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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. What do the 'a' and 'b' in Van Der Waal's equation allow for?
0 and 14
The Faraday or Faraday's constant.
a-IMFs - b-molecular volume
ion pairing

2. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
?H formation of an element in standard state=0
ion pairing
?H-kJ - ?S-J - ?G-kJ
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

3. Do you use J or kJ for ?H - ?S - and ?G?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
?H-kJ - ?S-J - ?G-kJ
catalyst=conc H2SO4
bent

4. What do you do to get rid of most of the solution from a precipitate?
Unsaturated - addition (ex: decolorize bromine solution)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Decant

5. What is precision?
How grouped results are
Concentration
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.
Eudiometer

6. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
do not change
MnO4?
ion pairing

7. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
an oxidized and reduced substance
K1 x K2
CnH2n
same KE - but PEice<PEwater

8. silver iodide
Pale yellow
Transition element compounds (except if it has a full or empty d shell)
redox reaction
K1 x K2

9. What shape is ammonia?
Trigonal pyramidal
All except for lithium
Purple
?H-kJ - ?S-J - ?G-kJ

10. Color (absorbance) is proportional to ________
Concentration
it reacts by substitution NOT addition
How close results are to the accepted value
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

11. A Bronsted-Lowry acid is...
S2O3²?
proton donor base
yellow
Exothermic (?H for ANY sa/sb = -57kJ/mol)

12. Does Kw increase or decrease with T? Why?
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
ionic and form hydrogen and hydroxide
different forms of the same element
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

13. A Bronsted-Lowry base is...
strong acids/bases are written as H+ or OH- ions
NH2?
proton acceptor.
0.10M HCl (more ions)

14. The definition of acidic basic and neutral aqueous solutions is:
The benzene ring (or more correctly the phenyl group - C6H5)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
CO3²?

15. What steps do organic labs consist of?
Synthesis - separation and purification of the product and its identification.
Purple
Salts (ex: CaO + SO2 ? CaSO3)
They stay the same.

16. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
non-metal oxides and hydrides are covalently bonded and are acidic.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Unsaturated - addition (ex: decolorize bromine solution)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

17. What electrons are lost/gained first in transition element ions?
acid + alcohol
voltaic: - electrolytic: +
ns² electrons (first in-first out)
E=q + w (negative is by system - positive is on system)

18. chromate
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
acid + alcohol
CrO4²?

19. What are amphoteric oxides?
Distillation
Most are soluble except Ag - Pb
Glowing splint (positive result=relights)
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?)

20. Which would cause the bulb in a conductivity apparatus to be brightest?
P2O5
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
benzene is less reactive than alkenes
0.10M HCl (more ions)

21. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
basic
No - it depends on the number of ions produced on dissolving.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
ROH

22. How does benzene compare in reactivity to alkenes?
fruit - fish - bases
benzene is less reactive than alkenes
T increases exponentially the proportion of molecules with E > Ea
No - it depends on the number of ions produced on dissolving.

23. chlorate
Increases down group 1 decreases down group 17
-Ea/R
ClO3?
Increases.

24. What are the formulas for q?
The compound with the lowest Ksp value.
Iodine and CO2 (dry ice)
q=mc?T q=mL (or n x ?h)
Selective absorption

25. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Insoluble except group 1 and ammonium
An active metal.

26. What do ions and electrons travel through in a voltaic/electrolytic cell?
A salt solution.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
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?)
brown volatile liquid

27. bromine
brown volatile liquid
Saturated - Substitution (which requires more radical conditions)
acids
Sigma bonds are stronger than pi bonds

28. If a free element is involved - what type of reaction must be involved?
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
q=mc?T q=mL (or n x ?h)
zero
redox reaction

29. An amphiprotic (amphoteric) species is...
Ksp = 4s³
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
allow for the vapor pressure of water and make sure to level levels

30. Which of the rates changes more when temperature is increased?
blue (BTB)
it is lower and occurs over less sharp a range
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
K1 x K2

31. Name some properties of Group 17
A) any range. b) 8-10 c) 4-6
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Reduction always takes place at the cathode (RED CAT) In both types of cell!
An active metal.

32. What do nonmetal oxides plus water form?
acids
it's lower and occurs over less sharp a range
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
are less dense than water

33. What do group I/II metal oxides and acids form?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
RNH2
same KE - but PEice<PEwater
Salt and water

34. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

35. How does group 1 metals' density compare to water's?
are less dense than water
different forms of the same element
Pipette (burette if need repetition)
Salt and water

36. What is the general formula of an alkane?
The Faraday or Faraday's constant.
CnH(2n+2)
Tetrahedral
redox reaction

37. What is HCOOCH3?
strong acids/bases are written as H+ or OH- ions
No - it depends on the number of ions produced on dissolving.
K2
Acids; HCOOCH3 is an ester

38. When the salt bridge is removed what happens to the cell reaction?
Increases.
Insoluble except nitrate and acetate
It ceases - the circuit is broken.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

39. How do you clean a buret/pipette for a titration?
bases
acid + alcohol
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Decant

40. What is the word equation for condensation polymerisation ?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
It ceases - the circuit is broken.
Disulfur dichloride

41. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
NH4?
Increases down group 1 decreases down group 17
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Current - time and charge on ion (moles of e used in half cell reaction)

42. What process do you use to separate two liquids with different boiling points?
Distillation
fractional distillation
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.
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

43. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
NH2?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Disulfur dichloride

44. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
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
basic
-Ea/R

45. A geometric (or cis-trans) isomer exists due to.....
OH?
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?)
RCHO (carbonyl at end)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

46. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Both electrons come from the same atom (just as good as a regular bond)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Pale purple - (orange)-yellow - red - blue - green.

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

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48. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
do not change
H+
Ksp = s²

49. What are isomers?
bright yellow
Molecules with the same molecular formulas - but different structural formulas
metal oxides and hydrides are ionically bonded and basic
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

50. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
More chaotic (ex: gases made)
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
Soluble
CnH2n-2