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. Lattice energy is high for ions with _____ size and _____ charge
water and substances with (s) less dense than
Pale purple - (orange)-yellow - red - blue - green.
Hg²?
small size and high charge


2. chromate
water and substances with (s) less dense than
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CrO4²?
chemically (ex: with carbon)


3. How does half life change for zero-th order - first order - and second order processes?
Ksp = 27s4
PO4³?
zero-th: decreases - first: constant - second: increases
proton donor base


4. What type of compounds do metals/non metals form?
An active metal.
Separating funnel
Ionic compounds
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)


5. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
lighted splint (positive result=pop)
Filtration
T increases exponentially the proportion of molecules with E > Ea
same KE - but PEice<PEwater


6. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Current - time and charge on ion (moles of e used in half cell reaction)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell


7. 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
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Suniverse increases for spontaneous processes
CnH2n+2


8. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Soluble except Ag - Pb - Ca - Sr Ba)
Exothermic (?H for ANY sa/sb = -57kJ/mol)


9. What type of compounds are almost always colored?
?G= -ve - E°= +ve
Transition element compounds (except if it has a full or empty d shell)
Tetrahedral
The Faraday or Faraday's constant.


10. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
atoms
CO (poisonous)
benzene is less reactive than alkenes


11. 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
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Acids; HCOOCH3 is an ester
Separating funnel


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

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

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14. What process do you use to obtain the solute from a solution?
Soluble
Evaporation
Glowing splint (positive result=relights)
bases


15. 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)
water and substances with (s) less dense than
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble


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

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17. What is an Alkyl group?

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18. What shape is methane?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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)
same KE - but PEice<PEwater
Tetrahedral


19. What is the general formula for alkyl halides?
Greenish-yellow gas
fruit - fish - bases
RX
Trigonal pyramidal


20. What causes the dramatic effect of T on rate?
blue (BTB)
Greenish-yellow gas
T increases exponentially the proportion of molecules with E > Ea
C4H10


21. primary colors
S crystal at 0K=0
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CN?
red - green - blue


22. What is the test for hydrogen?
fractional distillation
lighted splint (positive result=pop)
Read the bottom of the meniscus
CnH(2n+2)


23. dichromate (soln + most solids)
Most INsoluble except group 1 and ammonium
acids
Orange
Separating funnel


24. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
Insoluble except nitrate and acetate
O2 needs 4F/mol H2 needs 2F/mol
CnH2n+2


25. potassium permanganate
Both electrons come from the same atom (just as good as a regular bond)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CnH2n
Purple


26. Why are noble gases stable?
Combine the equations for the half reactions in the non-spontaneous direction
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.


27. What device would you use to measure a volume of gas?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Eudiometer
are less dense than water
basic


28. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
Big K=kf/kr
Iodine and CO2 (dry ice)
Acids; HCOOCH3 is an ester


29. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Clear
water and substances with (s) less dense than
MnO4?


30. What are hybrid orbitals used for?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Eudiometer
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
Making sigma bonds and holding lone pairs


31. Why are i factors (Van't Hoff factors) often less than ideal?
CO2 and H2O
Experimental mass/theoretical mass X 100
voltaic: - electrolytic: +
ion pairing


32. What is the formula for alkynes?
No - it depends on the number of ions produced on dissolving.
CnH2n-2
Ksp = 108s5
The dilution effect when the solutions mix. M1V1 = M2V2


33. permanganate
MnO4?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
C2O4²?


34. chlorate
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ClO3?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Distillation


35. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Big K=kf/kr
A) any range. b) 8-10 c) 4-6
benzene is less reactive than alkenes
P2O5


36. bromothymol
blue (BTB)
CH3COO?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K


37. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Graduated cylinder
Only temperature
Tetrahedral
Meth - eth - prop - but - pent - hex - hept - oct - non - dec


38. ammonium
?H formation of an element in standard state=0
NH4?
voltaic: + electrolytic: -
NH2?


39. Is the standard entropy (S°) of an element zero?
K2
RNH2
Graduated cylinder
But S° of element is not zero (except at 0K)


40. What is the general formula for an ether?
ROR
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
The one with most oxygen atoms (highest oxidation number)
Mono; di; tri; tetra; penta; hexa.


41. What is a coordinate covalent bond?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Pale purple - (orange)-yellow - red - blue - green.
are less dense than water
Both electrons come from the same atom (just as good as a regular bond)


42. phosphate
water and substances with (s) less dense than
But S° of element is not zero (except at 0K)
PO4³?
Hg²?


43. What are the signs for ?G and E° for spontaneous reactions?
left - ppt will form
?G= -ve - E°= +ve
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Soluble


44. Name some properties of Group 17
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.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
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 group 1 ammonium and Ba)


45. 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?
Sulfur
|experimental - accepted|/accepted X 100
Combine the equations for the half reactions in the non-spontaneous direction
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


46. What is the energy you must put into a reaction to make it start called?
Perform ICE BOX calculation based on K1
O2 needs 4F/mol H2 needs 2F/mol
Initiation energy (NOT Ea)
Conjugate pair (one must be a weak base or acid)


47. What equipment do you need for a titration?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Acid rain - dissolves marble buildings/statues and kills trees.
Hg2²?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask


48. If a free element is involved - what type of reaction must be involved?
redox reaction
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
S2O3²?
blue


49. What part of a liquid do you look at to measure its volume?
proton donor base
Transition element compounds (except if it has a full or empty d shell)
Read the bottom of the meniscus
The one with most oxygen atoms (highest oxidation number)


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

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