intermolecular attractions. what is the difference? what is the difference between: ...
TRANSCRIPT
What is the difference?
What is the difference between:What is the difference between: Inter-molecular?Inter-molecular? Intra-molecular?Intra-molecular?
More solidMore solid Moves lessMoves less These are the forces that hold our These are the forces that hold our
world together!world together!
Intermolecular Forces
Macro-covalentMacro-covalent IonicIonic MetallicMetallic HydrogenHydrogen Dipole-DipoleDipole-Dipole DispersionDispersion
Macrocovalent
The strongest of them all.The strongest of them all. Diamond (all Carbon atoms)Diamond (all Carbon atoms) Rocks (Silicon and Oxygen)Rocks (Silicon and Oxygen) See Toy ExamplesSee Toy Examples
Covalent• Lattice points occupied by atoms• Held together by covalent bonds• Hard, high melting point• Poor conductor of heat and electricity• Examples
diamond graphite
carbonatoms
Ionic
Very strongVery strong Permanent strong charge interactionsPermanent strong charge interactions Usually crystal in formationUsually crystal in formation Very high melting pointsVery high melting points See toy example.See toy example. Example of Latticeof Lattice
Metallic Bonding
Solids at room temperatureSolids at room temperature This means STRONG Intermolecular ForcesThis means STRONG Intermolecular Forces Metal Atoms give up electronsMetal Atoms give up electrons This creates many dipoles throughout the This creates many dipoles throughout the
atoms, they SHIFT but are always thereatoms, they SHIFT but are always there ““SEA of electrons”SEA of electrons”
Hydrogen Bonding
A strong intermolecular attractionsCaused by very strong dipole-dipole
attraction between molecules with N-H, O-H, and F-H bonds.
Responsible for many of water’s special properties.
Hydrogen Bond
The hydrogen bond is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom. IT IS NOT A BOND.
A H…B A H…Aor
A & B are N, O, or F
Dipole-Dipole Attraction
Caused by attraction of end of one polar molecule to of another polar molecule.
For a molecule to have dipoles it must be polar:A. Asymmetrical in shape
and B. With polar bonds
Molecular Polarity
In order for a molecule to be polar it must have polar bonds and be asymmetrical in shape. Lone pairs always lead to asymmetry.
Linear, trigonal planar, and tetrahedral are symmetrical shapes and dipoles will cancel if all bonds are equal.
Dipole-Dipole Forces
Attractive forces between polar molecules
Orientation of Polar Molecules in a Solid
Dispersion Forces (non polar molecules)
““Moving the Fat Around”Moving the Fat Around” Caused by momentary (temporary) Caused by momentary (temporary)
dipoles (pg. 444)dipoles (pg. 444) Get stronger with increase in massGet stronger with increase in mass Only attractive force between Only attractive force between non-polar non-polar
moleculesmolecules (symmetrical or those with (symmetrical or those with only non-polar bonds) or single atoms.only non-polar bonds) or single atoms.
London Dispersion Forces
Force that exits among noble gas atoms and nonpolar molecules
Can create a temporary dipole moment
Melting Points and Boiling Points of Similar Substances with Increasing Formula Weights
Substance FW (g/mol) mp (°C) bp (°C)
F2 38 -220 -188
Cl2 71 -100.98 -34.6
Br2 160 -7.2 58.78
I2 254 113.5 184.35
Boiling point is a true measure of the strength of intermolecular attractions. Why?
Let’s look at the effect of size on nonpolar molecules.
Conclusion?
Melting Points and Boiling Points of Substances with Similar Formula Weights
Substance FW (g/mol) mp (°C) bp (°C)
F2 38 -220 -188
NO 30 -164 -152
CH3OH 32 -94 65
Ca 40 893 1484
NaF 42 993 1695
Let’s compare strength of intermolecular attractions in molecules of the same size.
F2 = nonpolar, NO = dipole-dipole, CH3OH = hydrogen bonding, Ca = metal, NaF = ionic.
What does that say about the relative strength of these attractions?
State of Matter-(at room temp)• Ionic Compounds = Always Solid
• Covalent Compounds-Solid, liquid or gas
Depends on size and polarity.
Gas small and non-polar or dipole-dipole
Liquid small & H-bonding, or larger with non-polar or d/d
Solid large and polar, or very large and non-polar.
Practice – Label each with Phase and type of IMF Answers
SiO2 Solid, macrocovalent
Fe Solid, metallicCCl4 liquid, nonpolarNO gas, dipole-dipoleSO2 gas, dipole-dipole
C2H6 gas, non polar
C10H22 liquid, non-polarHg liquid, metallic
O3 gas, polar (assymetrical design)
CO2 gas, non polar (bent)
N2 gas, non-polar
C(diamond) solid, macrocovalent
C2H5OH liquid, H-bonding
C2H21OH liquid, H-bonding + dispersion
SO3 Gas, non polar (symmetrical)
CI4 gas, non polar
VolatilityAbility to evaporateHigh when attractions are weak. Why?Compare volatility of alcohol and water.
CapillarityAbility to climb up a tube or surfaceHigh when liquid molecules are attracted to
the tube or surface.Ex. Meniscus, paper towels, blood test
Surface Tension
A “skin” develops on the surface of liquids.
Water’s is very strong. High when molecules
are attracted to each other cohesion.
Ex. Paper clip “floating” Water striders
More Surface Tension Examples
“Don’t touch the tent”Rainx
•SurfactantsSurfactants Soaps and Soaps and detergentsdetergents
Surfactants
Molecules that act to disrupt a liquid’s surface tension “wetting agent”
Structure-long non-polar hydrocarbon tail and a polar or ionic head
Surfactants as Cleaning AgentsNon-polar hydrophobic (water-hating) tails
and polar or ionic hydrophilic (water-loving) heads form micelles.
Soap dissolves grease by taking grease molecules into the non-polar interior of the micelle.
Micelles are carried away during Micelles are carried away during rinsing.rinsing.
SolubilityWhat dissolves in what?I. Ionic substances dissolve in waterII. Covalent compounds:
A. Non-polar dissolves in non-polar solvents.B. Polar solutes dissolve in polar solvents.C. Partially polar (only polar in a small part of the molecule) solutes dissolve in partially polar solvents.
Like Dissolves Like!
The solute and the solvent have to be attracted to each other in order to dissolve.
Ionic solid dissolving in water