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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. What is the name of S2Cl2? (Know how to name others like this - too)
a-IMFs - b-molecular volume
q=mc?T q=mL (or n x ?h)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Disulfur dichloride

2. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
benzene has a delocalized pi ring structure
They stay the same.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Transition element compounds (except if it has a full or empty d shell)

3. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
Insoluble except nitrate and acetate
Pipette (burette if need repetition)
H+

4. bromine
Insoluble
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
brown volatile liquid
?G=negative - E° must be positive

5. Can you collect soluble gases over water?
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?)
OH?
No - NH3 and HCl gases are extremely soluble
CnH2n+1 often designated 'R' ex C3H7 is propyl

6. What equipment do you need for a titration?
White precipitate
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
0.10M HCl (more ions)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

7. What is the third law of thermodynamics?
S crystal at 0K=0
CnH(2n+2)
ion pairing
'non-active' metals such as Cu - Ag - Au - Pt - etc.

8. What are the units of the first order rate constant?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
H+
CO3²?

9. Esters smell like _______ and amines smell like _______ and are ______.
PO4³?
fruit - fish - bases
CO2 and H2O
Glowing splint (positive result=relights)

10. What device would you use to measure a volume of gas?
Group I metals (soft metals) are stored under oil
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
They stay the same.
Eudiometer

11. Which alkali metals float on water?
Soluble
Check for air bubbles in the buret and remove the buret funnel from the buret
Salt + water.
All except for lithium

12. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
Most are soluble except Ag - Pb
hydroxides (ex: Ba(OH)2)
ion pairing

13. ammonium/ammonium compounds
Cr2O7²?
ethers
Soluble
Synthetic condensation polymer (aka a polyamide)

14. How many faradays of electric charge do you need to produce one mole of O2? H2?
different forms of the same element
O2 needs 4F/mol H2 needs 2F/mol
Group I metals (soft metals) are stored under oil
H+

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

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16. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
water and substances with (s) less dense than
Transition element compounds (except if it has a full or empty d shell)
Soluble
same KE - but PEice<PEwater

17. What apparatus do you use to separate 2 immiscible liquids?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Separating funnel
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
?H formation of an element in standard state=0

18. How does the melting point of a mixture compare to the MP of a pure substance?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
neutralization: high K - H2O product dissociation: low K - H2O reactant
it is lower and occurs over less sharp a range
PO4³?

19. chlorine
Greenish-yellow gas
RCOOH
Pale purple - (orange)-yellow - red - blue - green.
Distillation

20. What measuring device would you use for very small volumes of liquids?
bent
Eudiometer
Synthetic condensation polymer (aka a polyamide)
Pipette (burette if need repetition)

21. chromate ion (soln + most solids)
OH?
hydroxides (ex: Ba(OH)2)
yellow
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

22. copper sulfate
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
fractional distillation
blue
CnH2n-2

23. What word is a clue for a redox reaction?
H+
A salt solution.
Concentration
Acidified

24. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
R=8.31 J/mol/K
metal oxides and hydrides are ionically bonded and basic
Making sigma bonds and holding lone pairs

25. What type of metals don't react with water or acids to form H2?

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26. 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.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Graduated cylinder

27. Generally - which oxy acid is strongest?
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?)
Anode
The one with most oxygen atoms (highest oxidation number)
by electrolysis

28. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
ClO4?
Insoluble (except group 1 ammonium and Ba)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

29. What do you use to look at burning magnesium? why?
Q=It (time in seconds)
by electrolysis
blue glass - it filters UV
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

30. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
No - NH3 and HCl gases are extremely soluble
CO (poisonous)
A) any range. b) 8-10 c) 4-6

31. What type of compounds are almost always colored?
Kc=Kp
blue (BTB)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Transition element compounds (except if it has a full or empty d shell)

32. What is the formula for alkenes?
P2O5
Check for air bubbles in the buret and remove the buret funnel from the buret
Purple
CnH2n

33. What is the general formula for a ketone?
RCOR
Soluble
ClO?
metal oxides and hydrides are ionically bonded and basic

34. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
0.10M HCl (more ions)
Only temperature
Increases down group 1 decreases down group 17
water and substances with (s) less dense than

35. What do you need to make a polymer?
Mn²? - Cr³? - Cr³
No - NH3 and HCl gases are extremely soluble
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)
ion pairing

36. What is the basic structure of an optical isomer?
ion pairing
atoms
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Pale purple - (orange)-yellow - red - blue - green.

37. For a dibasic acid (H2A) - [A²?]= ____ ?
C4H10
The one with most oxygen atoms (highest oxidation number)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
K2

38. What is the second law of thermodynamics?
Iodine and CO2 (dry ice)
ethers
Suniverse increases for spontaneous processes
zero

39. silver iodide
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ion pairing
Pale yellow
q=mc?T q=mL (or n x ?h)

40. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
blue glass - it filters UV
a-IMFs - b-molecular volume
Check for air bubbles in the buret and remove the buret funnel from the buret

41. What is the word equation for condensation polymerisation ?
Selective absorption
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Greenish-yellow gas
An active metal.

42. At what point during titration do you have the perfect buffer - and what is the pH at this point?
ClO3?
At half equivalence - pH=pKa
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ROR

43. What is the charge on a chlorine atom?
zero
Combine the equations for the half reactions in the non-spontaneous direction
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
brown volatile liquid

44. What is the general formula for an amine?
RNH2
hydroxides (ex: Ba(OH)2)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Hg²?

45. cyanide
Reduction always takes place at the cathode (RED CAT) In both types of cell!
?G= -ve - E°= +ve
CN?
O2 needs 4F/mol H2 needs 2F/mol

46. What is precision?
The benzene ring (or more correctly the phenyl group - C6H5)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
How grouped results are
no - they're written undissociated (HAaq)

47. Acid plus base make?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
The one with most oxygen atoms (highest oxidation number)
S2O3²?
Salt + water.

48. How many ligands attach to a central ion in a complex ion?
A salt solution.
C2O4²?
#ligands=charge x2
Synthetic condensation polymer (aka a polyamide)

49. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
chemically (ex: with carbon)
it's lower and occurs over less sharp a range

50. If a free element is involved - what type of reaction must be involved?
redox reaction
C4H10
Eudiometer
same KE - but PEice<PEwater

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AP Chemistry 2

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