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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. What is the formula for summation?

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2. group 1 ions/compounds
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Salt + water.
Soluble
fruit - fish - bases

3. How are primary alcohols turned into acids?
Synthetic condensation polymer (aka a polyamide)
Soluble
T increases exponentially the proportion of molecules with E > Ea
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

4. What is the test for oxygen?
Eudiometer
Glowing splint (positive result=relights)
-Ea/R
Molecules with the same molecular formulas - but different structural formulas

5. cyanide
CH3COO?
Acid rain - dissolves marble buildings/statues and kills trees.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
CN?

6. Color is due to ______ _______ of light.
Selective absorption
Insoluble (except group 1 ammonium and Ba)
left - ppt will form
Hg2²?

7. How do you dilute an acid?

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8. During a titration what is present in the beaker at the equivalence point?
water and substances with (s) less dense than
A salt solution.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ROH

9. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Soluble
NH4?
The Faraday or Faraday's constant.

10. Ions are not ______.
Eudiometer
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Soluble
atoms

11. nitrates
CrO4²?
Soluble
Check for air bubbles in the buret and remove the buret funnel from the buret
HClO4

12. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
O2 needs 4F/mol H2 needs 2F/mol
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)
allow for the vapor pressure of water and make sure to level levels

13. Acids + Carbonates (bicarbonates) make?
Filtration
basic
Clear
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

14. If Q < Ksp a ppt ______
Heptane
Ppt will NOT form (unsaturated)
ClO?
CnH2n

15. What is the difference between equivalence point and end point of a titration.
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
Purple
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
ionic and form hydrogen and hydroxide

16. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Orange
At half equivalence - pH=pKa
fruit - fish - bases
a-IMFs - b-molecular volume

17. What is the formula of copper (II) phosphate?
Pour liquids using a funnel or down a glass rod
Cu3(PO4)2
The Faraday or Faraday's constant.
[A?]/[HA] x 100 or [BH?]/[B] x 100

18. How does benzene compare in reactivity to alkenes?
Orange
benzene is less reactive than alkenes
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
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)

19. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
atoms
Graduated cylinder
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

20. What changes Keq?
Purple
Only temperature
RCHO (carbonyl at end)
?G=negative - E° must be positive

21. What is the formula for percent error?
RCHO (carbonyl at end)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ion pairing
|experimental - accepted|/accepted X 100

22. lead iodide
bright yellow
do not change
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Check for air bubbles in the buret and remove the buret funnel from the buret

23. What type of compounds do metals/non metals form?
Glacial acetic acid
blue
boiling without losing volatile solvents/reactants
Ionic compounds

24. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
q=mc?T q=mL (or n x ?h)
Iodine and CO2 (dry ice)
it reacts by substitution NOT addition

25. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
CH3COO?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
same KE - but PEice<PEwater
NH2?

26. What is the formula of butane?
NH4?
C4H10
Molecules with the same molecular formulas - but different structural formulas
bases

27. What element is used to vulcanize rubber?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Sulfur
ClO2?
it reacts by substitution NOT addition

28. What are allotropes?
different forms of the same element
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
O2 needs 4F/mol H2 needs 2F/mol
Pale yellow

29. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Most INsoluble except group 1 and ammonium
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

30. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Separating funnel
Mono; di; tri; tetra; penta; hexa.
allow for the vapor pressure of water and make sure to level levels
Unsaturated - addition (ex: decolorize bromine solution)

31. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
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?)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Silvery gray solid - brown - purple
CnH2n

32. A Bronsted-Lowry base is...
atoms
H+
A) any range. b) 8-10 c) 4-6
proton acceptor.

33. What is the energy you must put into a reaction to make it start called?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Initiation energy (NOT Ea)
But S° of element is not zero (except at 0K)
zero-th: decreases - first: constant - second: increases

34. Is the ?H formation of an element in standard state zero?
H2PO4?
Salt + water.
?H formation of an element in standard state=0
HClO4

35. Colorless doesn't mean ______
Clear
#ligands=charge x2
PO4³?
CO2 and H2O

36. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CrO4²?
Mn²? - Cr³? - Cr³
fractional distillation

37. What is the general formula for an alcohol?
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)
ROH
CO2 and H2O
RX

38. Give an example of a concentrated weak acid.
it is lower and occurs over less sharp a range
Glacial acetic acid
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
it reacts by substitution NOT addition

39. What process do you use to separate two liquids with different boiling points?
fractional distillation
HClO4
Glowing splint (positive result=relights)
Acid rain - dissolves marble buildings/statues and kills trees.

40. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
ClO3?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
CO2 and H2O
Distillation

41. mercury (I) ion
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Hg2²?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Anode - oxygen. Cathode - hydrogen

42. sulfate
A salt solution.
Identity and purity (impure compounds usually have broad & low melting points)
[A?]/[HA] x 100 or [BH?]/[B] x 100
SO4²?

43. How do you find the pH for a dibasic acid? (H2A)?
it reacts by substitution NOT addition
Perform ICE BOX calculation based on K1
NH4?
H2PO4?

44. BaSO4
allow for the vapor pressure of water and make sure to level levels
Group 1 hydroxides (ex: NaOH)
Insoluble
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

45. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Filtration
basic
K2

46. bromothymol
CnH2n
redox reaction
They stay the same.
blue (BTB)

47. What do ions and electrons travel through in a voltaic/electrolytic cell?
Soluble
Ions go through the salt bridge - electrons go through metal wires in the external circuit
atoms
acid + alcohol

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

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49. Why are noble gases stable?
Pour liquids using a funnel or down a glass rod
Soluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
linear

50. What is the catalyst for this reaction Ester + ?
The benzene ring (or more correctly the phenyl group - C6H5)
Sulfur
'non-active' metals such as Cu - Ag - Au - Pt - etc.
catalyst=conc H2SO4