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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 is the general formula of an alkane?
ClO2?
Soluble except Ag - Pb - Ca - Sr Ba)
H3PO4
CnH(2n+2)

2. What things should you remember to do when collecting gas over water?
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
Insoluble except group 1 and ammonium
Insoluble except nitrate and acetate
allow for the vapor pressure of water and make sure to level levels

3. acetate
CH3COO?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
bases
Ksp = 108s5

4. When a cell is 'flat' What is its voltage?
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero
More chaotic (ex: gases made)
allow for the vapor pressure of water and make sure to level levels

5. What is the formula for summation?

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6. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
H2O + CO2 (it decomposes readily)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
ClO4?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

7. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
catalyst=conc H2SO4
But S° of element is not zero (except at 0K)
The compound with the lowest Ksp value.
RX

8. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Concentration
-Ea/R
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

9. How many ligands attach to a central ion in a complex ion?
CO2 and H2O
#ligands=charge x2
Ppt will NOT form (unsaturated)
same KE - but PEice<PEwater

10. What is the slope of the graph of lnk vs. 1/T?
proton acceptor.
-Ea/R
Selective absorption
Add acid to water so that the acid doesn't boil and spit

11. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
All except for lithium
Graduated cylinder
H3PO4

12. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
[A?]/[HA] x 100 or [BH?]/[B] x 100
CnH(2n+2)
zero

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

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14. How do you get Ecell for spontaneous reactions?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
boiling without losing volatile solvents/reactants

15. What is accuracy?
How close results are to the accepted value
?G=negative - E° must be positive
The benzene ring (or more correctly the phenyl group - C6H5)
same KE - but PEice<PEwater

16. How does group 1 metals' density compare to water's?
Kc=Kp
are less dense than water
How grouped results are
CO2 and H2O

17. What is the pH of 1.0M HCl? 1M NaOH?
Read the bottom of the meniscus
0 and 14
A) any range. b) 8-10 c) 4-6
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.

18. An amphiprotic (amphoteric) species is...
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
allow for the vapor pressure of water and make sure to level levels
Decant

19. What is the general formula for an acid?
RCOOH
benzene is less reactive than alkenes
H+
S2O3²?

20. mercury (I) ion
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
The one with most oxygen atoms (highest oxidation number)
Acid rain - dissolves marble buildings/statues and kills trees.
Hg2²?

21. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Salts (ex: CaO + SO2 ? CaSO3)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
At half equivalence - pH=pKa
Ksp = 108s5

22. What are the prefixes for the naming of binary molecular compound formulas (up to six)
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)
How close results are to the accepted value
Mono; di; tri; tetra; penta; hexa.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

23. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Salt and water
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Ksp = 4s³

24. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
allow for the vapor pressure of water and make sure to level levels
K1 x K2
Conjugate pair (one must be a weak base or acid)

25. How do you find the pH for a dibasic acid? (H2A)?
zero
C2O4²?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Perform ICE BOX calculation based on K1

26. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
T increases exponentially the proportion of molecules with E > Ea
RCOOR
Both electrons come from the same atom (just as good as a regular bond)

27. nitrate
NO3?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Glacial acetic acid
same KE - but PEice<PEwater

28. What is the formula of butane?
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.
The benzene ring (or more correctly the phenyl group - C6H5)
Transition element compounds (except if it has a full or empty d shell)
C4H10

29. Esterification is...
Salts (ex: CaO + SO2 ? CaSO3)
Insoluble except for nitrate and acetate
Anode
acid + alcohol

30. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
it reacts by substitution NOT addition
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
it is lower and occurs over less sharp a range

31. Is the standard entropy (S°) of an element zero?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
But S° of element is not zero (except at 0K)
Glacial acetic acid
Heat a test tube at an angle at the side of the tube (not bottom)

32. What is the test for oxygen?
Glowing splint (positive result=relights)
Cr2O7²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Products - reactants (except for BDE when it's reactants - products)

33. chlorate
Insoluble except group 1 and ammonium
left - ppt will form
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ClO3?

34. If a weak acid is diluted more - what happens to its % dissociation value?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Increases.
NH2?
PO4³?

35. BaSO4
Trigonal pyramidal
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Insoluble
The one with most oxygen atoms (highest oxidation number)

36. Aromatic compounds contain what?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
bright yellow
Combine the equations for the half reactions in the non-spontaneous direction
The benzene ring (or more correctly the phenyl group - C6H5)

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

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38. Acid plus base make?
Salt + water.
R=8.31 J/mol/K
Salts (ex: CaO + SO2 ? CaSO3)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

39. How are more active metals reduced?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Distillation
metal oxides and hydrides are ionically bonded and basic
by electrolysis

40. What device would you use to measure a volume of gas?
P2O5
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
How grouped results are
Eudiometer

41. ammonium/ammonium compounds
Sulfur
CO (poisonous)
Soluble
CnH(2n+2)

42. What process do you use to obtain the precipitate from a solution?
#ligands=charge x2
OH?
Filtration
same KE - but PEice<PEwater

43. What is the general formula for an ether?
Check for air bubbles in the buret and remove the buret funnel from the buret
ROR
strong acids/bases are written as H+ or OH- ions
No - NH3 and HCl gases are extremely soluble

44. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
proton donor base
a-IMFs - b-molecular volume
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

45. What two compounds are great oxidizing agents?

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46. What causes the dramatic effect of T on rate?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Only temperature
T increases exponentially the proportion of molecules with E > Ea
At half equivalence - pH=pKa

47. What are allotropes?
Sulfur
different forms of the same element
q=mc?T q=mL (or n x ?h)
?G=negative - E° must be positive

48. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Anode
A salt solution.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

49. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
blue (BTB)
?H formation of an element in standard state=0
do not change

50. hydroxides
Initiation energy (NOT Ea)
atoms
Insoluble (except group 1 ammonium and Ba)
NH4?