Covalent and Metallic Bonds
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Transcript of Covalent and Metallic Bonds
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Covalent and Metallic Bonds
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How are these two items different?
Covalent bonds Metallic bonds
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Covalent Bonds
Most things are held together with covalent bonds.
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Characteristics• Usually low melting points• Brittle in solid state
Ex: Oxygen• low boiling point
• Gas at room temperature.
Ex: Wood: Brittle
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Covalent BondAtoms share one or more electronsNonmetals need energy to transfer electrons, so 2 nonmetals
will not transfer electrons but share them to fill the valence shells.
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Covalent Bonds and Molecules Substances made form covalent bonds consist of individual particles
called molecules. A molecule consists of two or more atoms joined in a definite ratio. Most molecules are composed two or more elements- like water.
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Electron Dot One way to represent atom and molecule bonding is with an
electron-dot diagram The diagram only shows the valence electrons of an atom.
• Can help you predict how an atom may bond
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Covalent Compounds and Molecules An atom is to an element
AsA molecule is to a compound
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Simplest Molecules
The simplest molecules contain 2 bonded atoms Diatomic
The elements Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, and Bromine are always found as diatomic molecules:
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More complex Molecules
Soap, plastic,& proteins are all complex molecules. Carbon is the base for a lot of these because it has a valence shell
of 4.
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Metallic Bonds Metals can be shaped because of metallic bonds.
A metallic bond is formed by the attraction between positive charged metal ions and the electrons in the metal.
The positive ions form as the metals lose electrons.
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Movement of Electrons throughout a Metal
Bonding in metals happens because the atoms are so close the outer energy shells overlap. This allows the valence electrons to “travel”
throughout the metal
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Properties of metals
Explain what each of the following are: Conductivity
Ductility Malleability
Why can metals be bent without breaking?