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AP Chemistry 2

Instructions:

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. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Hg2²?
-Ea/R
acid + alcohol

2. What kind of bonding structure does benzene have?
Ionic compounds
ionic and form hydrogen and hydroxide
Iodine and CO2 (dry ice)
benzene has a delocalized pi ring structure

3. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
How close results are to the accepted value
CnH2n+2
CnH2n+1 often designated 'R' ex C3H7 is propyl
Current - time and charge on ion (moles of e used in half cell reaction)

4. What do you use for an acid spill? base spill?
non-metal oxides and hydrides are covalently bonded and are acidic.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
?H-kJ - ?S-J - ?G-kJ

5. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Check for air bubbles in the buret and remove the buret funnel from the buret
It ceases - the circuit is broken.
H3PO4
do not change

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Ksp = 4s³
methyl formate
HClO4

7. What is the general formula for an acid?
Decant
a-IMFs - b-molecular volume
RCOOH
Molecules with the same molecular formulas - but different structural formulas

8. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
No - NH3 and HCl gases are extremely soluble
ClO4?

9. Esterification is...
Greenish-yellow gas
Insoluble except for nitrate and acetate
acid + alcohol
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

10. What word is a clue for a redox reaction?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CnH2n+2
+4-covalent - +2-ionic
Acidified

11. What is the test for hydrogen?
NH2?
lighted splint (positive result=pop)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

12. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
left - ppt will form
by electrolysis
0 and 14

13. primary colors
red - green - blue
Trigonal pyramidal
Silvery gray solid - brown - purple
CnH2n-2

14. What is the energy you must put into a reaction to make it start called?
Ksp = s²
Salts (ex: CaO + SO2 ? CaSO3)
Initiation energy (NOT Ea)
The benzene ring (or more correctly the phenyl group - C6H5)

15. A Bronsted-Lowry base is...
RX
H2O + CO2 (it decomposes readily)
They stay the same.
proton acceptor.

16. Neutralization is an ________ reaction.
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)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
proton donor base
Conjugate pair (one must be a weak base or acid)

17. carbonates
#ligands=charge x2
Saturated - Substitution (which requires more radical conditions)
Insoluble except group 1 and ammonium
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

18. ________ are Lewis bases - because they can donate a lone pair of electrons.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
OH- and NH3
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Iodine and CO2 (dry ice)

19. What is the formula for alkanes?
CnH2n+2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Ppt will NOT form (unsaturated)
The one with most oxygen atoms (highest oxidation number)

20. Give an example of a concentrated weak acid.
NH2?
Glacial acetic acid
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Salt and water

21. What two types of substances are present in all redox reactions?
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
fractional distillation
an oxidized and reduced substance
Insoluble except for nitrate and acetate

22. nitrates
Soluble
[A?]/[HA] x 100 or [BH?]/[B] x 100
CN?
Conjugate pair (one must be a weak base or acid)

23. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
ion pairing
zero
fruit - fish - bases
P2O5

24. How do you dilute an acid?

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25. What is accuracy?
No - NH3 and HCl gases are extremely soluble
How close results are to the accepted value
benzene is less reactive than alkenes
NO3?

26. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Mn²? - Cr³? - Cr³
H+

27. silver compounds
same KE - but PEice<PEwater
strong acids/bases are written as H+ or OH- ions
Insoluble except for nitrate and acetate
Pour liquids using a funnel or down a glass rod

28. Buffer capacity must contain decent amounts of a ________ ________
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
Conjugate pair (one must be a weak base or acid)
+4-covalent - +2-ionic
RCHO (carbonyl at end)

29. What are two substances that sublime at 1 atm when heated?
Purple
H2PO4?
Iodine and CO2 (dry ice)
Suniverse increases for spontaneous processes

30. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
S crystal at 0K=0
C2O4²?
Mono; di; tri; tetra; penta; hexa.

31. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
NO3?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
blue (BTB)

32. What process do you use to obtain a solvent from a solution?
O2 needs 4F/mol H2 needs 2F/mol
Distillation
Exothermic
H+

33. What is the formula for percent error?
metal oxides and hydrides are ionically bonded and basic
|experimental - accepted|/accepted X 100
K2
White precipitate

34. What is the word equation for condensation polymerisation ?
a-IMFs - b-molecular volume
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Monomer + monomer = polymer product + a simple molecule such as water or HCl
redox reaction

35. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Increases down group 1 decreases down group 17
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
OH?
Insoluble

36. sulfate
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
neutralization: high K - H2O product dissociation: low K - H2O reactant
Heptane
SO4²?

37. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Initiation energy (NOT Ea)
Mono; di; tri; tetra; penta; hexa.
Acidified

38. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Graduated cylinder
Cu3(PO4)2
zero-th: decreases - first: constant - second: increases
non-metal oxides and hydrides are covalently bonded and are acidic.

39. How do you get Ecell for spontaneous reactions?
are less dense than water
CN?
ClO2?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

40. What is the general formula for an amine?
RNH2
by electrolysis
H+
CnH2n+1 often designated 'R' ex C3H7 is propyl

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

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42. A geometric (or cis-trans) isomer exists due to.....
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Distillation
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
blue glass - it filters UV

43. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
acids
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
How close results are to the accepted value

44. When driving off water from a hydrate - how do you tell you're done?
RCHO (carbonyl at end)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ion pairing
|experimental - accepted|/accepted X 100

45. Both Acetic acid and ____________ are also functional isomers.
H2PO4?
O2 needs 4F/mol H2 needs 2F/mol
K2
methyl formate

46. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Clear
Suniverse increases for spontaneous processes
H2PO4?
a-IMFs - b-molecular volume

47. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
red - green - blue
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Kc=Kp
chemically (ex: with carbon)

48. What type of compounds are almost always colored?
strong acids/bases are written as H+ or OH- ions
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
a-IMFs - b-molecular volume
Transition element compounds (except if it has a full or empty d shell)

49. For a dibasic acid (H2A) - [A²?]= ____ ?
0 and 14
Sigma bonds are stronger than pi bonds
K2
Ionic compounds

50. Do you use J or kJ for ?H - ?S - and ?G?
proton donor base
?H-kJ - ?S-J - ?G-kJ
Experimental mass/theoretical mass X 100
0.10M HCl (more ions)