Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different...
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Transcript of Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different...
![Page 1: Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.](https://reader036.fdocuments.us/reader036/viewer/2022082819/56649f255503460f94c3c51a/html5/thumbnails/1.jpg)
Chemical bond
A mutual electrical attraction between the nuclei and valence
electrons of different atoms that binds the atoms together.
![Page 2: Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.](https://reader036.fdocuments.us/reader036/viewer/2022082819/56649f255503460f94c3c51a/html5/thumbnails/2.jpg)
Why Bond?
• Potential energy is lowered
• More stable
![Page 3: Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.](https://reader036.fdocuments.us/reader036/viewer/2022082819/56649f255503460f94c3c51a/html5/thumbnails/3.jpg)
Types of bonds
• Ionic
• Covalent
• metallic
![Page 4: Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.](https://reader036.fdocuments.us/reader036/viewer/2022082819/56649f255503460f94c3c51a/html5/thumbnails/4.jpg)
Ionic bonding
• Bonding that results from the electrical attraction between large numbers of cations and anions.
![Page 5: Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.](https://reader036.fdocuments.us/reader036/viewer/2022082819/56649f255503460f94c3c51a/html5/thumbnails/5.jpg)
Covalent bonding
• Results from the sharing of electrons pairs between two atoms.
![Page 6: Chemical bond A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.](https://reader036.fdocuments.us/reader036/viewer/2022082819/56649f255503460f94c3c51a/html5/thumbnails/6.jpg)
Metallic bonding
• Bonding that results from the attraction between metal atoms and the surrounding “sea of electrons”
– Delocalized electrons – electrons that freely move around; empty orbitals overlap, electrons very mobile making a “sea” of electrons
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How can you tell if a bond is ionic or covalent?
• A bond is rarely purely ionic or covalent. Usually falls somewhere between the two extremes.
• Diatomic – covalent
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electronegativity• Measure of an atom’s ability to attract
electrons.
• The degree to which bond is ionic or covalent depends on the difference in electronegativities.
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How to do
• Look up the electronegativities of the atoms involved on a chart.
• Subtract the two numbers
• Find where they fall on the ionic- covalent scale.
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Polar
• Polar – an unequal sharing of electrons that lends a molecule to be partially negative at one end and partially positive at another. Water is an example.
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Reading the chart
• Values above 1.7 are ionic, the closer you are to 3.3 the more ionic.
• Values under 1.7 are covalent.– Values under 0.3 are nonpolar -covalent– Values between 1.7 and .3 are polar -covalent