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5 Chemical Bonds
Chemical Bonding & Chemical Formulas
| Term | Definition |
|---|---|
| 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. |
Created by:
Ms O'Farrell
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