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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. acetate
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Pale purple - (orange)-yellow - red - blue - green.
CH3COO?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

2. Which value of R do you use for all energy and kinetics calculations?
But S° of element is not zero (except at 0K)
R=8.31 J/mol/K
Initiation energy (NOT Ea)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

3. Why are noble gases stable?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
The one with most oxygen atoms (highest oxidation number)
yellow
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

4. During a titration what is present in the beaker at the equivalence point?
A salt solution.
do not change
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

5. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Increases.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
an oxidized and reduced substance
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

6. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Products - reactants (except for BDE when it's reactants - products)
MnO4?

7. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
It ceases - the circuit is broken.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
q=mc?T q=mL (or n x ?h)
diamond and graphite

8. What process do you use to separate two liquids with different boiling points?
0.10M HCl (more ions)
Exothermic
fractional distillation
Ksp = 108s5

9. lead compounds
10?8
diamond and graphite
Mono; di; tri; tetra; penta; hexa.
Insoluble except nitrate and acetate

10. What equipment do you need for a titration?
Exothermic
Pale yellow
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
voltaic: - electrolytic: +

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

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12. What is the first law of thermodynamics?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mn²? - Cr³? - Cr³
E=q + w (negative is by system - positive is on system)
Heat a test tube at an angle at the side of the tube (not bottom)

13. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
ionic and form hydrogen and hydroxide
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

14. Both Acetic acid and ____________ are also functional isomers.
it's lower and occurs over less sharp a range
methyl formate
RCOOR
Concentration

15. What type of compounds do Group 14 form?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
+4-covalent - +2-ionic
do not change
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

16. How many ligands attach to a central ion in a complex ion?
water and substances with (s) less dense than
Read the bottom of the meniscus
#ligands=charge x2
How close results are to the accepted value

17. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Filtration
atoms
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
RX

18. How many faradays of electric charge do you need to produce one mole of O2? H2?
Heat a test tube at an angle at the side of the tube (not bottom)
Only temperature
O2 needs 4F/mol H2 needs 2F/mol
Initiation energy (NOT Ea)

19. acetates
basic
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Soluble
Ions go through the salt bridge - electrons go through metal wires in the external circuit

20. What do you use for an acid spill? base spill?
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
Soluble
Kc=Kp
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

21. What do ions and electrons travel through in a voltaic/electrolytic cell?
Add acid to water so that the acid doesn't boil and spit
Big K=kf/kr
H+
Ions go through the salt bridge - electrons go through metal wires in the external circuit

22. What are two substances that sublime at 1 atm when heated?
Pipette (burette if need repetition)
ClO2?
Iodine and CO2 (dry ice)
Pale yellow

23. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
catalyst=conc H2SO4
chemically (ex: with carbon)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

24. sulfate
Iodine and CO2 (dry ice)
E=q + w (negative is by system - positive is on system)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
SO4²?

25. Name 2 ways in which you can create a buffer?
O2 needs 4F/mol H2 needs 2F/mol
Distillation
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)
do not change

26. What device would you use to measure a volume of gas?
diamond and graphite
S2O3²?
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?)
Eudiometer

27. What causes the dramatic effect of T on rate?
CrO4²?
T increases exponentially the proportion of molecules with E > Ea
q=mc?T q=mL (or n x ?h)
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

28. What are isotopes?
E=q + w (negative is by system - positive is on system)
Big K=kf/kr
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Insoluble except nitrate and acetate

29. What is the test for hydrogen?
Ppt will NOT form (unsaturated)
blue
lighted splint (positive result=pop)
Soluble except Ag - Pb - Ca - Sr Ba)

30. What do you need to make a polymer?
ClO3?
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)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

31. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
basic
hydroxides (ex: Ba(OH)2)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
H+

32. Do you use J or kJ for ?H - ?S - and ?G?
At half equivalence - pH=pKa
Current - time and charge on ion (moles of e used in half cell reaction)
Separating funnel
?H-kJ - ?S-J - ?G-kJ

33. How are metal oxides and hydrides bonded? are they acidic or basic?
CnH(2n+2)
Making sigma bonds and holding lone pairs
metal oxides and hydrides are ionically bonded and basic
Reduction always takes place at the cathode (RED CAT) In both types of cell!

34. What is the general formula for an acid?
T increases exponentially the proportion of molecules with E > Ea
RCOOH
Greenish-yellow gas
Most INsoluble except group 1 and ammonium

35. bromothymol
blue (BTB)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
White precipitate

36. What is the second law of thermodynamics?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The dilution effect when the solutions mix. M1V1 = M2V2
proton acceptor.
Suniverse increases for spontaneous processes

37. Name six characteristics of transition elements (or their compounds)
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)
Salt + water.
a-IMFs - b-molecular volume
Identity and purity (impure compounds usually have broad & low melting points)

38. Which would cause the bulb in a conductivity apparatus to be brightest?
Products - reactants (except for BDE when it's reactants - products)
q=mc?T q=mL (or n x ?h)
How close results are to the accepted value
0.10M HCl (more ions)

39. What type of compounds do metals/non metals form?
Eudiometer
Ionic compounds
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
It ceases - the circuit is broken.

40. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
RCOR
Disulfur dichloride
Increases.

41. mercury (II) ion
CnH(2n+2)
Hg²?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

42. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
water and substances with (s) less dense than
Graduated cylinder
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

43. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Salt + water
Insoluble except nitrate and acetate
Kc=Kp

44. Which alkali metals float on water?
Acidified
The dilution effect when the solutions mix. M1V1 = M2V2
Heat a test tube at an angle at the side of the tube (not bottom)
All except for lithium

45. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
The compound with the lowest Ksp value.
Sigma bonds are stronger than pi bonds
CO (poisonous)
Acid rain - dissolves marble buildings/statues and kills trees.

46. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Soluble
zero-th: decreases - first: constant - second: increases
Synthetic condensation polymer (aka a polyamide)

47. dichromate
Cr2O7²?
Hg2²?
Combine the equations for the half reactions in the non-spontaneous direction
benzene has a delocalized pi ring structure

48. What is the general formula for an alcohol?
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)
0 and 14
CrO4²?
ROH

49. Nonmetals are good _____ agents. Metals are good _______ agents.
CH3COO?
Saturated - Substitution (which requires more radical conditions)
Ionic compounds
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

50. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Conjugate pair (one must be a weak base or acid)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Heat a test tube at an angle at the side of the tube (not bottom)
Group 1 hydroxides (ex: NaOH)