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 device would you use to measure a volume of gas?
Pale yellow
proton acceptor.
Eudiometer
voltaic: + electrolytic: -


2. Give an example of a concentrated weak acid.
metal oxides and hydrides are ionically bonded and basic
0 and 14
Glacial acetic acid
ClO4?


3. What is the formula for summation?

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4. How do you dilute an acid?

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5. Do anions flow to the cathode or anode?
Anode
RCHO (carbonyl at end)
bent
The compound with the lowest Ksp value.


6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
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
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Ksp = 4s³


7. What is the test for oxygen?
by electrolysis
The dilution effect when the solutions mix. M1V1 = M2V2
Q=It (time in seconds)
Glowing splint (positive result=relights)


8. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Group 1 hydroxides (ex: NaOH)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O


9. Alkanes are _________ and react by _________
Check for air bubbles in the buret and remove the buret funnel from the buret
Insoluble
CnH(2n+2)
Saturated - Substitution (which requires more radical conditions)


10. How do you clean a buret/pipette for a titration?
PO4³?
Group I metals (soft metals) are stored under oil
Nothing
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.


11. Which alkali metals float on water?
are less dense than water
O2 needs 4F/mol H2 needs 2F/mol
All except for lithium
Anode


12. How are strong ones written?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
strong acids/bases are written as H+ or OH- ions
same KE - but PEice<PEwater
zero


13. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Soluble except Ag - Pb - Ca - Sr Ba)
Ksp = s²
by electrolysis
C4H10


14. Is the standard entropy (S°) of an element zero?
Making sigma bonds and holding lone pairs
it reacts by substitution NOT addition
Time?¹ - (ex. s?¹ - hr?¹ - etc)
But S° of element is not zero (except at 0K)


15. group 1 ions/compounds
RX
metal oxides and hydrides are ionically bonded and basic
Soluble
same KE - but PEice<PEwater


16. Can you collect soluble gases over water?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
atoms
S crystal at 0K=0
No - NH3 and HCl gases are extremely soluble


17. What type of compounds do metals/non metals form?
Ionic compounds
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
chemically (ex: with carbon)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec


18. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
The compound with the lowest Ksp value.
Anode
Ppt will NOT form (unsaturated)


19. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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20. Which of the rates changes more when temperature is increased?
acids
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
it reacts by substitution NOT addition


21. silver compounds
T increases exponentially the proportion of molecules with E > Ea
Insoluble except for nitrate and acetate
benzene is less reactive than alkenes
HClO4


22. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
RX
do not change


23. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
OH- and NH3
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
The Faraday or Faraday's constant.


24. What are two substances that sublime at 1 atm when heated?
The one with most oxygen atoms (highest oxidation number)
Iodine and CO2 (dry ice)
Anode - oxygen. Cathode - hydrogen
redox reaction


25. nitrates
redox reaction
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
hydroxides (ex: Ba(OH)2)
Soluble


26. What is the general formula for an aldehyde?
ion pairing
H2O + CO2 (it decomposes readily)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
RCHO (carbonyl at end)


27. oxalate
zero
C2O4²?
Concentration
How grouped results are


28. chlorine
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
They decrease (or could be the same if the solid has ONLY JUST disappeared)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Greenish-yellow gas


29. What do the 'a' and 'b' in Van Der Waal's equation allow for?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
a-IMFs - b-molecular volume
Transition element compounds (except if it has a full or empty d shell)


30. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
[A?]/[HA] x 100 or [BH?]/[B] x 100
proton donor base
it reacts by substitution NOT addition


31. How does group 1 metals' density compare to water's?
ion pairing
Hg2²?
Combine the equations for the half reactions in the non-spontaneous direction
are less dense than water


32. An amphiprotic (amphoteric) species is...
Soluble except Ag - Pb - Ca - Sr Ba)
bases
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)


33. Acidic gases like SO2 in the atmosphere cause what environmental problems?
do not change
Combine the equations for the half reactions in the non-spontaneous direction
CnH2n+2
Acid rain - dissolves marble buildings/statues and kills trees.


34. What do metal oxides plus non- metal oxides form?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Salts (ex: CaO + SO2 ? CaSO3)
ClO2?
CO3²?


35. A Bronsted-Lowry base is...
Transition element compounds (except if it has a full or empty d shell)
Synthetic condensation polymer (aka a polyamide)
proton acceptor.
At half equivalence - pH=pKa


36. Does Kw increase or decrease with T? Why?
Soluble
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
R=8.31 J/mol/K
White precipitate


37. What are allotropes?
different forms of the same element
Insoluble (except group 1 ammonium and Ba)
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
Sulfur


38. What type of compounds are almost always colored?
An active metal.
Transition element compounds (except if it has a full or empty d shell)
boiling without losing volatile solvents/reactants
do not change


39. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
A salt solution.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)


40. What apparatus do you use to separate 2 immiscible liquids?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
left - ppt will form
P2O5
Separating funnel


41. Both Acetic acid and ____________ are also functional isomers.
methyl formate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
CO2 and H2O
Ksp = 108s5


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

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43. 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
+4-covalent - +2-ionic
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
same KE - but PEice<PEwater


44. bromine
acids
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The benzene ring (or more correctly the phenyl group - C6H5)
brown volatile liquid


45. Is a graduated cylinder or beaker more accurate?
it reacts by substitution NOT addition
H2O + CO2 (it decomposes readily)
NH4?
Graduated cylinder


46. phosphates
Most INsoluble except group 1 and ammonium
It ceases - the circuit is broken.
At half equivalence - pH=pKa
ROH


47. hydroxides
Insoluble (except group 1 ammonium and Ba)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
They stay the same.
0.10M HCl (more ions)


48. If a free element is involved - what type of reaction must be involved?
redox reaction
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Both electrons come from the same atom (just as good as a regular bond)
Ksp = 108s5


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

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50. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
K2
Cu3(PO4)2
Selective absorption