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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
|experimental - accepted|/accepted X 100
OH?
ion pairing

2. How do you dilute an acid?

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3. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Check for air bubbles in the buret and remove the buret funnel from the buret
neutralization: high K - H2O product dissociation: low K - H2O reactant
Heat a test tube at an angle at the side of the tube (not bottom)
The one with most oxygen atoms (highest oxidation number)

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

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5. sulfate
SO4²?
Saturated - Substitution (which requires more radical conditions)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

6. What shape is ammonia?
zero
PO4³?
it's lower and occurs over less sharp a range
Trigonal pyramidal

7. Alkanes are _________ and react by _________
bases
Ppt will NOT form (unsaturated)
Saturated - Substitution (which requires more radical conditions)
CnH2n+2

8. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
do not change
HClO4
The Faraday or Faraday's constant.

9. Do anions flow to the cathode or anode?
Anode
H3PO4
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Concentration

10. What is a coordinate covalent bond?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
At half equivalence - pH=pKa
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Both electrons come from the same atom (just as good as a regular bond)

11. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Read the bottom of the meniscus
bright yellow
The one with most oxygen atoms (highest oxidation number)
No - it depends on the number of ions produced on dissolving.

12. ammonium/ammonium compounds
Soluble
Filtration
Ksp = 108s5
Glowing splint (positive result=relights)

13. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
?H-kJ - ?S-J - ?G-kJ
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Pale purple - (orange)-yellow - red - blue - green.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

14. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Experimental mass/theoretical mass X 100
Pour liquids using a funnel or down a glass rod
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

15. 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?
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)
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
K2
+4-covalent - +2-ionic

16. What equipment do you need for a titration?
Transition element compounds (except if it has a full or empty d shell)
R=8.31 J/mol/K
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
it's lower and occurs over less sharp a range

17. Nonmetals are good _____ agents. Metals are good _______ agents.
Nothing
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Heat a test tube at an angle at the side of the tube (not bottom)
Tetrahedral

18. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
benzene has a delocalized pi ring structure
Acid rain - dissolves marble buildings/statues and kills trees.
redox reaction

19. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Soluble except Ag - Pb - Ca - Sr Ba)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Clear
Sulfur

20. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Clear
Experimental mass/theoretical mass X 100
Insoluble
Ksp = 108s5

21. What is the second law of thermodynamics?
Current - time and charge on ion (moles of e used in half cell reaction)
a-IMFs - b-molecular volume
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Suniverse increases for spontaneous processes

22. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
E=q + w (negative is by system - positive is on system)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
methyl formate

23. What should you check for before you begin titrating?
How grouped results are
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)
Check for air bubbles in the buret and remove the buret funnel from the buret
zero

24. What is the test for oxygen?
Trigonal pyramidal
Time?¹ - (ex. s?¹ - hr?¹ - etc)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Glowing splint (positive result=relights)

25. copper sulfate
a-IMFs - b-molecular volume
NH2?
blue
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

26. Metal hydrides are _____ and form _______ and _______ when added to water
diamond and graphite
Mn²? - Cr³? - Cr³
ionic and form hydrogen and hydroxide
catalyst=conc H2SO4

27. What are isomers?
brown volatile liquid
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
ClO?
Molecules with the same molecular formulas - but different structural formulas

28. potassium permanganate
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)
K1 x K2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Purple

29. What do the 'a' and 'b' in Van Der Waal's equation allow for?
All except for lithium
Sulfur
a-IMFs - b-molecular volume
benzene has a delocalized pi ring structure

30. Name C7H16
Heptane
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
chemically (ex: with carbon)
Ksp = 27s4

31. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
CnH2n-2
Anode - oxygen. Cathode - hydrogen
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Nothing

32. What process do you use to obtain a solvent from a solution?
proton acceptor.
an oxidized and reduced substance
Distillation
Acidified

33. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
K2
proton acceptor.

34. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
A) any range. b) 8-10 c) 4-6
Synthetic condensation polymer (aka a polyamide)
More chaotic (ex: gases made)
water and substances with (s) less dense than

35. What does saturated mean? Unsaturated?
CN?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
RCOOH
H3PO4

36. What is the general formula for an aldehyde?
strong acids/bases are written as H+ or OH- ions
Salts (ex: CaO + SO2 ? CaSO3)
voltaic: + electrolytic: -
RCHO (carbonyl at end)

37. What are the formulas for q?
S2O3²?
q=mc?T q=mL (or n x ?h)
H+
NH2?

38. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ionic and form hydrogen and hydroxide
Insoluble (except group 1 ammonium and Ba)
ethers

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

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40. What are the units of the first order rate constant?
CrO4²?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Greenish-yellow gas

41. What shape is water?
small size and high charge
Pipette (burette if need repetition)
bent
it's lower and occurs over less sharp a range

42. When combining half equations - what do you do to E° values when multiplying coefficients?
They stay the same.
Nothing
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

43. How do you find the pH for a dibasic acid? (H2A)?
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
left - ppt will form
Salt + water
Perform ICE BOX calculation based on K1

44. What is the word equation for condensation polymerisation ?
water and substances with (s) less dense than
Ionic compounds
ns² electrons (first in-first out)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

45. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
bases
P2O5

46. What is the general formula for a ketone?
CnH(2n+2)
Soluble
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?)
RCOR

47. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
CO (poisonous)
zero
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

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

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49. During a titration what is present in the beaker at the equivalence point?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
A salt solution.
CO (poisonous)
HClO4

50. What are the prefixes for the naming of binary molecular compound formulas (up to six)
boiling without losing volatile solvents/reactants
Mono; di; tri; tetra; penta; hexa.
Pipette (burette if need repetition)
Conjugate pair (one must be a weak base or acid)

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AP Chemistry 2

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