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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. What is the conjugate base of NH3?
?G=negative - E° must be positive
The compound with the lowest Ksp value.
NH2?
The one with most oxygen atoms (highest oxidation number)

2. What two compounds are great oxidizing agents?

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3. copper sulfate
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
a-IMFs - b-molecular volume
0 and 14
blue

4. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
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)
neutralization: high K - H2O product dissociation: low K - H2O reactant
The dilution effect when the solutions mix. M1V1 = M2V2

5. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Decant
boiling without losing volatile solvents/reactants
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
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

6. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
RCOOR
Ksp = s²
Group I metals (soft metals) are stored under oil

7. How many ligands attach to a central ion in a complex ion?
bright yellow
The Faraday or Faraday's constant.
#ligands=charge x2
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

8. Acid plus base make?
Perform ICE BOX calculation based on K1
Salt + water.
#ligands=charge x2
Cu3(PO4)2

9. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
It ceases - the circuit is broken.
An active metal.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

10. Is the ?H formation of an element in standard state zero?
CN?
RCOOR
Add acid to water so that the acid doesn't boil and spit
?H formation of an element in standard state=0

11. What is a coordinate covalent bond?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
H+
Both electrons come from the same atom (just as good as a regular bond)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

12. 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)
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.
Disulfur dichloride
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

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

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14. What part of a liquid do you look at to measure its volume?
linear
Read the bottom of the meniscus
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
All except for lithium

15. Does Kw increase or decrease with T? Why?
a-IMFs - b-molecular volume
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
it's lower and occurs over less sharp a range
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

16. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
basic
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
They decrease (or could be the same if the solid has ONLY JUST disappeared)

17. How can metals like iron and zinc be reduced?
Selective absorption
Q=It (time in seconds)
chemically (ex: with carbon)
blue glass - it filters UV

18. Name C7H16
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Experimental mass/theoretical mass X 100
No - it depends on the number of ions produced on dissolving.
Heptane

19. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
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)
RCOR
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

20. What process do you use to obtain the precipitate from a solution?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Filtration
CnH2n+2
RNH2

21. What is the formula for obtaining charge flowing in a cell?
strong acids/bases are written as H+ or OH- ions
Hg2²?
Q=It (time in seconds)
ion pairing

22. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Glowing splint (positive result=relights)
Ionic compounds
T increases exponentially the proportion of molecules with E > Ea

23. What complex ion does ammonia form with silver? copper? cadmium? zinc?
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)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
CN?
CO (poisonous)

24. Can you collect soluble gases over water?
blue
NH2?
No - NH3 and HCl gases are extremely soluble
blue glass - it filters UV

25. What is a dipeptide? polypeptide? protein?
Separating funnel
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Ksp = s²
boiling without losing volatile solvents/reactants

26. Give an example of a dilute strong acid.
Evaporation
HClO4
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
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.

27. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
K2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
No - NH3 and HCl gases are extremely soluble

28. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
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)

29. What shape is water?
Most are soluble except Ag - Pb
Ions go through the salt bridge - electrons go through metal wires in the external circuit
bent
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

30. What type of solutions do small - highly charged cations tend to form?
fractional distillation
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Read the bottom of the meniscus
non-metal oxides and hydrides are covalently bonded and are acidic.

31. What reacts with an acid to create hydrogen gas?
An active metal.
fractional distillation
K2
do not change

32. Buffer capacity must contain decent amounts of a ________ ________
Hg2²?
CO2 and H2O
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Conjugate pair (one must be a weak base or acid)

33. Is the freezing of ice endothermic or exothermic?
Ksp = s²
0 and 14
[A?]/[HA] x 100 or [BH?]/[B] x 100
Exothermic

34. mercury (I) ion
RX
Hg2²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
K1 x K2

35. What are allotropes?
Increases down group 1 decreases down group 17
different forms of the same element
It ceases - the circuit is broken.
S2O3²?

36. What things should you remember to do when collecting gas over water?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Products - reactants (except for BDE when it's reactants - products)
it's lower and occurs over less sharp a range
allow for the vapor pressure of water and make sure to level levels

37. Alkanes are _________ and react by _________
Evaporation
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)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Saturated - Substitution (which requires more radical conditions)

38. What is the conjugate acid of H2PO4?
small size and high charge
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
H3PO4
Sigma bonds are stronger than pi bonds

39. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
voltaic: + electrolytic: -
At half equivalence - pH=pKa

40. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ROR
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

41. What shape is methane?
benzene has a delocalized pi ring structure
Increases down group 1 decreases down group 17
Tetrahedral
zero-th: decreases - first: constant - second: increases

42. What is the test for hydrogen?
Making sigma bonds and holding lone pairs
At half equivalence - pH=pKa
lighted splint (positive result=pop)
C2O4²?

43. What do group I/II metal oxides and acids form?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
?G= -ve - E°= +ve
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Salt and water

44. What do group I/II metal oxides plus water form?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
0.10M HCl (more ions)
bases
Read the bottom of the meniscus

45. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
CO3²?
10?8
CO (poisonous)
Tetrahedral

46. Ions are not ______.
CnH2n+1 often designated 'R' ex C3H7 is propyl
Suniverse increases for spontaneous processes
atoms
Read the bottom of the meniscus

47. How are primary alcohols turned into acids?
acids
ROR
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

48. An amphiprotic (amphoteric) species is...
No - it depends on the number of ions produced on dissolving.
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
RCOOH
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

49. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Eudiometer
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

50. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Sulfur
Monomer + monomer = polymer product + a simple molecule such as water or HCl
acids

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AP Chemistry 2

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