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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 are isomers?
Heptane
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Current - time and charge on ion (moles of e used in half cell reaction)
Molecules with the same molecular formulas - but different structural formulas

2. What are the common strong bases?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Initiation energy (NOT Ea)
Group 1 hydroxides (ex: NaOH)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

3. What things should you remember to do when collecting gas over water?
non-metal oxides and hydrides are covalently bonded and are acidic.
Pale yellow
allow for the vapor pressure of water and make sure to level levels
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

4. How does group 1 metals' density compare to water's?
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)
voltaic: - electrolytic: +
are less dense than water
0 and 14

5. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ksp = s²
O2 needs 4F/mol H2 needs 2F/mol

6. What is the name of S2Cl2? (Know how to name others like this - too)
Soluble except Ag - Pb - Ca - Sr Ba)
Check for air bubbles in the buret and remove the buret funnel from the buret
All except for lithium
Disulfur dichloride

7. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
zero
|experimental - accepted|/accepted X 100
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

8. How many normal boiling points and boiling points are there?

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9. potassium permanganate
Purple
Transition element compounds (except if it has a full or empty d shell)
proton donor base
q=mc?T q=mL (or n x ?h)

10. What word is a clue for a redox reaction?
Concentration
O2 needs 4F/mol H2 needs 2F/mol
Making sigma bonds and holding lone pairs
Acidified

11. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
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
White precipitate
zero

12. How do you explain trends in atomic properties using Coulomb's Law?
Anode
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?)
P2O5
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

13. ammonium
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
fruit - fish - bases
NH4?

14. When a cell is 'flat' What is its voltage?
The benzene ring (or more correctly the phenyl group - C6H5)
zero
MnO4?
0.10M HCl (more ions)

15. What is reflux?
Combine the equations for the half reactions in the non-spontaneous direction
ROH
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
boiling without losing volatile solvents/reactants

16. What do hydrocarbons form when they burn in air (oxygen)?
voltaic: - electrolytic: +
CO2 and H2O
-Ea/R
Increases down group 1 decreases down group 17

17. At what point during titration do you have the perfect buffer - and what is the pH at this point?
atoms
At half equivalence - pH=pKa
No - NH3 and HCl gases are extremely soluble
ROH

18. When is ?G zero?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Mono; di; tri; tetra; penta; hexa.
K2

19. The definition of acidic basic and neutral aqueous solutions is:
OH?
Ionic compounds
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Current - time and charge on ion (moles of e used in half cell reaction)

20. What is the slope of the graph of lnk vs. 1/T?
red - green - blue
-Ea/R
catalyst=conc H2SO4
PO4³?

21. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Exothermic
neutralization: high K - H2O product dissociation: low K - H2O reactant
water and substances with (s) less dense than
linear

22. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Check for air bubbles in the buret and remove the buret funnel from the buret
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
zero

23. What do ions and electrons travel through in a voltaic/electrolytic cell?
Identity and purity (impure compounds usually have broad & low melting points)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Ppt will NOT form (unsaturated)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

24. If a free element is involved - what type of reaction must be involved?
redox reaction
voltaic: + electrolytic: -
blue (BTB)
Pale purple - (orange)-yellow - red - blue - green.

25. What is the charge on a chlorine atom?
zero
Selective absorption
left - ppt will form
an oxidized and reduced substance

26. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
?G= -ve - E°= +ve
Reduction always takes place at the cathode (RED CAT) In both types of cell!
RX
zero

27. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
A salt solution.
bases
Ksp = s²

28. How many faradays of electric charge do you need to produce one mole of O2? H2?
H3PO4
blue (BTB)
ROR
O2 needs 4F/mol H2 needs 2F/mol

29. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Q=It (time in seconds)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Most are soluble except Ag - Pb
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

30. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases down group 1 decreases down group 17
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
water and substances with (s) less dense than
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

31. What changes Keq?
Synthetic condensation polymer (aka a polyamide)
Insoluble except for nitrate and acetate
Only temperature
CnH2n+1 often designated 'R' ex C3H7 is propyl

32. What part of a liquid do you look at to measure its volume?
an oxidized and reduced substance
Read the bottom of the meniscus
zero-th: decreases - first: constant - second: increases
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

33. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CnH2n+1 often designated 'R' ex C3H7 is propyl
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Clear
a-IMFs - b-molecular volume

34. Name 2 ways in which you can create a buffer?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
K2
Iodine and CO2 (dry ice)
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)

35. What electrons are lost/gained first in transition element ions?
Conjugate pair (one must be a weak base or acid)
acids
Salt + water
ns² electrons (first in-first out)

36. Alkanes are _________ and react by _________
CnH2n-2
strong acids/bases are written as H+ or OH- ions
different forms of the same element
Saturated - Substitution (which requires more radical conditions)

37. What do group I/II metal oxides and acids form?
Salt and water
But S° of element is not zero (except at 0K)
Hg2²?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

38. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
RNH2
No - it depends on the number of ions produced on dissolving.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

39. mercury (I) ion
Hg2²?
C2O4²?
Group 1 hydroxides (ex: NaOH)
Iodine and CO2 (dry ice)

40. What things should you remember to do when collecting gas over water?
[A?]/[HA] x 100 or [BH?]/[B] x 100
allow for the vapor pressure of water and make sure to level levels
H2O + CO2 (it decomposes readily)
More chaotic (ex: gases made)

41. Do anions flow to the cathode or anode?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
OH- and NH3
Pale yellow
Anode

42. nitrate
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
NO3?

43. carbonates
Insoluble except group 1 and ammonium
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Initiation energy (NOT Ea)
Evaporation

44. Colorless doesn't mean ______
Insoluble except for nitrate and acetate
Clear
Insoluble (except group 1 ammonium and Ba)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

45. Name C7H16
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
Heptane
zero-th: decreases - first: constant - second: increases
Increases.

46. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
More chaotic (ex: gases made)

47. What is the formula of butane?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
The Faraday or Faraday's constant.
RCOOR
C4H10

48. What is the general formula for an ester?
RCOOR
ionic and form hydrogen and hydroxide
Tetrahedral
A) any range. b) 8-10 c) 4-6

49. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
CN?
Mn²? - Cr³? - Cr³
Insoluble except for nitrate and acetate
Making sigma bonds and holding lone pairs

50. If Q < Ksp a ppt ______
redox reaction
Ppt will NOT form (unsaturated)
Kc=Kp
P2O5