Download - Forming Compounds - Ms. Bunney's Classes
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Forming CompoundsUsing Bohr and Lewis Diagrams to show how electrons can be
transferred or shared to form bonds
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Compounds are of two basic types: IONIC and COVALENT
IONIC COMPOUNDS
• Contain a positive ion (usually a metal) and a negative ion (non-metal)
• In IONIC BONDING, one or more electrons TRANSFERS from each atom of the metal to each atom of the non-metal
Bohr Model:
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Covalent Compounds
• Atoms of many non-metals SHARE electrons with other non-metal atoms.
• In COVALENT BONDING, atoms overlap slightly, and one unpaired electron from each atom will pair together. Both atoms are attracted to the same pair of electrons forming a COVALENT BOND
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Representing Bonding with Lewis Dot DiagramsKey Concepts
• There are shorthand ways to represent how atoms form covalent or ionic bonds.
• Lewis dot diagrams use dots arranged around the atomic symbol to represent the electrons in the outermost energy level of an atom.
• Single bonds are represented by a pair of dots or one line between atoms.
• Double bonds are represented by two pairs of dots or two lines between atoms.
• Triple bonds are represented by three pairs of dots or three lines between atoms.
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Lewis Dot Diagrams
• A Lewis dot structure is like a simplified electron energy level model.
• The Lewis structure contains the element symbol with dots representing electrons.
• The only electrons shown are those on the outer energy level or valence electrons.
• The electrons are placed around the element symbol, one at a time, clockwise or counterclockwise, and then grouped in pairs as more electrons are added.
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Ionic Bonding of Sodium Chloride
• When sodium loses its only valence electron to become an ion, the Lewis structure shows it with no dots (electrons).
• The Na and Cl are near each other but the two dots from the Cl should not be interpreted as a covalent bond.
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Ionic Bonding in Calcium Chloride
• When calcium loses its two valence electrons to become an ion, the Lewis structure shows it with no dots (electrons).
• The Ca and Cls are near each other but the two dots from each Cl should not be interpreted as a covalent bond.
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Covalent Bonding in Hydrogen
• Lewis dot structures can also be used to show the bonded atoms in a molecule.
• The two dots together between the Hydrogens represent the electrons in the covalent bond between the hydrogen atoms.
• The line is a short-hand version of the two dots.
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Covalent Bonding in Water
• The Lewis dot structure for water shows the electron from hydrogen and an electron from oxygen being shared in a covalent bond.
• The other four valence electrons in oxygen are in pairs at the bottom.
• The lines are a short-hand version of the two dots representing the covalent bonds.
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Covalent Bonding in Oxygen
• The two pairs of dots between the Os represent the double covalent bond in the oxygen molecule.
• The two lines are a short-hand version of the two pairs of dots.
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Covalent Bonding in Carbon Dioxide
• The two pairs of dots between the C and the Os represent the double covalent bond between the carbon and each oxygen atom in the carbon dioxide molecule.
• The two sets of two lines are a short-hand version to show the two double covalent bonds.
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• http://www.bcscience10.com/pgs/quiz_section4.1.htm