Covalent Bonds Bonding of nonmetal to nonmetal. All elements want to gain electrons, so they must...
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Transcript of Covalent Bonds Bonding of nonmetal to nonmetal. All elements want to gain electrons, so they must...
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Covalent BondsCovalent BondsBonding of nonmetal to
nonmetal.
All elements want to gain electrons, so they must
SHARE valence electrons. Study your ion chart everyday!! Quiz this
Friday!
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A.6 Chemical Bonding
It’s a lot like dogs…
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ATOMIC STRUCTURE
HELIUM ATOM NEON ATOM
Label the protons, neutrons, and electrons in their correct locations on the diagrams below.
This first shell surrounding the nucleus can hold ________ electrons and the second shell can hold ________ electrons.
Where are the valence electrons??
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ELECTRON-DOT DIAGRAMS
The valence electrons of an atom can be written in the following way, where the electrons are represented by dots around the chemical symbol of the element.
Imagine that you are writing the dots on a square around the chemical symbol.
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Atomic Structure
NAME SYMBOL ATOMIC NUMBER NUMBER OF ELECTRONS IN OUTERMOST
ENERGY LEVEL
ELECTRON DOT FORMULA
HYDROGEN
H 1 1 H•
LITHIUM
BORON
NEON
FLUORINE
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Why do atoms bond together?
• Atoms bond together to become more like Noble Gases in electron arrangement.
• Bonding produces new substances.
• Involves only the 'outer shell' or 'valence' electrons
stablestable
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Atoms can bond in several ways …
• COVALENT BONDING – sharing electrons to form molecules withcovalent bonds
– formed between two nonmetals in a molecule.
• IONIC BONDING - By one atom transferring electrons to another atom.
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Covalent and Ionic Bonding
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Covalent Bonding• Example 1: 2 hydrogen atoms (1) form the molecule of the element hydrogen H2
Two hydrogen atoms with their valence electrons.
How many electrons would make these atoms stable? Both atoms need one electron to
fill their outer valence level, so they SHARE an electron.
Now they both have 2 electrons in the outer energy level.
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Covalent Bonding• Example: 2 atoms of hydrogen (1) combine
with 1 atom of oxygen to form water H2O
HH22OO
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Molecular shapes determine the chemical and physical properties
like boiling point and viscosityVSEPR Model
– Valence Shell Electron Pair Repulsionspecific bond angles are formed between terminal and central atoms.
Lone pairs of electrons occupy a slightly larger orbital and “push” shared electron bonding orbitals together.
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Molecular Shapese-pairs
Notation Name of VSEPR shape
Examples
2 AX2 Linear HgCl2 , ZnI2 , CS2 , CO2
3 AX3 Trigonal planar
BF3 , GaI3
AX2E Non-linear (Bent)
SO2 , SnCl2
4 AX4 Tetrahedral
CCl4 , CH4 , BF4-
AX3E (Trigonal) Pyramidal
NH3 , OH3-
AX2E2 Non-Linear (Bent)
H2O , SeCl2
5 AX5 Trigonal bipyramidal
PCl5 , PF5
AX4E Distorted tetrahedral (see-sawed)
TeCl4 , SF4
AX3E2 T-Shaped
ClF3 , BrF3
AX2E3 Linear I3- , ICl2
-
6 AX6 Octahedral
SF6 , PF6-
AX5E Square Pyramidal
IF5 , BrF5
AX4E2 Square Planar
ICl4- , BrF4
-
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Bond Polarity and ElectronegativityBond Polarity and Electronegativity
Electronegativity and Bond Polarity• There is no sharp distinction between bonding types.• The positive end (or pole) in a polar bond is represented
+ and the negative pole -.
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Electronegativity: measure of the tendency for an atom to attract bonding electrons
Trends: increases left to right within period and from bottom to top within group.
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covalent bonds revisited
• in a covalent bond between atoms with same electronegativity, there is “equal” probability of finding electrons around either bonded nucleus.
• in a polar covalent bond the more electronegative atom gains partial (-) charge, and the less electronegative atom gains partial (+) charge. This partial charge separation gives rise to “dipoles”.
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“polar” vs. “non-polar” molecules
• A molecule is considered “polar” if it has a net “dipole moment”. A molecule is “non-polar” if it has no net dipole moment (or if the dipole moment is negligibly small)
• Characteristics of a polar molecule: – Polar covalent bond(s)– Molecular geometry that gives rise to a net dipole moment
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Intermolecular forces
Van der Waals Forces
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Intramolecular vs. Intermolecular Forces
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Intramolecular Forces
Intermolecular Forces
Intramolecular vs. Intermolecular Forces (IMFs)
STRONGER
WEAKER
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Dispersion forceWeakest Intermolecular Force (IMFs)
• Present in all atoms and molecules.
• The random movement of electrons will sometimes result in their unequal distribution. – One area of the atom then
becomes more negatively charged and one more positively charged.
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• Element with more electrons have stronger dispersion forces since they have more charge.– Halogen family: explains why F & Cl
are gases. Br is liquid. I & At are solid.
Dispersion forces increase as atom size increases.
Dispersion forceWeakest Intermolecular Force
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Dipole-Dipole Forces (IMFs)
Attractions between oppositely charged regions of polar
molecules
http://www.elmhurst.edu/~chm/vchembook/160Aintermolec.html
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Intermolecular Forces (IMFs)
Hydrogen Bonding
Special Type of dipole-dipole attraction between molecules containing:
• a hydrogen atom (H)• a small, highly electronegative
atom (N,O,F)• at least one lone pairOf electrons
http://library.thinkquest.org/28751/review/biochem/2.html
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Complete the Chart:Intermolecular Forces
(IMFs) Dispersion Dipole-dipole
HydrogenRelativeStrength
How it’sFormed
Molecular Examples
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Identifying Intermolecular Forces
What type of intermolecular forces must be overcome to:
a. Melt ice?b. Boil water?c. Melt NaCl?d. Sublime I2
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Intermolecular Forces
Which of the following compounds can form dipole-dipole forces?
Cl2
CONOCH4
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States of Matter &Intermolecular Forces
Focus on the following criteria:How the Strengths of forces between molecules
Affect the properties of gases, liquids and solids
(like viscosity, melting point, and boiling point)
**Emphasize dispersion, dipole-dipole, & hydrogen IMFs
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Hydrocarbons:Hydrocarbons:PetroleumPetroleum
Phase Changes, IMFs, & Phase Changes, IMFs, & NamingNaming
Chapter Chapter
21.1-21.421.1-21.4
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Provides ½ of US energy needs for transportation, heat, & electricity
Provides raw materials for manufactured products
What is Petroleum used for?
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Crude oil is a mixture of hydrocarbons
What is in petroleum?
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Who has the oil? Who uses it? Where is it found?
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How is crude oil separated?
Fractional Fractional DistillationDistillation separates distinct mixtures from crude oil.
Fractions
Lowest bp = WEAK intermolecular forces
highest bp = STRONG intermolecular forces
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Separation by Distillation
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Separation by Distillation
• Liquid mixtures can be separated by their boiling points (bp).
• Every substance has it own specific bp.
• When a substance is undergoing a phase change, its temperature stays the same.
2-propanol
H2O
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Boiling Point/
Condensation Point
Freezing point/
Melting point
Phase Change Graph
Time
•The horizontal parts of the graph represent the temperatures at which a phase change will occur.
•All substances have their own specific melting and boiling points.
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Examining Petroleum’s Molecules
Intermolecular Forces are BETWEEN molecules
Lowest bp = weak intermolecular forces = small hydrocarbons
Highest bp = strong intermolecular forces = large hydrocarbons
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Examples:
Butane
Nonene
decyne
2-methylbutane
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