CHEM 202 Chapter Notes - Chapter 15: Colligative Properties, Semipermeable Membrane, Supersaturation

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an orbital that results from the mixing of different kinds of atomic orbitals on the same

atom. For

example. An sp3 hybrid results from the mixing of one s orbital and three p orbitals

hybridization

the mixing of different types of atomic orbitals to produce a set of equivalent new-hybrid

shape orbitals

delocalization

electrons that are spread over a number of atoms in a molecule or a crystal rather than

localized on a single

atom or pair of atoms

saturated

a solution in which undissolved solute and dissolved solute are in equilibrium

supersaturated

a solution containing more solute than an equivalent saturated solution

henrys law

states that the concentration of a gas in a solution, sg, is proportional to the pressure of

gas

over the solution.

Mole Fraction (χx)

concentration expressed using moles of one component divided by the total moles in

the solution

colligative properties

a property of a solvent the depends on the total concentration of solute particles

present.

• Vapor-Pressure Lowering

• Freezing-Point Depression

• Boiling-Point Elevation

• Osmotic Pressure

osmotic pressure

the pressure that must be applied to a solution to stop osmosis from pure solvent into

the

solution.

osmosis

the net movement of solvent through a semipermeable membrane toward the solution

with greater solute concentration

colloids

mixtures containing particles larger than normal solutes but small enough to remain

suspended in the dispersing medium.

tyndall effect

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Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one ? bond with another carbon atom and one ? and one ? bond with another carbon atom. Each carbon atom also forms one ? bond with a hydrogen atom. Identify which types of orbitals overlap to form the bonds between the atoms in a benzene molecule. Drag the appropriate labels to their respective targets.

Attached is picture. Please explain/show work, will give 5 stars to correct answer, thank you very much! :)

Chemical bonds are formed by linear combinations of atomic orbital's. These atomic orbital's should have compatible energies. An axial overlap of these orbitals results in the formation of a sigma bond, whereas a lateral overlap results in the formation of a pi bond. When two atomic orbitai's on different atoms approach each other, two molecular orbital's are formed: one bonding molecular orbital and one antibonding molecular orbital. The bonding molecular orbital has a lower energy than the corresponding atomic orbital's: antibonding orbital's have higher energies than the corresponding atomic orbital's. An example using the hydrogen molecule is shown here. However, the same rule applies to systems with multiple atomic orbital's. For each atomic orbital that overlaps, one molecular orbital must form. In the diagram below. 1s orbitais from two hydrogen atoms combine to form one bonding sigma1 orbital and one antibonding orbital. The total number of bonding and antibonding orbital's is always equal to the number of orbital's that overlap. Similarly, molecular orbital's can also be formed by the overlapping of hybrid orbital's. The hybrid orbital's are formed by the linear combination of different atomic orbital's of nearly equal energy on the same atom. The atomic orbital's of nearly equal energy undergo a process of mixing and reorientation to form new orbital's of lower energy. This process is called hybridization For example, hybridization of one s and two p orbital's on an atom forms three sp2 hybrid orbital's. Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one sigma bond with another carbon atom and one sigma and one pi bond with another carbon atom. Each carbon atom also forms one sigma bond with a hydrogen atom. Identify which types of orbital's overlap to form the bonds between the atoms in a benzene molecule.

Show transcribed image text LTIPLE CHOICE. Choose the one alternative that best completes the statement or answers th tion. 1) 1) How many lone pairs are on the Br atom in BrF2-? D) 3 A) 1 B) 0 C) 2 2) 2) Based on VSEPR theory, which should have the smallest XAX bond angle? D) A) B) C)
5) Arrange in order from the smallest to the largest bond angle: CH3+, NF3, NH4+, XeF4. 5) A) XeF4, NH4+, NF3, CH3+ C) NF3, NH4+, XeF4, CH3+ B) XeF4, NF3, NH4+, CH3+ D) CH3+, NF3, NH4+, XeF4
11) What is the bond angle in the following molecular model of NO2-? A) less than 109.5 B) 109.5 C) less than 120Â° but greater than 109.5 D) 120Â° 12) 12) What are the bond angles in the folowing molecular model of SO32-? ao A) less than 109.5 B) 109.5Â° C) less than 120Â° but greater than 109.5 D) 120 13) 13) How many of the following molecules are polar? B) 0 D) 3 E) 1 A) 2 14 14) Determine the electron geometry (eg, molecular geometry (mg. and polarity of Pa A) eg-trigonal pyramidal mg-trigonal pyramidal polar B) eg-tetrahedral mg-bent, polar C) eg-tetrahedral, mg-trigonal pyramidal polar D) eg-linear, mg-linear, nompolar E) eg-trigonal planar, mg-trigonal planar, nonpolar 15) Which orbital hybridization is associated with a tetrahedral charge cloud arrangement? 15)__ B) sp3 D) None of these C) sp 16) Which of the following is not true? 16 A) An sp3 hybrid orbital may hold a lone pair of electrons B) An sp3 hybrid orbital may form a pi bond by overlap with an orbital on another atom. C) An sp3 hybrid orbital may form a sigma bond by overlap with an orbital on another atom. D) The sp3 hybrid orbitals are degenerate.
chlo 17) What orbital hybridization is expected for the central atom in a molecule with a trigonal 17)_ planar geometry? A) sp2 C) sp B) sp3 D) None of these 18) Which atomic orbitals are involved in bonding and which as lone pair orbitals for 18) N2H2? H N N-H A) boading: s on H, sp2 and p on N B) bonding: s on H, sp2 on N C) bonding: sp2 on both H and N D) bonding: s on H, p on N lone pair: sp2 on N lone pair: p on N lone pair: p on N lone pair: sp2 on N 19) Place the following in order of increasing dipole moment 20) Give the hybridization for the O in OF2 21) Give the hybridization for the Br in BrCl3 22) Give the hybridization for the C in HCCH A)sp 20) E) sp3 Ð)sp3d 21) D) sp E)sp3 A)sp3 B) sp3d2 C) sp 22) D) sp3d E)sp2
23) Identify the set of hybrid orbitals shown below. A) sp C) sp3 B) sp2 D) None of these 24) Which molecule has a central atom that uses the set of hybrid orbitals shown below to form bonds 24) with the non-central atoms? A) NO2 B) H20 C) co2

HERE IS HOW THIS IS GOING TO WORK! IF YOU ANSWER THE QUESTIONS IWILL GIVE YOU THE 3K POINTS + MORE AFTER I REPOST IT.

2. The amount of heat involved in the synthesis of 1 mole of acompound from its elements, with all substances in their standardstates at 25*C, is called _________.

3. What is a valid unit for specific heat?

4. Use Hess's Law to find the heat of reaction in the examplebelow.

N2O4 (g) ----> 2NO2 (g)

Given that:

N2O4 (g) ----> N2 (g) + 2O2 (g) (Delta H =-9.7kJ)

2NO2 (g) ----> 2O2(g) + N2(g) ( Delta H= -67.7kJ)

5. Use Hess's Law to find the heat of reaction in the examplebelow. (Example doesn't exist btw.)

6. (Delta H) for the formation of rust (Fe2O3) is -826 kJ/mol. Howmuch energy is involved in the formation of 5 grams ofrust?

7. How many kilocalories of heat are required to raise thetemperature of 50g of aluminum from -5*C to 35*C? (Specific heat ofAluminum = 0.21 cal/g*C)

8.Calculate the (Delta H) for this reaction:

Zn(s) + Cu (2+ ion)(aq) ---> Zn(2+) + Cu(s)

(Delta H) for Cu(2+) = +64.4 kJ/Mol; (Delta H) for Zn(2+) = -152.4kJ/mol

9. The following equation shows the reaction that occurs whennitroglycerine explodes.

4C3H5O9N3 ----> 12CO2 + 6N2 + O2 +10H2O + 1725 Kcal

Is this reaction exothermic , endothermic, a combustion reaction ,or a combination reaction?

10. What does it mean for ammonia, (NH3) to have a (Delta H f) =-46 kJ/mol?

(for example: Define heat of formation. What does a negative heatof formation mean? what do the units of kJ/mol mean?)

11. What is the maximum amount of KCl that can dissolve in 500g ofwater?

(solubility of KCl is 34 g/ 100g of water at 20*C)

12.List the ways(operations) that can help make a substancedissolve faster in a solvent?

13. If a crystal added to an aqueous solution causes many particlesto come out of solution, the original solution was (saturate,unsaturated, supersaturated).

14. What is the number of moles of solute in 165 mL of a 0.82 Msolution?

15. What mass of NaCl is needed to make 350 mL of a 1.00 Msolution?

16. Colligative properties depend upon...

17. If one mole of each of these solutes in added to the sameamount of water, which solution has the highest boiling point?(glucose, aluminum sulfate, magnesium acetate, copper (I)chloride)

18. When an acid reacts with a base, what compounds areformed?

19. If the [H+] in a solution is 1x10^(-13) mol/L, what is the[OH-]?

20. If the [OH-] = 1x10^-6 mol/L, what is the pH of thesolution?

21. For a solution to be considered acidic what must be thehydrogen-ion concentration?

22. Which of the following represents a Bronsted-Lowry conjugateacid-base pair?

a) SO3(2-) and SO2 b) CO3(2-) and CO c) H3O and H2 d) NH4(+) and NH3

23. With solutions of "strong" acids and "strong" bases, the word"strong" refers to ...

24. What are the products of Al(OH)3 + H2CO3?

25.What is the concentration of hydrochloric acid if 5.0 mL of acidis neutralized by 30.0 mL of 2.00M sodium hydroxide.

26. At equilibrium, what is the rate of production of reactantscompared with the rate of production of products?

27. What is the equilibrium constant for the following reaction2SO3 ---> 2SO2 + O2

28. How does an increase in pressure affect the following reaction?2SO3 (g) --> 2SO2(g) +O2(g)

29.What stresses would shift the reaction to the right?

2SO3(g) ==> 2SO2(g) + O2(g)

30. The Keq of a reaction 4.9 x 10^(-7). Are products or reactantsfavored at equilibrium?

31. In which of these systems is the entropy decreasing?

a) air escaping from a tire b) snow melting c) a gas condensing d) salt dissolving inwater

32. If an atom is reduced in a redox reaction, what must occur toanother atom in the system?

33. Identify the oxidizing agent in the following reaction: 2Na + S---> Na2S

34. What are transferred in an oxidation -reductionreaction?

35. Give the oxidation number for each atom in KMnO4.

36. Which atom has a change in oxidation number of +4 in thefollowing reaction?

K2Cr2O7 + H2O + S ----> KOH + Cr2O3 +SO2

37. What is the oxidation number of sulfur in each of the following:

a. SO3 c.SO2(2-)

b. Na2SO4 d. S2O4 (2-)

38.Fe(3+) ----> Fe represents oxidation, reduction, orhydrolysis?

39. When the half reactions Br2+ 2e- -----> 2Br- and Na---->e- + Na(+) are combined the balanced redox equation is_____________________ ( WRITE the BALANCED REDOX eq)

40. To balance the oxygen and hydrogen for a redox reaction thattakes place in basic solution, it is necessary to use whichsubstance?

41. What particle completes this nuclear equation? 55/25 Mn + 2/1 H====> _____ +2 1/0 n

42. The half-life of tungsten-182 (182/74 W) is 1.1x10^(17) years.How long would it take for a 376.2 kg sample to decay until only123.0 grams remain?

43. After 3 days, the quantity of certain radioisotope is reducedfrom 13.6 grams to 1.9 grams. Calculate the half-life of theisotope.

44. What is the name of the compound having the formulaC8H18.

45. What is the name of the following compound:

CH3---CH2----CH---CH2--C

I \

CH3 OH

46. What is an isomer? Give an isomer of hexane (C6H14) and drawit's structure.

47. What is the name of the hydrocarbons with double covalentbonds?

48. Draw the stucture for 3-methylbutanoic acid.

49. Draw the structure for methylbenzene?

50. What is the name of the following compound:

CH3----C-----CH3

CH3

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CHEM 202 Chapter Notes - Chapter 15: Colligative Properties, Semipermeable Membrane, Supersaturation

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