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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. What changes Keq?
Ksp = 108s5
Only temperature
RCOOR
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

2. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
same KE - but PEice<PEwater
small size and high charge
-Ea/R

3. Generally - which oxy acid is strongest?
non-metal oxides and hydrides are covalently bonded and are acidic.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The one with most oxygen atoms (highest oxidation number)
No - it depends on the number of ions produced on dissolving.

4. Ions are not ______.
atoms
P2O5
Anode - oxygen. Cathode - hydrogen
Reduction always takes place at the cathode (RED CAT) In both types of cell!

5. nitrate
A substance that can act as an acid or a base. ex. water - HCO3? ion 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
NO3?
boiling without losing volatile solvents/reactants

6. Where are group I metals stored?
The Faraday or Faraday's constant.
proton acceptor.
Group I metals (soft metals) are stored under oil
H2O + CO2 (it decomposes readily)

7. When a cell is 'flat' What is its voltage?
?H-kJ - ?S-J - ?G-kJ
zero
Both electrons come from the same atom (just as good as a regular bond)
Disulfur dichloride

8. What is the relationship in strength between sigma and pi bonds?
same KE - but PEice<PEwater
Synthesis - separation and purification of the product and its identification.
Sigma bonds are stronger than pi bonds
Most are soluble except Ag - Pb

9. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
#ligands=charge x2
SO4²?
H+
Increases.

10. What does the solubility of organic compounds depend on?
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)
The Faraday or Faraday's constant.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
ClO?

11. What is the test for oxygen?
Glowing splint (positive result=relights)
SO4²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
OH- and NH3

12. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Synthesis - separation and purification of the product and its identification.
a-IMFs - b-molecular volume
Big K=kf/kr
Insoluble

13. primary colors
An active metal.
?H formation of an element in standard state=0
Conjugate pair (one must be a weak base or acid)
red - green - blue

14. hydroxides
Synthetic condensation polymer (aka a polyamide)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Insoluble (except group 1 ammonium and Ba)
?G=negative - E° must be positive

15. What is the formula for obtaining charge flowing in a cell?
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)
Insoluble except nitrate and acetate
Clear
Q=It (time in seconds)

16. How does the melting point of a mixture compare to the MP of a pure substance?

17. carbonates
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Insoluble except group 1 and ammonium
The benzene ring (or more correctly the phenyl group - C6H5)
?H formation of an element in standard state=0

18. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
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.
ClO4?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

19. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
zero-th: decreases - first: constant - second: increases
different forms of the same element
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

20. bromothymol
red - green - blue
blue (BTB)
Pale purple - (orange)-yellow - red - blue - green.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

21. What is the general formula for a ketone?
RCOR
same KE - but PEice<PEwater
No - NH3 and HCl gases are extremely soluble
Hg²?

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

23. When the salt bridge is removed what happens to the cell reaction?
atoms
How grouped results are
Insoluble except for nitrate and acetate
It ceases - the circuit is broken.

24. How do you clean a buret/pipette for a titration?
Selective absorption
?G= -ve - E°= +ve
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
O2 needs 4F/mol H2 needs 2F/mol

25. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
0.10M HCl (more ions)
ns² electrons (first in-first out)
Greenish-yellow gas

26. How are primary alcohols turned into acids?
The dilution effect when the solutions mix. M1V1 = M2V2
Iodine and CO2 (dry ice)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
strong acids/bases are written as H+ or OH- ions

27. The definition of acidic basic and neutral aqueous solutions is:
A) any range. b) 8-10 c) 4-6
Heptane
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
allow for the vapor pressure of water and make sure to level levels

28. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Silvery gray solid - brown - purple

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

30. What is the formula for percent yield?
Insoluble except for nitrate and acetate
Experimental mass/theoretical mass X 100
acid + alcohol
CnH2n+1 often designated 'R' ex C3H7 is propyl

31. What are isotopes?
The dilution effect when the solutions mix. M1V1 = M2V2
ROR
q=mc?T q=mL (or n x ?h)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

32. When can supercooling occur? What does it look like on a cooling curve?

33. Which of the rates changes more when temperature is increased?
NO3?
CnH2n+2
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
allow for the vapor pressure of water and make sure to level levels

34. BaSO4
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Soluble except Ag - Pb - Ca - Sr Ba)
Insoluble
do not change

35. What is the first law of thermodynamics?
Ppt will NOT form (unsaturated)
q=mc?T q=mL (or n x ?h)
Sigma bonds are stronger than pi bonds
E=q + w (negative is by system - positive is on system)

36. What is the charge on a chlorine atom?
S crystal at 0K=0
Salt + water
fractional distillation
zero

37. How does group 1 metals' density compare to water's?
are less dense than water
CrO4²?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
RCOR

38. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Eudiometer
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
RCOR
Soluble

39. What is the sign of the anode in voltaic cells? in electrolytic cells?
water and substances with (s) less dense than
voltaic: - electrolytic: +
bent
Eudiometer

40. mercury (II) ion
Hg²?
Anode - oxygen. Cathode - hydrogen
Ksp = 4s³
non-metal oxides and hydrides are covalently bonded and are acidic.

41. The oxidation # for acid base reactions...
H2PO4?
do not change
Kc=Kp
Insoluble

42. dichromate
Cr2O7²?
Q=It (time in seconds)
Perform ICE BOX calculation based on K1
Combine the equations for the half reactions in the non-spontaneous direction

43. What causes the dramatic effect of T on rate?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
proton acceptor.
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)
T increases exponentially the proportion of molecules with E > Ea

44. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
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
10?8
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
a-IMFs - b-molecular volume

45. Give an example of a concentrated weak acid.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble except group 1 and ammonium
fruit - fish - bases
Glacial acetic acid

46. Give an example of a dilute strong acid.
HClO4
?G= -ve - E°= +ve
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ksp = 4s³

47. sulfate
linear
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Salt + water
SO4²?

48. hydroxide
Combine the equations for the half reactions in the non-spontaneous direction
OH?
Ksp = 4s³
Q=It (time in seconds)

49. When can supercooling occur? What does it look like on a cooling curve?

50. For a dibasic acid (H2A) - [A²?]= ____ ?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
K2