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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. What is the general formula for a ketone?
RCOR
Soluble
Hg²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

2. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
RX
Soluble
Add acid to water so that the acid doesn't boil and spit

3. What are two allotropes of carbon?
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
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
diamond and graphite
No - NH3 and HCl gases are extremely soluble

4. Is the ?H formation of an element in standard state zero?
Iodine and CO2 (dry ice)
allow for the vapor pressure of water and make sure to level levels
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
?H formation of an element in standard state=0

5. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
diamond and graphite
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
At half equivalence - pH=pKa

6. Metal hydrides are _____ and form _______ and _______ when added to water
Distillation
CnH2n+2
ionic and form hydrogen and hydroxide
'non-active' metals such as Cu - Ag - Au - Pt - etc.

7. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
S2O3²?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
R=8.31 J/mol/K

8. What two types of substances are present in all redox reactions?
Soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
an oxidized and reduced substance
P2O5

9. Can you collect soluble gases over water?
strong acids/bases are written as H+ or OH- ions
No - NH3 and HCl gases are extremely soluble
catalyst=conc H2SO4
Increases down group 1 decreases down group 17

10. A geometric (or cis-trans) isomer exists due to.....
The Faraday or Faraday's constant.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

11. Color is due to ______ _______ of light.
NH2?
Selective absorption
Salt + water
Reduction always takes place at the cathode (RED CAT) In both types of cell!

12. What is the test for oxygen?
Check for air bubbles in the buret and remove the buret funnel from the buret
q=mc?T q=mL (or n x ?h)
Glowing splint (positive result=relights)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

13. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Big K=kf/kr
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
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
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

14. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
No - NH3 and HCl gases are extremely soluble
Big K=kf/kr
same KE - but PEice<PEwater
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

15. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Mono; di; tri; tetra; penta; hexa.
proton acceptor.
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)

16. carbonates
A) any range. b) 8-10 c) 4-6
Insoluble except for nitrate and acetate
Insoluble except group 1 and ammonium
H3PO4

17. Give an example of a concentrated weak acid.
Glacial acetic acid
an oxidized and reduced substance
Initiation energy (NOT Ea)
H2O + CO2 (it decomposes readily)

18. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
At half equivalence - pH=pKa
Synthesis - separation and purification of the product and its identification.
Eudiometer

19. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
0.10M HCl (more ions)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

20. What do hydrocarbons form when they burn in air (oxygen)?
voltaic: + electrolytic: -
+4-covalent - +2-ionic
PO4³?
CO2 and H2O

21. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Group 1 hydroxides (ex: NaOH)
RX

22. How do you dilute an acid?

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23. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
CnH2n+1 often designated 'R' ex C3H7 is propyl
CnH2n-2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

24. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
H2O + CO2 (it decomposes readily)

25. Esterification is...
Molecules with the same molecular formulas - but different structural formulas
acid + alcohol
diamond and graphite
blue glass - it filters UV

26. What type of compounds do Group 14 form?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
+4-covalent - +2-ionic
?H formation of an element in standard state=0
CO3²?

27. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
bright yellow
Selective absorption
RCOOR

28. Alcohols and _______ are FG isomers
allow for the vapor pressure of water and make sure to level levels
ethers
Filtration
acids

29. The definition of acidic basic and neutral aqueous solutions is:
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
NO3?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
C4H10

30. What two compounds are great oxidizing agents?

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31. Name C7H16
Soluble
H2O + CO2 (it decomposes readily)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Heptane

32. What is the general formula for an amine?
Only temperature
RNH2
The dilution effect when the solutions mix. M1V1 = M2V2
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

33. Is the standard entropy (S°) of an element zero?
RCOOH
But S° of element is not zero (except at 0K)
Synthetic condensation polymer (aka a polyamide)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

34. 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?
Heat a test tube at an angle at the side of the tube (not bottom)
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
a-IMFs - b-molecular volume
The one with most oxygen atoms (highest oxidation number)

35. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Eudiometer
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.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
basic

36. What is the test for hydrogen?
Acids; HCOOCH3 is an ester
lighted splint (positive result=pop)
strong acids/bases are written as H+ or OH- ions
NO3?

37. Both Acetic acid and ____________ are also functional isomers.
ion pairing
Synthetic condensation polymer (aka a polyamide)
Ksp = s²
methyl formate

38. What is the formula for alkenes?
CnH2n
Kc=Kp
Separating funnel
allow for the vapor pressure of water and make sure to level levels

39. nitrate
Increases down group 1 decreases down group 17
NO3?
allow for the vapor pressure of water and make sure to level levels
PO4³?

40. What type of compounds are almost always colored?
?H formation of an element in standard state=0
Synthesis - separation and purification of the product and its identification.
Transition element compounds (except if it has a full or empty d shell)
O2 needs 4F/mol H2 needs 2F/mol

41. How do you clean a buret/pipette for a titration?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Eudiometer

42. What is the general formula for an ether?
Heptane
Soluble except Ag - Pb - Ca - Sr Ba)
ROR
Insoluble

43. What is an Alkyl group?

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44. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
left - ppt will form
?H-kJ - ?S-J - ?G-kJ
Time?¹ - (ex. s?¹ - hr?¹ - etc)

45. What is the second law of thermodynamics?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Suniverse increases for spontaneous processes
blue
But S° of element is not zero (except at 0K)

46. group 1 ions/compounds
bent
Soluble
They stay the same.
red - green - blue

47. oxalate
C2O4²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
allow for the vapor pressure of water and make sure to level levels
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

48. What is the formula of copper (II) phosphate?
Eudiometer
yellow
Salt and water
Cu3(PO4)2

49. How many faradays of electric charge do you need to produce one mole of O2? H2?
SO4²?
O2 needs 4F/mol H2 needs 2F/mol
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Tetrahedral

50. ammonium/ammonium compounds
Soluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
H+
CnH2n

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AP Chemistry 2

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