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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. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Molecules with the same molecular formulas - but different structural formulas
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Current - time and charge on ion (moles of e used in half cell reaction)
atoms

2. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
allow for the vapor pressure of water and make sure to level levels
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
P2O5
The dilution effect when the solutions mix. M1V1 = M2V2

3. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
#ligands=charge x2
ion pairing

4. What process do you use to obtain a solvent from a solution?
Distillation
Acidified
RX
CrO4²?

5. What type of compounds are almost always colored?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
White precipitate
it's lower and occurs over less sharp a range
Transition element compounds (except if it has a full or empty d shell)

6. Acids + Carbonates (bicarbonates) make?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
it is lower and occurs over less sharp a range
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)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

7. What is the general formula for an acid?
Most are soluble except Ag - Pb
ionic and form hydrogen and hydroxide
RCOOH
Soluble

8. What are the names and formulas of the 6 strong acids?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
NH4?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

9. chlorite
same KE - but PEice<PEwater
Acid rain - dissolves marble buildings/statues and kills trees.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ClO2?

10. Nonmetals are good _____ agents. Metals are good _______ agents.
Salts (ex: CaO + SO2 ? CaSO3)
do not change
Kc=Kp
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

11. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Increases.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
a-IMFs - b-molecular volume
NH4?

12. The definition of acidic basic and neutral aqueous solutions is:
no - they're written undissociated (HAaq)
NH2?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Orange

13. What is the general formula for alkyl halides?
RX
Soluble
lighted splint (positive result=pop)
#ligands=charge x2

14. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
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
Soluble
Anode - oxygen. Cathode - hydrogen

15. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Anode - oxygen. Cathode - hydrogen
ClO4?

16. mercury (II) ion
Hg²?
are less dense than water
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
it reacts by substitution NOT addition

17. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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18. hypochlorite
ClO?
Exothermic
PO4³?
left - ppt will form

19. hydroxides
Insoluble (except group 1 ammonium and Ba)
But S° of element is not zero (except at 0K)
They stay the same.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

20. Colorless doesn't mean ______
Clear
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ROH

21. Does Benzene react by addition or substitution?
Pipette (burette if need repetition)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
it reacts by substitution NOT addition
RCOOH

22. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Suniverse increases for spontaneous processes
zero
blue (BTB)

23. During a titration what is present in the beaker at the equivalence point?
A salt solution.
ClO2?
ionic and form hydrogen and hydroxide
Separating funnel

24. What type of compounds do Group 14 form?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
+4-covalent - +2-ionic
same KE - but PEice<PEwater
acid + alcohol

25. What are the units of the first order rate constant?
|experimental - accepted|/accepted X 100
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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
Acidified

26. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
The compound with the lowest Ksp value.
Distillation
The one with most oxygen atoms (highest oxidation number)
water and substances with (s) less dense than

27. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Perform ICE BOX calculation based on K1
Acidified
The compound with the lowest Ksp value.

28. phosphates
Most INsoluble except group 1 and ammonium
acids
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
MnO4?

29. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Suniverse increases for spontaneous processes
acid + alcohol
Hg²?

30. permanganate
Orange
acids
MnO4?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

31. What are isotopes?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Most are soluble except Ag - Pb
Glacial acetic acid

32. Is the freezing of ice endothermic or exothermic?
bases
Exothermic
Saturated - Substitution (which requires more radical conditions)
|experimental - accepted|/accepted X 100

33. What are the formulas for q?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
q=mc?T q=mL (or n x ?h)
red - green - blue

34. Why are i factors (Van't Hoff factors) often less than ideal?
+4-covalent - +2-ionic
Salts (ex: CaO + SO2 ? CaSO3)
ion pairing
RNH2

35. dichromate
a-IMFs - b-molecular volume
Cr2O7²?
Heat a test tube at an angle at the side of the tube (not bottom)
RCHO (carbonyl at end)

36. How does the melting point of a mixture compare to the MP of a pure substance?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Both electrons come from the same atom (just as good as a regular bond)
it is lower and occurs over less sharp a range
S2O3²?

37. Color is due to ______ _______ of light.
Soluble
Pour liquids using a funnel or down a glass rod
an oxidized and reduced substance
Selective absorption

38. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
bent
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
OH?

39. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
They stay the same.
?G= -ve - E°= +ve
How close results are to the accepted value

40. What do acids plus active metals form?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
catalyst=conc H2SO4
Evaporation
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

41. What word is a clue for a redox reaction?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Kc=Kp
Synthetic condensation polymer (aka a polyamide)
Acidified

42. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
it is lower and occurs over less sharp a range
Reduction always takes place at the cathode (RED CAT) In both types of cell!
PO4³?

43. What electrons are lost/gained first in transition element ions?
-Ea/R
ns² electrons (first in-first out)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
No - NH3 and HCl gases are extremely soluble

44. What is the general formula for an ether?
MnO4?
Most are soluble except Ag - Pb
NO3?
ROR

45. Give an example of a concentrated weak acid.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Clear
Glacial acetic acid

46. When driving off water from a hydrate - how do you tell you're done?
ROR
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Insoluble except nitrate and acetate
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

47. cyanide
K1 x K2
CN?
zero-th: decreases - first: constant - second: increases
No - NH3 and HCl gases are extremely soluble

48. What is the formula for alkenes?
fractional distillation
CnH2n
Saturated - Substitution (which requires more radical conditions)
Molecules with the same molecular formulas - but different structural formulas

49. What is accuracy?
Distillation
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
How close results are to the accepted value

50. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
?H-kJ - ?S-J - ?G-kJ
Experimental mass/theoretical mass X 100
Glowing splint (positive result=relights)