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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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1. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Pour liquids using a funnel or down a glass rod
neutralization: high K - H2O product dissociation: low K - H2O reactant
RX
Mono; di; tri; tetra; penta; hexa.

2. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
More chaotic (ex: gases made)
All except for lithium
allow for the vapor pressure of water and make sure to level levels

3. What is the name of S2Cl2? (Know how to name others like this - too)
At half equivalence - pH=pKa
Disulfur dichloride
zero
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

4. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
They stay the same.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

5. silver compounds
Insoluble except for nitrate and acetate
proton acceptor.
RNH2
voltaic: + electrolytic: -

6. sulfates
bases
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Soluble except Ag - Pb - Ca - Sr Ba)
+4-covalent - +2-ionic

7. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
water and substances with (s) less dense than
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)
PO4³?

8. How are more active metals reduced?
by electrolysis
Insoluble (except group 1 ammonium and Ba)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Heptane

9. nitrate
NO3?
Increases.
Mono; di; tri; tetra; penta; hexa.
?H formation of an element in standard state=0

10. What type of compounds are almost always colored?
NH4?
strong acids/bases are written as H+ or OH- ions
Transition element compounds (except if it has a full or empty d shell)
Most INsoluble except group 1 and ammonium

11. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
At half equivalence - pH=pKa
Suniverse increases for spontaneous processes
0 and 14

12. For a dibasic acid (H2A) - [A²?]= ____ ?
do not change
K2
Concentration
A) any range. b) 8-10 c) 4-6

13. At what point during titration do you have the perfect buffer - and what is the pH at this point?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
|experimental - accepted|/accepted X 100
MnO4?
At half equivalence - pH=pKa

14. Name six characteristics of transition elements (or their compounds)
Soluble
RCOOH
are less dense than water
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)

15. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
ion pairing
Monomer + monomer = polymer product + a simple molecule such as water or HCl
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

16. What are the names and formulas of the 6 strong acids?
by electrolysis
Greenish-yellow gas
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Orange

17. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
#ligands=charge x2
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
The one with most oxygen atoms (highest oxidation number)

18. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
bases
Group 1 hydroxides (ex: NaOH)
basic
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

19. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Greenish-yellow gas
The benzene ring (or more correctly the phenyl group - C6H5)
water and substances with (s) less dense than

20. What is accuracy?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
How close results are to the accepted value
Kc=Kp

21. What do metal oxides plus acids form?
Combine the equations for the half reactions in the non-spontaneous direction
Salt + water
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Separating funnel

22. What shape is carbon dioxide?
RCOR
NH4?
Separating funnel
linear

23. How does group 1 metals' density compare to water's?
+4-covalent - +2-ionic
red - green - blue
CnH2n+1 often designated 'R' ex C3H7 is propyl
are less dense than water

24. What is the basic structure of an optical isomer?
Greenish-yellow gas
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
RCHO (carbonyl at end)
Disulfur dichloride

25. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
RCHO (carbonyl at end)
Current - time and charge on ion (moles of e used in half cell reaction)
Anode

26. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
Clear
yellow
blue glass - it filters UV

27. What is precision?
zero
How grouped results are
Combine the equations for the half reactions in the non-spontaneous direction
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

28. What is the relationship in strength between sigma and pi bonds?
Soluble
redox reaction
Sigma bonds are stronger than pi bonds
Insoluble

29. What is the word equation for addition polymerisation?
Initiation energy (NOT Ea)
It ceases - the circuit is broken.
OH?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

30. What is reflux?
boiling without losing volatile solvents/reactants
redox reaction
diamond and graphite
ROR

31. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
ion pairing
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)
Initiation energy (NOT Ea)

32. acetates
Soluble
zero
bases
CO2 and H2O

33. What is an Alkyl group?

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34. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Separating funnel
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.

35. What are two allotropes of carbon?
How grouped results are
diamond and graphite
Sulfur
It ceases - the circuit is broken.

36. What is the sign of the anode in voltaic cells? in electrolytic cells?
do not change
voltaic: - electrolytic: +
H3PO4
red - green - blue

37. What word is a clue for a redox reaction?
linear
Acidified
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

38. How are strong ones written?
Purple
strong acids/bases are written as H+ or OH- ions
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
red - green - blue

39. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Increases down group 1 decreases down group 17
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
[A?]/[HA] x 100 or [BH?]/[B] x 100
'non-active' metals such as Cu - Ag - Au - Pt - etc.

40. Do you use J or kJ for ?H - ?S - and ?G?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
?H-kJ - ?S-J - ?G-kJ
benzene has a delocalized pi ring structure
RCOOH

41. What process do you use to obtain the precipitate from a solution?
Anode
Filtration
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

42. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
allow for the vapor pressure of water and make sure to level levels
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
it is lower and occurs over less sharp a range

43. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
blue
look for changes in oxidation # - the one that goes up is oxidized and is the RA
K1 x K2
non-metal oxides and hydrides are covalently bonded and are acidic.

44. Acidic gases like SO2 in the atmosphere cause what environmental problems?
How close results are to the accepted value
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acid rain - dissolves marble buildings/statues and kills trees.

45. bromothymol
blue (BTB)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
The one with most oxygen atoms (highest oxidation number)
Making sigma bonds and holding lone pairs

46. What changes Keq?
proton acceptor.
acids
Only temperature
Conjugate pair (one must be a weak base or acid)

47. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Current - time and charge on ion (moles of e used in half cell reaction)
bases
Pale purple - (orange)-yellow - red - blue - green.
voltaic: + electrolytic: -

48. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Acidified
The benzene ring (or more correctly the phenyl group - C6H5)

49. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Both electrons come from the same atom (just as good as a regular bond)
Perform ICE BOX calculation based on K1
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Kc=Kp

50. mercury (II) ion
RCOOH
Purple
Hg²?
an oxidized and reduced substance

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AP Chemistry 2

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