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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
yellow
-Ea/R
voltaic: + electrolytic: -

2. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Heptane
Experimental mass/theoretical mass X 100
OH- and NH3
H+

3. What are the formulas for q?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
q=mc?T q=mL (or n x ?h)
P2O5
Molecules with the same molecular formulas - but different structural formulas

4. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
it is lower and occurs over less sharp a range
Mn²? - Cr³? - Cr³
Reduction always takes place at the cathode (RED CAT) In both types of cell!

5. Acid plus base make?
Salt + water.
Decant
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
+4-covalent - +2-ionic

6. How do you find the pH for a dibasic acid? (H2A)?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Big K=kf/kr
Perform ICE BOX calculation based on K1

7. What is the pH of 1.0M HCl? 1M NaOH?
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
-Ea/R
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

8. What do group I/II metal oxides and acids form?
ClO4?
methyl formate
CnH2n
Salt and water

9. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
acids
do not change
lighted splint (positive result=pop)
small size and high charge

10. Which alkali metals float on water?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
All except for lithium
Suniverse increases for spontaneous processes
T increases exponentially the proportion of molecules with E > Ea

11. What is the second law of thermodynamics?
Trigonal pyramidal
Add acid to water so that the acid doesn't boil and spit
Suniverse increases for spontaneous processes
CnH(2n+2)

12. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
White precipitate
An active metal.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

13. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Insoluble (except group 1 ammonium and Ba)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Iodine and CO2 (dry ice)

14. Why are i factors (Van't Hoff factors) often less than ideal?
A) any range. b) 8-10 c) 4-6
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ion pairing
Insoluble except group 1 and ammonium

15. What is the test for oxygen?
NO3?
Glowing splint (positive result=relights)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Soluble

16. chromate ion (soln + most solids)
yellow
At half equivalence - pH=pKa
Ksp = s²
K2

17. What is the general formula for a ketone?
bases
RCOR
Heat a test tube at an angle at the side of the tube (not bottom)
Selective absorption

18. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
HClO4
a-IMFs - b-molecular volume
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

19. What are allotropes?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Soluble
different forms of the same element
ethers

20. Give an example of a concentrated weak acid.
Glacial acetic acid
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
yellow
CO3²?

21. What is HCOOCH3?
RCHO (carbonyl at end)
Acids; HCOOCH3 is an ester
Selective absorption
Both electrons come from the same atom (just as good as a regular bond)

22. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
boiling without losing volatile solvents/reactants
an oxidized and reduced substance
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acid rain - dissolves marble buildings/statues and kills trees.

23. 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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24. halides
blue
Most are soluble except Ag - Pb
Hg2²?
it's lower and occurs over less sharp a range

25. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
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)
CnH2n
How close results are to the accepted value

26. Why are noble gases stable?
Making sigma bonds and holding lone pairs
CO (poisonous)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

27. Acids + Carbonates (bicarbonates) make?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
basic
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
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

28. How are primary alcohols turned into acids?
CO3²?
RCHO (carbonyl at end)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
More chaotic (ex: gases made)

29. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Soluble except Ag - Pb - Ca - Sr Ba)
NH2?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

30. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
All except for lithium
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
diamond and graphite

31. What steps do organic labs consist of?
Tetrahedral
Orange
Synthesis - separation and purification of the product and its identification.
T increases exponentially the proportion of molecules with E > Ea

32. acetates
Soluble
SO4²?
Heptane
PO4³?

33. carbonates
ClO2?
Filtration
Insoluble except group 1 and ammonium
?G=negative - E° must be positive

34. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
metal oxides and hydrides are ionically bonded and basic
?G= -ve - E°= +ve
Pale purple - (orange)-yellow - red - blue - green.
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?)

35. How are more active metals reduced?
by electrolysis
ion pairing
?G=negative - E° must be positive
CnH2n+1 often designated 'R' ex C3H7 is propyl

36. Which value of R do you use for all energy and kinetics calculations?
acid + alcohol
Insoluble except for nitrate and acetate
R=8.31 J/mol/K
No - it depends on the number of ions produced on dissolving.

37. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
The dilution effect when the solutions mix. M1V1 = M2V2
Greenish-yellow gas
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
Perform ICE BOX calculation based on K1

38. What is reflux?
boiling without losing volatile solvents/reactants
Big K=kf/kr
E=q + w (negative is by system - positive is on system)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

39. What are isotopes?
Pale yellow
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
neutralization: high K - H2O product dissociation: low K - H2O reactant
ClO4?

40. Neutralization is an ________ reaction.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ROH

41. Are weak acids (and bases) written dissociated?

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42. permanganate
Cu3(PO4)2
MnO4?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Ionic compounds

43. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
CnH2n-2
A) any range. b) 8-10 c) 4-6
An active metal.
Acid rain - dissolves marble buildings/statues and kills trees.

44. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
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
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Iodine and CO2 (dry ice)

45. What is the energy you must put into a reaction to make it start called?
water and substances with (s) less dense than
same KE - but PEice<PEwater
Initiation energy (NOT Ea)
Mn²? - Cr³? - Cr³

46. Both Acetic acid and ____________ are also functional isomers.
ethers
red - green - blue
methyl formate
It ceases - the circuit is broken.

47. mercury (I) ion
Silvery gray solid - brown - purple
Anode - oxygen. Cathode - hydrogen
Hg2²?
E=q + w (negative is by system - positive is on system)

48. Do anions flow to the cathode or anode?
Anode
S2O3²?
Pale yellow
?H-kJ - ?S-J - ?G-kJ

49. What is the conjugate acid of H2PO4?
But S° of element is not zero (except at 0K)
Check for air bubbles in the buret and remove the buret funnel from the buret
H3PO4
CO2 and H2O

50. What is the basic structure of an optical isomer?
At half equivalence - pH=pKa
S2O3²?
same KE - but PEice<PEwater
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.