Test your basic knowledge |

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. Metal hydrides are _____ and form _______ and _______ when added to water
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ClO?
ionic and form hydrogen and hydroxide
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.

2. When the salt bridge is removed what happens to the cell reaction?
Salt + water.
It ceases - the circuit is broken.
+4-covalent - +2-ionic
Check for air bubbles in the buret and remove the buret funnel from the buret

3. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ksp = s²
CO2 and H2O
Clear

4. What type of compounds do metals/non metals form?
Hg2²?
Ionic compounds
Heat a test tube at an angle at the side of the tube (not bottom)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

5. How does group 1 metals' density compare to water's?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
?G= -ve - E°= +ve
are less dense than water
Saturated - Substitution (which requires more radical conditions)

6. bromothymol
blue (BTB)
Tetrahedral
The benzene ring (or more correctly the phenyl group - C6H5)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

7. 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
basic
CnH(2n+2)
Acid rain - dissolves marble buildings/statues and kills trees.

8. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
?H formation of an element in standard state=0
It ceases - the circuit is broken.
blue (BTB)

9. A Bronsted-Lowry base is...
ion pairing
A salt solution.
proton acceptor.
O2 needs 4F/mol H2 needs 2F/mol

10. What shape is methane?
Tetrahedral
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Iodine and CO2 (dry ice)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

11. iodine - iodine solution - iodine vapor
different forms of the same element
atoms
Silvery gray solid - brown - purple
lighted splint (positive result=pop)

12. Ions are not ______.
Increases down group 1 decreases down group 17
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
Soluble
atoms

13. acetates
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
diamond and graphite
Mono; di; tri; tetra; penta; hexa.
Soluble

14. What two types of substances are present in all redox reactions?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
H2O + CO2 (it decomposes readily)
an oxidized and reduced substance
ionic and form hydrogen and hydroxide

15. What do hydrocarbons form when they burn in air (oxygen)?
Check for air bubbles in the buret and remove the buret funnel from the buret
The compound with the lowest Ksp value.
Ppt will NOT form (unsaturated)
CO2 and H2O

16. If a weak acid is diluted more - what happens to its % dissociation value?
Salts (ex: CaO + SO2 ? CaSO3)
fractional distillation
Increases.
yellow

17. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Kc=Kp
small size and high charge
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Anode

18. What is the general formula for an amine?
H2PO4?
RCOOR
RNH2
Ksp = 4s³

19. Name some properties of Group 17
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

20. What electrons are lost/gained first in transition element ions?
Glowing splint (positive result=relights)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ns² electrons (first in-first out)
RNH2

21. phosphate
PO4³?
Salt + water
strong acids/bases are written as H+ or OH- ions
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.

22. What part of a liquid do you look at to measure its volume?
Glowing splint (positive result=relights)
Ksp = 27s4
Read the bottom of the meniscus
ion pairing

23. Is the standard entropy (S°) of an element zero?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
H2PO4?
The one with most oxygen atoms (highest oxidation number)
But S° of element is not zero (except at 0K)

24. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Ksp = 108s5
atoms
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
E=q + w (negative is by system - positive is on system)

25. What things should you remember to do when collecting gas over water?
Ionic compounds
No - it depends on the number of ions produced on dissolving.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
allow for the vapor pressure of water and make sure to level levels

26. What are two allotropes of carbon?
zero
diamond and graphite
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
different forms of the same element

27. What process do you use to obtain the precipitate from a solution?
Filtration
Unsaturated - addition (ex: decolorize bromine solution)
Anode - oxygen. Cathode - hydrogen
CnH2n+1 often designated 'R' ex C3H7 is propyl

28. What is the charge on a chlorine atom?
Current - time and charge on ion (moles of e used in half cell reaction)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
zero
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

29. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Sigma bonds are stronger than pi bonds
zero

30. What is H2CO3 (carbonate acid) usually written as?
H2O + CO2 (it decomposes readily)
Read the bottom of the meniscus
boiling without losing volatile solvents/reactants
Soluble except Ag - Pb - Ca - Sr Ba)

31. cyanide
linear
CN?
catalyst=conc H2SO4
Heat a test tube at an angle at the side of the tube (not bottom)

32. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Increases.
methyl formate
-Ea/R

33. What is the conjugate base of NH3?
NH2?
Molecules with the same molecular formulas - but different structural formulas
Acid rain - dissolves marble buildings/statues and kills trees.
Mono; di; tri; tetra; penta; hexa.

34. Color (absorbance) is proportional to ________
ROH
Concentration
More chaotic (ex: gases made)
Making sigma bonds and holding lone pairs

35. What is the test for oxygen?
H+
Salt + water
Glowing splint (positive result=relights)
Greenish-yellow gas

36. mercury (II) ion
basic
blue glass - it filters UV
P2O5
Hg²?

37. What are the units of the first order rate constant?
zero
are less dense than water
Time?¹ - (ex. s?¹ - hr?¹ - etc)
A salt solution.

38. dichromate (soln + most solids)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Orange
ionic and form hydrogen and hydroxide

39. dihydrogen phosphate
RCOR
H2PO4?
Current - time and charge on ion (moles of e used in half cell reaction)
SO4²?

40. Do anions flow to the cathode or anode?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
More chaotic (ex: gases made)
Salts (ex: CaO + SO2 ? CaSO3)
Anode

41. What is the formula for obtaining charge flowing in a cell?
S2O3²?
The compound with the lowest Ksp value.
Q=It (time in seconds)
The one with most oxygen atoms (highest oxidation number)

42. nitrates
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
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)
HClO4

43. carbonate
CO3²?
blue (BTB)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
CO (poisonous)

44. What is the name of S2Cl2? (Know how to name others like this - too)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Disulfur dichloride
left - ppt will form
ethers

45. Why are noble gases stable?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
boiling without losing volatile solvents/reactants
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Time?¹ - (ex. s?¹ - hr?¹ - etc)

46. group 1 ions/compounds
boiling without losing volatile solvents/reactants
Soluble
ethers
do not change

47. What do the 'a' and 'b' in Van Der Waal's equation allow for?
yellow
Add acid to water so that the acid doesn't boil and spit
a-IMFs - b-molecular volume
Insoluble except for nitrate and acetate

48. How does half life change for zero-th order - first order - and second order processes?
K1 x K2
Acids; HCOOCH3 is an ester
zero-th: decreases - first: constant - second: increases
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

49. What is the general formula of an alkane?
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
Acidified
CnH(2n+2)
K2

50. What is the second law of thermodynamics?
Tetrahedral
blue (BTB)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Suniverse increases for spontaneous processes