Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are...
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Transcript of Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are...
![Page 1: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/1.jpg)
Unit 6 Notes – Part II
Mr Nelson 2010
![Page 2: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/2.jpg)
Bonding & Lone Pairs
• Electron pairs that are shared are called bonding pairs
• Electron pairs that are not bonded or shared are called lone or unshared pairs
![Page 3: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/3.jpg)
Steric Number• The total electron
pairs as the steric number.
• Double or Triple bonds count as 1 steric number.
• The central atom in this molecule, A, has a steric number of four.
![Page 4: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/4.jpg)
Determining the shape of molecules
• Electrons, whether they be bonding or lone pairs, repel each other.
• By assuming the electron pairs are placed as far as possible from each other, we can predict the shape of the molecule.
![Page 5: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/5.jpg)
VSEPR
• VSEPR: Valence Shell Electron Pair Repulsion
– Electron pairs will arrange so they are as far apart as possible. ALL HAVE NEGATIVE CHARGES
– ALL e- pairs determine the shape, bonded or not, but ONLY bonded pairs determine the name of the shape.
![Page 6: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/6.jpg)
Molecular Shapes
• The shape of a molecule plays an important role in its reactivity.
• By noting the number of bonding and lone pairs we can easily predict the shape of the molecule.
![Page 7: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/7.jpg)
Different Bond Types
• Ionic (extremely polar)– Electrons are transferred
• Covalent– Polar – uneven sharing of electrons– Nonpolar – even sharing of electrons
![Page 8: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/8.jpg)
Nonpolar Covalent Bonds
![Page 9: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/9.jpg)
Polar Covalent Bonds
![Page 10: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/10.jpg)
Ionic Bonds
![Page 11: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/11.jpg)
Nonpolar, polar, and ionic bonds
• (a) – a nonpolar covalent bond
• (b) – a polar covalent bond
• (c) – an ionic bond
![Page 12: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/12.jpg)
Electronegativity• Electronegativity is the ability of atoms in a molecule
to attract electrons to themselves.
• On the PT, EN increases:– …from left to right across a row.
• EN decreases– …from the top to bottom of a group (column).
![Page 13: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/13.jpg)
Bond Properties and Electronegativity
![Page 14: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/14.jpg)
Bond properties and electronegativity
• Any bond can be classified by subtracting the EN of the 2 elements involved
![Page 15: Unit 6 Notes – Part II Mr Nelson 2010. Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.](https://reader036.fdocuments.us/reader036/viewer/2022062421/56649e245503460f94b128e5/html5/thumbnails/15.jpg)
Polar Covalent Bonds
• Electrons are not always shared equally in compounds.
• Oxygen pulls harder on the electrons it shares with hydrogen than hydrogen does.
• Oxygen’s end of the molecule has more electron density than the hydrogen end.