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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. The oxidation # for acid base reactions...
RX
do not change
Soluble except Ag - Pb - Ca - Sr Ba)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

2. What is the conjugate acid of H2PO4?
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.
H3PO4
acid + alcohol
Saturated - Substitution (which requires more radical conditions)

3. What is the energy you must put into a reaction to make it start called?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Concentration
Initiation energy (NOT Ea)

4. Why are i factors (Van't Hoff factors) often less than ideal?
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.
methyl formate
ion pairing
CO2 and H2O

5. What do metal oxides plus non- metal oxides form?
Most INsoluble except group 1 and ammonium
it is lower and occurs over less sharp a range
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Salts (ex: CaO + SO2 ? CaSO3)

6. What shape is water?
bent
Nothing
All except for lithium
CO3²?

7. chlorate
Sulfur
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ClO3?
fruit - fish - bases

8. What do you do to get rid of most of the solution from a precipitate?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Decant
allow for the vapor pressure of water and make sure to level levels

9. Acids + Carbonates (bicarbonates) make?
Current - time and charge on ion (moles of e used in half cell reaction)
PO4³?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Anode

10. How are metal oxides and hydrides bonded? are they acidic or basic?
no - they're written undissociated (HAaq)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
metal oxides and hydrides are ionically bonded and basic
SO4²?

11. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Read the bottom of the meniscus
Acids; HCOOCH3 is an ester
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

12. What is the test for oxygen?
Glowing splint (positive result=relights)
Clear
E=q + w (negative is by system - positive is on system)
proton donor base

13. 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?
10?8
ionic and form hydrogen and hydroxide
?H-kJ - ?S-J - ?G-kJ
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

14. What is the formula for obtaining charge flowing in a cell?
0.10M HCl (more ions)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
blue glass - it filters UV
Q=It (time in seconds)

15. Ions are not ______.
diamond and graphite
Reduction always takes place at the cathode (RED CAT) In both types of cell!
benzene is less reactive than alkenes
atoms

16. halides
0.10M HCl (more ions)
Greenish-yellow gas
Most are soluble except Ag - Pb
Experimental mass/theoretical mass X 100

17. Where are group I metals stored?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Q=It (time in seconds)
Group I metals (soft metals) are stored under oil
Soluble

18. What process do you use to obtain the solute from a solution?
Evaporation
CO (poisonous)
Mono; di; tri; tetra; penta; hexa.
Group 1 hydroxides (ex: NaOH)

19. For a dibasic acid (H2A) - [A²?]= ____ ?
Purple
K2
RNH2
Suniverse increases for spontaneous processes

20. What do hydrocarbons form when they burn in air (oxygen)?
ClO?
?G=negative - E° must be positive
No - NH3 and HCl gases are extremely soluble
CO2 and H2O

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

22. How does benzene compare in reactivity to alkenes?
Anode - oxygen. Cathode - hydrogen
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
benzene is less reactive than alkenes

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

24. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
do not change
Making sigma bonds and holding lone pairs

25. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Ksp = s²
Mono; di; tri; tetra; penta; hexa.
Kc=Kp
Insoluble except group 1 and ammonium

26. What does a short - sharp melting point indicate?
NO3?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Unsaturated - addition (ex: decolorize bromine solution)
Identity and purity (impure compounds usually have broad & low melting points)

27. Alkenes are ________ and react by __________
Products - reactants (except for BDE when it's reactants - products)
q=mc?T q=mL (or n x ?h)
Unsaturated - addition (ex: decolorize bromine solution)
catalyst=conc H2SO4

28. acetates
Soluble
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Hg²?
a-IMFs - b-molecular volume

29. copper sulfate
blue
Making sigma bonds and holding lone pairs
acid + alcohol
Sulfur

30. What are the units of the first order rate constant?
Ionic compounds
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Big K=kf/kr
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

31. bromothymol
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
More chaotic (ex: gases made)
blue (BTB)
Products - reactants (except for BDE when it's reactants - products)

32. What type of metals don't react with water or acids to form H2?

33. What things should you remember to do when collecting gas over water?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
allow for the vapor pressure of water and make sure to level levels
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

34. What type of compounds are almost always colored?
Acid rain - dissolves marble buildings/statues and kills trees.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Transition element compounds (except if it has a full or empty d shell)

35. What do you use to look at burning magnesium? why?
blue glass - it filters UV
Saturated - Substitution (which requires more radical conditions)
Separating funnel
Acidified

36. hydroxide
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)
RCOOR
OH?
Evaporation

37. What equipment do you need for a titration?
proton donor base
Evaporation
an oxidized and reduced substance
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

38. How many ligands attach to a central ion in a complex ion?
At half equivalence - pH=pKa
+4-covalent - +2-ionic
#ligands=charge x2
OH?

39. Does Benzene react by addition or substitution?
ion pairing
it reacts by substitution NOT addition
PO4³?
acids

40. What two compounds are great oxidizing agents?

41. What is the formula for summation?

42. primary colors
CO (poisonous)
voltaic: - electrolytic: +
red - green - blue
Most are soluble except Ag - Pb

43. Color is due to ______ _______ of light.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Selective absorption
The dilution effect when the solutions mix. M1V1 = M2V2

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

45. How does half life change for zero-th order - first order - and second order processes?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
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
are less dense than water
zero-th: decreases - first: constant - second: increases

46. Is the standard entropy (S°) of an element zero?
Hg2²?
blue (BTB)
Products - reactants (except for BDE when it's reactants - products)
But S° of element is not zero (except at 0K)

47. Nonmetals are good _____ agents. Metals are good _______ agents.
Eudiometer
CrO4²?
Acidified
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

48. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
Initiation energy (NOT Ea)
water and substances with (s) less dense than
SO4²?

49. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
no - they're written undissociated (HAaq)
blue glass - it filters UV

50. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
hydroxides (ex: Ba(OH)2)
boiling without losing volatile solvents/reactants
acids