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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. chlorate
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Saturated - Substitution (which requires more radical conditions)
ClO3?
no - they're written undissociated (HAaq)

2. 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.
blue (BTB)
acid + alcohol
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

3. What electrons are lost/gained first in transition element ions?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
are less dense than water
ns² electrons (first in-first out)
PO4³?

4. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ionic compounds
blue glass - it filters UV
Orange
Ions go through the salt bridge - electrons go through metal wires in the external circuit

5. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
ROH
Big K=kf/kr
P2O5
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

6. Name six characteristics of transition elements (or their compounds)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
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)
Q=It (time in seconds)
Iodine and CO2 (dry ice)

7. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
10?8
-Ea/R
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

8. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
CO3²?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Glowing splint (positive result=relights)

9. What is an Alkyl group?

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10. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
a-IMFs - b-molecular volume
diamond and graphite

11. What is the first law of thermodynamics?
RCOR
They stay the same.
proton acceptor.
E=q + w (negative is by system - positive is on system)

12. Lattice energy is high for ions with _____ size and _____ charge
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
small size and high charge
ion pairing
basic

13. Nonmetals are good _____ agents. Metals are good _______ agents.
allow for the vapor pressure of water and make sure to level levels
Sulfur
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Molecules with the same molecular formulas - but different structural formulas

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

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15. hydroxides
RX
Insoluble (except group 1 ammonium and Ba)
Mono; di; tri; tetra; penta; hexa.
Decant

16. carbonates
Insoluble except group 1 and ammonium
Unsaturated - addition (ex: decolorize bromine solution)
H3PO4
Evaporation

17. How does half life change for zero-th order - first order - and second order processes?
Insoluble except nitrate and acetate
zero-th: decreases - first: constant - second: increases
HClO4
lighted splint (positive result=pop)

18. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
CnH2n+2
yellow
same KE - but PEice<PEwater

19. What steps do organic labs consist of?
Exothermic
Synthesis - separation and purification of the product and its identification.
Kc=Kp
Evaporation

20. 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?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
0 and 14
Salts (ex: CaO + SO2 ? CaSO3)
The compound with the lowest Ksp value.

21. If Q < Ksp a ppt ______
T increases exponentially the proportion of molecules with E > Ea
Ppt will NOT form (unsaturated)
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
zero

22. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
Saturated - Substitution (which requires more radical conditions)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Disulfur dichloride

23. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Synthetic condensation polymer (aka a polyamide)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

24. What is H2CO3 (carbonate acid) usually written as?
T increases exponentially the proportion of molecules with E > Ea
Pale yellow
H2O + CO2 (it decomposes readily)
Soluble

25. What things should you remember to do when collecting gas over water?
Disulfur dichloride
allow for the vapor pressure of water and make sure to level levels
ClO2?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

26. What are amphoteric oxides?
Trigonal pyramidal
CrO4²?
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?)
benzene has a delocalized pi ring structure

27. During a titration what is present in the beaker at the equivalence point?
Hg2²?
Silvery gray solid - brown - purple
do not change
A salt solution.

28. thiosulfate
CrO4²?
?G=negative - E° must be positive
Evaporation
S2O3²?

29. Does Kw increase or decrease with T? Why?
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.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
ion pairing

30. What changes Keq?
Only temperature
water and substances with (s) less dense than
ClO2?
bases

31. How do you explain trends in atomic properties using Coulomb's Law?
Increases.
Salts (ex: CaO + SO2 ? CaSO3)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
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

32. potassium permanganate
Anode - oxygen. Cathode - hydrogen
Purple
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

33. What do group I/II metal oxides plus water form?
Ionic compounds
bases
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.
ClO4?

34. dihydrogen phosphate
H2PO4?
Insoluble except nitrate and acetate
R=8.31 J/mol/K
benzene is less reactive than alkenes

35. permanganate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Synthetic condensation polymer (aka a polyamide)
MnO4?
Distillation

36. halides
Nothing
Most are soluble except Ag - Pb
Cr2O7²?
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

37. Does reactivity increase/decrease going down group 1 and group 17?
No - NH3 and HCl gases are extremely soluble
Increases down group 1 decreases down group 17
CH3COO?
Eudiometer

38. Does Benzene react by addition or substitution?
Perform ICE BOX calculation based on K1
hydroxides (ex: Ba(OH)2)
proton donor base
it reacts by substitution NOT addition

39. What is accuracy?
Saturated - Substitution (which requires more radical conditions)
#ligands=charge x2
How close results are to the accepted value
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)

40. What reacts with an acid to create hydrogen gas?
An active metal.
voltaic: + electrolytic: -
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Unsaturated - addition (ex: decolorize bromine solution)

41. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Separating funnel
Big K=kf/kr
it reacts by substitution NOT addition

42. What shape is methane?
Tetrahedral
10?8
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Kc=Kp

43. What word is a clue for a redox reaction?
CO3²?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Current - time and charge on ion (moles of e used in half cell reaction)
Acidified

44. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
blue glass - it filters UV
same KE - but PEice<PEwater

45. chlorite
Pour liquids using a funnel or down a glass rod
different forms of the same element
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
ClO2?

46. What is the relationship in strength between sigma and pi bonds?
Disulfur dichloride
Sigma bonds are stronger than pi bonds
Greenish-yellow gas
Purple

47. What things should you remember to do when collecting gas over water?
Heptane
allow for the vapor pressure of water and make sure to level levels
?H-kJ - ?S-J - ?G-kJ
Current - time and charge on ion (moles of e used in half cell reaction)

48. What is the general formula for a ketone?
Cr2O7²?
Anode - oxygen. Cathode - hydrogen
Pale yellow
RCOR

49. Where are group I metals stored?
brown volatile liquid
CO3²?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Group I metals (soft metals) are stored under oil

50. What are the prefixes for the naming of binary molecular compound formulas (up to six)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Ppt will NOT form (unsaturated)
Mono; di; tri; tetra; penta; hexa.
ionic and form hydrogen and hydroxide

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AP Chemistry 2

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