Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does...
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Transcript of Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does...
![Page 1: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/1.jpg)
Chapter 6
Sections 6.1 – 6.4
![Page 2: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/2.jpg)
6.1 – Chemical Bonds
Chemical Bond = A link between atoms
Why does it occur?
The nucleus of one atom is attracted to the electrons of another.
![Page 3: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/3.jpg)
Types of Bonds (an overview)(You will see all of these again later in the chapter!)
1. Ionic BondIon = Atom which has gained or lost
electron(s)Metal =
-LEFT side of Periodic Table-Weak nucleus / Low Electronegativity-LOSERS of electrons-Become + charged ions
![Page 4: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/4.jpg)
Types of Bonds (an overview)
1. Ionic Bond
Nonmetal =
-RIGHT side of Periodic Table
-Strong nucleus / High Electronegativity
-GRABBERS of electrons
-Become - charged ions
![Page 5: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/5.jpg)
Types of Bonds1. Ionic Bonds
Atoms gain or lose valence electrons to become a NOBLE GAS CONFIGURATION
Examples:
Na =
Na ION =
Cl =
Cl ION =
![Page 6: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/6.jpg)
Types of Bonds
1. Ionic Bonds
Ionic bond = A chemical bond between a cation (+) and an anion (-). Caused by a TRANSFER of electron(s).
Usually a metal + a nonmetal
![Page 7: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/7.jpg)
Types of Bonds (an overview)(You will see all of these again later in the chapter!)
2. Covalent Bond = A bond caused by a SHARING of electrons
Usually a nonmetal + a nonmetal
Nonpolar Covalent = Equal sharing of the electrons. Atoms are close in strength
Polar Covalent = Unequal sharing of the electrons. One atom is a little bit stronger than the other World of Chemistry; #8
Chemical Bonds; End at 16:25 – formation of Hydrogen molecule
![Page 8: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/8.jpg)
Types of BondsHow do you tell which type of bond it is?
-By ELECTRONEGATIVITY
A chart of electronegativity will be provided to you:
-The greater the difference in electronegativity – the more ionic the bond.
-Electrons spend more time closer to the element with higher electronegativity.
![Page 9: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/9.jpg)
Types of BondsIf the ABSOLUTE VALUE of the electronegativity
difference is:
GREATER THAN 1.7 = IONIC Bond
LESS THAN 0.3 = NONPOLAR COVALENT Bond
0.3 – 1.7 = POLAR COVALENT Bond
Examples:
![Page 10: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/10.jpg)
Types of Bonds (an overview)
3. Metallic bond
Usually metals only
-The metal gives up valence electrons.
-Electrons are free to move about.Atom
Electron Sea
![Page 11: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/11.jpg)
More Detail on the Bond Types6.2 – Covalent Bonds
Covalent Bond = A sharing of electronsMolecule = A group of atoms held by
covalent bonds (ex – water)Diatomic Molecule = Molecule with only 2
atomsMolecular Compound = Compound made of
moleculesMolecular Formula = The type and number
of atoms in a molecule (ex – H2O)
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Formation of Covalent Bonds
Sharing electrons in a covalent bond makes the atoms more stable and decreases the energy of the atoms. Energy is released when a bond is FORMED.
Overlapping of Orbitals – Example H2:
H H
+
H2
![Page 13: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/13.jpg)
The Octet Rule
Atoms in a compound obtain the electron configuration of a NOBLE GAS to gain stability
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Drawing Lewis Structures
-A picture of the covalent bonds in a molecule
-Connect valence electrons with LINES
-For Academic classes, atoms follow the octet rule unless stated
Examples:
![Page 15: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/15.jpg)
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Single Bond = 1 pair of electrons (2 e-s total) shared between two atoms
Double Bond = 2 pairs of electrons (4 total e-s) shared between two atoms
Triple Bond = 3 pairs of electrons (6 total e-s) shared between two atoms
*Single bonds are the LONGEST in length; Triple are the SHORTEST
*Single bonds have the LOWEST bond energy; Triple have the HIGHEST
![Page 18: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/18.jpg)
Ionic Bond = Bond formed by the attraction of a cation (lost electrons) to an anion (gained electrons)
Crystal Lattice = 3-Dimensional network of ions
Formula Unit = Simplest ratio of ions
More Detail on the Bond Types6.3 – Ionic Bonds
NaCl
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Dot structures for Ionic Compounds:
-Will reach noble gas configuration
-Draw an ARROW to show the transfer of e-
-Draw as many of each ion as needed
Examples:
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Comparison of Ionic and Molecular
Molecular Compounds IONIC Compounds
Bond Type Covalent Bonds Ionic
Structure Individual Molecules
Crystal Lattice
Strength of Bond
Strong Bonds Very Strong Bonds
mp/bp Low mp / bp High mp / bp
Drawing Connect Dots Arrows with Charges
Other Conduct electricity when melted or in water
![Page 21: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/21.jpg)
Drawing the Pictures – when you’re not told the TYPE of substance
• Do electronegativity difference first!!
• Examples:
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6. 4- Metallic Bonding
Metals have LOW electronegativity – Will LOSE electrons
The steps:
-Donate valence electrons to electron sea
-Electrons free to move about
-All electrons in sea are shared by all atoms
![Page 23: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/23.jpg)
6.4 – Metallic BondingProperties of Metals:1. Good conductors of heat – e- sea shakes
2. Good conductors of electricity – e- in sea can move
3. Malleable – atoms can be pushed closer
4. Ductile – atoms can be pushed closer
5. Luster – light bounces off e- sea
![Page 24: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/24.jpg)
Chapter 6
Section 6.5
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Putting Partial Charges on Molecules
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Properties of MOLECULAR Compounds
VSEPR = Valence Shell Electron Pair Repulsion Theory
Valence electrons move as far away from each other as possible
1. Draw Lewis Structure2. Look at Central Atom3. Count electron areas (bonds + lone pairs)4. Use chart info
*Academic will be given a WORD BANK and the option to use Model Kits*
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VSEPRAreas Bonds Lone
pairsShape Bond
AnglesStructure Example
2 2 0 Linear 180o http://cheminfo.chem.ou.edu/~mra/jmol/jmol.php
BeCl2;CO2
3 3 0 Trigonal Planar 120o http://cheminfo.chem.ou.edu/~mra/jmol/jmol.php
BF3
3 2 1 Bent <120o http://cheminfo.chem.ou.edu/~mra/jmol/jmol.php
SO2
4 4 0 Tetrahedral 109.5o http://cheminfo.chem.ou.edu/~mra/jmol/jmol.php
CH4
4 3 1 TrigonalPyramidal
<109.5o http://cheminfo.chem.ou.edu/~mra/jmol/jmol.php
NH3
4 2 2 Bent <109.5o http://cheminfo.chem.ou.edu/~mra/jmol/jmol.php
H2O
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VSEPR
Examples:
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VSEPR
Examples:
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VSEPR
Examples:
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Hybridization
Combination of equal energy orbitals to form new orbitals which all have the same shape and energy
Carbon:
C
BECOMES
C
1s22s22p2 four sp3 hybrid
![Page 32: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/32.jpg)
Types of Molecules
FIRST – Draw Lewis Structure & Include Partial Charges!
1. Dipole = Molecule with overall charge
2. NonPolar With Polar Sites = Molecules with area of charge which cancel out
3. Nonpolar = Molecule with no areas of charge
![Page 33: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/33.jpg)
Types of Molecules
How do you tell the difference?-Ask yourself these questions…
1. Is there charge on the molecule?
Yes2. Can it be sliced?
YES = Dipole NO = NPWPS
No = Nonpolar
![Page 34: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/34.jpg)
Examples
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Intermolecular ForcesAKA – EXTERNAL BONDS
The attraction BETWEEN Molecules
Types of External Bonds:
1. Dipole-Dipole Interactions
-Occur due to attraction between partial charges
-Occur between two dipoles (Fix notes) – the strongest external bond
Hydrogen Bond = External bond that involves a hydrogen atom
![Page 36: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/36.jpg)
Intermolecular Forces2. London Force
-Occurs between Nonpolar (or Nonpolar With Polar Sites) molecules – CHANGE THIS IN THE NOTES!!
-Very weak connection (nonpolar to nonpolar is the weakest)
The Steps: (only needed for Honors)
A. Electrons in one molecule shift instantaneously to one side
B. Instantaneous charge results
C. Electrons in another molecule are repelled
D. Very weak attraction results
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Properties Based on Number / Strength of External Bonds
1. State of Matters>l>g
2. Evaporation (*volatility)slow>fast
3. Thickness (*viscosity)thick>thin
4. Wetness (*adhesion)To feel wet the substance must bond to your skin (to the Na+Cl-)
5. DissolvingLIKE DISSOLVES LIKE
![Page 38: Chapter 6 Sections 6.1 – 6.4. 6.1 – Chemical Bonds Chemical Bond = A link between atoms Why does it occur? The nucleus of one atom is attracted to the.](https://reader036.fdocuments.net/reader036/viewer/2022062304/56649e245503460f94b128fa/html5/thumbnails/38.jpg)
Demonstrations