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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.
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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. What steps do organic labs consist of?
basic
zero
Synthesis - separation and purification of the product and its identification.
Increases down group 1 decreases down group 17

2. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
More chaotic (ex: gases made)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

3. What shape is ammonia?
#ligands=charge x2
ROR
Trigonal pyramidal
CrO4²?

4. What are two allotropes of carbon?
Heptane
Time?¹ - (ex. s?¹ - hr?¹ - etc)
diamond and graphite
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

5. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
acid + alcohol
Greenish-yellow gas
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

6. What shape is methane?
H2O + CO2 (it decomposes readily)
CO3²?
Tetrahedral
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

7. What electrons are lost/gained first in transition element ions?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
ns² electrons (first in-first out)
?G=negative - E° must be positive
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

8. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
|experimental - accepted|/accepted X 100
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

9. What is the pH of 1.0M HCl? 1M NaOH?
diamond and graphite
The compound with the lowest Ksp value.
0 and 14
Ions go through the salt bridge - electrons go through metal wires in the external circuit

10. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
|experimental - accepted|/accepted X 100
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
The compound with the lowest Ksp value.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

11. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Kc=Kp
Mn²? - Cr³? - Cr³
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
ClO2?

12. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
At half equivalence - pH=pKa
neutralization: high K - H2O product dissociation: low K - H2O reactant
different forms of the same element
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

13. sulfates
CO (poisonous)
White precipitate
Soluble except Ag - Pb - Ca - Sr Ba)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

14. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
Acidified
ClO3?
catalyst=conc H2SO4

15. What is the general formula for alkyl halides?
NH2?
do not change
RX
fractional distillation

16. Acids + Carbonates (bicarbonates) make?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
S crystal at 0K=0
CnH2n-2
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

17. What shape is carbon dioxide?
Group I metals (soft metals) are stored under oil
linear
Heptane
zero

18. What kind of bonding structure does benzene have?
Sigma bonds are stronger than pi bonds
Unsaturated - addition (ex: decolorize bromine solution)
benzene has a delocalized pi ring structure
chemically (ex: with carbon)

19. When the salt bridge is removed what happens to the cell reaction?
Increases down group 1 decreases down group 17
Molecules with the same molecular formulas - but different structural formulas
It ceases - the circuit is broken.
Combine the equations for the half reactions in the non-spontaneous direction

20. The oxidation # for acid base reactions...
zero-th: decreases - first: constant - second: increases
SO4²?
do not change
OH?

21. One mole of electrons carries 96500Coulombs - what is this quantity called?

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22. What is the formula of butane?
Synthetic condensation polymer (aka a polyamide)
C4H10
neutralization: high K - H2O product dissociation: low K - H2O reactant
They decrease (or could be the same if the solid has ONLY JUST disappeared)

23. What are isotopes?
left - ppt will form
Ppt will NOT form (unsaturated)
Ksp = 4s³
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

24. During a titration what is present in the beaker at the equivalence point?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Synthesis - separation and purification of the product and its identification.
A salt solution.
Glowing splint (positive result=relights)

25. phosphates
Heptane
Most INsoluble except group 1 and ammonium
But S° of element is not zero (except at 0K)
same KE - but PEice<PEwater

26. hydroxide
OH?
Products - reactants (except for BDE when it's reactants - products)
basic
bent

27. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
Ksp = 27s4
Acids; HCOOCH3 is an ester
blue glass - it filters UV

28. Neutralization is an ________ reaction.
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
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Insoluble except group 1 and ammonium
Exothermic (?H for ANY sa/sb = -57kJ/mol)

29. Ions are not ______.
Ksp = 4s³
atoms
0 and 14
left - ppt will form

30. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Initiation energy (NOT Ea)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Decant

31. What causes the dramatic effect of T on rate?
NH4?
T increases exponentially the proportion of molecules with E > Ea
Silvery gray solid - brown - purple
Filtration

32. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
PO4³?
Soluble
H2O + CO2 (it decomposes readily)

33. What type of polymer is nylon?
RX
Synthetic condensation polymer (aka a polyamide)
Current - time and charge on ion (moles of e used in half cell reaction)
Making sigma bonds and holding lone pairs

34. What is an Alkyl group?

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35. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
H2PO4?
Synthesis - separation and purification of the product and its identification.
HClO4

36. nitrate
metal oxides and hydrides are ionically bonded and basic
blue
NO3?
Hg2²?

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

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38. ________ are Lewis bases - because they can donate a lone pair of electrons.
brown volatile liquid
OH- and NH3
Transition element compounds (except if it has a full or empty d shell)
Group I metals (soft metals) are stored under oil

39. What process do you use to obtain the solute from a solution?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Insoluble (except group 1 ammonium and Ba)
Evaporation
HClO4

40. perchlorate
Silvery gray solid - brown - purple
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Acids; HCOOCH3 is an ester
ClO4?

41. What type of compounds do metals/non metals form?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
fractional distillation
Ionic compounds
Pale purple - (orange)-yellow - red - blue - green.

42. How are strong ones written?
bent
same KE - but PEice<PEwater
?H formation of an element in standard state=0
strong acids/bases are written as H+ or OH- ions

43. When a cell is 'flat' What is its voltage?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero
Sigma bonds are stronger than pi bonds

44. What is the word equation for condensation polymerisation ?
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)
Mono; di; tri; tetra; penta; hexa.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Glowing splint (positive result=relights)

45. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
T increases exponentially the proportion of molecules with E > Ea
Disulfur dichloride
benzene is less reactive than alkenes

46. acetate
Only temperature
CH3COO?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
it reacts by substitution NOT addition

47. How does the melting point of a mixture compare to the MP of a pure substance?
|experimental - accepted|/accepted X 100
0.10M HCl (more ions)
it is lower and occurs over less sharp a range
Salt + water.

48. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
At half equivalence - pH=pKa
K1 x K2
Perform ICE BOX calculation based on K1

49. What is the difference between equivalence point and end point of a titration.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Group 1 hydroxides (ex: NaOH)
Clear
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

50. What is the formula of copper (II) phosphate?
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
Cu3(PO4)2
Soluble
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)