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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.
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 are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
neutralization: high K - H2O product dissociation: low K - H2O reactant
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

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

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3. Colorless doesn't mean ______
lighted splint (positive result=pop)
Clear
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Heptane

4. What is the general formula for an aldehyde?
O2 needs 4F/mol H2 needs 2F/mol
look for changes in oxidation # - the one that goes up is oxidized and is the RA
RCHO (carbonyl at end)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

5. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
CnH(2n+2)
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.
Ksp = 4s³
Transition element compounds (except if it has a full or empty d shell)

6. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
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.
SO4²?
Ksp = s²
RCHO (carbonyl at end)

7. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ClO3?
left - ppt will form

8. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
CnH2n+2
Mono; di; tri; tetra; penta; hexa.
water and substances with (s) less dense than

9. What type of compounds do Group 14 form?
The benzene ring (or more correctly the phenyl group - C6H5)
?H-kJ - ?S-J - ?G-kJ
+4-covalent - +2-ionic
OH- and NH3

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

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11. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
White precipitate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

12. What electrons are lost/gained first in transition element ions?
neutralization: high K - H2O product dissociation: low K - H2O reactant
CnH2n-2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
ns² electrons (first in-first out)

13. Ca - Sr - Ba
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
hydroxides (ex: Ba(OH)2)
OH- and NH3

14. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Group 1 hydroxides (ex: NaOH)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Current - time and charge on ion (moles of e used in half cell reaction)

15. dichromate
Salts (ex: CaO + SO2 ? CaSO3)
Pale yellow
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Cr2O7²?

16. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
It ceases - the circuit is broken.
Group I metals (soft metals) are stored under oil
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

17. Which alkali metals float on water?
non-metal oxides and hydrides are covalently bonded and are acidic.
[A?]/[HA] x 100 or [BH?]/[B] x 100
All except for lithium
do not change

18. The definition of acidic basic and neutral aqueous solutions is:
Check for air bubbles in the buret and remove the buret funnel from the buret
The compound with the lowest Ksp value.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Add acid to water so that the acid doesn't boil and spit

19. chlorate
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
water and substances with (s) less dense than
ClO3?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

20. What should you check for before you begin titrating?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
no - they're written undissociated (HAaq)
ClO2?
Check for air bubbles in the buret and remove the buret funnel from the buret

21. Is the standard entropy (S°) of an element zero?
Orange
10?8
But S° of element is not zero (except at 0K)
Initiation energy (NOT Ea)

22. Which of the rates changes more when temperature is increased?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
K1 x K2
Products - reactants (except for BDE when it's reactants - products)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

23. ________ are Lewis bases - because they can donate a lone pair of electrons.
PO4³?
White precipitate
OH- and NH3
Greenish-yellow gas

24. Is the freezing of ice endothermic or exothermic?
Exothermic
different forms of the same element
basic
atoms

25. What do you use for an acid spill? base spill?
OH?
blue (BTB)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
S crystal at 0K=0

26. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Distillation
a-IMFs - b-molecular volume
OH?
Ksp = 27s4

27. Acids + Carbonates (bicarbonates) make?
C2O4²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
basic
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

28. What is the third law of thermodynamics?
do not change
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)
water and substances with (s) less dense than
S crystal at 0K=0

29. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
same KE - but PEice<PEwater
Soluble except Ag - Pb - Ca - Sr Ba)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
They stay the same.

30. What does the solubility of organic compounds depend on?
Experimental mass/theoretical mass X 100
benzene is less reactive than alkenes
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

31. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
no - they're written undissociated (HAaq)
linear
Big K=kf/kr
zero

32. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
it is lower and occurs over less sharp a range
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Q=It (time in seconds)

33. What do you need to make a polymer?
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)
At half equivalence - pH=pKa
Perform ICE BOX calculation based on K1
RCOOR

34. What shape is water?
RX
A salt solution.
bent
MnO4?

35. primary colors
red - green - blue
bright yellow
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Most are soluble except Ag - Pb

36. Is the ?H formation of an element in standard state zero?
H2PO4?
small size and high charge
Insoluble except for nitrate and acetate
?H formation of an element in standard state=0

37. What is the first law of thermodynamics?
R=8.31 J/mol/K
#ligands=charge x2
ethers
E=q + w (negative is by system - positive is on system)

38. When driving off water from a hydrate - how do you tell you're done?
S2O3²?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Iodine and CO2 (dry ice)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

39. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
Saturated - Substitution (which requires more radical conditions)
do not change
yellow

40. What is the charge on a chlorine atom?
zero
bent
Soluble
CnH2n+2

41. Aromatic compounds contain what?
Making sigma bonds and holding lone pairs
The benzene ring (or more correctly the phenyl group - C6H5)
0.10M HCl (more ions)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

42. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Greenish-yellow gas
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CO2 and H2O
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

43. What are amphoteric oxides?
Insoluble (except group 1 ammonium and Ba)
lighted splint (positive result=pop)
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)
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?)

44. How does the melting point of a mixture compare to the MP of a pure substance?
The one with most oxygen atoms (highest oxidation number)
it is lower and occurs over less sharp a range
Add acid to water so that the acid doesn't boil and spit
Soluble

45. lead compounds
|experimental - accepted|/accepted X 100
Insoluble except nitrate and acetate
catalyst=conc H2SO4
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

46. If ?S is positive - are the products more or less chaotic than the reactants?
small size and high charge
no - they're written undissociated (HAaq)
More chaotic (ex: gases made)
boiling without losing volatile solvents/reactants

47. What are two substances that sublime at 1 atm when heated?
Suniverse increases for spontaneous processes
Iodine and CO2 (dry ice)
Q=It (time in seconds)
RCOR

48. What is the difference between equivalence point and end point of a titration.
Pipette (burette if need repetition)
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
Greenish-yellow gas
Increases.

49. How are metal oxides and hydrides bonded? are they acidic or basic?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
S crystal at 0K=0
metal oxides and hydrides are ionically bonded and basic

50. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Evaporation
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
strong acids/bases are written as H+ or OH- ions