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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.
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. mercury (II) ion
fruit - fish - bases
Hg²?
Synthetic condensation polymer (aka a polyamide)
zero

2. Name 2 ways in which you can create a buffer?
But S° of element is not zero (except at 0K)
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)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Iodine and CO2 (dry ice)

3. What do ions and electrons travel through in a voltaic/electrolytic cell?
RNH2
Ions go through the salt bridge - electrons go through metal wires in the external circuit
0.10M HCl (more ions)
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)

4. What process do you use to obtain the precipitate from a solution?
Filtration
Products - reactants (except for BDE when it's reactants - products)
?G=negative - E° must be positive
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

5. Is the ?H formation of an element in standard state zero?
Experimental mass/theoretical mass X 100
it reacts by substitution NOT addition
Products - reactants (except for BDE when it's reactants - products)
?H formation of an element in standard state=0

6. What do acids plus active metals form?
non-metal oxides and hydrides are covalently bonded and are acidic.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
basic
Silvery gray solid - brown - purple

7. What are two substances that sublime at 1 atm when heated?
Orange
hydroxides (ex: Ba(OH)2)
Iodine and CO2 (dry ice)
T increases exponentially the proportion of molecules with E > Ea

8. One mole of electrons carries 96500Coulombs - what is this quantity called?

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9. For a dibasic acid (H2A) - [A²?]= ____ ?
?H-kJ - ?S-J - ?G-kJ
K2
non-metal oxides and hydrides are covalently bonded and are acidic.
White precipitate

10. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
H2PO4?
|experimental - accepted|/accepted X 100
zero
Graduated cylinder

11. iodine - iodine solution - iodine vapor
a-IMFs - b-molecular volume
CN?
Pale yellow
Silvery gray solid - brown - purple

12. What is the test for oxygen?
Glowing splint (positive result=relights)
non-metal oxides and hydrides are covalently bonded and are acidic.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
zero

13. What is the general formula for an ether?
Glacial acetic acid
ROR
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
proton donor base

14. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
do not change
Ksp = s²
zero-th: decreases - first: constant - second: increases
?G=negative - E° must be positive

15. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
same KE - but PEice<PEwater
Ppt will NOT form (unsaturated)
ClO2?

16. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
The compound with the lowest Ksp value.
blue (BTB)
An active metal.

17. How does half life change for zero-th order - first order - and second order processes?
CnH2n+2
zero-th: decreases - first: constant - second: increases
P2O5
ClO4?

18. How do you heat a test tube?
#ligands=charge x2
Heat a test tube at an angle at the side of the tube (not bottom)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Group 1 hydroxides (ex: NaOH)

19. carbonates
basic
Purple
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Insoluble except group 1 and ammonium

20. Esterification is...
acid + alcohol
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
More chaotic (ex: gases made)
acids

21. The definition of acidic basic and neutral aqueous solutions is:
Pour liquids using a funnel or down a glass rod
Group 1 hydroxides (ex: NaOH)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
voltaic: - electrolytic: +

22. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Increases down group 1 decreases down group 17
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ksp = 4s³
They stay the same.

23. What two compounds are great oxidizing agents?

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24. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
zero-th: decreases - first: constant - second: increases
10?8
ethers

25. What is the formula for alkanes?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Combine the equations for the half reactions in the non-spontaneous direction
O2 needs 4F/mol H2 needs 2F/mol
CnH2n+2

26. Ions are not ______.
Orange
yellow
atoms
Pale yellow

27. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
Exothermic
Ionic compounds
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

28. What are the formulas for q?
A salt solution.
q=mc?T q=mL (or n x ?h)
Trigonal pyramidal
zero

29. primary colors
Hg²?
CnH2n
red - green - blue
S2O3²?

30. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
same KE - but PEice<PEwater
Insoluble (except group 1 ammonium and Ba)
Glowing splint (positive result=relights)

31. Color is due to ______ _______ of light.
OH?
Selective absorption
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.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

32. What reacts with an acid to create hydrogen gas?
blue
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
An active metal.
Read the bottom of the meniscus

33. What do you use for an acid spill? base spill?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Products - reactants (except for BDE when it's reactants - products)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
RCOR

34. How do you identify which is oxidized or otherwise?
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)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
look for changes in oxidation # - the one that goes up is oxidized and is the RA

35. If ?S is positive - are the products more or less chaotic than the reactants?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
blue glass - it filters UV
More chaotic (ex: gases made)
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)

36. Why are noble gases stable?
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)
ClO?
acid + alcohol
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

37. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
CnH2n
At half equivalence - pH=pKa
+4-covalent - +2-ionic
They decrease (or could be the same if the solid has ONLY JUST disappeared)

38. What things should you remember to do when collecting gas over water?
Eudiometer
benzene has a delocalized pi ring structure
Iodine and CO2 (dry ice)
allow for the vapor pressure of water and make sure to level levels

39. What do metal oxides plus non- metal oxides form?
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
Tetrahedral
Salts (ex: CaO + SO2 ? CaSO3)
Mono; di; tri; tetra; penta; hexa.

40. nitrate
q=mc?T q=mL (or n x ?h)
small size and high charge
NO3?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

41. What is the general formula for alkyl halides?
Suniverse increases for spontaneous processes
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
RX
Q=It (time in seconds)

42. group 1 ions/compounds
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Orange
Soluble
atoms

43. If a weak acid is diluted more - what happens to its % dissociation value?
Sigma bonds are stronger than pi bonds
But S° of element is not zero (except at 0K)
Increases.
Ppt will NOT form (unsaturated)

44. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ksp = s²
The dilution effect when the solutions mix. M1V1 = M2V2
NH4?

45. What is the word equation for addition polymerisation?
CO3²?
basic
Combine the equations for the half reactions in the non-spontaneous direction
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

46. Acids + Carbonates (bicarbonates) make?
NH2?
-Ea/R
Big K=kf/kr
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

47. A geometric (or cis-trans) isomer exists due to.....
lighted splint (positive result=pop)
RCOR
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
OH- and NH3

48. sulfates
ethers
Group 1 hydroxides (ex: NaOH)
zero
Soluble except Ag - Pb - Ca - Sr Ba)

49. What is the relationship in strength between sigma and pi bonds?
Kc=Kp
it reacts by substitution NOT addition
Sigma bonds are stronger than pi bonds
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

50. What shape is ammonia?
chemically (ex: with carbon)
S2O3²?
Trigonal pyramidal
The dilution effect when the solutions mix. M1V1 = M2V2