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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. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Salt + water
water and substances with (s) less dense than
[A?]/[HA] x 100 or [BH?]/[B] x 100
linear

2. What is the catalyst for this reaction Ester + ?
PO4³?
catalyst=conc H2SO4
Selective absorption
Both electrons come from the same atom (just as good as a regular bond)

3. What do you do to get rid of most of the solution from a precipitate?
Decant
Check for air bubbles in the buret and remove the buret funnel from the buret
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Insoluble except nitrate and acetate

4. What is the test for oxygen?
boiling without losing volatile solvents/reactants
Add acid to water so that the acid doesn't boil and spit
Glowing splint (positive result=relights)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

5. What value of R do you use for thermo calculations? gas calculations?
yellow
C4H10
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
proton acceptor.

6. What shape is methane?
Glowing splint (positive result=relights)
Sigma bonds are stronger than pi bonds
voltaic: - electrolytic: +
Tetrahedral

7. What causes the dramatic effect of T on rate?
non-metal oxides and hydrides are covalently bonded and are acidic.
Orange
[A?]/[HA] x 100 or [BH?]/[B] x 100
T increases exponentially the proportion of molecules with E > Ea

8. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Tetrahedral
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
|experimental - accepted|/accepted X 100
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

9. What is the general formula for an aldehyde?
ionic and form hydrogen and hydroxide
Suniverse increases for spontaneous processes
RCHO (carbonyl at end)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

10. What is the general formula for an ether?
Cr2O7²?
linear
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
ROR

11. An amphiprotic (amphoteric) species is...
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CO (poisonous)
Ionic compounds

12. Color (absorbance) is proportional to ________
Nothing
Concentration
zero
ClO3?

13. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Molecules with the same molecular formulas - but different structural formulas
Anode - oxygen. Cathode - hydrogen
Combine the equations for the half reactions in the non-spontaneous direction
water and substances with (s) less dense than

14. bromothymol
ethers
blue (BTB)
Initiation energy (NOT Ea)
ClO2?

15. lead compounds
Insoluble except nitrate and acetate
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
small size and high charge
Iodine and CO2 (dry ice)

16. 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?
RCHO (carbonyl at end)
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
Distillation
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

17. What is the difference between equivalence point and end point of a titration.
neutralization: high K - H2O product dissociation: low K - H2O reactant
#ligands=charge x2
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
Transition element compounds (except if it has a full or empty d shell)

18. What type of compounds do metals/non metals form?
No - it depends on the number of ions produced on dissolving.
Ionic compounds
proton acceptor.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

19. When is ?G zero?
RCOOH
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Glowing splint (positive result=relights)

20. Buffer capacity must contain decent amounts of a ________ ________
CnH2n+1 often designated 'R' ex C3H7 is propyl
Most INsoluble except group 1 and ammonium
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)
Conjugate pair (one must be a weak base or acid)

21. Esters smell like _______ and amines smell like _______ and are ______.
Suniverse increases for spontaneous processes
Ksp = 4s³
NH4?
fruit - fish - bases

22. What are allotropes?
chemically (ex: with carbon)
different forms of the same element
zero
hydroxides (ex: Ba(OH)2)

23. Alkenes are ________ and react by __________
Add acid to water so that the acid doesn't boil and spit
Unsaturated - addition (ex: decolorize bromine solution)
zero
Read the bottom of the meniscus

24. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
0.10M HCl (more ions)
allow for the vapor pressure of water and make sure to level levels
basic
Read the bottom of the meniscus

25. Does Kw increase or decrease with T? Why?
At half equivalence - pH=pKa
Salts (ex: CaO + SO2 ? CaSO3)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
K2

26. If Q > Ksp - then system shifts _______ and ppt ______
Salts (ex: CaO + SO2 ? CaSO3)
Transition element compounds (except if it has a full or empty d shell)
left - ppt will form
Cr2O7²?

27. cyanide
CN?
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.
Distillation
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

28. What do the 'a' and 'b' in Van Der Waal's equation allow for?
OH?
a-IMFs - b-molecular volume
Increases down group 1 decreases down group 17
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

29. How do you get Ecell for spontaneous reactions?
Saturated - Substitution (which requires more radical conditions)
Exothermic
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Eudiometer

30. What is H2CO3 (carbonate acid) usually written as?
H2O + CO2 (it decomposes readily)
CnH2n+2
water and substances with (s) less dense than
Unsaturated - addition (ex: decolorize bromine solution)

31. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
zero
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
water and substances with (s) less dense than

32. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Distillation
Pale yellow

33. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble except Ag - Pb - Ca - Sr Ba)
neutralization: high K - H2O product dissociation: low K - H2O reactant
PO4³?

34. Name 2 ways in which you can create a buffer?
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)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Making sigma bonds and holding lone pairs
?H-kJ - ?S-J - ?G-kJ

35. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Ionic compounds
?G=negative - E° must be positive
Ksp = s²

36. When driving off water from a hydrate - how do you tell you're done?
ROH
brown volatile liquid
Big K=kf/kr
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

37. How are primary alcohols turned into acids?
water and substances with (s) less dense than
More chaotic (ex: gases made)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
CnH(2n+2)

38. chlorite
yellow
ClO2?
RCOOH
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

39. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Acid rain - dissolves marble buildings/statues and kills trees.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Selective absorption

40. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
E=q + w (negative is by system - positive is on system)
ROH
Check for air bubbles in the buret and remove the buret funnel from the buret

41. What is the third law of thermodynamics?
RCOOH
it is lower and occurs over less sharp a range
voltaic: - electrolytic: +
S crystal at 0K=0

42. What process do you use to obtain the solute from a solution?
fractional distillation
Evaporation
Initiation energy (NOT Ea)
zero-th: decreases - first: constant - second: increases

43. What is the test for hydrogen?
lighted splint (positive result=pop)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
boiling without losing volatile solvents/reactants

44. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
redox reaction
water and substances with (s) less dense than
allow for the vapor pressure of water and make sure to level levels

45. Name C7H16
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Heptane
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Greenish-yellow gas

46. What is the formula for alkynes?
CnH2n-2
same KE - but PEice<PEwater
OH?
RNH2

47. Lattice energy is high for ions with _____ size and _____ charge
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Soluble
metal oxides and hydrides are ionically bonded and basic
small size and high charge

48. What are the names and formulas of the 6 strong acids?
?H-kJ - ?S-J - ?G-kJ
Monomer + monomer = polymer product + a simple molecule such as water or HCl
are less dense than water
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

49. What is the first law of thermodynamics?
T increases exponentially the proportion of molecules with E > Ea
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
RCOR
E=q + w (negative is by system - positive is on system)

50. What do metal oxides plus non- metal oxides form?
Ksp = 108s5
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
P2O5
Salts (ex: CaO + SO2 ? CaSO3)