Test your basic knowledge |

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. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
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.
same KE - but PEice<PEwater
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
H3PO4

2. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
are less dense than water
All except for lithium
look for changes in oxidation # - the one that goes up is oxidized and is the RA

3. barium sulfate
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.
0.10M HCl (more ions)
White precipitate
blue glass - it filters UV

4. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
diamond and graphite
Iodine and CO2 (dry ice)
More chaotic (ex: gases made)

5. What is the general formula for an acid?
RCOOH
Purple
?H formation of an element in standard state=0
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

6. How many ligands attach to a central ion in a complex ion?
Iodine and CO2 (dry ice)
by electrolysis
#ligands=charge x2
Synthetic condensation polymer (aka a polyamide)

7. lead iodide
bright yellow
P2O5
SO4²?
Most are soluble except Ag - Pb

8. What type of compounds are almost always colored?
RCOOR
Read the bottom of the meniscus
Transition element compounds (except if it has a full or empty d shell)
No - it depends on the number of ions produced on dissolving.

9. What are isomers?
bent
Current - time and charge on ion (moles of e used in half cell reaction)
OH- and NH3
Molecules with the same molecular formulas - but different structural formulas

10. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Clear
No - NH3 and HCl gases are extremely soluble
[A?]/[HA] x 100 or [BH?]/[B] x 100

11. phosphate
How close results are to the accepted value
bases
CrO4²?
PO4³?

12. What is the general formula for an ester?
RCOOR
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
Glowing splint (positive result=relights)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

13. Alcohols and _______ are FG isomers
ion pairing
ethers
Experimental mass/theoretical mass X 100
benzene is less reactive than alkenes

14. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Hg2²?
Products - reactants (except for BDE when it's reactants - products)
Insoluble except for nitrate and acetate
K1 x K2

15. Esters smell like _______ and amines smell like _______ and are ______.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
fruit - fish - bases
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Making sigma bonds and holding lone pairs

16. What are the names and formulas of the 6 strong acids?
hydroxides (ex: Ba(OH)2)
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
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)

17. What things should you remember to do when collecting gas over water?
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.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Separating funnel

18. Is the freezing of ice endothermic or exothermic?
Exothermic
different forms of the same element
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Insoluble

19. If a free element is involved - what type of reaction must be involved?
No - it depends on the number of ions produced on dissolving.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Both electrons come from the same atom (just as good as a regular bond)
redox reaction

20. A geometric (or cis-trans) isomer exists due to.....
Pour liquids using a funnel or down a glass rod
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
HClO4
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

21. What is the formula for alkynes?
Ksp = 27s4
HClO4
CnH2n-2
Salts (ex: CaO + SO2 ? CaSO3)

22. What are the signs of ?G and E° for spontaneous reactions?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
?G= -ve - E°= +ve
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
?G=negative - E° must be positive

23. What is the formula of butane?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
C4H10
SO4²?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

24. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Soluble except Ag - Pb - Ca - Sr Ba)
CnH2n+1 often designated 'R' ex C3H7 is propyl
10?8
Glacial acetic acid

25. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
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)
Both electrons come from the same atom (just as good as a regular bond)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Current - time and charge on ion (moles of e used in half cell reaction)

26. What is the general formula for an alcohol?
No - NH3 and HCl gases are extremely soluble
ROH
bright yellow
Most INsoluble except group 1 and ammonium

27. Is the standard entropy (S°) of an element zero?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
blue (BTB)
OH?
But S° of element is not zero (except at 0K)

28. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
zero-th: decreases - first: constant - second: increases
CN?

29. What are allotropes?
Sulfur
H2PO4?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
different forms of the same element

30. oxalate
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Initiation energy (NOT Ea)
C2O4²?
NO3?

31. What is the formula for obtaining charge flowing in a cell?
Pour liquids using a funnel or down a glass rod
ion pairing
Combine the equations for the half reactions in the non-spontaneous direction
Q=It (time in seconds)

32. What do you do to get rid of most of the solution from a precipitate?
Eudiometer
Decant
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Iodine and CO2 (dry ice)

33. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
CnH2n-2
Ksp = 108s5
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
different forms of the same element

34. chromate
CrO4²?
How grouped results are
Reduction always takes place at the cathode (RED CAT) In both types of cell!
NH2?

35. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
acid + alcohol
Pale purple - (orange)-yellow - red - blue - green.
C4H10

36. A Bronsted-Lowry acid is...
Exothermic
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)
proton donor base
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

37. How are primary alcohols turned into acids?
zero-th: decreases - first: constant - second: increases
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Heat a test tube at an angle at the side of the tube (not bottom)

38. An amphiprotic (amphoteric) species is...
Reduction always takes place at the cathode (RED CAT) In both types of cell!
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
RNH2
Salt + water

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

40. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
a-IMFs - b-molecular volume
redox reaction
Anode - oxygen. Cathode - hydrogen
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

41. Name C7H16
Heptane
Anode
10?8
H2PO4?

42. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Ksp = s²
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
a-IMFs - b-molecular volume
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

43. What type of polymer is nylon?
Read the bottom of the meniscus
Synthetic condensation polymer (aka a polyamide)
by electrolysis
Insoluble (except group 1 ammonium and Ba)

44. When combining half equations - what do you do to E° values when multiplying coefficients?
bases
Nothing
?G=negative - E° must be positive
H2PO4?

45. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
-Ea/R
neutralization: high K - H2O product dissociation: low K - H2O reactant
CnH2n-2

46. Which alkali metals float on water?
Filtration
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
All except for lithium
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)

47. How are metal oxides and hydrides bonded? are they acidic or basic?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
benzene has a delocalized pi ring structure
metal oxides and hydrides are ionically bonded and basic
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

48. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
No - NH3 and HCl gases are extremely soluble
OH?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
H+

49. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Salt + water.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ClO?
A salt solution.

50. What two compounds are great oxidizing agents?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183