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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Purple
ns² electrons (first in-first out)
Insoluble (except group 1 ammonium and Ba)

2. What is the charge on a chlorine atom?
-Ea/R
zero
an oxidized and reduced substance
q=mc?T q=mL (or n x ?h)

3. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
All except for lithium
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Identity and purity (impure compounds usually have broad & low melting points)

4. Do anions flow to the cathode or anode?
Anode
lighted splint (positive result=pop)
CnH(2n+2)
CO (poisonous)

5. Acid plus base make?
Anode - oxygen. Cathode - hydrogen
Salt + water.
Current - time and charge on ion (moles of e used in half cell reaction)
Anode

6. What are isotopes?
?H-kJ - ?S-J - ?G-kJ
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acid rain - dissolves marble buildings/statues and kills trees.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

7. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Heptane
brown volatile liquid
Glowing splint (positive result=relights)

8. Color (absorbance) is proportional to ________
CnH2n+1 often designated 'R' ex C3H7 is propyl
Anode - oxygen. Cathode - hydrogen
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Concentration

9. How are more active metals reduced?
fruit - fish - bases
by electrolysis
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
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)

10. ammonium
bent
Acids; HCOOCH3 is an ester
NH4?
CnH2n

11. Ca - Sr - Ba
RCOOH
H2PO4?
hydroxides (ex: Ba(OH)2)
Acidified

12. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CnH(2n+2)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
redox reaction
a-IMFs - b-molecular volume

13. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Soluble
Glowing splint (positive result=relights)
benzene has a delocalized pi ring structure

14. Esterification is...
acid + alcohol
S2O3²?
CrO4²?
Both electrons come from the same atom (just as good as a regular bond)

15. sulfates
Cu3(PO4)2
different forms of the same element
CO (poisonous)
Soluble except Ag - Pb - Ca - Sr Ba)

16. Acidic gases like SO2 in the atmosphere cause what environmental problems?
CrO4²?
metal oxides and hydrides are ionically bonded and basic
Acid rain - dissolves marble buildings/statues and kills trees.
blue (BTB)

17. What is the general formula for a ketone?
Mn²? - Cr³? - Cr³
RCOR
Clear
NO3?

18. How do you explain trends in atomic properties using Coulomb's Law?
Ksp = 27s4
Most INsoluble except group 1 and ammonium
allow for the vapor pressure of water and make sure to level levels
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

19. Why are i factors (Van't Hoff factors) often less than ideal?
an oxidized and reduced substance
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Tetrahedral
ion pairing

20. What do acids plus active metals form?
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?)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Greenish-yellow gas
H2PO4?

21. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
by electrolysis
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

22. How are metal oxides and hydrides bonded? are they acidic or basic?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Heat a test tube at an angle at the side of the tube (not bottom)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
metal oxides and hydrides are ionically bonded and basic

23. 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!
Cr2O7²?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Synthesis - separation and purification of the product and its identification.

24. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
?G=negative - E° must be positive
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

25. phosphate
PO4³?
Hg2²?
allow for the vapor pressure of water and make sure to level levels
A salt solution.

26. What are the products of the reaction between group 1 metals and water?

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27. bromine
water and substances with (s) less dense than
brown volatile liquid
Exothermic (?H for ANY sa/sb = -57kJ/mol)
RCOR

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

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29. What is the first law of thermodynamics?
voltaic: - electrolytic: +
E=q + w (negative is by system - positive is on system)
zero
Disulfur dichloride

30. What are the prefixes for the naming of binary molecular compound formulas (up to six)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Group I metals (soft metals) are stored under oil
water and substances with (s) less dense than
Mono; di; tri; tetra; penta; hexa.

31. How do you heat a test tube?
CH3COO?
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.
Q=It (time in seconds)
Heat a test tube at an angle at the side of the tube (not bottom)

32. How do you find the pH for a dibasic acid? (H2A)?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Perform ICE BOX calculation based on K1
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Most are soluble except Ag - Pb

33. silver iodide
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Pale yellow
No - it depends on the number of ions produced on dissolving.
Q=It (time in seconds)

34. dichromate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Molecules with the same molecular formulas - but different structural formulas
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)
Cr2O7²?

35. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Soluble
MnO4?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Ksp = s²

36. 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
Perform ICE BOX calculation based on K1
Combine the equations for the half reactions in the non-spontaneous direction
Ionic compounds

37. What is the general formula for an amine?
Synthetic condensation polymer (aka a polyamide)
-Ea/R
RNH2
But S° of element is not zero (except at 0K)

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

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

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40. potassium permanganate
Silvery gray solid - brown - purple
Purple
same KE - but PEice<PEwater
catalyst=conc H2SO4

41. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Ksp = 108s5
Pale purple - (orange)-yellow - red - blue - green.
E=q + w (negative is by system - positive is on system)
Big K=kf/kr

42. What reacts with an acid to create hydrogen gas?
Identity and purity (impure compounds usually have broad & low melting points)
An active metal.
Products - reactants (except for BDE when it's reactants - products)
RNH2

43. Alkenes are ________ and react by __________
ethers
Unsaturated - addition (ex: decolorize bromine solution)
methyl formate
Distillation

44. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Increases.
Greenish-yellow gas
Hg²?
K1 x K2

45. What is H2CO3 (carbonate acid) usually written as?
-Ea/R
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
ion pairing
H2O + CO2 (it decomposes readily)

46. How do you compute % dissociation?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Distillation
Pale yellow

47. Alkanes are _________ and react by _________
do not change
H+
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Saturated - Substitution (which requires more radical conditions)

48. Neutralization is an ________ reaction.
More chaotic (ex: gases made)
benzene is less reactive than alkenes
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Disulfur dichloride

49. perchlorate
ClO4?
CnH2n+1 often designated 'R' ex C3H7 is propyl
CO2 and H2O
same KE - but PEice<PEwater

50. What changes Keq?
non-metal oxides and hydrides are covalently bonded and are acidic.
bent
Only temperature
A salt solution.