formulas - but different structural formulas
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
MnO4?

40. silver compounds
brown volatile liquid
Insoluble except for nitrate and acetate
Sulfur
ionic and form hydrogen and hydroxide

41. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
#ligands=charge x2
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

42. What is the charge on a chlorine atom?
metal oxides and hydrides are ionically bonded and basic
zero
same KE - but PEice<PEwater
Pale yellow

43. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Trigonal pyramidal
non-metal oxides and hydrides are covalently bonded and are acidic.
Q=It (time in seconds)

44. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
allow for the vapor pressure of water and make sure to level levels
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
do not change
Acid rain - dissolves marble buildings/statues and kills trees.

45. What do you need to make a polymer?
Exothermic
Cu3(PO4)2
Products - reactants (except for BDE when it's reactants - products)
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)

46. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Exothermic
S2O3²?
K1 x K2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

47. Give an example of a concentrated weak acid.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Glacial acetic acid
zero
Most INsoluble except group 1 and ammonium

48. What is the formula for alkanes?
NH2?
CnH2n+2
Perform ICE BOX calculation based on K1
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

49. perchlorate
ClO4?
The Faraday or Faraday's constant.
Soluble
S2O3²?

50. Is the freezing of ice endothermic or exothermic?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
same KE - but PEice<PEwater
Exothermic
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

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AP Chemistry 2

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