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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 do you dilute an acid?

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2. acetates
NH4?
Pale purple - (orange)-yellow - red - blue - green.
Soluble
blue

3. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Soluble
methyl formate
C4H10

4. What do you do to get rid of most of the solution from a precipitate?
PO4³?
Decant
Insoluble (except group 1 ammonium and Ba)
All except for lithium

5. What is reflux?
boiling without losing volatile solvents/reactants
NO3?
bent
Soluble except Ag - Pb - Ca - Sr Ba)

6. What shape is methane?
At half equivalence - pH=pKa
metal oxides and hydrides are ionically bonded and basic
Experimental mass/theoretical mass X 100
Tetrahedral

7. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
methyl formate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
water and substances with (s) less dense than
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

8. What is the test for hydrogen?
it is lower and occurs over less sharp a range
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?)
lighted splint (positive result=pop)
q=mc?T q=mL (or n x ?h)

9. When combining half equations - what do you do to E° values when multiplying coefficients?
ion pairing
do not change
water and substances with (s) less dense than
Nothing

10. What is the formula for summation?

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11. mercury (II) ion
by electrolysis
Hg²?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
How grouped results are

12. What is the formula for alkenes?
CnH2n
Making sigma bonds and holding lone pairs
an oxidized and reduced substance
No - NH3 and HCl gases are extremely soluble

13. Do anions flow to the cathode or anode?
Pipette (burette if need repetition)
Anode
Hg²?
strong acids/bases are written as H+ or OH- ions

14. What does saturated mean? Unsaturated?
Salt + water
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Ionic compounds

15. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Combine the equations for the half reactions in the non-spontaneous direction
water and substances with (s) less dense than
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

16. What are the common strong bases?
Initiation energy (NOT Ea)
CN?
acids
Group 1 hydroxides (ex: NaOH)

17. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
ionic and form hydrogen and hydroxide
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

18. What are two substances that sublime at 1 atm when heated?
CnH2n-2
Iodine and CO2 (dry ice)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
it is lower and occurs over less sharp a range

19. What are the formulas for q?
?H formation of an element in standard state=0
ion pairing
q=mc?T q=mL (or n x ?h)
Combine the equations for the half reactions in the non-spontaneous direction

20. Which value of R do you use for all energy and kinetics calculations?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Read the bottom of the meniscus
R=8.31 J/mol/K

21. What is the formula of copper (II) phosphate?
The dilution effect when the solutions mix. M1V1 = M2V2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Cu3(PO4)2
do not change

22. Metal hydrides are _____ and form _______ and _______ when added to water
Big K=kf/kr
Soluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ionic and form hydrogen and hydroxide

23. Buffer capacity must contain decent amounts of a ________ ________
ion pairing
#ligands=charge x2
Conjugate pair (one must be a weak base or acid)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

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

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25. Ca - Sr - Ba
Add acid to water so that the acid doesn't boil and spit
The benzene ring (or more correctly the phenyl group - C6H5)
hydroxides (ex: Ba(OH)2)
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)

26. What is the general formula for alkyl halides?
Evaporation
water and substances with (s) less dense than
RX
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

27. What is the formula for percent error?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
All except for lithium
|experimental - accepted|/accepted X 100
How close results are to the accepted value

28. What process do you use to obtain the precipitate from a solution?
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)
The compound with the lowest Ksp value.
methyl formate
Filtration

29. What type of compounds do Group 14 form?
water and substances with (s) less dense than
water and substances with (s) less dense than
+4-covalent - +2-ionic
it reacts by substitution NOT addition

30. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
CnH2n-2
Soluble except Ag - Pb - Ca - Sr Ba)
Insoluble except for nitrate and acetate

31. What is the energy you must put into a reaction to make it start called?
Identity and purity (impure compounds usually have broad & low melting points)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Initiation energy (NOT Ea)
Salt + water.

32. hydroxide
OH?
NO3?
water and substances with (s) less dense than
Salt + water

33. What is H2CO3 (carbonate acid) usually written as?
H2O + CO2 (it decomposes readily)
Transition element compounds (except if it has a full or empty d shell)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Anode - oxygen. Cathode - hydrogen

34. Color is due to ______ _______ of light.
Selective absorption
no - they're written undissociated (HAaq)
The Faraday or Faraday's constant.
redox reaction

35. dichromate (soln + most solids)
Orange
No - it depends on the number of ions produced on dissolving.
Acid rain - dissolves marble buildings/statues and kills trees.
Cr2O7²?

36. What element is used to vulcanize rubber?
Heat a test tube at an angle at the side of the tube (not bottom)
Making sigma bonds and holding lone pairs
bent
Sulfur

37. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Salt + water
Both electrons come from the same atom (just as good as a regular bond)

38. Generally - which oxy acid is strongest?
Kc=Kp
The one with most oxygen atoms (highest oxidation number)
+4-covalent - +2-ionic
The dilution effect when the solutions mix. M1V1 = M2V2

39. How many faradays of electric charge do you need to produce one mole of O2? H2?
OH?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
O2 needs 4F/mol H2 needs 2F/mol
Experimental mass/theoretical mass X 100

40. What is the conjugate acid of H2PO4?
Acid rain - dissolves marble buildings/statues and kills trees.
H3PO4
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
How close results are to the accepted value

41. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Salt + water.
A salt solution.
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)

42. What are the signs of ?G and E° for spontaneous reactions?
NH2?
SO4²?
?G=negative - E° must be positive
Q=It (time in seconds)

43. What are allotropes?
RX
Salt + water
different forms of the same element
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

44. carbonates
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Acids; HCOOCH3 is an ester
Insoluble except group 1 and ammonium
Read the bottom of the meniscus

45. Where are group I metals stored?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Group I metals (soft metals) are stored under oil
Glacial acetic acid
Most INsoluble except group 1 and ammonium

46. What is the general formula for a ketone?
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
it's lower and occurs over less sharp a range
?G= -ve - E°= +ve
RCOR

47. What type of solutions do small - highly charged cations tend to form?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Soluble
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
benzene has a delocalized pi ring structure

48. What do you use to look at burning magnesium? why?
White precipitate
atoms
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
blue glass - it filters UV

49. barium sulfate
Add acid to water so that the acid doesn't boil and spit
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
White precipitate
Distillation

50. chromate
water and substances with (s) less dense than
R=8.31 J/mol/K
CrO4²?
bases