F Consider the bonding in HF: H Obviously they will share an electron to form a covalent bond.

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Presentation transcript:

F Consider the bonding in HF: H Obviously they will share an electron to form a covalent bond

F Consider the bonding in HF: H Obviously they will share an electron to form a covalent bond

Consider the bonding in HF: H Lets redraw it showing only the bonding electrons F

Consider the bonding in HF: H Fluorine is more electronegative than hydrogen. This means the bonding pair of electrons will be more attracted to the fluorine atom giving a polar covalent bond. F -- ++

Consider the bonding in HF: H What if the hydrogen was an element that was less electronegative? F -- ++

Consider the bonding in HF: The bonding electrons would move even further towards the fluorine atom. F -- ++

Consider the bonding in HF: A point will be reached where the bonding electrons are no longer shared. Fluorine has taken both of the bonding pair electrons. Its own, and the one donated from the lesser electronegative atom. The covalent bond no longer exists. F -- ++

Consider the bonding in HF: Fluorine has gained an electron, fluorine now has a 1- charge and is an ion. The other atom has lost an electron to have a 1+ charge. F 1+1-

Consider the bonding in HF: Lets look at the full dot and cross diagram: F 1+1-

Consider the bonding in HF: Lets look at the full dot and cross diagram: F 1+1-

Consider the bonding in HF: If the 2 atoms are very different in electronegativities then the bonding electrons are so far towards the more electronegative that ionic bonding now occurs. 1+ F 1-