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5 Chemical Bonds

Chemical Bonding & Chemical Formulas

TermDefinition
Octet rule In bonding atoms tend to reach an electron arrangement with eight electrons in their outermost energy level.
Ion Charged atom or group of atoms
Ionic Bond Force of electrostatic attraction between oppositely charged ions in a compound. Formed by complete transfer of electrons from one atom to another.
Crystal Lattice Three dimensional arrangement of ions
Transition Metal One that forms at least one ion with a partially filled d sublevel
Characteristics of transition metals Exhibit Variable valency, usually form coloured compounds, are widely used as catalysts
Compound is a substance made up of two or more different elements chemically combined
Molecule group of atoms joined together, smallest part of an element or compound that can exist independently.
Lone pair a pair (2) of electrons that are not involved in bonding
Bond Pair A pair of electrons involved in bonding (Covalent Bonds)
Covalent Bond Sharing a pair of electrons
Sigma Bond Head-on overlap of two orbitals to form a bond ( single Bond)
pi Bond sideways overlap of p orbitals (Double/Triple bonds)
Characteristics of Ionic Compounds Network of ions, Hard, High melting & boiling points, Usually solid & conduct electricity when molten or dissolved in water.
Characteristics of Covalent Compounds Individual Molecules, Soft, Low melting & Boiling points, usually liquids, gases or soft solids, do not conduct electricity.
Valence Shell Electron Pair Repulsion Theory (VSEPR Theory) Lone Pair|| Lone Pair greater than Lone pair ||Bond Pair greater than Bond Pair|| Bond Pair (|| = repulsion)
Linear two bond pairs about the central atom, 180 degrees
Trigonal Planar/ Triangular planar three bond pairs about the central atom, 120 degrees
Tetrahedral Four Bond pairs about the central atom, 109.5 degrees.
Pyramidal Three Bond Pair and one Lone pair about the central atom, 107 degrees
V-Shaped Two Bond Pairs and two Lone Pairs about the central atom, 104.5 degrees
Electronegativity the measure of the relative attraction and atom has for the shared pair of electrons in a single covalent bond
Polar Means that bonding electrons are not shared equally, and that there is a partial positive charge & a partial negative charge separated by some distance.
Polar Covalent bond is a bond where there is unequal sharing of electrons, causing one end to be delta + and the other delta -.
Pure Covalent There is equal sharing of electrons within the bond. EN diff = 0 to 0.4
Intramolecular Bonding Bonding within a molecule holding atoms together i.e. Ionic or Covalent
Intermolecular Bonding Forces of attraction between molecules i.e. Van der Waals Forces, Dipole-Dipole Forces and Hydrogen bonding.
Van der Waals Forces Small attractive forces due to the temporary internal shifts in the distribution of electrons within a molecule. Exist in non-polar molecules. Weakest Intermolecular force
Dipole-Dipole Forces Forces of attration between the negative pole of one polar molecule & the positive pole of another polar molecule. Stronger than Van der Waals Forces but weaker than Hydrogen Bonds.
Hydrogen Bonds Hydrogen is bonded to Nitrogen, Oxygen or Flourine. The Hydrogen carries a partial positive charge and is attracted to the electronegative atom in another molecule, creating a bridge between the atoms . A special Dipole-Dipole Force.
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