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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. Which alkali metals float on water?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
All except for lithium
Acidified
Evaporation

2. group 1 ions/compounds
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
RNH2
Soluble
water and substances with (s) less dense than

3. phosphates
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Most INsoluble except group 1 and ammonium
Pour liquids using a funnel or down a glass rod
chemically (ex: with carbon)

4. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acids; HCOOCH3 is an ester
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acid rain - dissolves marble buildings/statues and kills trees.

5. During a titration what is present in the beaker at the equivalence point?
A salt solution.
water and substances with (s) less dense than
Group 1 hydroxides (ex: NaOH)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

6. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Greenish-yellow gas
RCHO (carbonyl at end)
ClO?

7. Why are noble gases stable?
fruit - fish - bases
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Filtration
CnH2n-2

8. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
Mono; di; tri; tetra; penta; hexa.
Ksp = 4s³
Sulfur

9. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
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)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

10. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
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)
RCOOH
Salt + water
K1 x K2

11. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
A) any range. b) 8-10 c) 4-6
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble except Ag - Pb - Ca - Sr Ba)
ionic and form hydrogen and hydroxide

12. What is the test for oxygen?
#ligands=charge x2
Glowing splint (positive result=relights)
Q=It (time in seconds)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

13. What shape is ammonia?
basic
Filtration
Trigonal pyramidal
small size and high charge

14. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
C4H10
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?)
NO3?

15. Which of the rates changes more when temperature is increased?
The dilution effect when the solutions mix. M1V1 = M2V2
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
proton donor base
red - green - blue

16. How are non-metal oxides and hydrides bonded? are they acidic or basic?
#ligands=charge x2
non-metal oxides and hydrides are covalently bonded and are acidic.
OH- and NH3
brown volatile liquid

17. mercury (II) ion
?H formation of an element in standard state=0
do not change
Hg²?
Combine the equations for the half reactions in the non-spontaneous direction

18. Color (absorbance) is proportional to ________
Concentration
S2O3²?
Insoluble except nitrate and acetate
HClO4

19. copper sulfate
K2
blue
small size and high charge
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

20. Name C7H16
Heptane
Ions go through the salt bridge - electrons go through metal wires in the external circuit
CnH(2n+2)
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.

21. sulfate
Acidified
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)
Increases down group 1 decreases down group 17
SO4²?

22. What equipment do you need for a titration?
Evaporation
Eudiometer
red - green - blue
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

23. primary colors
water and substances with (s) less dense than
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
red - green - blue
SO4²?

24. What are the common strong bases?
same KE - but PEice<PEwater
ethers
Group 1 hydroxides (ex: NaOH)
blue

25. Acids + Carbonates (bicarbonates) make?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Clear
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

26. 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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27. ________ are Lewis bases - because they can donate a lone pair of electrons.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RNH2
Acids; HCOOCH3 is an ester
OH- and NH3

28. What type of compounds do metals/non metals form?
H3PO4
?H-kJ - ?S-J - ?G-kJ
Ionic compounds
small size and high charge

29. What do group I/II metal oxides and acids form?
acid + alcohol
ClO3?
Salt and water
0.10M HCl (more ions)

30. chlorite
ClO2?
Only temperature
H+
yellow

31. nitrate
Silvery gray solid - brown - purple
water and substances with (s) less dense than
NO3?
acids

32. carbonates
Distillation
an oxidized and reduced substance
Sigma bonds are stronger than pi bonds
Insoluble except group 1 and ammonium

33. An amphiprotic (amphoteric) species is...
#ligands=charge x2
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
How close results are to the accepted value
NO3?

34. What is the charge on a chlorine atom?
zero
An active metal.
Anode
PO4³?

35. Color is due to ______ _______ of light.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
CnH2n+1 often designated 'R' ex C3H7 is propyl
How grouped results are
Selective absorption

36. What is the general formula for an ether?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Filtration
ROR
No - NH3 and HCl gases are extremely soluble

37. What is the formula for alkynes?
catalyst=conc H2SO4
|experimental - accepted|/accepted X 100
CnH2n-2
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

38. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Increases down group 1 decreases down group 17
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

39. How are metal oxides and hydrides bonded? are they acidic or basic?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
metal oxides and hydrides are ionically bonded and basic
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
zero

40. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
The Faraday or Faraday's constant.
q=mc?T q=mL (or n x ?h)
lighted splint (positive result=pop)

41. What is reflux?
Orange
Exothermic
boiling without losing volatile solvents/reactants
Suniverse increases for spontaneous processes

42. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Insoluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Mono; di; tri; tetra; penta; hexa.
They stay the same.

43. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
H3PO4
neutralization: high K - H2O product dissociation: low K - H2O reactant
Disulfur dichloride
Anode - oxygen. Cathode - hydrogen

44. dichromate (soln + most solids)
MnO4?
Orange
Evaporation
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

45. What device would you use to measure a volume of gas?
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?)
Salts (ex: CaO + SO2 ? CaSO3)
Eudiometer
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

46. halides
Most are soluble except Ag - Pb
hydroxides (ex: Ba(OH)2)
Pale yellow
acids

47. What type of metals don't react with water or acids to form H2?

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48. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
diamond and graphite
Making sigma bonds and holding lone pairs
Check for air bubbles in the buret and remove the buret funnel from the buret

49. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
At half equivalence - pH=pKa
Pale purple - (orange)-yellow - red - blue - green.
Soluble

50. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
CnH2n-2
The one with most oxygen atoms (highest oxidation number)
Silvery gray solid - brown - purple