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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. What is the name of S2Cl2? (Know how to name others like this - too)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Disulfur dichloride

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

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3. What do the 'a' and 'b' in Van Der Waal's equation allow for?
blue glass - it filters UV
a-IMFs - b-molecular volume
Sigma bonds are stronger than pi bonds
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

4. When driving off water from a hydrate - how do you tell you're done?
Exothermic
Cu3(PO4)2
HClO4
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

5. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Add acid to water so that the acid doesn't boil and spit
Suniverse increases for spontaneous processes
water and substances with (s) less dense than

6. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble except group 1 and ammonium
No - it depends on the number of ions produced on dissolving.
Ksp = 4s³

7. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Evaporation
Ionic compounds
Identity and purity (impure compounds usually have broad & low melting points)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

8. chromate ion (soln + most solids)
Disulfur dichloride
yellow
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Group I metals (soft metals) are stored under oil

9. Acid plus base make?
All except for lithium
Salt + water.
Conjugate pair (one must be a weak base or acid)
Group 1 hydroxides (ex: NaOH)

10. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
voltaic: + electrolytic: -
The one with most oxygen atoms (highest oxidation number)
Read the bottom of the meniscus

11. How do you find the pH for a dibasic acid? (H2A)?
allow for the vapor pressure of water and make sure to level levels
Pipette (burette if need repetition)
Perform ICE BOX calculation based on K1
C4H10

12. A Bronsted-Lowry base is...
it reacts by substitution NOT addition
proton acceptor.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
fractional distillation

13. What is the third law of thermodynamics?
S crystal at 0K=0
An active metal.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Making sigma bonds and holding lone pairs

14. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
C4H10
blue glass - it filters UV
same KE - but PEice<PEwater

15. What do you do to get rid of most of the solution from a precipitate?
Decant
They stay the same.
Hg²?
Read the bottom of the meniscus

16. What electrons are lost/gained first in transition element ions?
K1 x K2
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.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
ns² electrons (first in-first out)

17. Is the freezing of ice endothermic or exothermic?
fruit - fish - bases
More chaotic (ex: gases made)
Exothermic
RCOOR

18. What is the formula for alkanes?
an oxidized and reduced substance
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
CnH2n+2

19. How do you dilute an acid?

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20. primary colors
red - green - blue
Only temperature
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Soluble except Ag - Pb - Ca - Sr Ba)

21. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
The one with most oxygen atoms (highest oxidation number)
Concentration
P2O5
hydroxides (ex: Ba(OH)2)

22. What is a coordinate covalent bond?
0 and 14
Both electrons come from the same atom (just as good as a regular bond)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Distillation

23. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
SO4²?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Soluble
NH2?

24. One mole of electrons carries 96500Coulombs - what is this quantity called?

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25. What things should you remember to do when collecting gas over water?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
allow for the vapor pressure of water and make sure to level levels
proton acceptor.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

26. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
it reacts by substitution NOT addition
Ksp = 108s5
Acidified
T increases exponentially the proportion of molecules with E > Ea

27. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
a-IMFs - b-molecular volume
Synthetic condensation polymer (aka a polyamide)

28. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
benzene is less reactive than alkenes
Kc=Kp
neutralization: high K - H2O product dissociation: low K - H2O reactant

29. What is the general formula for alkyl halides?
CrO4²?
RX
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

30. What is the formula for alkynes?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
allow for the vapor pressure of water and make sure to level levels
CnH2n-2
NO3?

31. Is the standard entropy (S°) of an element zero?
Synthetic condensation polymer (aka a polyamide)
But S° of element is not zero (except at 0K)
A salt solution.
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.

32. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Concentration
allow for the vapor pressure of water and make sure to level levels
No - it depends on the number of ions produced on dissolving.

33. How many faradays of electric charge do you need to produce one mole of O2? H2?
Sulfur
It ceases - the circuit is broken.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
O2 needs 4F/mol H2 needs 2F/mol

34. Esters smell like _______ and amines smell like _______ and are ______.
#ligands=charge x2
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)
fruit - fish - bases
Salt + water.

35. Alkenes are ________ and react by __________
Monomer + monomer = polymer product + a simple molecule such as water or HCl
allow for the vapor pressure of water and make sure to level levels
Mono; di; tri; tetra; penta; hexa.
Unsaturated - addition (ex: decolorize bromine solution)

36. sulfates
Anode - oxygen. Cathode - hydrogen
Soluble except Ag - Pb - Ca - Sr Ba)
allow for the vapor pressure of water and make sure to level levels
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

37. What is the formula for obtaining charge flowing in a cell?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Q=It (time in seconds)
bright yellow
Salts (ex: CaO + SO2 ? CaSO3)

38. What are the prefixes for the naming of binary molecular compound formulas (up to six)
ClO3?
Mono; di; tri; tetra; penta; hexa.
But S° of element is not zero (except at 0K)
More chaotic (ex: gases made)

39. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
are less dense than water
They decrease (or could be the same if the solid has ONLY JUST disappeared)
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.

40. What is the general formula for an ester?
Mono; di; tri; tetra; penta; hexa.
More chaotic (ex: gases made)
RCOOR
it is lower and occurs over less sharp a range

41. ammonium
Increases.
Sigma bonds are stronger than pi bonds
linear
NH4?

42. For a dibasic acid (H2A) - [A²?]= ____ ?
NH4?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Perform ICE BOX calculation based on K1
K2

43. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
red - green - blue
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
K1 x K2

44. How are primary alcohols turned into acids?
Iodine and CO2 (dry ice)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Sigma bonds are stronger than pi bonds
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

45. Esterification is...
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.
same KE - but PEice<PEwater
SO4²?
acid + alcohol

46. What shape is ammonia?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Trigonal pyramidal
Soluble
10?8

47. When the salt bridge is removed what happens to the cell reaction?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
It ceases - the circuit is broken.
CO (poisonous)
Glacial acetic acid

48. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
strong acids/bases are written as H+ or OH- ions
They stay the same.
bright yellow
Eudiometer

49. What should you check for before you begin titrating?
CrO4²?
Check for air bubbles in the buret and remove the buret funnel from the buret
zero
Iodine and CO2 (dry ice)

50. Which would cause the bulb in a conductivity apparatus to be brightest?
Eudiometer
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
yellow
0.10M HCl (more ions)