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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 shape is methane?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Tetrahedral
RX
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.

2. cyanide
CN?
PO4³?
NH4?
ClO4?

3. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
RCHO (carbonyl at end)
diamond and graphite

4. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
Ionic compounds
No - NH3 and HCl gases are extremely soluble
metal oxides and hydrides are ionically bonded and basic

5. ________ are Lewis bases - because they can donate a lone pair of electrons.
Group 1 hydroxides (ex: NaOH)
OH- and NH3
strong acids/bases are written as H+ or OH- ions
ClO2?

6. 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?
ClO3?
The compound with the lowest Ksp value.
Graduated cylinder
Decant

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

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8. What do you use for an acid spill? base spill?
Iodine and CO2 (dry ice)
No - it depends on the number of ions produced on dissolving.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
ClO3?

9. Give an example of a concentrated weak acid.
Ppt will NOT form (unsaturated)
Perform ICE BOX calculation based on K1
Glacial acetic acid
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

10. How are more active metals reduced?
All except for lithium
0.10M HCl (more ions)
Silvery gray solid - brown - purple
by electrolysis

11. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Selective absorption
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
water and substances with (s) less dense than

12. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
proton donor base
Graduated cylinder

13. hydroxides
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Insoluble (except group 1 ammonium and Ba)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
?G= -ve - E°= +ve

14. What causes the dramatic effect of T on rate?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
are less dense than water
?H-kJ - ?S-J - ?G-kJ
T increases exponentially the proportion of molecules with E > Ea

15. ammonium/ammonium compounds
Pipette (burette if need repetition)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Soluble
benzene is less reactive than alkenes

16. Lattice energy is high for ions with _____ size and _____ charge
S crystal at 0K=0
small size and high charge
0.10M HCl (more ions)
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

17. How does group 1 metals' density compare to water's?
Saturated - Substitution (which requires more radical conditions)
OH- and NH3
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
are less dense than water

18. phosphates
small size and high charge
RCOOH
Most INsoluble except group 1 and ammonium
Ionic compounds

19. What is the formula for percent error?
|experimental - accepted|/accepted X 100
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ion pairing

20. Ions are not ______.
T increases exponentially the proportion of molecules with E > Ea
H2PO4?
C4H10
atoms

21. What type of polymer is nylon?
benzene is less reactive than alkenes
small size and high charge
K2
Synthetic condensation polymer (aka a polyamide)

22. hypochlorite
boiling without losing volatile solvents/reactants
ClO?
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)
Insoluble (except group 1 ammonium and Ba)

23. What is the general formula for alkyl halides?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Anode
Ksp = 4s³
RX

24. Name six characteristics of transition elements (or their compounds)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
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)
Increases.
The Faraday or Faraday's constant.

25. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Combine the equations for the half reactions in the non-spontaneous direction
How close results are to the accepted value
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

26. primary colors
Greenish-yellow gas
Most INsoluble except group 1 and ammonium
Only temperature
red - green - blue

27. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Perform ICE BOX calculation based on K1
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

28. chromate
CrO4²?
Sulfur
same KE - but PEice<PEwater
Ksp = 108s5

29. What are hybrid orbitals used for?
fruit - fish - bases
Cr2O7²?
acids
Making sigma bonds and holding lone pairs

30. Color is due to ______ _______ of light.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Filtration
bright yellow
Selective absorption

31. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
#ligands=charge x2
Glowing splint (positive result=relights)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

32. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
Decant
Anode - oxygen. Cathode - hydrogen
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

33. What are two substances that sublime at 1 atm when heated?
S crystal at 0K=0
Iodine and CO2 (dry ice)
blue glass - it filters UV
OH?

34. The definition of acidic basic and neutral aqueous solutions is:
left - ppt will form
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
fractional distillation
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

35. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
How grouped results are
Anode - oxygen. Cathode - hydrogen

36. barium sulfate
White precipitate
benzene is less reactive than alkenes
Distillation
ns² electrons (first in-first out)

37. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Mono; di; tri; tetra; penta; hexa.
left - ppt will form
Acid rain - dissolves marble buildings/statues and kills trees.

38. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
S crystal at 0K=0
ClO4?
Kc=Kp

39. What changes Keq?
Only temperature
Unsaturated - addition (ex: decolorize bromine solution)
basic
-Ea/R

40. If ?S is positive - are the products more or less chaotic than the reactants?
Orange
Evaporation
Group I metals (soft metals) are stored under oil
More chaotic (ex: gases made)

41. Ca - Sr - Ba
ClO2?
R=8.31 J/mol/K
The Faraday or Faraday's constant.
hydroxides (ex: Ba(OH)2)

42. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
red - green - blue
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Ksp = 108s5
+4-covalent - +2-ionic

43. Metal hydrides are _____ and form _______ and _______ when added to water
How close results are to the accepted value
ion pairing
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ionic and form hydrogen and hydroxide

44. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
H2O + CO2 (it decomposes readily)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
ns² electrons (first in-first out)

45. What is HCOOCH3?
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?)
Acids; HCOOCH3 is an ester
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)
by electrolysis

46. Give an example of a dilute strong acid.
HClO4
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Iodine and CO2 (dry ice)
Add acid to water so that the acid doesn't boil and spit

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

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48. What process do you use to obtain the precipitate from a solution?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ClO2?
Filtration
O2 needs 4F/mol H2 needs 2F/mol

49. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Acidified
Check for air bubbles in the buret and remove the buret funnel from the buret
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Insoluble except for nitrate and acetate

50. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Add acid to water so that the acid doesn't boil and spit
CrO4²?
RCOOR
do not change

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AP Chemistry 2

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