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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 shape is water?
acid + alcohol
Ksp = 108s5
bent
ROR

2. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
10?8
Exothermic (?H for ANY sa/sb = -57kJ/mol)
RCOOH
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

3. How does benzene compare in reactivity to alkenes?
Soluble
benzene is less reactive than alkenes
Purple
Exothermic (?H for ANY sa/sb = -57kJ/mol)

4. The oxidation # for acid base reactions...
do not change
T increases exponentially the proportion of molecules with E > Ea
CrO4²?
Tetrahedral

5. What do you do to get rid of most of the solution from a precipitate?
ion pairing
Decant
Acids; HCOOCH3 is an ester
RNH2

6. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Ksp = 27s4
methyl formate
H2PO4?

7. lead compounds
H3PO4
water and substances with (s) less dense than
Pipette (burette if need repetition)
Insoluble except nitrate and acetate

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

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9. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
OH- and NH3
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
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?)

10. How are metal oxides and hydrides bonded? are they acidic or basic?
?H-kJ - ?S-J - ?G-kJ
metal oxides and hydrides are ionically bonded and basic
by electrolysis
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

11. What is the general formula for an ether?
Trigonal pyramidal
ROR
a-IMFs - b-molecular volume
S crystal at 0K=0

12. How are more active metals reduced?
by electrolysis
Time?¹ - (ex. s?¹ - hr?¹ - etc)
strong acids/bases are written as H+ or OH- ions
Combine the equations for the half reactions in the non-spontaneous direction

13. Ions are not ______.
allow for the vapor pressure of water and make sure to level levels
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)
atoms
Only temperature

14. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble (except group 1 ammonium and Ba)

15. A Bronsted-Lowry acid is...
Selective absorption
Hg2²?
RCHO (carbonyl at end)
proton donor base

16. How does group 1 metals' density compare to water's?
are less dense than water
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ROR
CH3COO?

17. chromate
Insoluble except nitrate and acetate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CrO4²?
S crystal at 0K=0

18. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Purple
But S° of element is not zero (except at 0K)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

19. bromine
More chaotic (ex: gases made)
CH3COO?
brown volatile liquid
Glacial acetic acid

20. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
diamond and graphite
RCHO (carbonyl at end)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

21. What is the formula for summation?

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22. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salt + water.
Increases down group 1 decreases down group 17

23. What is the slope of the graph of lnk vs. 1/T?
NO3?
Read the bottom of the meniscus
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
-Ea/R

24. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
'non-active' metals such as Cu - Ag - Au - Pt - etc.
do not change
zero

25. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
ROH
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
RX

26. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
hydroxides (ex: Ba(OH)2)
Both electrons come from the same atom (just as good as a regular bond)
ethers
zero

27. How are non-metal oxides and hydrides bonded? are they acidic or basic?
methyl formate
-Ea/R
Insoluble (except group 1 ammonium and Ba)
non-metal oxides and hydrides are covalently bonded and are acidic.

28. Why are i factors (Van't Hoff factors) often less than ideal?
Salt and water
ion pairing
allow for the vapor pressure of water and make sure to level levels
Trigonal pyramidal

29. A Bronsted-Lowry base is...
Disulfur dichloride
Pour liquids using a funnel or down a glass rod
SO4²?
proton acceptor.

30. dihydrogen phosphate
Salts (ex: CaO + SO2 ? CaSO3)
H2PO4?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Trigonal pyramidal

31. hydroxide
Ionic compounds
H2O + CO2 (it decomposes readily)
OH?
Anode

32. Is the ?H formation of an element in standard state zero?
CO (poisonous)
?H formation of an element in standard state=0
Suniverse increases for spontaneous processes
CN?

33. Why are i factors (Van't Hoff factors) often less than ideal?
Disulfur dichloride
S2O3²?
Ionic compounds
ion pairing

34. barium sulfate
blue (BTB)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
White precipitate
Mono; di; tri; tetra; penta; hexa.

35. How are primary alcohols turned into acids?
H3PO4
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Mn²? - Cr³? - Cr³
Unsaturated - addition (ex: decolorize bromine solution)

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

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37. What kind of bonding structure does benzene have?
?H formation of an element in standard state=0
benzene has a delocalized pi ring structure
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Silvery gray solid - brown - purple

38. What are two allotropes of carbon?
diamond and graphite
It ceases - the circuit is broken.
Most are soluble except Ag - Pb
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

39. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
Greenish-yellow gas
S2O3²?
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.

40. acetate
Ksp = 27s4
CH3COO?
Ksp = 4s³
Ksp = 108s5

41. What type of compounds do metals/non metals form?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Soluble
Ionic compounds
ROR

42. How do you identify which is oxidized or otherwise?
O2 needs 4F/mol H2 needs 2F/mol
zero-th: decreases - first: constant - second: increases
look for changes in oxidation # - the one that goes up is oxidized and is the RA
allow for the vapor pressure of water and make sure to level levels

43. sulfates
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Soluble except Ag - Pb - Ca - Sr Ba)
zero
How close results are to the accepted value

44. carbonate
Add acid to water so that the acid doesn't boil and spit
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CO3²?
Ppt will NOT form (unsaturated)

45. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Increases down group 1 decreases down group 17
Ksp = 108s5
NO3?
Soluble

46. What are hybrid orbitals used for?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
it's lower and occurs over less sharp a range
Pour liquids using a funnel or down a glass rod
Making sigma bonds and holding lone pairs

47. When driving off water from a hydrate - how do you tell you're done?
0.10M HCl (more ions)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Soluble
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

48. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
RCOR
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
lighted splint (positive result=pop)

49. What do nonmetal oxides plus water form?
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)
an oxidized and reduced substance
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
acids

50. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
HClO4
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Both electrons come from the same atom (just as good as a regular bond)