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Course: CHEM 1212, Fall 2011School: Kennesaw
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Word Count: 617
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Properties Relating to IM Forces 12.4-12.6, 13.1 12.4 Liquids Consider a liquid: Surface Interior A molecule on the interior can experience more intermolecular forces than a molecule on the surface Thus molecules in the interior are more stable The number of molecules on the surface is minimized Surface Tension 12.4 Surface Tension Surface tension describes a liquids tendency to minimize the...
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Properties Relating to IM
Forces
12.4-12.6, 13.1
12.4 Liquids
Consider a liquid:
Surface
Interior
A molecule on the interior can experience
more intermolecular forces than a
molecule on the surface
Thus molecules in the interior are more stable
The number of molecules on the surface is
minimized
Surface Tension
12.4 Surface Tension
Surface tension describes a liquids
tendency to minimize the surface area
Stronger intermolecular forces Larger
value for surface tension
Order the following liquids in terms of
increasing surface tension:
H2O, CH3Br, I2
Capillarity
Glass
Tube
Adhesive forces between water
molecules and Glass wall
(Hydrogen bonds)
Simplified
Water
Molecules
Cohesive forces between water
molecules (Hydrogen bonds)
Adhesive stronger than cohesive
leads to the meniscus, which
maximizes the number of stronger
adhesive forces
Cohesive forces
are identical to
surface tension
Viscosity
Viscosity: resistance to flow
Flow requires breaking intermolecular
forces (see below)
Stronger intermol forces, higher viscosity
Raising temperature reduces viscosity,
why?
Flow
12.5 Water
Intermolecular forces: All H-bonds
Very strong intermolecular force
Leads to certain properties:
Very good solvent
many things can dissolve in it, especially polar
molecules
What cannot dissolve in water?
12.5 Water
Strong H-bond forces:
Very high boiling and melting points
Very high specific heat
High heat of vaporization
These attributes make water a stabilizing force for
many temperature changes
Also high surface tension
12.5 Water
The H-bonds, and the
length of the water
molecule, lead to an
open pattern of ice
Ice is less dense than
water
Means water can pack
together more
efficiently
IM Forces Recap
Intermolecular forces determine many
properties:
Strong Intermolecular Forces are associated with:
High Boiling Point
High Surface Tension
High Melting Point
High Viscosity
High values for Hvap and Hfusion
Low Vapor Pressure
12.6 Solids
Atomic Solids: Dispersion Forces only
Only for Noble Gases
Molecular Solids: Dispersion, Dipole-Dipole,
H-bond
Covalent bonds (non-metal to non-metal)
Ionic Solids: bonds Ionic are stronger than
almost all intermolecular forces
Ionic bonds: metal to non-metal
12.6 Solids
Metallic bonds: delocalized electrons
responsible, wide range of strength
Metal to metal bonds
Covalent network solids: covalent bonds
in a giant lattice, not intermolecular forces
Covalent bonds are stronger, these have
some of the highest melting/boiling points
12.6 Solids
Classification relates to intermolecular
forces
Strong
Intermolecular
Forces
Weak
Intermolecular
Forces
Ionic Solids
Atomic solids
Molecular Solids
Metallic Bonds
Covalent Network Solids
13.1 Solutions
Solute
Solvent
13.1 Solutions
Solution
13.1 Solutions
Intermolecular forces are responsible for things
dissolving
Polar
Solvent
Example
Non-polar
Solvent
Example
Ion-dipole
forces
KCl in water
Ion-induced
dipoles
KCl in
C5H12
Hydrogen
bonding
CH3OH in
water
Dipole-induced
dipole
H2O in
C2H6
Dipole-Dipole
CH3Cl in
water
Dispersion
Forces
C4H8 in
C5H12
13.1 Solutions
Regarding polarity: Like dissolves Like
Polar compounds dissolve in polar solutions
Non-polar compounds dissolve in non-polar
solutions
Polar solutions
Non- Polar solutions
H2O
CH4
CH3CH2OH
C5H12
CH3F
Hydro-carbons (only C and
H present)
13.1 Solutions
Ion-dipole forces (KCl in H2O)
First, break the ions: KCl K+ + Cl
Second, break solvent-solvent force to make
room
Requires a lot of energy
Requires some energy
Second the ion-dipole forces stabilize the ions
in solution
Gives back a lot of energy (enough to make it
happen)
13.1 Solutions
All dissolutions work in this way:
intermolecular forces of solvent-to-solute
replace the intermolecular forces of
solute-to-solute and solvent-to solvent
H
K
Cl
H
H
O
Cl
O
K+
H
K
H
Cl-
H
H
O
H
O
13.1 Solutions
Consider O2 as a solute
What are the solute-to-solute forces?
Now consider O2 in a solution where H2O
is the solvent
What are the solvent-to-solute forces?
Which forces are stronger? Solute-to-solute
or solvent-to-solute
Recap
Properties of water
Role of IM Forces on properties
Intermolecular forces in solids
Solubility and intermolecular forces
Three IM Forces to consider
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CHEM 1212Chapter 21 Practice1. Balance the following redox reaction:Fe3+ (aq) + I (aq) I2 (s) + FeO (s) [acidic]2. Given the following values in kJ/mol, solve for G0 for the balanced redox reaction:G0(Fe3+) = -10.5; G0(FeO) = -251.4; G0(I) = -51.67;
Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
CHEM 1212Review of Chem 1211 material:1. How many moles are in 21.3 g of O2?2. Balance the chemical reaction:Al + O2 Al2O3What is the mass of O2 needed to react 72 g of Al? What is the mass of Al2O3 formed?3. How much water is added to 12 mL of 1.0
Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
Colligative Properties1. List the four colligative properties2. Solve for the freezing point of benzene if 215 g of CO2 are added to 1.55 kg of benzene. TheKf of benzene is 4.90 C/m and the freezing point of pure benzene is 5.5 Celsius.3. Determine th
Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
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Kennesaw - CHEM - 1212
CHEM 1212Rate Law PracticeFor a reaction of:2 H2 + C2H2 C2H6You have the following experimental data:Rate0.1502.4002.400[H2]0.01000.01000.0300[C2H2]0.01000.04000.04001. Determine a rate law for the above reaction including a value for k.
Kennesaw - CHEM - 1212
Reaction Mechanism Practice1. Determine if the reaction mechanism below is plausible for the overall reaction: A + 3 B CB + B D [slow]A+DEB+ECGiven the following experimental data: The elementary steps do add up to the overall reaction mechanism (D
Kennesaw - CHEM - 1212
D ue:2l4ll0Chapter1 6 P ractice. Usethe folRate(mol/L-s)rq 0.0800.720t,2.880vt t/0.080t,3.6000.160Ztt.,Seco.ri'fnrrnqfinntH2l(mol/L)0.01r0.010.01 I^I0.02v0.010.02q rate l* td e r r e l n n a r c t e l c aw[CoHr+](mol/L)0.02r,
Kennesaw - CHEM - 1212
CHEM 1212Review of Chem 1211 material:1. How many moles are in 21.3 g of O2?21.3 g * (1 mol / 32 g) = 0.666 mol of O22. Balance the chemical reaction:Al + O2 Al2O3What is the mass of O2 needed to react 72 g of Al? What is the mass of Al2O3 formed?4
Kennesaw - CHEM - 1212
Chem 1212Test 1Form APERIODIC TABLE OF THE ELEMENTS1IA2IIA3IIIB4IVB5VB6VIB7VIIB8-9VIIB10-11IB12IIB13IIIA14IVA15VA16VIA17VIIA1H18VIIIA2He1.0084.0033Li4Be5B6C7N8O9F10Ne6.9419.01210.8112.0114.
Kennesaw - CHEM - 1212
Chem 1212Test 1Form BPERIODIC TABLE OF THE ELEMENTS1IA2IIA3IIIB4IVB5VB6VIB7VIIB8-9VIIB10-11IB12IIB13IIIA14IVA15VA16VIA17VIIA1H18VIIIA2He1.0084.0033Li4Be5B6C7N8O9F10Ne6.9419.01210.8112.0114.
Kennesaw - CHEM - 1212
CHEM 1212Test 2Form CPERIODIC TABLE OF THE ELEMENTS1IA2IIA3IIIB4IVB5VB6VIB7VIIB8-9VIIB10-11IB12IIB13IIIA14IVA15VA16VIA17VIIA18VIIIA1H2He1.0084.0033Li4Be5B6C7N8O9F10Ne6.9419.01210.8112.0114.
Kennesaw - CHEM - 1212
CHEM 1212Test 2Form DPERIODIC TABLE OF THE ELEMENTS1IA2IIA3IIIB4IVB5VB6VIB7VIIB8-9VIIB10-11IB12IIB13IIIA14IVA15VA16VIA17VIIA18VIIIA1H2He1.0084.0033Li4Be5B6C7N8O9F10Ne6.9419.01210.8112.0114.
Kennesaw - CHEM - 1212
CHEM 1212 PracticeThis is only to help you prepare for the upcoming test. Of course you should bereviewing and using all available resources for your preparation.1. Determine the rate law when given the following data (at 25 Celsius):3 A(aq) + 2 B(aq)
Kennesaw - CHEM - 1212
The Test 2 ReviewChapters 16 and 17ReviewGiven a reaction:H2 + Cl2 2 HClRate0.001150.001150.018400.01840H2 (mol/L)0.1480.1480.5920.592Cl2 (mol/L)0.2150.4300.2150.215Solve for the rate law including a value for k with the appropriate un
Kennesaw - CHEM - 1212
CHEM 1212Units of Concentration / Colligative Properties1. For a solution that has 28 g of FePO4 dissolved in water, the total mass of solution is 1.350 kg.What is the molality of this solution?28 g of FePO4 * ( 1 mol / 150.82 g) = 0.1857 molm = 0.18
Kennesaw - CHEM - 1212
CHEM 1212Units of Concentration / Colligative Properties1. For a solution that has 28 g of FePO4 dissolved in water, the total mass of solution is 1.350 kg.What is the molality of this solution?2. Assume the above solution has a density of 1.10 g/mL.
Kennesaw - CHEM - 1212
Vapor Pressure Calculations1. Given that a substance has a vapor pressure of 85 torr at 15 Celsius, solve for the vaporpressure at -15 Celsius. The Hvap = 65 kJ/mol for this substance.ln (P2 / 85) = (65000 / 8.314) * (1 / 258.15 1 / 288.15)ln (P2 / 85
Kennesaw - CHEM - 1212
Vapor Pressure Calculations1. Given that a substance has a vapor pressure of 85 torr at 15 Celsius, solve for the vaporpressure at -15 Celsius. The Hvap = 65 kJ/mol for this substance.2. In the above problem, solve the temperature (in Celsius) where th
Kennesaw - CHEM - 1212
Chapter 18 PracticeHCN (Ka = 6.2 * 1010)C6H5NH2 (Kb = 4.0 * 1010)1. Solve for the pH of a 0.0160 M solution of HCN.2. Solve for the pH of a 0.0160 M solution of NaCN.3. Solve for the pH of a 0.0160 M solution of C6H5NH24. Would a salt of C6H5NH3CN b
Kennesaw - CHEM - 1212
Chapter 18 ReactionsWrite reactions for each of the following behaving as an acid or a base in water:CH3NH2C6H5COOHCa(OH)2 [need to write two reactions]NH4NO3KCH3COO
Kennesaw - CHEM - 1212
Acids and Bases18.1 18.3From Chem I Acids are anything that donates an H+ ionin waterThe H+ ion is usually stabilized by a water moleculeand is often written as H3O+ Bases are anything that donates an OHion in water Well be expanding these definit
Kennesaw - CHEM - 1212
Weak Acids/Bases18.4 18.6Last time General equations:HA(aq) + H2O(l) H3O+(aq) + A-(aq)KaFor weak basesB(aq) + H2O(l) BH+(aq) + OH-(aq)KbStrong bases are usually BOH B+ + OH-Weak acids and bases disassociate only partly,they reach equilibriumWe
Kennesaw - CHEM - 1212
Making Acids out of Nothing atAll18.7, 18.9From Chem 1 Salts are any ionic compound Cation Positive charge Metal (left side of periodic table) Or NH4+ Anion Negative charge Non-metal (right side of periodic table) Or polyatomic ions (SO42-, Cr
Kennesaw - CHEM - 1212
Name _Homework: More Acid-BaseHClO (Ka = 2.9 * 108)NH3 (Kb = 1.76 * 10-5)1. Identify the conjugate base of HClO.2. Solve for the pH of a solution that is 0.150 M of HClO.3. Solve for the pH of a solution that is 0.150 M of LiClO.4. Would a solution