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

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2. chlorite
Insoluble except for nitrate and acetate
Acid rain - dissolves marble buildings/statues and kills trees.
?G=negative - E° must be positive
ClO2?

3. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
H3PO4
Concentration
Soluble except Ag - Pb - Ca - Sr Ba)

4. nitrate
Salts (ex: CaO + SO2 ? CaSO3)
NO3?
voltaic: + electrolytic: -
More chaotic (ex: gases made)

5. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
do not change
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

6. Color (absorbance) is proportional to ________
Heptane
small size and high charge
Concentration
CnH(2n+2)

7. silver iodide
NH4?
Insoluble
R=8.31 J/mol/K
Pale yellow

8. What is the name of S2Cl2? (Know how to name others like this - too)
Ionic compounds
H+
How grouped results are
Disulfur dichloride

9. 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 -
zero-th: decreases - first: constant - second: increases
The dilution effect when the solutions mix. M1V1 = M2V2
Nothing

10. sulfates
At half equivalence - pH=pKa
K2
?G= -ve - E°= +ve
Soluble except Ag - Pb - Ca - Sr Ba)

11. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
The one with most oxygen atoms (highest oxidation number)
NH4?
10?8

12. 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
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Pale purple - (orange)-yellow - red - blue - green.
diamond and graphite

13. Generally - which oxy acid is strongest?
Kc=Kp
The one with most oxygen atoms (highest oxidation number)
Pour liquids using a funnel or down a glass rod
Ksp = 4s³

14. Which alkali metals float on water?
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 compound with the lowest Ksp value.
Check for air bubbles in the buret and remove the buret funnel from the buret
All except for lithium

15. What apparatus do you use to separate 2 immiscible liquids?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Separating funnel
Ksp = s²

16. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Increases down group 1 decreases down group 17
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
C4H10

17. What is the basic structure of an optical isomer?
basic
Big K=kf/kr
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Mono; di; tri; tetra; penta; hexa.

18. What equipment do you need for a titration?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
MnO4?
Insoluble (except group 1 ammonium and Ba)

19. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Hg2²?
atoms

20. What is the general formula for an amine?
Exothermic
blue (BTB)
NH4?
RNH2

21. What is the formula of butane?
C4H10
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Graduated cylinder
Acid rain - dissolves marble buildings/statues and kills trees.

22. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Time?¹ - (ex. s?¹ - hr?¹ - etc)

23. 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?)
ClO?
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
HClO4

24. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Silvery gray solid - brown - purple
No - it depends on the number of ions produced on dissolving.
Clear
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

25. What does saturated mean? Unsaturated?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Big K=kf/kr
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

26. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
an oxidized and reduced substance
Silvery gray solid - brown - purple

27. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
NH2?
H+
Insoluble except for nitrate and acetate
RNH2

28. What are two substances that sublime at 1 atm when heated?
Unsaturated - addition (ex: decolorize bromine solution)
H3PO4
Iodine and CO2 (dry ice)
fractional distillation

29. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Add acid to water so that the acid doesn't boil and spit
blue (BTB)
Pale purple - (orange)-yellow - red - blue - green.
Increases down group 1 decreases down group 17

30. Both Acetic acid and ____________ are also functional isomers.
Sigma bonds are stronger than pi bonds
MnO4?
methyl formate
voltaic: - electrolytic: +

31. Does Benzene react by addition or substitution?
ClO?
it reacts by substitution NOT addition
Sulfur
Ksp = 27s4

32. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
MnO4?
Insoluble except nitrate and acetate

33. When is ?G zero?
Trigonal pyramidal
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
T increases exponentially the proportion of molecules with E > Ea
voltaic: + electrolytic: -

34. What are the signs of ?G and E° for spontaneous reactions?
At half equivalence - pH=pKa
?G=negative - E° must be positive
left - ppt will form
H2PO4?

35. How do you clean a buret/pipette for a titration?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
it reacts by substitution NOT addition

36. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
#ligands=charge x2
K2
same KE - but PEice<PEwater
CO (poisonous)

37. How does benzene compare in reactivity to alkenes?
Insoluble except group 1 and ammonium
ClO3?
An active metal.
benzene is less reactive than alkenes

38. How are primary alcohols turned into acids?
Synthesis - separation and purification of the product and its identification.
Experimental mass/theoretical mass X 100
Iodine and CO2 (dry ice)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

39. Ions are not ______.
PO4³?
atoms
basic
left - ppt will form

40. What are two allotropes of carbon?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
diamond and graphite
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Clear

41. What is the conjugate acid of H2PO4?
H3PO4
OH- and NH3
Soluble
bright yellow

42. What do you need to make a polymer?
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)
How close results are to the accepted value
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
hydroxides (ex: Ba(OH)2)

43. What type of compounds do Group 14 form?
Disulfur dichloride
+4-covalent - +2-ionic
RX
10?8

44. What changes Keq?
Sigma bonds are stronger than pi bonds
Only temperature
Insoluble except for nitrate and acetate
Soluble

45. What steps do organic labs consist of?
ClO2?
Synthesis - separation and purification of the product and its identification.
#ligands=charge x2
The dilution effect when the solutions mix. M1V1 = M2V2

46. What should you check for before you begin titrating?
Soluble except Ag - Pb - Ca - Sr Ba)
Soluble
Clear
Check for air bubbles in the buret and remove the buret funnel from the buret

47. Do you use J or kJ for ?H - ?S - and ?G?
?H formation of an element in standard state=0
Ionic compounds
Add acid to water so that the acid doesn't boil and spit
?H-kJ - ?S-J - ?G-kJ

48. Color is due to ______ _______ of light.
Saturated - Substitution (which requires more radical conditions)
benzene is less reactive than alkenes
Selective absorption
voltaic: + electrolytic: -

49. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
ClO2?
No - it depends on the number of ions produced on dissolving.
Orange

50. What shape is ammonia?
no - they're written undissociated (HAaq)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Trigonal pyramidal
Check for air bubbles in the buret and remove the buret funnel from the buret