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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. How do you find the pH for a dibasic acid? (H2A)?
Heptane
Perform ICE BOX calculation based on K1
?G=negative - E° must be positive
neutralization: high K - H2O product dissociation: low K - H2O reactant

2. What is Big K in terms of kf and kr?
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)
acid + alcohol
Big K=kf/kr
benzene has a delocalized pi ring structure

3. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
0 and 14
Add acid to water so that the acid doesn't boil and spit
neutralization: high K - H2O product dissociation: low K - H2O reactant
NH4?

4. carbonate
CO3²?
ClO?
Big K=kf/kr
Time?¹ - (ex. s?¹ - hr?¹ - etc)

5. Both Acetic acid and ____________ are also functional isomers.
methyl formate
allow for the vapor pressure of water and make sure to level levels
catalyst=conc H2SO4
Increases down group 1 decreases down group 17

6. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
zero-th: decreases - first: constant - second: increases
A) any range. b) 8-10 c) 4-6
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

7. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
0 and 14
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Ksp = 27s4

8. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
ClO4?
zero
Ksp = s²
Glacial acetic acid

9. Can you collect soluble gases over water?
The Faraday or Faraday's constant.
No - NH3 and HCl gases are extremely soluble
0 and 14
Exothermic

10. At what point during titration do you have the perfect buffer - and what is the pH at this point?
CnH2n-2
brown volatile liquid
allow for the vapor pressure of water and make sure to level levels
At half equivalence - pH=pKa

11. Is the standard entropy (S°) of an element zero?
Pale purple - (orange)-yellow - red - blue - green.
RNH2
CnH2n
But S° of element is not zero (except at 0K)

12. Acids + Carbonates (bicarbonates) make?
RCOOH
Evaporation
Check for air bubbles in the buret and remove the buret funnel from the buret
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

13. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
fractional distillation
Initiation energy (NOT Ea)

14. The oxidation # for acid base reactions...
CnH(2n+2)
RCOOH
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
do not change

15. How are more active metals reduced?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
acids
by electrolysis
yellow

16. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H2O + CO2 (it decomposes readily)
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.
H+
'non-active' metals such as Cu - Ag - Au - Pt - etc.

17. What process do you use to obtain the solute from a solution?
a-IMFs - b-molecular volume
Evaporation
bases
Soluble

18. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Q=It (time in seconds)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Eudiometer
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)

19. What is the test for hydrogen?
Molecules with the same molecular formulas - but different structural formulas
Pour liquids using a funnel or down a glass rod
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.
lighted splint (positive result=pop)

20. chlorine
Glacial acetic acid
Greenish-yellow gas
RCHO (carbonyl at end)
ion pairing

21. Do you use J or kJ for ?H - ?S - and ?G?
Conjugate pair (one must be a weak base or acid)
P2O5
methyl formate
?H-kJ - ?S-J - ?G-kJ

22. chlorite
E=q + w (negative is by system - positive is on system)
ClO2?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH(2n+2)

23. If Q < Ksp a ppt ______
ethers
Ppt will NOT form (unsaturated)
Insoluble
fruit - fish - bases

24. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Only temperature
methyl formate
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
basic

25. What is the formula of butane?
allow for the vapor pressure of water and make sure to level levels
Concentration
C4H10
Group 1 hydroxides (ex: NaOH)

26. What word is a clue for a redox reaction?
Acidified
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
zero
The compound with the lowest Ksp value.

27. What is the basic structure of an optical isomer?
benzene is less reactive than alkenes
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acids; HCOOCH3 is an ester

28. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
RCOR
water and substances with (s) less dense than
Mono; di; tri; tetra; penta; hexa.

29. What kind of bonding structure does benzene have?
R=8.31 J/mol/K
Cu3(PO4)2
benzene has a delocalized pi ring structure
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

30. What is the general formula for an alcohol?
bases
small size and high charge
C2O4²?
ROH

31. When a cell is 'flat' What is its voltage?
?G=negative - E° must be positive
zero
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
strong acids/bases are written as H+ or OH- ions

32. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
The compound with the lowest Ksp value.
H3PO4

33. Lattice energy is high for ions with _____ size and _____ charge
A salt solution.
0.10M HCl (more ions)
small size and high charge
Acidified

34. What process do you use to obtain a solvent from a solution?
diamond and graphite
Kc=Kp
neutralization: high K - H2O product dissociation: low K - H2O reactant
Distillation

35. What do you use for an acid spill? base spill?
Soluble
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
The Faraday or Faraday's constant.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

36. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
?H-kJ - ?S-J - ?G-kJ
Ksp = 4s³
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
CnH2n

37. What part of a liquid do you look at to measure its volume?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Read the bottom of the meniscus
it reacts by substitution NOT addition
boiling without losing volatile solvents/reactants

38. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
Synthetic condensation polymer (aka a polyamide)
Iodine and CO2 (dry ice)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

39. Nonmetals are good _____ agents. Metals are good _______ agents.
proton donor base
S2O3²?
Insoluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

40. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
O2 needs 4F/mol H2 needs 2F/mol
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
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.
basic

41. Alcohols and _______ are FG isomers
ethers
Read the bottom of the meniscus
K1 x K2
The one with most oxygen atoms (highest oxidation number)

42. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Hg²?
neutralization: high K - H2O product dissociation: low K - H2O reactant
It ceases - the circuit is broken.

43. dichromate
no - they're written undissociated (HAaq)
acids
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
Cr2O7²?

44. Buffer capacity must contain decent amounts of a ________ ________
How grouped results are
Conjugate pair (one must be a weak base or acid)
ClO?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

45. Ions are not ______.
Ksp = 108s5
atoms
strong acids/bases are written as H+ or OH- ions
S crystal at 0K=0

46. What is the conjugate base of NH3?
Combine the equations for the half reactions in the non-spontaneous direction
NH2?
water and substances with (s) less dense than
Purple

47. What shape is carbon dioxide?
Salt + water.
Ksp = 27s4
ns² electrons (first in-first out)
linear

48. What do you use to look at burning magnesium? why?
same KE - but PEice<PEwater
?H formation of an element in standard state=0
Pale yellow
blue glass - it filters UV

49. What is the second law of thermodynamics?
Silvery gray solid - brown - purple
yellow
Suniverse increases for spontaneous processes
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

50. bromothymol
blue (BTB)
Decant
RCOOR
HClO4

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AP Chemistry 2

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