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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. Name C7H16
Pour liquids using a funnel or down a glass rod
Heptane
CnH2n+1 often designated 'R' ex C3H7 is propyl
Identity and purity (impure compounds usually have broad & low melting points)

2. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
Soluble
RCOOH
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)

3. What are isomers?
10?8
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
blue
Molecules with the same molecular formulas - but different structural formulas

4. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Pale yellow
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
+4-covalent - +2-ionic

5. What is the formula for obtaining charge flowing in a cell?
Only temperature
Q=It (time in seconds)
Acidified
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

6. What shape is water?
zero
bent
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Suniverse increases for spontaneous processes

7. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
lighted splint (positive result=pop)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

8. What are allotropes?
H2PO4?
Iodine and CO2 (dry ice)
different forms of the same element
CN?

9. What is the general formula for an acid?
White precipitate
zero
CN?
RCOOH

10. phosphate
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Experimental mass/theoretical mass X 100
PO4³?
Insoluble

11. What is the first law of thermodynamics?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
blue
blue (BTB)
E=q + w (negative is by system - positive is on system)

12. chlorite
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?)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
ClO2?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

13. When a cell is 'flat' What is its voltage?
K2
zero
Combine the equations for the half reactions in the non-spontaneous direction
CnH2n

14. Aromatic compounds contain what?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
The benzene ring (or more correctly the phenyl group - C6H5)
Evaporation
Acid rain - dissolves marble buildings/statues and kills trees.

15. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Disulfur dichloride
Read the bottom of the meniscus
Mn²? - Cr³? - Cr³
voltaic: + electrolytic: -

16. What do you use to look at burning magnesium? why?
an oxidized and reduced substance
Most are soluble except Ag - Pb
blue
blue glass - it filters UV

17. What is the conjugate acid of H2PO4?
Tetrahedral
Acidified
H3PO4
0 and 14

18. The definition of acidic basic and neutral aqueous solutions is:
ClO?
Iodine and CO2 (dry ice)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Pour liquids using a funnel or down a glass rod

19. What do you do to get rid of most of the solution from a precipitate?
Decant
H2O + CO2 (it decomposes readily)
Insoluble except group 1 and ammonium
?H formation of an element in standard state=0

20. What is the general formula for an ether?
Eudiometer
ROR
Big K=kf/kr
Increases down group 1 decreases down group 17

21. What is the third law of thermodynamics?
Group 1 hydroxides (ex: NaOH)
H2O + CO2 (it decomposes readily)
All except for lithium
S crystal at 0K=0

22. What is the formula for alkenes?
CnH2n
are less dense than water
RCOOH
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?)

23. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
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?)
diamond and graphite
by electrolysis

24. What is H2CO3 (carbonate acid) usually written as?
[A?]/[HA] x 100 or [BH?]/[B] x 100
methyl formate
All except for lithium
H2O + CO2 (it decomposes readily)

25. Alcohols and _______ are FG isomers
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.
ethers
CO (poisonous)
bases

26. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CrO4²?
#ligands=charge x2
Ions go through the salt bridge - electrons go through metal wires in the external circuit

27. What does a short - sharp melting point indicate?
But S° of element is not zero (except at 0K)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Identity and purity (impure compounds usually have broad & low melting points)
Soluble

28. When the salt bridge is removed what happens to the cell reaction?
CnH2n
It ceases - the circuit is broken.
Big K=kf/kr
RCHO (carbonyl at end)

29. What are the signs of ?G and E° for spontaneous reactions?
OH- and NH3
?G=negative - E° must be positive
acids
Hg2²?

30. ammonium/ammonium compounds
brown volatile liquid
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.
allow for the vapor pressure of water and make sure to level levels
Soluble

31. sulfates
do not change
Soluble except Ag - Pb - Ca - Sr Ba)
Filtration
red - green - blue

32. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Combine the equations for the half reactions in the non-spontaneous direction
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
The dilution effect when the solutions mix. M1V1 = M2V2

33. Generally - which oxy acid is strongest?
Q=It (time in seconds)
Anode - oxygen. Cathode - hydrogen
The one with most oxygen atoms (highest oxidation number)
by electrolysis

34. chlorate
|experimental - accepted|/accepted X 100
Making sigma bonds and holding lone pairs
ClO3?
diamond and graphite

35. What value of R do you use for thermo calculations? gas calculations?
CO (poisonous)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
?G=negative - E° must be positive
ethers

36. Acids + Carbonates (bicarbonates) make?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
NO3?

37. What shape is ammonia?
Pale yellow
non-metal oxides and hydrides are covalently bonded and are acidic.
H2PO4?
Trigonal pyramidal

38. What are two allotropes of carbon?
Both electrons come from the same atom (just as good as a regular bond)
Ppt will NOT form (unsaturated)
ClO4?
diamond and graphite

39. What is the energy you must put into a reaction to make it start called?
10?8
Initiation energy (NOT Ea)
blue
Acids; HCOOCH3 is an ester

40. chlorine
bent
Soluble
a-IMFs - b-molecular volume
Greenish-yellow gas

41. What are the signs for ?G and E° for spontaneous reactions?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
?G= -ve - E°= +ve
The dilution effect when the solutions mix. M1V1 = M2V2

42. Which alkali metals float on water?
Increases down group 1 decreases down group 17
S crystal at 0K=0
ionic and form hydrogen and hydroxide
All except for lithium

43. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
zero-th: decreases - first: constant - second: increases
Heptane
+4-covalent - +2-ionic
10?8

44. What word is a clue for a redox reaction?
Acidified
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Salt and water
The dilution effect when the solutions mix. M1V1 = M2V2

45. What electrons are lost/gained first in transition element ions?
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?)
ns² electrons (first in-first out)
different forms of the same element
O2 needs 4F/mol H2 needs 2F/mol

46. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
H2O + CO2 (it decomposes readily)
HClO4
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

47. When is ?G zero?
Cr2O7²?
?G= -ve - E°= +ve
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
different forms of the same element

48. BaSO4
Insoluble
+4-covalent - +2-ionic
S2O3²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

49. If a free element is involved - what type of reaction must be involved?
C2O4²?
OH?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
redox reaction

50. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Evaporation
ClO2?
do not change
Unsaturated - addition (ex: decolorize bromine solution)

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AP Chemistry 2

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