Unit 11: States of Matter Ch. 13, Sections 2-4. ++ -- Types of Covalent Bonds Polar Covalent Bond...
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Transcript of Unit 11: States of Matter Ch. 13, Sections 2-4. ++ -- Types of Covalent Bonds Polar Covalent Bond...
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Types of Covalent Bonds
• Polar Covalent Bond– e- are shared unequally– asymmetrical e- density– results in partial charges (dipole)
• Nonpolar Covalent Bond– e- are shared equally– symmetrical e- density– usually identical atoms
Types of Covalent Bonds
If ΔEN is: Bond type is:
< 0.4 Nonpolar covalent
0.4 < Δ EN < 1.7 Polar covalent
> 1.7 Ionic
Given: Electronegativities of these elements
H = 2.2 C = 2.55 N = 3.04 O = 3.44 F = 3.98Na = 0.93K = 0.82 P = 2.19 S = 2.58 Cl = 3.16
Determine bond type for the following bonds:
H – H _____________________ H – O ________________________H – C _____________________ Na – Cl ________________________C – Cl _____________________ F – F ________________________K – F _____________________ H – N ________________________
Take the absolute value of the difference!
Intermolecular Forces (IMF)Intermolecular Forces (IMF)
• Attractive forces between molecules.
• Much weaker than
chemical bonds
within molecules.
• a.k.a. van der Waals forces
Types of IMFTypes of IMF
• London dispersion forces– Exist in all atoms and molecules
(temporary dipoles)– Attraction between two
instantaneous dipoles– Weakest– Larger the molecule, larger the
dispersion force.
Types of IMFTypes of IMF
• London Dispersion Forces
View animation online.
Types of IMFTypes of IMF
-Dipole-Dipole forces
-Attraction between two permanent dipoles
-Polar molecules
-Medium strength
-Stronger when molecules are closer together
Types of IMF Types of IMF
• Dipole-Dipole Forces
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View animation online.
Types of IMFTypes of IMF
• Hydrogen bonding– Special kind of dipole-
dipole– Occurs between
molecules that have an H bonded to either O, N, or F.
– Extremely polar bonds– Strongest– Not chemical bonding
Types of IMF• The hydrogen bonds in water explain its relatively high boiling
point, considering that it is a small molecule. The H-bonds hold the water molecules together as a liquid, so you have to heat it a lot before it will change to a gas. Compare boiling points of these molecules:
Molecule IMF (s) present Molar Mass (g/mol)
Boiling Point (oC)
CH4 16.05 - 164
HCl 36.46 - 85
H2O 18.02 100
London Disp.
London Disp.
Dipole-DipoleLondon Disp./Dipole-Dipole/Hydrogen Bonding
Properties of Liquids
• Density:– Higher in liquids than gases
• Intermolecular forces hold liquid particles together• Gas particles are far apart and have minimal
attraction between particles.
• Compressibility:– Only slightly in liquids
• Molecules already closely packed• Gases have a lot of empty space between particles
and can be compressed.
Liquid PropertiesLiquid Properties
• Viscosity– Resistance to flow
Viscosity Demo
Liquid PropertiesLiquid Properties
• Surface Tension– attractive force between particles in a liquid that
minimizes surface area
Action of detergents:• Detergents are used to clean dirt/oil from clothing, dishes, etc. • How does this work?
– The detergent interacts with water in such a way that the hydrogen bonding is disrupted, and this breaks the surface tension of the water, so that the dirt can mix with the water. Detergents are called surfactants, because they are surface active agents.
• Detergents have a special structure that aids the cleaning process. A micelle is formed when detergents interact with dirt/oil and water. – Water is polar. – Dirt and oils are nonpolar.– Detergents are long molecules that have polar “heads” and
nonpolar “tails”. – “like dissolves like”
• Because detergents have a dual nature, they can dissolve grease and carry it away in the water at the same time.
Cohesion and Adhesion
• Cohesion is the force of attraction between identical molecules in a liquid (cohesion is a result of intermolecular forces).
• Adhesion is the force of attraction between liquid molecules and a solid that is touching them.
Liquid PropertiesLiquid Properties• Capillary Action
– attractive force between the surface of a liquid and the surface of a solid
water mercury
Meniscus of water in a glass tube is concave: adhesion > cohesion
Meniscus of Hg in a glass tube is convex: cohesion > adhesion
PROPERTIES OF SOLIDS
• Density: In general, the particles of a solid are more closely packed than those of a liquid. So most solids are more dense than most liquids, but there are exceptions (wax, cork). When solid and liquid states of a substance coexist, the solid is more dense than the liquid, so the solid will sink in the liquid. Water is an important exception (ice floats in water). This is because the H2O molecules are less closely packed in ice than in liquid water.
Types of SolidsTypes of Solids
• Crystalline - repeating geometric pattern– covalent network– metallic– ionic– covalent molecular
• Amorphous –
– no geometric pattern
decreasingm.p.
Crystalline vs. Amorphous:
• A crystalline solid has particles which are arranged in an orderly, geometric, 3-D structure.
– Examples: sodium chloride, ice, gems and minerals
• In an amorphous solid, the particles are not arranged in any particular pattern.
– Examples: rubber, plastics.
Types of SolidsTypes of Solids
CovalentMolecular
(H2O)
CovalentNetwork
(SiO2 - quartz)
Amorphous(SiO2 - glass)
Phase ChangesT
em
pe
ratu
re E. Q=mCΔT
D. Q= mHv Tb B. Q =mHf
C. Q=mCΔTTm A. Q= mCΔT
Thermal Energy (Heat)
Thermal Energy (heat)
• Phase Changes:– B and D represent phase changes– Occur at constant temperature
• Temperature Changes– A,C, and E– Temp is changing– Sloping portion of the graph
Thermal Energy (heat )
• What is happening at each part of the graph:• A. Substance is a solid. Can heat it up or cool it
down along this line.• B. Phase change: solid-liquid. The temperature
at B (Tm) is the melting (freezing) point. • C. Substance is a liquid. Can heat it up or cool it
down along this line.• D. Phase change: liquid-gas. The temperature at
D (Tb) is the boiling (condensation) point.• E. Substance is a gas. Can heat it up or cool it
down along this line.
Heat Calculations
• Q = m c ∆ T– Q = heat or thermal energy in Joules (J) or
calories (cal)– m= mass in grams (g)– C = specific heat in J/(g oC) or cal/(g oC)– ∆T= change in temperature in oC
Heat Calculations
• Q =mHf
– Q = heat or thermal energy in Joules (J) or calories (cal)
– m= mass in grams (g)
– Hf = Heat of fusion (J/g or cal/g); use for liquid-solid phase change
Heat Calculations
• Q =mHv
– Q = heat or thermal energy in Joules (J) or calories (cal)
– m= mass in grams (g)– Hv = Heat of vaporization (J/g or cal/g); use for
gas-liquid phase change
Things to remember
• You can move from left to right or right to left along the curve.
• If you move left to right:– all the processes are endothermic (heat must
be supplied). – Your answer for heat calculations will be
positive.