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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. halides
Group I metals (soft metals) are stored under oil
Most are soluble except Ag - Pb
bent
C4H10

2. What do group I/II metal oxides and acids form?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Tetrahedral
It ceases - the circuit is broken.
Salt and water

3. What do group I/II metal oxides plus water form?
bases
Making sigma bonds and holding lone pairs
hydroxides (ex: Ba(OH)2)
Distillation

4. Color is due to ______ _______ of light.
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
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
ethers
Selective absorption

5. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
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.
CrO4²?

6. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
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
Insoluble
left - ppt will form

7. What shape is carbon dioxide?
linear
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Glacial acetic acid
CN?

8. What is H2CO3 (carbonate acid) usually written as?
Ksp = s²
Ions go through the salt bridge - electrons go through metal wires in the external circuit
0.10M HCl (more ions)
H2O + CO2 (it decomposes readily)

9. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
linear
Exothermic (?H for ANY sa/sb = -57kJ/mol)
C2O4²?

10. What is the test for hydrogen?
q=mc?T q=mL (or n x ?h)
RX
lighted splint (positive result=pop)
Evaporation

11. What type of compounds do metals/non metals form?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ionic compounds
hydroxides (ex: Ba(OH)2)
Anode - oxygen. Cathode - hydrogen

12. How do you get Ecell for spontaneous reactions?
Perform ICE BOX calculation based on K1
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Increases down group 1 decreases down group 17
An active metal.

13. silver compounds
Unsaturated - addition (ex: decolorize bromine solution)
red - green - blue
Pale purple - (orange)-yellow - red - blue - green.
Insoluble except for nitrate and acetate

14. permanganate
MnO4?
K1 x K2
Tetrahedral
Sigma bonds are stronger than pi bonds

15. What is the difference between equivalence point and end point of a titration.
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
OH- and NH3
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
All except for lithium

16. What things should you remember to do when collecting gas over water?
H2PO4?
Distillation
allow for the vapor pressure of water and make sure to level levels
Eudiometer

17. What measuring device would you use for very small volumes of liquids?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
C4H10
Pipette (burette if need repetition)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

18. What process do you use to obtain the solute from a solution?
allow for the vapor pressure of water and make sure to level levels
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.
Evaporation
No - NH3 and HCl gases are extremely soluble

19. What is the formula of copper (II) phosphate?
The one with most oxygen atoms (highest oxidation number)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Cu3(PO4)2
voltaic: + electrolytic: -

20. Why are i factors (Van't Hoff factors) often less than ideal?
ClO?
allow for the vapor pressure of water and make sure to level levels
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
ion pairing

21. An amphiprotic (amphoteric) species is...
But S° of element is not zero (except at 0K)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Purple
ns² electrons (first in-first out)

22. What is accuracy?
SO4²?
How close results are to the accepted value
methyl formate
Silvery gray solid - brown - purple

23. What do acids plus active metals form?
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
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
How grouped results are
Cr2O7²?

24. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
The dilution effect when the solutions mix. M1V1 = M2V2
Soluble

25. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
+4-covalent - +2-ionic
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero
E=q + w (negative is by system - positive is on system)

26. cyanide
MnO4?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Unsaturated - addition (ex: decolorize bromine solution)
CN?

27. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
C4H10
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
H2PO4?
basic

28. What is the formula for alkenes?
Mono; di; tri; tetra; penta; hexa.
CnH2n
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Anode

29. What is Big K in terms of kf and kr?
Big K=kf/kr
fruit - fish - bases
are less dense than water
an oxidized and reduced substance

30. What electrons are lost/gained first in transition element ions?
OH?
basic
OH- and NH3
ns² electrons (first in-first out)

31. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
a-IMFs - b-molecular volume
Ksp = 27s4
SO4²?

32. What is the basic structure of an optical isomer?
ClO4?
Ksp = 4s³
Eudiometer
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

33. If a free element is involved - what type of reaction must be involved?
redox reaction
Perform ICE BOX calculation based on K1
The benzene ring (or more correctly the phenyl group - C6H5)
small size and high charge

34. What part of a liquid do you look at to measure its volume?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Glacial acetic acid
Read the bottom of the meniscus
diamond and graphite

35. What is the formula for percent error?
acids
Kc=Kp
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
|experimental - accepted|/accepted X 100

36. When can supercooling occur? What does it look like on a cooling curve?

37. How many ligands attach to a central ion in a complex ion?
q=mc?T q=mL (or n x ?h)
#ligands=charge x2
Products - reactants (except for BDE when it's reactants - products)
K1 x K2

38. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
bright yellow
CN?
A) any range. b) 8-10 c) 4-6

39. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
blue (BTB)
At half equivalence - pH=pKa
same KE - but PEice<PEwater
S2O3²?

40. What is the sign of the anode in voltaic cells? in electrolytic cells?
Combine the equations for the half reactions in the non-spontaneous direction
voltaic: - electrolytic: +
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Group 1 hydroxides (ex: NaOH)

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

42. mercury (II) ion
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Hg²?
left - ppt will form
It ceases - the circuit is broken.

43. What are hybrid orbitals used for?
No - NH3 and HCl gases are extremely soluble
Making sigma bonds and holding lone pairs
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

44. What should you check for before you begin titrating?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Check for air bubbles in the buret and remove the buret funnel from the buret
Mono; di; tri; tetra; penta; hexa.
But S° of element is not zero (except at 0K)

45. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Sulfur
Orange
Cr2O7²?

46. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Anode
zero-th: decreases - first: constant - second: increases
Sigma bonds are stronger than pi bonds

47. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Ksp = 108s5
brown volatile liquid
Cr2O7²?

48. What shape is ammonia?
zero
Trigonal pyramidal
by electrolysis
Perform ICE BOX calculation based on K1

49. What are two substances that sublime at 1 atm when heated?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
MnO4?
Iodine and CO2 (dry ice)
Pale purple - (orange)-yellow - red - blue - green.

50. What is reflux?
boiling without losing volatile solvents/reactants
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Iodine and CO2 (dry ice)
Most INsoluble except group 1 and ammonium