What you’ve learned so far…..  Atoms form bonds in more than one way  In IONIC bonding, atoms give up or gain electrons  In COVALENT bonding, atoms.

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Presentation transcript:

What you’ve learned so far….

 Atoms form bonds in more than one way  In IONIC bonding, atoms give up or gain electrons  In COVALENT bonding, atoms share electrons

 Valence electrons and bonding can be shown by using ELECTRON DOT DIAGRAMS (aka Lewis Structures)  Ionic bonds form due to the attraction of positive & negative ions  Ionic bonds are NEUTRAL because the opposite charges cancel each other out  Covalent bonds are held together by the attraction of each atom’s nucleus for the shared pair of electrons

 Ionic bonds occur between metals & non- metals; covalent bonds between non-metals & non-metals  Covalent bonds form MOLECULAR COMPOUNDS  Molecular compounds consist of electrically neutral molecules, NOT IONS, so they do not have charged particles to conduct electricity

 Ionic Bonding

 Covalent Bonds / Molecular Compounds Example of a single covalent bond CH 4

Double Bond Example Using O 2

 Polar molecules are covalent bonds in which electrons are shared unequally  Some atoms pull more strongly on the shared electrons than other atoms do.  This results in the electrons moving closer to one atom, causing the atoms to have slight electrical charges.

Water molecules are good examples of polar covalent bonds

Shared equally = non-polar bond Carbon Dioxide

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