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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. lead iodide
bright yellow
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Add acid to water so that the acid doesn't boil and spit
chemically (ex: with carbon)

2. How many faradays of electric charge do you need to produce one mole of O2? H2?
ROR
O2 needs 4F/mol H2 needs 2F/mol
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
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.

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

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4. What is the general formula of an alkane?
do not change
Pour liquids using a funnel or down a glass rod
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH(2n+2)

5. What is a coordinate covalent bond?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
No - it depends on the number of ions produced on dissolving.
Both electrons come from the same atom (just as good as a regular bond)
Glacial acetic acid

6. What are the names and formulas of the 6 strong acids?
water and substances with (s) less dense than
How grouped results are
lighted splint (positive result=pop)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

7. What type of polymer is nylon?
are less dense than water
Mono; di; tri; tetra; penta; hexa.
Synthetic condensation polymer (aka a polyamide)
water and substances with (s) less dense than

8. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
[A?]/[HA] x 100 or [BH?]/[B] x 100
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

9. Which of the rates changes more when temperature is increased?
H+
ethers
Initiation energy (NOT Ea)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

10. What part of a liquid do you look at to measure its volume?
proton acceptor.
Read the bottom of the meniscus
Orange
linear

11. What is the formula for alkynes?
But S° of element is not zero (except at 0K)
CnH2n-2
Sulfur
Anode - oxygen. Cathode - hydrogen

12. Ca - Sr - Ba
Mono; di; tri; tetra; penta; hexa.
hydroxides (ex: Ba(OH)2)
Heat a test tube at an angle at the side of the tube (not bottom)
small size and high charge

13. Alkenes are ________ and react by __________
Current - time and charge on ion (moles of e used in half cell reaction)
Unsaturated - addition (ex: decolorize bromine solution)
Heptane
Anode - oxygen. Cathode - hydrogen

14. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The Faraday or Faraday's constant.
Mono; di; tri; tetra; penta; hexa.
Most INsoluble except group 1 and ammonium

15. If a free element is involved - what type of reaction must be involved?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
redox reaction
RCHO (carbonyl at end)

16. BaSO4
Concentration
Heat a test tube at an angle at the side of the tube (not bottom)
RCOOH
Insoluble

17. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
OH?
RCOR
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
basic

18. Nonmetals are good _____ agents. Metals are good _______ agents.
O2 needs 4F/mol H2 needs 2F/mol
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Trigonal pyramidal
?G=negative - E° must be positive

19. mercury (I) ion
The benzene ring (or more correctly the phenyl group - C6H5)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Hg2²?
RCHO (carbonyl at end)

20. What shape is ammonia?
Trigonal pyramidal
ClO3?
-Ea/R
water and substances with (s) less dense than

21. What is the formula for alkenes?
Insoluble except group 1 and ammonium
blue (BTB)
P2O5
CnH2n

22. What changes Keq?
Only temperature
T increases exponentially the proportion of molecules with E > Ea
ethers
Soluble

23. Acids + Carbonates (bicarbonates) make?
Soluble except Ag - Pb - Ca - Sr Ba)
brown volatile liquid
CnH2n-2
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

24. acetate
water and substances with (s) less dense than
CH3COO?
CO (poisonous)
water and substances with (s) less dense than

25. If Q > Ksp - then system shifts _______ and ppt ______
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
P2O5
left - ppt will form
?G=negative - E° must be positive

26. What do metal oxides plus acids form?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
allow for the vapor pressure of water and make sure to level levels
Salt + water
Molecules with the same molecular formulas - but different structural formulas

27. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Anode
Acid rain - dissolves marble buildings/statues and kills trees.
Check for air bubbles in the buret and remove the buret funnel from the buret

28. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

29. What are allotropes?
Saturated - Substitution (which requires more radical conditions)
different forms of the same element
same KE - but PEice<PEwater
0.10M HCl (more ions)

30. What is the pH of 1.0M HCl? 1M NaOH?
a-IMFs - b-molecular volume
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.
Graduated cylinder
0 and 14

31. What process do you use to obtain the solute from a solution?
K1 x K2
Both electrons come from the same atom (just as good as a regular bond)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Evaporation

32. chromate
bent
They stay the same.
CrO4²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

33. What is the general formula for a ketone?
blue
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
chemically (ex: with carbon)
RCOR

34. phosphate
strong acids/bases are written as H+ or OH- ions
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
PO4³?
OH- and NH3

35. hydroxides
Insoluble (except group 1 ammonium and Ba)
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
Combine the equations for the half reactions in the non-spontaneous direction
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

36. primary colors
red - green - blue
atoms
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

37. silver iodide
red - green - blue
All except for lithium
Pale yellow
Clear

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

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39. What is the general formula for an ether?
blue glass - it filters UV
linear
ROR
bright yellow

40. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
methyl formate
RCOR
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

41. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Current - time and charge on ion (moles of e used in half cell reaction)
zero
Silvery gray solid - brown - purple
+4-covalent - +2-ionic

42. For a dibasic acid (H2A) - [A²?]= ____ ?
Salt and water
K2
Mono; di; tri; tetra; penta; hexa.
Ions go through the salt bridge - electrons go through metal wires in the external circuit

43. Colorless doesn't mean ______
Silvery gray solid - brown - purple
Clear
CnH2n+1 often designated 'R' ex C3H7 is propyl
At half equivalence - pH=pKa

44. Aromatic compounds contain what?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Heat a test tube at an angle at the side of the tube (not bottom)
The benzene ring (or more correctly the phenyl group - C6H5)
Decant

45. What is the general formula for an ester?
RCOOR
proton donor base
Heat a test tube at an angle at the side of the tube (not bottom)
water and substances with (s) less dense than

46. What is reflux?
White precipitate
Hg2²?
boiling without losing volatile solvents/reactants
Both electrons come from the same atom (just as good as a regular bond)

47. Does reactivity increase/decrease going down group 1 and group 17?
Anode
Increases down group 1 decreases down group 17
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

48. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
acid + alcohol

49. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Current - time and charge on ion (moles of e used in half cell reaction)
redox reaction
Combine the equations for the half reactions in the non-spontaneous direction
They stay the same.

50. Name 2 ways in which you can create a buffer?
CN?
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)
Heptane
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)