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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.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. bromothymol
Eudiometer
Greenish-yellow gas
blue (BTB)
blue

2. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Graduated cylinder
Insoluble except group 1 and ammonium
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

3. 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.
Saturated - Substitution (which requires more radical conditions)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

4. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
?H formation of an element in standard state=0
R=8.31 J/mol/K
A salt solution.

5. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
a-IMFs - b-molecular volume
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
it's lower and occurs over less sharp a range
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

6. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Insoluble except group 1 and ammonium
Soluble
?H-kJ - ?S-J - ?G-kJ

7. Which of the rates changes more when temperature is increased?
Saturated - Substitution (which requires more radical conditions)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Transition element compounds (except if it has a full or empty d shell)
Increases down group 1 decreases down group 17

8. carbonate
RCHO (carbonyl at end)
0.10M HCl (more ions)
CO3²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

9. ________ are Lewis bases - because they can donate a lone pair of electrons.
Synthetic condensation polymer (aka a polyamide)
OH- and NH3
an oxidized and reduced substance
neutralization: high K - H2O product dissociation: low K - H2O reactant

10. What is the formula for percent error?
CnH2n-2
|experimental - accepted|/accepted X 100
zero
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

11. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
a-IMFs - b-molecular volume
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
do not change

12. Why are i factors (Van't Hoff factors) often less than ideal?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Pipette (burette if need repetition)
ion pairing

13. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
?G= -ve - E°= +ve
Ksp = 108s5
zero
CnH2n

14. What are the signs for ?G and E° for spontaneous reactions?
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
?G= -ve - E°= +ve
S2O3²?
C4H10

15. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
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)
diamond and graphite
Ksp = 27s4

16. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Clear
catalyst=conc H2SO4
S2O3²?

17. What is the energy you must put into a reaction to make it start called?
Acidified
Initiation energy (NOT Ea)
CnH(2n+2)
Anode

18. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
Salt + water.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Soluble

19. Is a graduated cylinder or beaker more accurate?
Decant
Graduated cylinder
Synthesis - separation and purification of the product and its identification.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

20. What do nonmetal oxides plus water form?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Current - time and charge on ion (moles of e used in half cell reaction)
acids
Acids; HCOOCH3 is an ester

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

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22. A Bronsted-Lowry base is...
Orange
Most are soluble except Ag - Pb
But S° of element is not zero (except at 0K)
proton acceptor.

23. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
Separating funnel
ionic and form hydrogen and hydroxide
Increases down group 1 decreases down group 17

24. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Both electrons come from the same atom (just as good as a regular bond)
Acids; HCOOCH3 is an ester
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

25. chromate ion (soln + most solids)
brown volatile liquid
[A?]/[HA] x 100 or [BH?]/[B] x 100
yellow
strong acids/bases are written as H+ or OH- ions

26. bromine
brown volatile liquid
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
How grouped results are
OH?

27. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
small size and high charge
?G=negative - E° must be positive
Trigonal pyramidal

28. What equipment do you need for a titration?
?G= -ve - E°= +ve
non-metal oxides and hydrides are covalently bonded and are acidic.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Separating funnel

29. What two types of substances are present in all redox reactions?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Kc=Kp
Increases down group 1 decreases down group 17
an oxidized and reduced substance

30. What electrons are lost/gained first in transition element ions?
A) any range. b) 8-10 c) 4-6
acid + alcohol
ns² electrons (first in-first out)
by electrolysis

31. Both Acetic acid and ____________ are also functional isomers.
methyl formate
it reacts by substitution NOT addition
Salt + water.
The dilution effect when the solutions mix. M1V1 = M2V2

32. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
?G= -ve - E°= +ve
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

33. What is a dipeptide? polypeptide? protein?
?G=negative - E° must be positive
benzene is less reactive than alkenes
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Orange

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

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35. sulfate
Disulfur dichloride
Insoluble except group 1 and ammonium
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
SO4²?

36. chlorate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
No - it depends on the number of ions produced on dissolving.
ClO3?
boiling without losing volatile solvents/reactants

37. What is HCOOCH3?
Ppt will NOT form (unsaturated)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acids; HCOOCH3 is an ester
linear

38. At what point during titration do you have the perfect buffer - and what is the pH at this point?
K1 x K2
'non-active' metals such as Cu - Ag - Au - Pt - etc.
At half equivalence - pH=pKa
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

39. How do you find the pH for a dibasic acid? (H2A)?
allow for the vapor pressure of water and make sure to level levels
Synthesis - separation and purification of the product and its identification.
Perform ICE BOX calculation based on K1
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.

40. 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?)
CH3COO?
Suniverse increases for spontaneous processes
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

41. 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)
Clear
Disulfur dichloride
Heptane

42. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Sigma bonds are stronger than pi bonds
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ClO2?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

43. Alcohols and _______ are FG isomers
RCOOH
Acidified
catalyst=conc H2SO4
ethers

44. How do you compute % dissociation?
do not change
NO3?
Evaporation
[A?]/[HA] x 100 or [BH?]/[B] x 100

45. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
Tetrahedral
fruit - fish - bases
NH4?

46. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Pale yellow
The dilution effect when the solutions mix. M1V1 = M2V2
Products - reactants (except for BDE when it's reactants - products)
Only temperature

47. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Nothing
non-metal oxides and hydrides are covalently bonded and are acidic.
same KE - but PEice<PEwater
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

48. What process do you use to obtain the precipitate from a solution?
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
Filtration
voltaic: + electrolytic: -
strong acids/bases are written as H+ or OH- ions

49. hypochlorite
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ClO?
Separating funnel
[A?]/[HA] x 100 or [BH?]/[B] x 100

50. What type of compounds do metals/non metals form?
HClO4
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Ionic compounds
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