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

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2. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
neutralization: high K - H2O product dissociation: low K - H2O reactant
ClO2?
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
Silvery gray solid - brown - purple

3. Alcohols and _______ are FG isomers
ethers
C4H10
it reacts by substitution NOT addition
Clear

4. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Soluble
H+

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

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6. Are weak acids (and bases) written dissociated?

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7. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Identity and purity (impure compounds usually have broad & low melting points)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
boiling without losing volatile solvents/reactants
a-IMFs - b-molecular volume

8. What is a dipeptide? polypeptide? protein?
yellow
do not change
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
They decrease (or could be the same if the solid has ONLY JUST disappeared)

9. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Sulfur
Ppt will NOT form (unsaturated)
metal oxides and hydrides are ionically bonded and basic

10. If Q < Ksp a ppt ______
RCOOH
Identity and purity (impure compounds usually have broad & low melting points)
atoms
Ppt will NOT form (unsaturated)

11. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
blue (BTB)
Eudiometer
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Soluble

12. What is the formula for alkynes?
RCOR
CnH2n-2
CO (poisonous)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

13. bromothymol
blue (BTB)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Saturated - Substitution (which requires more radical conditions)
allow for the vapor pressure of water and make sure to level levels

14. If a weak acid is diluted more - what happens to its % dissociation value?
voltaic: - electrolytic: +
basic
It ceases - the circuit is broken.
Increases.

15. What are allotropes?
fruit - fish - bases
different forms of the same element
Ppt will NOT form (unsaturated)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

16. Esters smell like _______ and amines smell like _______ and are ______.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
fruit - fish - bases
yellow
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

17. chlorate
Orange
ClO3?
Molecules with the same molecular formulas - but different structural formulas
CnH(2n+2)

18. Name some properties of Group 17
OH- and NH3
An active metal.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
catalyst=conc H2SO4

19. What process do you use to obtain a solvent from a solution?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
q=mc?T q=mL (or n x ?h)
Distillation
Mn²? - Cr³? - Cr³

20. What is the conjugate acid of H2PO4?
H3PO4
T increases exponentially the proportion of molecules with E > Ea
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
-Ea/R

21. What do ions and electrons travel through in a voltaic/electrolytic cell?
lighted splint (positive result=pop)
ionic and form hydrogen and hydroxide
-Ea/R
Ions go through the salt bridge - electrons go through metal wires in the external circuit

22. What does the solubility of organic compounds depend on?
brown volatile liquid
Soluble
Insoluble
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

23. Acid plus base make?
Salt + water.
left - ppt will form
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

24. When a cell is 'flat' What is its voltage?
redox reaction
zero
voltaic: + electrolytic: -
E=q + w (negative is by system - positive is on system)

25. What element is used to vulcanize rubber?
bright yellow
non-metal oxides and hydrides are covalently bonded and are acidic.
Sulfur
zero

26. dichromate
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Cr2O7²?
Ionic compounds
Graduated cylinder

27. Ions are not ______.
yellow
catalyst=conc H2SO4
White precipitate
atoms

28. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
?G=negative - E° must be positive
Synthetic condensation polymer (aka a polyamide)
blue (BTB)
same KE - but PEice<PEwater

29. Is the freezing of ice endothermic or exothermic?
Exothermic
At half equivalence - pH=pKa
Acid rain - dissolves marble buildings/statues and kills trees.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

30. What type of solutions do small - highly charged cations tend to form?
fruit - fish - bases
it is lower and occurs over less sharp a range
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
NH2?

31. When the salt bridge is removed what happens to the cell reaction?
do not change
it is lower and occurs over less sharp a range
It ceases - the circuit is broken.
E=q + w (negative is by system - positive is on system)

32. What device would you use to measure a volume of gas?
Kc=Kp
Sigma bonds are stronger than pi bonds
Eudiometer
left - ppt will form

33. Ca - Sr - Ba
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Pale yellow
hydroxides (ex: Ba(OH)2)
CrO4²?

34. What is the test for hydrogen?
lighted splint (positive result=pop)
CO2 and H2O
water and substances with (s) less dense than
RCHO (carbonyl at end)

35. What changes Keq?
Only temperature
0 and 14
boiling without losing volatile solvents/reactants
HClO4

36. What is the general formula for an aldehyde?
Most INsoluble except group 1 and ammonium
RCHO (carbonyl at end)
OH- and NH3
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?)

37. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
H2PO4?
Unsaturated - addition (ex: decolorize bromine solution)
But S° of element is not zero (except at 0K)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

38. How do you heat a test tube?
voltaic: + electrolytic: -
Heat a test tube at an angle at the side of the tube (not bottom)
Silvery gray solid - brown - purple
Salt and water

39. Name C7H16
Heptane
A salt solution.
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
HClO4

40. What measuring device would you use for very small volumes of liquids?
H2O + CO2 (it decomposes readily)
blue
ClO4?
Pipette (burette if need repetition)

41. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
voltaic: + electrolytic: -
Clear
The dilution effect when the solutions mix. M1V1 = M2V2
Ksp = 108s5

42. acetates
Soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
acid + alcohol
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

43. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
ionic and form hydrogen and hydroxide
Anode - oxygen. Cathode - hydrogen
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

44. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
But S° of element is not zero (except at 0K)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
linear

45. mercury (II) ion
Ksp = 27s4
S crystal at 0K=0
Hg²?
White precipitate

46. If a free element is involved - what type of reaction must be involved?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
10?8
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
redox reaction

47. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
But S° of element is not zero (except at 0K)
Disulfur dichloride
Orange

48. 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.
atoms
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

49. What should you check for before you begin titrating?
Hg²?
Salt + water.
#ligands=charge x2
Check for air bubbles in the buret and remove the buret funnel from the buret

50. What is the first law of thermodynamics?
ClO?
different forms of the same element
E=q + w (negative is by system - positive is on system)
zero