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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. For a dibasic acid (H2A) - [A²?]= ____ ?
Synthetic condensation polymer (aka a polyamide)
K2
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ROH

2. How do you get the equation for a net electrolysis reaction?
Trigonal pyramidal
Combine the equations for the half reactions in the non-spontaneous direction
ROH
Ksp = s²

3. Alkanes are _________ and react by _________
CrO4²?
Saturated - Substitution (which requires more radical conditions)
At half equivalence - pH=pKa
C4H10

4. What is the general formula for an acid?
linear
atoms
allow for the vapor pressure of water and make sure to level levels
RCOOH

5. What is the name of S2Cl2? (Know how to name others like this - too)
Read the bottom of the meniscus
an oxidized and reduced substance
Disulfur dichloride
Exothermic (?H for ANY sa/sb = -57kJ/mol)

6. What process do you use to obtain the precipitate from a solution?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
The dilution effect when the solutions mix. M1V1 = M2V2
Filtration
Distillation

7. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Ionic compounds
How grouped results are
catalyst=conc H2SO4

8. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
boiling without losing volatile solvents/reactants
Insoluble (except group 1 ammonium and Ba)
atoms
H+

9. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Iodine and CO2 (dry ice)
At half equivalence - pH=pKa
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

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

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11. When is ?G zero?
voltaic: - electrolytic: +
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Transition element compounds (except if it has a full or empty d shell)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

12. What is the formula for percent error?
|experimental - accepted|/accepted X 100
lighted splint (positive result=pop)
water and substances with (s) less dense than
CO (poisonous)

13. 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!
ionic and form hydrogen and hydroxide
linear
metal oxides and hydrides are ionically bonded and basic

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

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15. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
How grouped results are
All except for lithium
RCOOR
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

16. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
strong acids/bases are written as H+ or OH- ions
Read the bottom of the meniscus
CO2 and H2O

17. oxalate
C2O4²?
#ligands=charge x2
ClO3?
boiling without losing volatile solvents/reactants

18. Acids + Carbonates (bicarbonates) make?
Mono; di; tri; tetra; penta; hexa.
Insoluble except nitrate and acetate
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Only temperature

19. What is the general formula for an amine?
Saturated - Substitution (which requires more radical conditions)
metal oxides and hydrides are ionically bonded and basic
RNH2
bent

20. primary colors
hydroxides (ex: Ba(OH)2)
red - green - blue
blue glass - it filters UV
Iodine and CO2 (dry ice)

21. silver iodide
CO2 and H2O
Pale yellow
H2PO4?
it reacts by substitution NOT addition

22. What do nonmetal oxides plus water form?
Salts (ex: CaO + SO2 ? CaSO3)
acid + alcohol
zero
acids

23. When driving off water from a hydrate - how do you tell you're done?
Sigma bonds are stronger than pi bonds
voltaic: + electrolytic: -
CnH2n-2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

24. What is the formula of butane?
C4H10
NH2?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
RCHO (carbonyl at end)

25. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Initiation energy (NOT Ea)
OH?
Selective absorption

26. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Salt + water
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
Insoluble except for nitrate and acetate

27. What shape is carbon dioxide?
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)
linear
Perform ICE BOX calculation based on K1
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

28. What is the test for hydrogen?
lighted splint (positive result=pop)
Check for air bubbles in the buret and remove the buret funnel from the buret
Group I metals (soft metals) are stored under oil
Soluble

29. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
different forms of the same element
Pipette (burette if need repetition)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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)

30. chlorate
But S° of element is not zero (except at 0K)
Tetrahedral
ClO3?
look for changes in oxidation # - the one that goes up is oxidized and is the RA

31. What is the formula of copper (II) phosphate?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Synthesis - separation and purification of the product and its identification.
Increases down group 1 decreases down group 17
Cu3(PO4)2

32. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
?G=negative - E° must be positive
Heptane
Reduction always takes place at the cathode (RED CAT) In both types of cell!

33. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Hg2²?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Silvery gray solid - brown - purple

34. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
#ligands=charge x2

35. What does saturated mean? Unsaturated?
Separating funnel
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Cr2O7²?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

36. Do you use J or kJ for ?H - ?S - and ?G?
CnH2n+2
voltaic: - electrolytic: +
?H-kJ - ?S-J - ?G-kJ
O2 needs 4F/mol H2 needs 2F/mol

37. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Big K=kf/kr
Graduated cylinder
More chaotic (ex: gases made)
Anode - oxygen. Cathode - hydrogen

38. What are the products of the reaction between group 1 metals and water?

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39. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
it's lower and occurs over less sharp a range
Pale purple - (orange)-yellow - red - blue - green.
redox reaction
Heat a test tube at an angle at the side of the tube (not bottom)

40. ________ are Lewis bases - because they can donate a lone pair of electrons.
CnH2n
CnH2n+1 often designated 'R' ex C3H7 is propyl
bases
OH- and NH3

41. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
NO3?
Selective absorption
blue (BTB)

42. How are metal oxides and hydrides bonded? are they acidic or basic?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
metal oxides and hydrides are ionically bonded and basic
ClO3?
Monomer + monomer = polymer product + a simple molecule such as water or HCl

43. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Identity and purity (impure compounds usually have broad & low melting points)
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
A) any range. b) 8-10 c) 4-6
Only temperature

44. A Bronsted-Lowry acid is...
proton donor base
Silvery gray solid - brown - purple
Hg²?
voltaic: + electrolytic: -

45. What is the formula for alkenes?
An active metal.
NO3?
CnH2n
Nothing

46. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
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.
CO (poisonous)
Pale yellow

47. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Sigma bonds are stronger than pi bonds
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

48. dihydrogen phosphate
no - they're written undissociated (HAaq)
H2PO4?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
An active metal.

49. What is the general formula for an ester?
Hg²?
ClO?
RCOOR
CnH(2n+2)

50. What type of compounds do Group 14 form?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
P2O5
+4-covalent - +2-ionic
neutralization: high K - H2O product dissociation: low K - H2O reactant