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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Glowing splint (positive result=relights)
bright yellow
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)

2. Does reactivity increase/decrease going down group 1 and group 17?
Synthesis - separation and purification of the product and its identification.
it is lower and occurs over less sharp a range
R=8.31 J/mol/K
Increases down group 1 decreases down group 17

3. What type of polymer is nylon?
R=8.31 J/mol/K
Only temperature
Sulfur
Synthetic condensation polymer (aka a polyamide)

4. What is the catalyst for this reaction Ester + ?
Hg²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H2PO4?
catalyst=conc H2SO4

5. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
RCOOR
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Anode
K1 x K2

6. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
atoms
linear

7. What is the conjugate base of NH3?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
red - green - blue
it is lower and occurs over less sharp a range
NH2?

8. Is the standard entropy (S°) of an element zero?
Acidified
Pipette (burette if need repetition)
ethers
But S° of element is not zero (except at 0K)

9. What is the second law of thermodynamics?
CrO4²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Suniverse increases for spontaneous processes
Ksp = 4s³

10. nitrates
Soluble
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ClO3?
ClO2?

11. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
zero-th: decreases - first: constant - second: increases
Trigonal pyramidal
They stay the same.

12. Alkanes are _________ and react by _________
Identity and purity (impure compounds usually have broad & low melting points)
Saturated - Substitution (which requires more radical conditions)
NH4?
Products - reactants (except for BDE when it's reactants - products)

13. What do the 'a' and 'b' in Van Der Waal's equation allow for?
RCOOH
Mono; di; tri; tetra; penta; hexa.
a-IMFs - b-molecular volume
benzene has a delocalized pi ring structure

14. What is precision?
How grouped results are
Reduction always takes place at the cathode (RED CAT) In both types of cell!
K1 x K2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

15. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Insoluble
E=q + w (negative is by system - positive is on system)
At half equivalence - pH=pKa
They stay the same.

16. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
ionic and form hydrogen and hydroxide
The one with most oxygen atoms (highest oxidation number)
Iodine and CO2 (dry ice)
same KE - but PEice<PEwater

17. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
zero
ethers
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

18. Give an example of a concentrated weak acid.
Glacial acetic acid
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
The benzene ring (or more correctly the phenyl group - C6H5)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

19. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Tetrahedral
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Insoluble except group 1 and ammonium

20. BaSO4
Molecules with the same molecular formulas - but different structural formulas
R=8.31 J/mol/K
Insoluble
Selective absorption

21. How do you find the pH for a dibasic acid? (H2A)?
Only temperature
E=q + w (negative is by system - positive is on system)
Synthesis - separation and purification of the product and its identification.
Perform ICE BOX calculation based on K1

22. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
proton acceptor.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
bases

23. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
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
Cu3(PO4)2
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Current - time and charge on ion (moles of e used in half cell reaction)

24. Both Acetic acid and ____________ are also functional isomers.
methyl formate
10?8
Insoluble except for nitrate and acetate
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

25. cyanide
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CnH2n-2
CN?

26. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
ethers
RX

27. What are isotopes?
zero
Pale yellow
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
RCOOH

28. What value of R do you use for thermo calculations? gas calculations?
proton donor base
lighted splint (positive result=pop)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Trigonal pyramidal

29. What do you need to make a polymer?
Unsaturated - addition (ex: decolorize bromine solution)
+4-covalent - +2-ionic
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)
do not change

30. What do group I/II metal oxides plus water form?
Salts (ex: CaO + SO2 ? CaSO3)
Molecules with the same molecular formulas - but different structural formulas
zero
bases

31. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
fractional distillation
It ceases - the circuit is broken.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
R=8.31 J/mol/K

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

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33. What two types of substances are present in all redox reactions?
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)
an oxidized and reduced substance
Combine the equations for the half reactions in the non-spontaneous direction
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

34. Esterification is...
RCOR
E=q + w (negative is by system - positive is on system)
Tetrahedral
acid + alcohol

35. What are the signs of ?G and E° for spontaneous reactions?
linear
Glacial acetic acid
?G=negative - E° must be positive
Current - time and charge on ion (moles of e used in half cell reaction)

36. nitrate
NH2?
OH- and NH3
Transition element compounds (except if it has a full or empty d shell)
NO3?

37. What is HCOOCH3?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Acids; HCOOCH3 is an ester
[A?]/[HA] x 100 or [BH?]/[B] x 100

38. What kind of bonding structure does benzene have?
Selective absorption
But S° of element is not zero (except at 0K)
benzene has a delocalized pi ring structure
Experimental mass/theoretical mass X 100

39. 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?
White precipitate
Concentration
ion pairing
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

40. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
catalyst=conc H2SO4
Salt and water
Most INsoluble except group 1 and ammonium
water and substances with (s) less dense than

41. What is the word equation for condensation polymerisation ?
RCHO (carbonyl at end)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Soluble
allow for the vapor pressure of water and make sure to level levels

42. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
an oxidized and reduced substance
The dilution effect when the solutions mix. M1V1 = M2V2
ion pairing

43. What is a coordinate covalent bond?
CO3²?
Hg2²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Both electrons come from the same atom (just as good as a regular bond)

44. What are amphoteric oxides?
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?)
acid + alcohol
redox reaction
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

45. For a dibasic acid (H2A) - [A²?]= ____ ?
Filtration
ClO2?
C4H10
K2

46. What is the general formula for an ether?
ROR
CnH2n+2
Exothermic (?H for ANY sa/sb = -57kJ/mol)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

47. Color is due to ______ _______ of light.
Soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Selective absorption
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

48. What element is used to vulcanize rubber?
Sulfur
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
H+
H2PO4?

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

50. What type of compounds do metals/non metals form?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ionic compounds
ns² electrons (first in-first out)

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AP Chemistry 2

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