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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 is the name of S2Cl2? (Know how to name others like this - too)
An active metal.
Disulfur dichloride
C4H10
Only temperature

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

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3. What things should you remember to do when collecting gas over water?
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.
CO2 and H2O
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
allow for the vapor pressure of water and make sure to level levels

4. What is a dipeptide? polypeptide? protein?
NO3?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Products - reactants (except for BDE when it's reactants - products)

5. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Big K=kf/kr
Products - reactants (except for BDE when it's reactants - products)
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
ROR

6. What do you use to look at burning magnesium? why?
Read the bottom of the meniscus
blue glass - it filters UV
CrO4²?
Evaporation

7. What complex ion does ammonia form with silver? copper? cadmium? zinc?
same KE - but PEice<PEwater
?G=negative - E° must be positive
Eudiometer
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

8. What are the units of the first order rate constant?
Purple
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Products - reactants (except for BDE when it's reactants - products)
K2

9. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
K1 x K2
basic
S2O3²?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

10. What are the products of the reaction between group 1 metals and water?

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11. What is the formula for alkanes?
Kc=Kp
CnH2n+2
Molecules with the same molecular formulas - but different structural formulas
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

12. Ions are not ______.
atoms
basic
Greenish-yellow gas
Decant

13. Esters smell like _______ and amines smell like _______ and are ______.
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
Ksp = 4s³
Most INsoluble except group 1 and ammonium
fruit - fish - bases

14. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Trigonal pyramidal
At half equivalence - pH=pKa
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
The dilution effect when the solutions mix. M1V1 = M2V2

15. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Making sigma bonds and holding lone pairs
RCOOH
#ligands=charge x2
A) any range. b) 8-10 c) 4-6

16. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
Insoluble except nitrate and acetate
water and substances with (s) less dense than
It ceases - the circuit is broken.

17. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Cr2O7²?
yellow
Filtration

18. hydroxide
OH?
Insoluble
It ceases - the circuit is broken.
boiling without losing volatile solvents/reactants

19. cyanide
Decant
Insoluble except group 1 and ammonium
NH2?
CN?

20. What are hybrid orbitals used for?
methyl formate
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
S2O3²?
Making sigma bonds and holding lone pairs

21. lead compounds
Ksp = 4s³
Insoluble except nitrate and acetate
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)
Exothermic (?H for ANY sa/sb = -57kJ/mol)

22. What value of R do you use for thermo calculations? gas calculations?
allow for the vapor pressure of water and make sure to level levels
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Insoluble (except group 1 ammonium and Ba)
Concentration

23. What process do you use to obtain the solute from a solution?
Evaporation
Kc=Kp
left - ppt will form
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

24. What do nonmetal oxides plus water form?
No - it depends on the number of ions produced on dissolving.
Ksp = 4s³
Pale purple - (orange)-yellow - red - blue - green.
acids

25. What is the formula of butane?
C4H10
zero
Disulfur dichloride
RCOR

26. chromate ion (soln + most solids)
Salt + water
Selective absorption
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
yellow

27. What is the sign of the anode in voltaic cells? in electrolytic cells?
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)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
voltaic: - electrolytic: +
Tetrahedral

28. Is the freezing of ice endothermic or exothermic?
|experimental - accepted|/accepted X 100
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Exothermic
Sulfur

29. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
It ceases - the circuit is broken.
catalyst=conc H2SO4
10?8

30. How do you identify which is oxidized or otherwise?
At half equivalence - pH=pKa
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Molecules with the same molecular formulas - but different structural formulas
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

31. What causes the dramatic effect of T on rate?
Exothermic
But S° of element is not zero (except at 0K)
T increases exponentially the proportion of molecules with E > Ea
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

32. What should you check for before you begin titrating?
Molecules with the same molecular formulas - but different structural formulas
CN?
Products - reactants (except for BDE when it's reactants - products)
Check for air bubbles in the buret and remove the buret funnel from the buret

33. Where are group I metals stored?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Group I metals (soft metals) are stored under oil
voltaic: - electrolytic: +
acids

34. chlorine
fractional distillation
All except for lithium
Greenish-yellow gas
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

35. Do anions flow to the cathode or anode?
ClO4?
Anode
ClO?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

36. What do the 'a' and 'b' in Van Der Waal's equation allow for?
ionic and form hydrogen and hydroxide
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acidified
a-IMFs - b-molecular volume

37. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Molecules with the same molecular formulas - but different structural formulas
Exothermic (?H for ANY sa/sb = -57kJ/mol)
a-IMFs - b-molecular volume
acid + alcohol

38. What is the conjugate base of NH3?
Insoluble
T increases exponentially the proportion of molecules with E > Ea
NH2?
Combine the equations for the half reactions in the non-spontaneous direction

39. Lattice energy is high for ions with _____ size and _____ charge
The compound with the lowest Ksp value.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
P2O5
small size and high charge

40. acetates
Soluble
CH3COO?
The benzene ring (or more correctly the phenyl group - C6H5)
CO3²?

41. If a weak acid is diluted more - what happens to its % dissociation value?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
The dilution effect when the solutions mix. M1V1 = M2V2
Increases.
Filtration

42. What is the formula for percent error?
|experimental - accepted|/accepted X 100
look for changes in oxidation # - the one that goes up is oxidized and is the RA
it reacts by substitution NOT addition
It ceases - the circuit is broken.

43. chlorite
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.
same KE - but PEice<PEwater
ClO2?
A salt solution.

44. Ca - Sr - Ba
proton acceptor.
hydroxides (ex: Ba(OH)2)
CN?
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

45. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
water and substances with (s) less dense than
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H3PO4
Concentration

46. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
red - green - blue
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

47. 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?]
Hg²?
fractional distillation
allow for the vapor pressure of water and make sure to level levels

48. What are isomers?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Molecules with the same molecular formulas - but different structural formulas
Glowing splint (positive result=relights)
?H formation of an element in standard state=0

49. What steps do organic labs consist of?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Synthesis - separation and purification of the product and its identification.
Products - reactants (except for BDE when it's reactants - products)

50. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Both electrons come from the same atom (just as good as a regular bond)
Hg2²?
CnH2n+2

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AP Chemistry 2

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