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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. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Group 1 hydroxides (ex: NaOH)
SO4²?

2. primary colors
H+
Pour liquids using a funnel or down a glass rod
Sigma bonds are stronger than pi bonds
red - green - blue

3. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
boiling without losing volatile solvents/reactants
Distillation
look for changes in oxidation # - the one that goes up is oxidized and is the RA

4. carbonates
All except for lithium
Pipette (burette if need repetition)
ion pairing
Insoluble except group 1 and ammonium

5. bromine
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
brown volatile liquid
atoms
T increases exponentially the proportion of molecules with E > Ea

6. What are the prefixes for the naming of binary molecular compound formulas (up to six)
ion pairing
Mono; di; tri; tetra; penta; hexa.
Soluble except Ag - Pb - Ca - Sr Ba)
A) any range. b) 8-10 c) 4-6

7. Aromatic compounds contain what?
Tetrahedral
No - it depends on the number of ions produced on dissolving.
The benzene ring (or more correctly the phenyl group - C6H5)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

8. Name 2 ways in which you can create a buffer?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
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)
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

9. If a weak acid is diluted more - what happens to its % dissociation value?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
No - it depends on the number of ions produced on dissolving.
Increases.
ns² electrons (first in-first out)

10. group 1 ions/compounds
Initiation energy (NOT Ea)
Soluble
diamond and graphite
Separating funnel

11. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Orange
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
yellow

12. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
Insoluble except for nitrate and acetate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

13. When a cell is 'flat' What is its voltage?
zero
K2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Pale yellow

14. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
?H-kJ - ?S-J - ?G-kJ
Iodine and CO2 (dry ice)
Most INsoluble except group 1 and ammonium

15. What changes Keq?
Distillation
Evaporation
Only temperature
catalyst=conc H2SO4

16. At what point during titration do you have the perfect buffer - and what is the pH at this point?
ROH
?G= -ve - E°= +ve
At half equivalence - pH=pKa
proton acceptor.

17. perchlorate
ClO4?
CnH(2n+2)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Graduated cylinder

18. What is the general formula for an amine?
RX
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
0 and 14
RNH2

19. When is ?G zero?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Pale purple - (orange)-yellow - red - blue - green.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

20. What word is a clue for a redox reaction?
Distillation
Acidified
Both electrons come from the same atom (just as good as a regular bond)
CO3²?

21. When combining half equations - what do you do to E° values when multiplying coefficients?
Insoluble
Experimental mass/theoretical mass X 100
Nothing
PO4³?

22. Give an example of a concentrated weak acid.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Glacial acetic acid
left - ppt will form
H3PO4

23. copper sulfate
Glowing splint (positive result=relights)
Group I metals (soft metals) are stored under oil
blue
Soluble except Ag - Pb - Ca - Sr Ba)

24. During a titration what is present in the beaker at the equivalence point?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Transition element compounds (except if it has a full or empty d shell)
CO2 and H2O
A salt solution.

25. What steps do organic labs consist of?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Synthesis - separation and purification of the product and its identification.
non-metal oxides and hydrides are covalently bonded and are acidic.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

26. What is the general formula for an ester?
RCOOR
They stay the same.
Trigonal pyramidal
CO3²?

27. Both Acetic acid and ____________ are also functional isomers.
benzene is less reactive than alkenes
methyl formate
allow for the vapor pressure of water and make sure to level levels
Nothing

28. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
K2
The compound with the lowest Ksp value.
Anode - oxygen. Cathode - hydrogen

29. What is the formula for percent yield?
proton acceptor.
Experimental mass/theoretical mass X 100
Hg2²?
zero

30. A Bronsted-Lowry base is...
Increases.
Group I metals (soft metals) are stored under oil
H+
proton acceptor.

31. 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?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
water and substances with (s) less dense than
Sulfur
The compound with the lowest Ksp value.

32. What are the common strong bases?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Group 1 hydroxides (ex: NaOH)
No - it depends on the number of ions produced on dissolving.
ROH

33. What is the test for oxygen?
Glowing splint (positive result=relights)
Tetrahedral
CnH2n
basic

34. How are metal oxides and hydrides bonded? are they acidic or basic?
Eudiometer
hydroxides (ex: Ba(OH)2)
metal oxides and hydrides are ionically bonded and basic
Iodine and CO2 (dry ice)

35. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
a-IMFs - b-molecular volume
ion pairing
CnH2n+2

36. Name six characteristics of transition elements (or their compounds)
Soluble
blue
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)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

37. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
ROR
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ksp = 4s³

38. What is a coordinate covalent bond?
ClO3?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
|experimental - accepted|/accepted X 100
Both electrons come from the same atom (just as good as a regular bond)

39. Are weak acids (and bases) written dissociated?

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40. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Salt and water
Current - time and charge on ion (moles of e used in half cell reaction)
Experimental mass/theoretical mass X 100
Decant

41. What is the basic structure of an optical isomer?
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)
CnH(2n+2)
by electrolysis

42. What is a dipeptide? polypeptide? protein?
no - they're written undissociated (HAaq)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

43. What are the signs for ?G and E° for spontaneous reactions?
How close results are to the accepted value
?G= -ve - E°= +ve
small size and high charge
At half equivalence - pH=pKa

44. What equipment do you need for a titration?
different forms of the same element
Salt + water
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
it's lower and occurs over less sharp a range

45. mercury (I) ion
Hg2²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
NH4?
C4H10

46. What is the general formula for an ether?
fractional distillation
R=8.31 J/mol/K
ROR
HClO4

47. How many faradays of electric charge do you need to produce one mole of O2? H2?
Cr2O7²?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Monomer + monomer = polymer product + a simple molecule such as water or HCl
O2 needs 4F/mol H2 needs 2F/mol

48. What is the first law of thermodynamics?
OH- and NH3
redox reaction
E=q + w (negative is by system - positive is on system)
The Faraday or Faraday's constant.

49. carbonate
?H formation of an element in standard state=0
basic
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
CO3²?

50. What is the general formula for an alcohol?
Sigma bonds are stronger than pi bonds
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
C4H10
ROH

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AP Chemistry 2

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