Bonds The eternal mystery of the world is its comprehensibility - Albert Einstein.
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Transcript of Bonds The eternal mystery of the world is its comprehensibility - Albert Einstein.
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Bonds
The eternal mystery of the world is its comprehensibility
- Albert Einstein
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Chemical Bonds• Chemical compounds
are formed by the joining of two or more atoms.
• This point of union is called a bond.
• The bond means there is an attractive force between the atoms.
• Bonds are more like springs then sticks. Some atom movement is possible.
• There are 3 main types of bonds, Ionic, Metallic and Covalent.
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Ionic Bonds• Ionic bonds are formed by a transfer of electrons.
• One of the atoms gains the electron(s) that the other lost.
• Both end up with full outer energy levels and opposite charges.
• The oppositely charged ions are attracted to each other.
• Many ions bond together forming networks.
• This is shown in the diagram of NaCl to the right.
• In the diagram, Na is red and Cl is green.
• In this situation there really is no single molecule but there is a simplest formula..
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Ionic Bonds
• Ionic bonds are formed by a transfer of electrons.
• One of the atoms gains the electron(s) that the other lost.
• Both end up with full outer energy levels and opposite charges.
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Ionic compounds and conduction• Electric current is
moving charges.• Solid ionic
compounds do not conduct electricity because the charged ions are locked in place.
• When dissolved, ionic compounds disassociate or separate into their ions.
• The solution can now conduct electricity because the ions are free to move.
• A solid block of salt and a beaker of distilled water will not conduct electricity, but a beaker of salty water will!
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Metallic Bonds
• The attraction between a metal atom’s nucleus and a neighboring atoms electrons is strong and packs the atoms closely together.
• This causes the outermost energy levels of the atoms to overlap.
• These outermost electrons are free to move from atom to atom.
• This explains why metals are good conductors and why they are so flexible and malleable when compared to the non-metals.
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Covalent Bonds• A covalent bond
forms when two or more atoms share valence electrons.
• This occurs most often between elements in groups IVA, VA, VIA and VIIA.
• The sharing of electrons allows each atom in the molecule to have a stable octet in its outermost energy level.
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Methane (CH4) • The methane molecule illustrated has 4 covalent bonds.
• The bonds are between each hydrogen atom and the carbon atom.
• The sharing of electrons means sometimes they are going around the carbon and sometimes they are going around the hydrogens.
• In this way each element gets to have a full outer energy orbital.
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Polar Covalent bonds
• The shared electrons in a covalent bond may not be shared equally.
• Electrons are strongly attracted to atoms located to the upper right of the periodic table.
• In the water molecule, the oxygen atom has a much stronger attraction for the electrons then either hydrogen.
• This means that the electrons from the two hydrogens spend most of their time orbiting the oxygen atom.
• Because of this unequal sharing a molecule of water has a negative and a positive end (poles).
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Water is Special!
• Because of the polar nature of the water molecule it is attracted to itself!
• Water molecules are attracted to each other and this is the main reason that such a small molecule is a liquid at room temperature!
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Many water molecules showing hydrogen bonding
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Ice Structure - note similarities to snowflakes!
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Glacial Blue ice - ice that is formed by the recrystallization of snow that is compacted in a glacier.
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Huge tabular iceberg from Antarctica
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Blue ice berg, Antarctica
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Carbon dioxide, polar covalent but with a twist!
• In the CO2 molecule the oxygen atoms have the electrons more often than the carbon atoms.
• This makes the oxygen ends of the molecule negative and the area between the oxygen and the carbon positive.
• How does this explain the fact the CO2 is a gas at room temperature even though it is a much bigger molecule than water?
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Dry Ice
• Dry ice is the solid form of the gas carbon dioxide.
• A full block, measuring about 10 inches square, weighs 50 lbs.
• The temperature of dry ice is 110° below zero.
• When handling dry ice, wear work gloves as the extremely low temperature will cause frostbite.
• Dry ice has many uses, chief among them as a refrigerant to prevent food form perishing and to ship blood products.
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