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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. What value of R do you use for thermo calculations? gas calculations?
Insoluble (except group 1 ammonium and Ba)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
acids
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

2. Both Acetic acid and ____________ are also functional isomers.
Pale yellow
methyl formate
Trigonal pyramidal
non-metal oxides and hydrides are covalently bonded and are acidic.

3. Can you collect soluble gases over water?
Group I metals (soft metals) are stored under oil
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
zero
No - NH3 and HCl gases are extremely soluble

4. What is the formula for obtaining charge flowing in a cell?
Purple
strong acids/bases are written as H+ or OH- ions
Check for air bubbles in the buret and remove the buret funnel from the buret
Q=It (time in seconds)

5. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
bright yellow
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?)

6. What measuring device would you use for very small volumes of liquids?
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)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Pipette (burette if need repetition)
ROR

7. What is the formula for alkynes?
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
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CnH2n-2

8. What is the slope of the graph of lnk vs. 1/T?
CN?
The Faraday or Faraday's constant.
Greenish-yellow gas
-Ea/R

9. sulfates
Suniverse increases for spontaneous processes
Soluble except Ag - Pb - Ca - Sr Ba)
Soluble
neutralization: high K - H2O product dissociation: low K - H2O reactant

10. How many faradays of electric charge do you need to produce one mole of O2? H2?
C4H10
O2 needs 4F/mol H2 needs 2F/mol
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Acids; HCOOCH3 is an ester

11. How are more active metals reduced?
Insoluble except nitrate and acetate
Acidified
by electrolysis
proton donor base

12. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
?H formation of an element in standard state=0
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Cu3(PO4)2

13. What do metal oxides plus acids form?
it reacts by substitution NOT addition
Salt + water
Insoluble except nitrate and acetate
PO4³?

14. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
How close results are to the accepted value
water and substances with (s) less dense than
0.10M HCl (more ions)
Group 1 hydroxides (ex: NaOH)

15. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
strong acids/bases are written as H+ or OH- ions
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)
Pale purple - (orange)-yellow - red - blue - green.
Mn²? - Cr³? - Cr³

16. What is the conjugate acid of H2PO4?
H3PO4
K2
ROH
Big K=kf/kr

17. What is H2CO3 (carbonate acid) usually written as?
0 and 14
H2O + CO2 (it decomposes readily)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Pour liquids using a funnel or down a glass rod

18. What is the general formula for a ketone?
small size and high charge
RCOR
S crystal at 0K=0
Cr2O7²?

19. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
a-IMFs - b-molecular volume
different forms of the same element
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

20. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
neutralization: high K - H2O product dissociation: low K - H2O reactant
CO3²?
Selective absorption

21. What is the conjugate base of NH3?
NH2?
How close results are to the accepted value
Selective absorption
bases

22. Neutralization is an ________ reaction.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
S crystal at 0K=0
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Anode

23. hydroxides
Insoluble (except group 1 ammonium and Ba)
Salt + water.
Sigma bonds are stronger than pi bonds
Acid rain - dissolves marble buildings/statues and kills trees.

24. What shape is carbon dioxide?
?H formation of an element in standard state=0
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Group 1 hydroxides (ex: NaOH)
linear

25. chlorate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
All except for lithium
ClO3?
zero-th: decreases - first: constant - second: increases

26. What are allotropes?
different forms of the same element
Ksp = 108s5
ion pairing
Transition element compounds (except if it has a full or empty d shell)

27. Buffer capacity must contain decent amounts of a ________ ________
ionic and form hydrogen and hydroxide
S2O3²?
Conjugate pair (one must be a weak base or acid)
Separating funnel

28. How are non-metal oxides and hydrides bonded? are they acidic or basic?
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.
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 -
non-metal oxides and hydrides are covalently bonded and are acidic.

29. What are two allotropes of carbon?
diamond and graphite
Clear
Combine the equations for the half reactions in the non-spontaneous direction
Disulfur dichloride

30. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
ion pairing
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

31. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
CnH(2n+2)
CN?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ksp = 4s³

32. What element is used to vulcanize rubber?
Selective absorption
Soluble
Sulfur
K1 x K2

33. If ?S is positive - are the products more or less chaotic than the reactants?
boiling without losing volatile solvents/reactants
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
More chaotic (ex: gases made)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

34. hypochlorite
methyl formate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ClO?
Experimental mass/theoretical mass X 100

35. A Bronsted-Lowry acid is...
red - green - blue
Salt + water
proton donor base
Insoluble except group 1 and ammonium

36. Alkanes are _________ and react by _________
Soluble
redox reaction
Current - time and charge on ion (moles of e used in half cell reaction)
Saturated - Substitution (which requires more radical conditions)

37. What is the formula for alkanes?
MnO4?
CnH2n+2
Clear
Perform ICE BOX calculation based on K1

38. chlorine
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Greenish-yellow gas
-Ea/R
it reacts by substitution NOT addition

39. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
?G=negative - E° must be positive
+4-covalent - +2-ionic
But S° of element is not zero (except at 0K)

40. How many ligands attach to a central ion in a complex ion?
White precipitate
Anode - oxygen. Cathode - hydrogen
#ligands=charge x2
Greenish-yellow gas

41. What is the basic structure of an optical isomer?
CnH2n
HClO4
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Anode

42. sulfate
fractional distillation
SO4²?
hydroxides (ex: Ba(OH)2)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

43. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
10?8
it is lower and occurs over less sharp a range
Selective absorption

44. What is the formula of butane?
T increases exponentially the proportion of molecules with E > Ea
do not change
C4H10
CH3COO?

45. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Sigma bonds are stronger than pi bonds
H+
Mono; di; tri; tetra; penta; hexa.
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.

46. dihydrogen phosphate
Disulfur dichloride
no - they're written undissociated (HAaq)
H2PO4?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

47. Alkenes are ________ and react by __________
Salt + water.
Unsaturated - addition (ex: decolorize bromine solution)
#ligands=charge x2
Time?¹ - (ex. s?¹ - hr?¹ - etc)

48. Does Kw increase or decrease with T? Why?
Current - time and charge on ion (moles of e used in half cell reaction)
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.
NH4?

49. What do hydrocarbons form when they burn in air (oxygen)?
CnH2n+2
a-IMFs - b-molecular volume
CO2 and H2O
CN?

50. What are the names and formulas of the 6 strong acids?
RCOOH
HClO4
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

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AP Chemistry 2

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