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Bonding
vocab 3
Term | Definition |
---|---|
Alloy | A mixture of two or more elements, at least one of which is a metal |
Lewis Electron Dot Structure | Diagrams that show valence electrons in the atoms of an element as dots |
Ionic Bond | A compound with a metal and non-metal . Results from valence electrons are transferred. |
Metallic Bonds | Bonding between atoms of the same metal (pure metals only) and different metals can never bond together. Results from mobile valence electrons in pure metal samples only |
Octet Rule | Neutral atoms will gain, lose, or share valence electrons to get to 8 valence electrons and become stable like the Noble Gases. |
Valence Electrons | The electrons in the outermost energy level. The last number in the electron configuration on the Periodic Table. |
Covalent Bond | Atoms of two non-metals combine together. The valence electrons are shared between the two non-metals |
Diatomic Molecule | A molecule that contains two atoms. |
Non-Polar Covalent Bonds | Bonds formed when atoms in a bond pull equally on each other. Equal distribution of electrons between two atoms, no difference in electronegativity. |
Polar Covalent Bonds | Covalent bonds where atoms in the bond are shared unequally. Unequal distribution of electrons between two atoms, IS different in electronegativity |
Non-Polar Covalent Molecule | Symmetrical in shape, all polar covalent bonds cancel out |
Polar Covalent Molecule | Non symmetrical in shape, polar covalent bonds DO NOT all cancel out |
Subscript | Balances out the charges in a compound. The small numbers to the bottom right of elements |