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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 are primary alcohols turned into acids?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Trigonal pyramidal
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

2. 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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3. What are allotropes?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
different forms of the same element
Experimental mass/theoretical mass X 100
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

4. What is the formula of butane?
C4H10
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Q=It (time in seconds)

5. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
OH- and NH3
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
More chaotic (ex: gases made)

6. What is the formula for summation?

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7. When a cell is 'flat' What is its voltage?
zero
K1 x K2
acids
It ceases - the circuit is broken.

8. BaSO4
Insoluble
RCOOH
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

9. What do nonmetal oxides plus water form?
acids
a-IMFs - b-molecular volume
P2O5
Perform ICE BOX calculation based on K1

10. Which value of R do you use for all energy and kinetics calculations?
Conjugate pair (one must be a weak base or acid)
A) any range. b) 8-10 c) 4-6
R=8.31 J/mol/K
At half equivalence - pH=pKa

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

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12. What reacts with an acid to create hydrogen gas?
RNH2
An active metal.
boiling without losing volatile solvents/reactants
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

13. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
Molecules with the same molecular formulas - but different structural formulas
Big K=kf/kr
ClO2?

14. silver iodide
ClO2?
catalyst=conc H2SO4
Pale yellow
?H formation of an element in standard state=0

15. What is the second law of thermodynamics?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Suniverse increases for spontaneous processes
S crystal at 0K=0
Trigonal pyramidal

16. What is the general formula for an amine?
RNH2
Experimental mass/theoretical mass X 100
Heptane
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

17. How does half life change for zero-th order - first order - and second order processes?
ion pairing
Sigma bonds are stronger than pi bonds
zero-th: decreases - first: constant - second: increases
Pale yellow

18. barium sulfate
proton acceptor.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
White precipitate
At half equivalence - pH=pKa

19. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
ROH
ionic and form hydrogen and hydroxide
CH3COO?

20. What are two substances that sublime at 1 atm when heated?
Glowing splint (positive result=relights)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Iodine and CO2 (dry ice)
NH2?

21. Color (absorbance) is proportional to ________
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Concentration
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

22. What is reflux?
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?)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
NH2?
boiling without losing volatile solvents/reactants

23. During a titration what is present in the beaker at the equivalence point?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
A salt solution.
Soluble
chemically (ex: with carbon)

24. What is the difference between equivalence point and end point of a titration.
MnO4?
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
RCOR
But S° of element is not zero (except at 0K)

25. What is Big K in terms of kf and kr?
Big K=kf/kr
No - it depends on the number of ions produced on dissolving.
metal oxides and hydrides are ionically bonded and basic
it reacts by substitution NOT addition

26. hypochlorite
Group 1 hydroxides (ex: NaOH)
blue
ClO?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

27. What electrons are lost/gained first in transition element ions?
Glowing splint (positive result=relights)
ns² electrons (first in-first out)
RCOOR
Conjugate pair (one must be a weak base or acid)

28. copper sulfate
blue
Salt + water.
CN?
Mn²? - Cr³? - Cr³

29. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
RCOOR
left - ppt will form
?G=negative - E° must be positive

30. ammonium
Increases down group 1 decreases down group 17
NH4?
S2O3²?
look for changes in oxidation # - the one that goes up is oxidized and is the RA

31. Ions are not ______.
Making sigma bonds and holding lone pairs
Soluble except Ag - Pb - Ca - Sr Ba)
atoms
blue glass - it filters UV

32. carbonates
SO4²?
P2O5
Insoluble except group 1 and ammonium
Sigma bonds are stronger than pi bonds

33. What is the general formula of an alkane?
RCOOH
catalyst=conc H2SO4
NH2?
CnH(2n+2)

34. What is the formula for alkanes?
blue (BTB)
CnH2n+2
Ions go through the salt bridge - electrons go through metal wires in the external circuit
acids

35. What shape is carbon dioxide?
HClO4
Ksp = 108s5
linear
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

36. Generally - which oxy acid is strongest?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CrO4²?
The one with most oxygen atoms (highest oxidation number)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

37. Does Benzene react by addition or substitution?
chemically (ex: with carbon)
it reacts by substitution NOT addition
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Exothermic (?H for ANY sa/sb = -57kJ/mol)

38. nitrate
T increases exponentially the proportion of molecules with E > Ea
Ionic compounds
NO3?
Most INsoluble except group 1 and ammonium

39. What is the general formula for an ether?
Silvery gray solid - brown - purple
ROR
E=q + w (negative is by system - positive is on system)
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

40. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Filtration
Add acid to water so that the acid doesn't boil and spit
Silvery gray solid - brown - purple

41. Is the standard entropy (S°) of an element zero?
Eudiometer
But S° of element is not zero (except at 0K)
CH3COO?
They stay the same.

42. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
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)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ClO3?

43. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Soluble except Ag - Pb - Ca - Sr Ba)
Initiation energy (NOT Ea)
Ksp = 108s5
Suniverse increases for spontaneous processes

44. What causes the dramatic effect of T on rate?
RCOOH
Experimental mass/theoretical mass X 100
Ppt will NOT form (unsaturated)
T increases exponentially the proportion of molecules with E > Ea

45. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
The compound with the lowest Ksp value.
Synthesis - separation and purification of the product and its identification.
Kc=Kp
it's lower and occurs over less sharp a range

46. What process do you use to separate two liquids with different boiling points?
Nothing
RCOOR
Concentration
fractional distillation

47. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
redox reaction
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Kc=Kp

48. An amphiprotic (amphoteric) species is...
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?)
ClO2?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

49. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
CnH2n+2
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)
Salt + water.

50. What is the general formula for an ester?
|experimental - accepted|/accepted X 100
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
0 and 14
RCOOR