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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. phosphates
CrO4?
basic
Most INsoluble except group 1 and ammonium
Mn? - Cr? - Cr

2. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
HClO4
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Insoluble except for nitrate and acetate
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2

3. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
E=q + w (negative is by system - positive is on system)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
basic
ClO?

4. nitrate
Kc=Kp
it's lower and occurs over less sharp a range
NO3?
a-IMFs - b-molecular volume

5. What is the general formula for an ester?
RCOOR
blue glass - it filters UV
Salts (ex: CaO + SO2 ? CaSO3)
Acidified

6. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Soluble
Combine the equations for the half reactions in the non-spontaneous direction
Increases.

7. Is the freezing of ice endothermic or exothermic?
Orange
MnO4?
ion pairing
Exothermic

8. What is the relationship in strength between sigma and pi bonds?
Purple
Combine the equations for the half reactions in the non-spontaneous direction
Sigma bonds are stronger than pi bonds
H2PO4?

9. cyanide
CN?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Ksp = 27s4
Synthetic condensation polymer (aka a polyamide)

10. What are the formulas for q?
chemically (ex: with carbon)
H+
bent
q=mc?T q=mL (or n x ?h)

11. group 1 ions/compounds
blue glass - it filters UV
Group 1 hydroxides (ex: NaOH)
Salt and water
Soluble

12. bromothymol
blue (BTB)
Group 1 hydroxides (ex: NaOH)
It ceases - the circuit is broken.
Acidic solutions (Ex: [Fe(H2O)6]? + H2O = Fe(H2O)5OH]? + H3O?)

13. phosphate
PO4?
Identity and purity (impure compounds usually have broad & low melting points)
boiling without losing volatile solvents/reactants
Cr2O7?

14. Is the ?H formation of an element in standard state zero?
by electrolysis
?H formation of an element in standard state=0
ROH
Increases.

15. How are strong ones written?
Decant
lighted splint (positive result=pop)
The one with most oxygen atoms (highest oxidation number)
strong acids/bases are written as H+ or OH- ions

16. What is H2CO3 (carbonate acid) usually written as?
Current - time and charge on ion (moles of e used in half cell reaction)
NH4?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
H2O + CO2 (it decomposes readily)

17. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Most are soluble except Ag - Pb
R=8.31 J/mol/K
water and substances with (s) less dense than
Suniverse increases for spontaneous processes

18. Esterification is...
acid + alcohol
The compound with the lowest Ksp value.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CnH(2n+2)

19. How many normal boiling points and boiling points are there?
Transition element compounds (except if it has a full or empty d shell)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Decant
NH2?

20. What electrons are lost/gained first in transition element ions?
The dilution effect when the solutions mix. M1V1 = M2V2
S crystal at 0K=0
Salt + water.
ns electrons (first in-first out)

21. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Most INsoluble except group 1 and ammonium
Only temperature
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ksp = 108s5

22. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Exothermic
a-IMFs - b-molecular volume
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
CO3?

23. What do you need to make a polymer?
C4H10
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)
Greenish-yellow gas
Insoluble

24. When can supercooling occur? What does it look like on a cooling curve?
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.
Synthesis - separation and purification of the product and its identification.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Trigonal pyramidal

25. When a cell is 'flat' What is its voltage?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Saturated - Substitution (which requires more radical conditions)
zero
How grouped results are

26. What type of compounds do metals/non metals form?
Ionic compounds
Monomer + monomer = polymer product + a simple molecule such as water or HCl
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Ksp = s

27. dichromate (soln + most solids)
same KE - but PEice<PEwater
Suniverse increases for spontaneous processes
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2
Orange

28. What is the formula for obtaining charge flowing in a cell?
S crystal at 0K=0
Ionic compounds
Q=It (time in seconds)
It ceases - the circuit is broken.

29. What is the formula for summation?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Tetrahedral
Products - reactants (except for BDE when it's reactants - products)
Hydrogen (active metals are metals with more negative reduction potentials in E chart)

30. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
ROH

31. carbonate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CO3?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

32. acetates
HClO4
r1/r2=(M2/M1)^ - v1/v2=(T1/T2)^ - E1/E2=T1/T2
Soluble
All except for lithium

33. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
bright yellow
NO3?

34. What does a short - sharp melting point indicate?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
?H formation of an element in standard state=0
Identity and purity (impure compounds usually have broad & low melting points)
allow for the vapor pressure of water and make sure to level levels

35. chromate
fruit - fish - bases
Ksp = s
acids
CrO4?

36. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
it reacts by substitution NOT addition
Iodine and CO2 (dry ice)

37. Do anions flow to the cathode or anode?
RX
More chaotic (ex: gases made)
Anode
?G=negative - E must be positive

38. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
A) any range. b) 8-10 c) 4-6
Q=It (time in seconds)
Increases.

39. chlorine
Kc=Kp
it's lower and occurs over less sharp a range
Greenish-yellow gas
SO4?

40. How does the KE and PE of ice at 0C compare to the KE and PE of water at 0C?
same KE - but PEice<PEwater
Reverse most negative E and add voltages to get Ecell (or take absolute difference between Ered values)
Most INsoluble except group 1 and ammonium
CnH2n+2

41. Acidic gases like SO2 in the atmosphere cause what environmental problems?
it's lower and occurs over less sharp a range
Conjugate pair (one must be a weak base or acid)
Acid rain - dissolves marble buildings/statues and kills trees.
voltaic: + electrolytic: -

42. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Heptane
blue (BTB)
The benzene ring (or more correctly the phenyl group - C6H5)

43. What is the energy you must put into a reaction to make it start called?
methyl formate
Initiation energy (NOT Ea)
Group 1 hydroxides (ex: NaOH)
Insoluble except for nitrate and acetate

44. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Salt and water
hydroxides (ex: Ba(OH)2)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Trigonal pyramidal

45. Name C7H16
no - they're written undissociated (HAaq)
?G= -ve - E= +ve
Making sigma bonds and holding lone pairs
Heptane

46. What two compounds are great oxidizing agents?
an oxidized and reduced substance
Ksp = 27s4
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

47. What is the charge on a chlorine atom?
Insoluble
Mn? - Cr? - Cr
Acids; HCOOCH3 is an ester
zero

48. Which of the rates changes more when temperature is increased?
zero
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Insoluble
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

49. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CN?
Reduction always takes place at the cathode (RED CAT) In both types of cell!

50. silver iodide
OH- and NH3
Pale yellow
NO3?
fruit - fish - bases

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