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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 Big K in terms of kf and kr?
Acidified
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Big K=kf/kr
voltaic: + electrolytic: -

2. What should you check for before you begin titrating?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Mono; di; tri; tetra; penta; hexa.
Check for air bubbles in the buret and remove the buret funnel from the buret

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

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4. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
10?8
How close results are to the accepted value
same KE - but PEice<PEwater

5. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Hg²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
bases

6. mercury (II) ion
zero
Synthetic condensation polymer (aka a polyamide)
S crystal at 0K=0
Hg²?

7. What process do you use to separate two liquids with different boiling points?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
fractional distillation
ROR

8. Alkenes are ________ and react by __________
H2O + CO2 (it decomposes readily)
Silvery gray solid - brown - purple
Unsaturated - addition (ex: decolorize bromine solution)
by electrolysis

9. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
redox reaction

10. The definition of acidic basic and neutral aqueous solutions is:
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
ClO4?
bases
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

11. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
All except for lithium
Ppt will NOT form (unsaturated)
OH?

12. What word is a clue for a redox reaction?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
+4-covalent - +2-ionic
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Acidified

13. Alcohols and _______ are FG isomers
ethers
Iodine and CO2 (dry ice)
acids
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

14. What is the conjugate base of NH3?
Salt + water
10?8
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
NH2?

15. phosphates
OH?
?H-kJ - ?S-J - ?G-kJ
Most INsoluble except group 1 and ammonium
K2

16. What do you need to make a polymer?
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)
At half equivalence - pH=pKa
Pale purple - (orange)-yellow - red - blue - green.
CN?

17. acetates
Soluble
CO3²?
basic
White precipitate

18. What is the word equation for condensation polymerisation ?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Silvery gray solid - brown - purple
Monomer + monomer = polymer product + a simple molecule such as water or HCl
But S° of element is not zero (except at 0K)

19. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
MnO4?
CnH2n
All except for lithium

20. What is the name of S2Cl2? (Know how to name others like this - too)
an oxidized and reduced substance
At half equivalence - pH=pKa
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Disulfur dichloride

21. lead compounds
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Insoluble except for nitrate and acetate
The dilution effect when the solutions mix. M1V1 = M2V2
Insoluble except nitrate and acetate

22. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Silvery gray solid - brown - purple
They stay the same.
Selective absorption
They decrease (or could be the same if the solid has ONLY JUST disappeared)

23. Acid plus base make?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Salt + water.
Soluble except Ag - Pb - Ca - Sr Ba)
-Ea/R

24. chlorate
?H-kJ - ?S-J - ?G-kJ
All except for lithium
ClO3?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

25. What is the formula for alkenes?
it is lower and occurs over less sharp a range
Transition element compounds (except if it has a full or empty d shell)
CnH2n
do not change

26. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Most INsoluble except group 1 and ammonium
chemically (ex: with carbon)

27. What is the general formula for an ester?
All except for lithium
RCOOR
How close results are to the accepted value
fruit - fish - bases

28. What do group I/II metal oxides plus water form?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
CnH2n-2
hydroxides (ex: Ba(OH)2)
bases

29. Do you use J or kJ for ?H - ?S - and ?G?
Cu3(PO4)2
A salt solution.
?H-kJ - ?S-J - ?G-kJ
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

30. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
catalyst=conc H2SO4
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salt + water

31. Give an example of a concentrated weak acid.
H3PO4
Synthetic condensation polymer (aka a polyamide)
Glacial acetic acid
ethers

32. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
CnH2n+2
do not change
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

33. What two compounds are great oxidizing agents?

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34. hydroxides
Ksp = 27s4
Insoluble (except group 1 ammonium and Ba)
atoms
basic

35. What is the general formula of an alkane?
acid + alcohol
Current - time and charge on ion (moles of e used in half cell reaction)
CnH(2n+2)
CO3²?

36. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Selective absorption
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Transition element compounds (except if it has a full or empty d shell)
CO2 and H2O

37. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
it's lower and occurs over less sharp a range
CnH2n
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

38. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ClO2?
K2

39. What is the general formula for an amine?
Salt + water
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
RNH2
zero

40. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
ion pairing
allow for the vapor pressure of water and make sure to level levels
Greenish-yellow gas

41. 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?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
RNH2
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
The compound with the lowest Ksp value.

42. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Greenish-yellow gas
Acidified
Sigma bonds are stronger than pi bonds

43. What is the pH of 1.0M HCl? 1M NaOH?
At half equivalence - pH=pKa
Iodine and CO2 (dry ice)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
0 and 14

44. What reacts with an acid to create hydrogen gas?
An active metal.
Insoluble except for nitrate and acetate
|experimental - accepted|/accepted X 100
basic

45. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Ppt will NOT form (unsaturated)
No - NH3 and HCl gases are extremely soluble
Read the bottom of the meniscus

46. How does benzene compare in reactivity to alkenes?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
benzene is less reactive than alkenes
chemically (ex: with carbon)
CnH(2n+2)

47. What electrons are lost/gained first in transition element ions?
Synthetic condensation polymer (aka a polyamide)
ns² electrons (first in-first out)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
No - NH3 and HCl gases are extremely soluble

48. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
Transition element compounds (except if it has a full or empty d shell)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Soluble

49. What type of metals don't react with water or acids to form H2?

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50. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Both electrons come from the same atom (just as good as a regular bond)
NH4?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

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AP Chemistry 2

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