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. dichromate (soln + most solids)
ethers
[A?]/[HA] x 100 or [BH?]/[B] x 100
water and substances with (s) less dense than
Orange

2. What steps do organic labs consist of?
fruit - fish - bases
Synthesis - separation and purification of the product and its identification.
Clear
No - NH3 and HCl gases are extremely soluble

3. Acid plus base make?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Salt + water.
S2O3²?
K2

4. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH2n-2
Salt and water
Mn²? - Cr³? - Cr³

5. hydroxide
Insoluble except group 1 and ammonium
No - NH3 and HCl gases are extremely soluble
Disulfur dichloride
OH?

6. What does the solubility of organic compounds depend on?
Products - reactants (except for BDE when it's reactants - products)
Soluble except Ag - Pb - Ca - Sr Ba)
by electrolysis
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

7. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
catalyst=conc H2SO4
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Salts (ex: CaO + SO2 ? CaSO3)
H+

8. ammonium
NH4?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Saturated - Substitution (which requires more radical conditions)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

9. Do anions flow to the cathode or anode?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
How grouped results are
Anode
Time?¹ - (ex. s?¹ - hr?¹ - etc)

10. How are more active metals reduced?
PO4³?
by electrolysis
-Ea/R
look for changes in oxidation # - the one that goes up is oxidized and is the RA

11. What is the catalyst for this reaction Ester + ?
do not change
Ksp = 4s³
an oxidized and reduced substance
catalyst=conc H2SO4

12. Which would cause the bulb in a conductivity apparatus to be brightest?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Separating funnel
0.10M HCl (more ions)

13. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Identity and purity (impure compounds usually have broad & low melting points)
CO2 and H2O

14. What is the general formula for alkyl halides?
?H-kJ - ?S-J - ?G-kJ
RX
Acidified
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

15. thiosulfate
White precipitate
S2O3²?
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
q=mc?T q=mL (or n x ?h)

16. What equipment do you need for a titration?
Decant
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Good catalysts - form multiple oxidation states - often paramagnetic - good structural metals - form a host of alloys (similar sized atoms) - have similar I energies (inner filling)
redox reaction

17. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Q=It (time in seconds)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
non-metal oxides and hydrides are covalently bonded and are acidic.
No - NH3 and HCl gases are extremely soluble

18. ________ are Lewis bases - because they can donate a lone pair of electrons.
atoms
fruit - fish - bases
OH- and NH3
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

19. Color (absorbance) is proportional to ________
Concentration
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
|experimental - accepted|/accepted X 100
ROH

20. What things should you remember to do when collecting gas over water?
RCOR
Acidified
Ppt will NOT form (unsaturated)
allow for the vapor pressure of water and make sure to level levels

21. How does the melting point of a mixture compare to the MP of a pure substance?
non-metal oxides and hydrides are covalently bonded and are acidic.
Ksp = 108s5
it is lower and occurs over less sharp a range
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

22. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
No - NH3 and HCl gases are extremely soluble
Iodine and CO2 (dry ice)
0 and 14
Ksp = s²

23. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
K2
RCHO (carbonyl at end)
atoms
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

24. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
Heat a test tube at an angle at the side of the tube (not bottom)
Cr2O7²?
MnO4?

25. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
C4H10
Ksp = 108s5
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)
The dilution effect when the solutions mix. M1V1 = M2V2

26. What is the sign of the anode in voltaic cells? in electrolytic cells?
K1 x K2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
voltaic: - electrolytic: +
boiling without losing volatile solvents/reactants

27. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Mn²? - Cr³? - Cr³
CO2 and H2O

28. If a weak acid is diluted more - what happens to its % dissociation value?
linear
Distillation
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Increases.

29. What is the formula for obtaining charge flowing in a cell?
The dilution effect when the solutions mix. M1V1 = M2V2
Check for air bubbles in the buret and remove the buret funnel from the buret
CN?
Q=It (time in seconds)

30. silver iodide
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Pale yellow
methyl formate
zero

31. What electrons are lost/gained first in transition element ions?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Transition element compounds (except if it has a full or empty d shell)
ns² electrons (first in-first out)
K2

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

33. How do you explain trends in atomic properties using Coulomb's Law?
Increases down group 1 decreases down group 17
ns² electrons (first in-first out)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

34. iodine - iodine solution - iodine vapor
small size and high charge
[A?]/[HA] x 100 or [BH?]/[B] x 100
The Faraday or Faraday's constant.
Silvery gray solid - brown - purple

35. When the salt bridge is removed what happens to the cell reaction?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
It ceases - the circuit is broken.
Glacial acetic acid
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

36. How many faradays of electric charge do you need to produce one mole of O2? H2?
The dilution effect when the solutions mix. M1V1 = M2V2
O2 needs 4F/mol H2 needs 2F/mol
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
Distillation

37. What do nonmetal oxides plus water form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Current - time and charge on ion (moles of e used in half cell reaction)
Exothermic
acids

38. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
The one with most oxygen atoms (highest oxidation number)
S crystal at 0K=0
ion pairing

39. A Bronsted-Lowry base is...
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Increases down group 1 decreases down group 17
proton acceptor.

40. What shape is carbon dioxide?
yellow
The Faraday or Faraday's constant.
linear
ionic and form hydrogen and hydroxide

41. Color is due to ______ _______ of light.
left - ppt will form
Selective absorption
Anode - oxygen. Cathode - hydrogen
Synthesis - separation and purification of the product and its identification.

42. How do you find the pH for a dibasic acid? (H2A)?
H2O + CO2 (it decomposes readily)
CO3²?
Perform ICE BOX calculation based on K1
red - green - blue

43. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
CN?
Salts (ex: CaO + SO2 ? CaSO3)
0.10M HCl (more ions)

44. What is the general formula for an alcohol?
SO4²?
ROH
A) any range. b) 8-10 c) 4-6
Ions go through the salt bridge - electrons go through metal wires in the external circuit

45. What is the formula for summation?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

46. Metal hydrides are _____ and form _______ and _______ when added to water
Saturated - Substitution (which requires more radical conditions)
10?8
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ionic and form hydrogen and hydroxide

47. phosphate
An active metal.
Exothermic
Salt + water
PO4³?

48. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
S crystal at 0K=0
Current - time and charge on ion (moles of e used in half cell reaction)
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
ionic and form hydrogen and hydroxide

49. What is the test for oxygen?
K1 x K2
diamond and graphite
Acids; HCOOCH3 is an ester
Glowing splint (positive result=relights)

50. mercury (II) ion
Hg²?
Filtration
K2
H+