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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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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. If Q > Ksp - then system shifts _______ and ppt ______
blue
left - ppt will form
?G= -ve - E°= +ve
fractional distillation

2. silver iodide
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
Most are soluble except Ag - Pb
Pale yellow
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

3. What do group I/II metal oxides plus water form?
bases
an oxidized and reduced substance
Glowing splint (positive result=relights)
Combine the equations for the half reactions in the non-spontaneous direction

4. How does the melting point of a mixture compare to the MP of a pure substance?

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5. What complex ion does ammonia form with silver? copper? cadmium? zinc?
basic
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Group I metals (soft metals) are stored under oil
Acidified

6. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Ksp = 27s4
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Q=It (time in seconds)

7. Neutralization is an ________ reaction.
blue
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Orange

8. What is the formula for percent yield?
Current - time and charge on ion (moles of e used in half cell reaction)
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?)
Experimental mass/theoretical mass X 100
NH4?

9. The definition of acidic basic and neutral aqueous solutions is:
0.10M HCl (more ions)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Hg2²?
Insoluble except nitrate and acetate

10. How does group 1 metals' density compare to water's?
basic
Ionic compounds
ionic and form hydrogen and hydroxide
are less dense than water

11. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
T increases exponentially the proportion of molecules with E > Ea
acids
Soluble
Kc=Kp

12. Ions are not ______.
atoms
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
NH4?
0.10M HCl (more ions)

13. potassium permanganate
ROR
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Clear
Purple

14. What type of solutions do small - highly charged cations tend to form?
acids
Both electrons come from the same atom (just as good as a regular bond)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
H3PO4

15. How can metals like iron and zinc be reduced?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ROH
chemically (ex: with carbon)
CnH2n

16. What is the formula of copper (II) phosphate?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Cu3(PO4)2
0.10M HCl (more ions)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

17. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
proton acceptor.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Unsaturated - addition (ex: decolorize bromine solution)

18. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Anode - oxygen. Cathode - hydrogen

19. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
proton donor base
yellow
H+

20. ammonium/ammonium compounds
boiling without losing volatile solvents/reactants
Big K=kf/kr
Soluble
Initiation energy (NOT Ea)

21. What are isotopes?
Mono; di; tri; tetra; penta; hexa.
CO3²?
Combine the equations for the half reactions in the non-spontaneous direction
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

22. What do you use for an acid spill? base spill?
Unsaturated - addition (ex: decolorize bromine solution)
SO4²?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

23. Do you use J or kJ for ?H - ?S - and ?G?
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
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?)
?H-kJ - ?S-J - ?G-kJ
Pour liquids using a funnel or down a glass rod

24. When is ?G zero?
Acidified
Disulfur dichloride
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
it reacts by substitution NOT addition

25. What are two substances that sublime at 1 atm when heated?
lighted splint (positive result=pop)
blue
Iodine and CO2 (dry ice)
water and substances with (s) less dense than

26. What type of compounds do Group 14 form?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
+4-covalent - +2-ionic
Disulfur dichloride
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

27. What is accuracy?
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)
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
T increases exponentially the proportion of molecules with E > Ea
How close results are to the accepted value

28. Name some properties of Group 17
Ions go through the salt bridge - electrons go through metal wires in the external circuit
CO3²?
ClO?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

29. Is the freezing of ice endothermic or exothermic?
Exothermic
Soluble except Ag - Pb - Ca - Sr Ba)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Mn²? - Cr³? - Cr³

30. What is the word equation for condensation polymerisation ?
diamond and graphite
Monomer + monomer = polymer product + a simple molecule such as water or HCl
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ns² electrons (first in-first out)

31. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
Glacial acetic acid
No - it depends on the number of ions produced on dissolving.
Salt + water

32. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Heat a test tube at an angle at the side of the tube (not bottom)
yellow

33. Can you collect soluble gases over water?
redox reaction
Ppt will NOT form (unsaturated)
No - NH3 and HCl gases are extremely soluble
Glowing splint (positive result=relights)

34. phosphates
Most INsoluble except group 1 and ammonium
same KE - but PEice<PEwater
K2
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

35. What do metal oxides plus non- metal oxides form?
The benzene ring (or more correctly the phenyl group - C6H5)
Salts (ex: CaO + SO2 ? CaSO3)
RCHO (carbonyl at end)
Selective absorption

36. perchlorate
Trigonal pyramidal
ClO4?
boiling without losing volatile solvents/reactants
proton donor base

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

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38. What is the difference between equivalence point and end point of a titration.
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
yellow
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
fruit - fish - bases

39. What apparatus do you use to pour liquids?
Orange
Pour liquids using a funnel or down a glass rod
Exothermic
RCOOR

40. 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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41. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
Silvery gray solid - brown - purple
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
zero

42. What is the general formula of an alkane?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
OH- and NH3
ns² electrons (first in-first out)
CnH(2n+2)

43. Which of the rates changes more when temperature is increased?
zero-th: decreases - first: constant - second: increases
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Products - reactants (except for BDE when it's reactants - products)
CnH2n-2

44. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
small size and high charge
CnH2n+2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
How close results are to the accepted value

45. What two compounds are great oxidizing agents?

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46. What do you need to make a polymer?
non-metal oxides and hydrides are covalently bonded and are acidic.
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)
E=q + w (negative is by system - positive is on system)

47. sulfate
Products - reactants (except for BDE when it's reactants - products)
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero
SO4²?

48. What are amphoteric oxides?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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?)
Experimental mass/theoretical mass X 100
hydroxides (ex: Ba(OH)2)

49. bromine
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Salt + water.
ns² electrons (first in-first out)
brown volatile liquid

50. What are the signs of ?G and E° for spontaneous reactions?
Kc=Kp
E=q + w (negative is by system - positive is on system)
Filtration
?G=negative - E° must be positive

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AP Chemistry 2

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