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Chapter 6 Chemical bonding
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Do now Draw a web with pure substance as the main concepts Pure substance
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3 different types of substances
Molecular substances (only non metal atoms) Ionic compounds (metal and non metal ions) Metallic compounds (only metal atoms)
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Molecular substances Composed of molecules in which elements share electrons. Elements: molecules are made of 1 type of atom. Ex. H2 ; O2 Compounds: molecules are made of 2 or more types of atoms. Ex. H2O ; NH3 ; CO2
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Molecular formula Definition: shows the numbers and kinds of atoms present in a molecule of a compound. Ex. CO ( 1 molecule exist of 1 atom of carbon and 1 atom of oxygen) CH4 (1 molecule exist of 1 atom of carbon and 4 atoms of hydrogen)
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Molecular compounds Just one type of atom? H2 Hydrogen N2 Nitrogen O2 Oxygen C Carbon S8 Sulfur
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Molecular compounds (binary compounds)
Prefixes are used to show how many atoms are present in each molecule. mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca (prefix + element root + ide)
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Naming compounds (binary compounds)
CO2 * No mono prefix is used on the first element Carbon dioxide Di means 2 oxygen atoms
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Naming compounds (binary compounds)
N2O PCl3
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Monatomic vs. Diatomic Molecules
Most molecules can be monatomic or diatomic Diatomic Molecule is a molecule consisting of two atoms There are 7 diatomic molecules (SUPER 7) – N2, O2, F2, Cl2, Br2, I2, H2 You can also remember them as: H2O2F2Br2I2N2Cl2
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Bonding in molecules Covalent compounds form by sharing electrons to attain a noble gas electron configuration. Regardless of the type of bond, the Octet Rule still must be obeyed (8 valence electrons)
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Single Covalent Bond A Single Covalent Bond consists of two atoms held together by sharing 1 pair of electrons (2 e-)
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Double Covalent Bonds Sometimes atoms attain noble gas configuration by sharing 2 or 3 pairs of electrons A Double Covalent Bond is a bond that involves 2 shared pairs of electrons (4 e-)
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Triple Covalent Bond A Triple Covalent Bond is a bond that involves 3 shared pairs of electrons (6 e-)
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