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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Where are group I metals stored?
P2O5
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)
Group I metals (soft metals) are stored under oil

2. What do the 'a' and 'b' in Van Der Waal's equation allow for?
ROH
a-IMFs - b-molecular volume
A salt solution.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

3. When a cell is 'flat' What is its voltage?
acids
Salts (ex: CaO + SO2 ? CaSO3)
CnH(2n+2)
zero

4. perchlorate
ClO4?
Unsaturated - addition (ex: decolorize bromine solution)
All except for lithium
Ksp = 27s4

5. What process do you use to obtain a solvent from a solution?
Distillation
Trigonal pyramidal
Glowing splint (positive result=relights)
Heat a test tube at an angle at the side of the tube (not bottom)

6. Alcohols and _______ are FG isomers
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
RCOOR
HClO4
ethers

7. How does benzene compare in reactivity to alkenes?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Suniverse increases for spontaneous processes
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
benzene is less reactive than alkenes

8. Color is due to ______ _______ of light.
Conjugate pair (one must be a weak base or acid)
linear
Acid rain - dissolves marble buildings/statues and kills trees.
Selective absorption

9. What part of a liquid do you look at to measure its volume?
lighted splint (positive result=pop)
Eudiometer
zero-th: decreases - first: constant - second: increases
Read the bottom of the meniscus

10. How do you get the equation for a net electrolysis reaction?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
are less dense than water
blue
Combine the equations for the half reactions in the non-spontaneous direction

11. What process do you use to obtain the solute from a solution?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Group I metals (soft metals) are stored under oil
Evaporation
S2O3²?

12. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Sigma bonds are stronger than pi bonds
Ksp = s²
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
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

13. ammonium/ammonium compounds
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
H3PO4
Soluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

14. What do group I/II metal oxides plus water form?
How grouped results are
bases
ion pairing
HClO4

15. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
It ceases - the circuit is broken.
CO (poisonous)
T increases exponentially the proportion of molecules with E > Ea

16. What is the catalyst for this reaction Ester + ?
[A?]/[HA] x 100 or [BH?]/[B] x 100
K1 x K2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
catalyst=conc H2SO4

17. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
NH4?
Exothermic (?H for ANY sa/sb = -57kJ/mol)

18. 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
No - NH3 and HCl gases are extremely soluble
K2
zero

19. What electrons are lost/gained first in transition element ions?
ROH
diamond and graphite
acids
ns² electrons (first in-first out)

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

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21. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Acids; HCOOCH3 is an ester
fruit - fish - bases
T increases exponentially the proportion of molecules with E > Ea

22. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Ksp = 108s5
zero
brown volatile liquid
C4H10

23. What are two substances that sublime at 1 atm when heated?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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.
Iodine and CO2 (dry ice)
basic

24. What does saturated mean? Unsaturated?
Cr2O7²?
Salts (ex: CaO + SO2 ? CaSO3)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
atoms

25. 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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26. What two compounds are great oxidizing agents?

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27. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Both electrons come from the same atom (just as good as a regular bond)
The benzene ring (or more correctly the phenyl group - C6H5)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
proton donor base

28. What is the conjugate base of NH3?
same KE - but PEice<PEwater
NH2?
Initiation energy (NOT Ea)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

29. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Combine the equations for the half reactions in the non-spontaneous direction
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
water and substances with (s) less dense than
Kc=Kp

30. What is the formula for obtaining charge flowing in a cell?
Iodine and CO2 (dry ice)
Q=It (time in seconds)
Soluble
Ksp = 27s4

31. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Insoluble except nitrate and acetate
Separating funnel
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Synthetic condensation polymer (aka a polyamide)

32. sulfate
SO4²?
Insoluble except nitrate and acetate
Q=It (time in seconds)
Salt and water

33. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
do not change
Trigonal pyramidal

34. Why are i factors (Van't Hoff factors) often less than ideal?
?H-kJ - ?S-J - ?G-kJ
Molecules with the same molecular formulas - but different structural formulas
ion pairing
O2 needs 4F/mol H2 needs 2F/mol

35. Esterification is...
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
acid + alcohol
Mono; di; tri; tetra; penta; hexa.
brown volatile liquid

36. How does the melting point of a mixture compare to the MP of a pure substance?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
it is lower and occurs over less sharp a range
Transition element compounds (except if it has a full or empty d shell)
CN?

37. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
CO (poisonous)
blue
different forms of the same element
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

38. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Glacial acetic acid
ethers

39. barium sulfate
ROH
water and substances with (s) less dense than
White precipitate
NH4?

40. What is the formula for percent error?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
The one with most oxygen atoms (highest oxidation number)
R=8.31 J/mol/K
|experimental - accepted|/accepted X 100

41. lead compounds
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Insoluble except nitrate and acetate
[A?]/[HA] x 100 or [BH?]/[B] x 100

42. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ClO3?
Tetrahedral
CnH2n+1 often designated 'R' ex C3H7 is propyl

43. What do metal oxides plus non- metal oxides form?
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
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.
Salts (ex: CaO + SO2 ? CaSO3)

44. What are isomers?
hydroxides (ex: Ba(OH)2)
Molecules with the same molecular formulas - but different structural formulas
Most are soluble except Ag - Pb
Pale purple - (orange)-yellow - red - blue - green.

45. How does group 1 metals' density compare to water's?
chemically (ex: with carbon)
RCOOH
are less dense than water
Exothermic (?H for ANY sa/sb = -57kJ/mol)

46. Lattice energy is high for ions with _____ size and _____ charge
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
An active metal.
small size and high charge
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

47. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Soluble
Ppt will NOT form (unsaturated)
q=mc?T q=mL (or n x ?h)

48. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
The one with most oxygen atoms (highest oxidation number)
same KE - but PEice<PEwater
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Making sigma bonds and holding lone pairs

49. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
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
Iodine and CO2 (dry ice)
Silvery gray solid - brown - purple

50. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ksp = 27s4
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
The compound with the lowest Ksp value.

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AP Chemistry 2

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