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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.
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. bromine
ClO?
brown volatile liquid
a-IMFs - b-molecular volume
Purple

2. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
allow for the vapor pressure of water and make sure to level levels
Insoluble (except group 1 ammonium and Ba)
it reacts by substitution NOT addition
do not change

3. What do acids plus active metals form?
a-IMFs - b-molecular volume
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Selective absorption

4. A geometric (or cis-trans) isomer exists due to.....
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
allow for the vapor pressure of water and make sure to level levels
an oxidized and reduced substance

5. ammonium
Iodine and CO2 (dry ice)
NH4?
ion pairing
by electrolysis

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
acid + alcohol
Ksp = 4s³
it is lower and occurs over less sharp a range
zero-th: decreases - first: constant - second: increases

7. What is a coordinate covalent bond?
Tetrahedral
voltaic: + electrolytic: -
Both electrons come from the same atom (just as good as a regular bond)
H3PO4

8. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
Read the bottom of the meniscus
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)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

9. What type of compounds are almost always colored?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
bent
metal oxides and hydrides are ionically bonded and basic
Transition element compounds (except if it has a full or empty d shell)

10. What is the charge on a chlorine atom?
Initiation energy (NOT Ea)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
zero
No - it depends on the number of ions produced on dissolving.

11. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
benzene is less reactive than alkenes
basic
small size and high charge
S2O3²?

12. What is the formula for alkynes?
redox reaction
CnH2n-2
Iodine and CO2 (dry ice)
a-IMFs - b-molecular volume

13. 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
H2O + CO2 (it decomposes readily)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

14. carbonate
CO3²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Sulfur
RX

15. What is reflux?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
boiling without losing volatile solvents/reactants
No - it depends on the number of ions produced on dissolving.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

16. 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?
CnH2n+1 often designated 'R' ex C3H7 is propyl
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
ethers
Read the bottom of the meniscus

17. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
The benzene ring (or more correctly the phenyl group - C6H5)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
strong acids/bases are written as H+ or OH- ions

18. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
Identity and purity (impure compounds usually have broad & low melting points)
CO2 and H2O
bent

19. Esters smell like _______ and amines smell like _______ and are ______.
atoms
Transition element compounds (except if it has a full or empty d shell)
basic
fruit - fish - bases

20. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
ClO4?
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)

21. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
#ligands=charge x2
Cr2O7²?
How grouped results are

22. hydroxides
Insoluble (except group 1 ammonium and Ba)
Greenish-yellow gas
Ions go through the salt bridge - electrons go through metal wires in the external circuit
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

23. Alkenes are ________ and react by __________
no - they're written undissociated (HAaq)
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.
Unsaturated - addition (ex: decolorize bromine solution)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

24. Esterification is...
benzene is less reactive than alkenes
?G=negative - E° must be positive
acid + alcohol
Hg2²?

25. How are primary alcohols turned into acids?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
lighted splint (positive result=pop)
atoms

26. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
The compound with the lowest Ksp value.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Ionic compounds
Combine the equations for the half reactions in the non-spontaneous direction

27. What are the formulas for q?
All except for lithium
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
RX
q=mc?T q=mL (or n x ?h)

28. What is the pH of 1.0M HCl? 1M NaOH?
Ksp = 27s4
Ions go through the salt bridge - electrons go through metal wires in the external circuit
0 and 14
Ppt will NOT form (unsaturated)

29. What device would you use to measure a volume of gas?
Eudiometer
No - it depends on the number of ions produced on dissolving.
Salt + water
benzene is less reactive than alkenes

30. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
H2PO4?
ROR
are less dense than water

31. What is the difference between equivalence point and end point of a titration.
Glowing splint (positive result=relights)
strong acids/bases are written as H+ or OH- ions
small size and high charge
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

32. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
blue (BTB)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
NH2?
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

33. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Clear
CN?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

34. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
No - it depends on the number of ions produced on dissolving.
H3PO4
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
HClO4

35. silver compounds
HClO4
acid + alcohol
Kc=Kp
Insoluble except for nitrate and acetate

36. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
RCHO (carbonyl at end)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
zero
10?8

37. Both Acetic acid and ____________ are also functional isomers.
methyl formate
Transition element compounds (except if it has a full or empty d shell)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

38. oxalate
Transition element compounds (except if it has a full or empty d shell)
Suniverse increases for spontaneous processes
C2O4²?
Experimental mass/theoretical mass X 100

39. Is the ?H formation of an element in standard state zero?
water and substances with (s) less dense than
?H formation of an element in standard state=0
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
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

40. sulfates
RNH2
Soluble except Ag - Pb - Ca - Sr Ba)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Heptane

41. What are the signs for ?G and E° for spontaneous reactions?
OH?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
?G= -ve - E°= +ve
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

42. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
RCOOH
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
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)

43. chlorate
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
?G= -ve - E°= +ve
Most INsoluble except group 1 and ammonium
ClO3?

44. Which alkali metals float on water?
Add acid to water so that the acid doesn't boil and spit
All except for lithium
linear
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)

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

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46. If ?S is positive - are the products more or less chaotic than the reactants?
Soluble
fractional distillation
More chaotic (ex: gases made)
by electrolysis

47. If a free element is involved - what type of reaction must be involved?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Trigonal pyramidal
Check for air bubbles in the buret and remove the buret funnel from the buret
redox reaction

48. What do ions and electrons travel through in a voltaic/electrolytic cell?
metal oxides and hydrides are ionically bonded and basic
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Making sigma bonds and holding lone pairs

49. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
P2O5
Read the bottom of the meniscus
different forms of the same element

50. How does the melting point of a mixture compare to the MP of a pure substance?
Sulfur
it is lower and occurs over less sharp a range
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Salt + water