# 2.2.5 Bond Polarity

* Polarity is related to the way the electrons are distributed withinonds and molecules
  * Shared pairs of electrons are not necessarily shared equally  between two atoms
* Bond polarity is resulted from the difference of Electronegativity of bonded atoms
* For $$F\_2$$--> same bond strength  ( **Pure covalent bond )** 
  * **Non-polar**
  * **No dipole moment**
* For $$HF$$ $$\because$$$$EN\_F>EN\_H$$, so flourine pulls more than Hydrogen

  * This is a **Polar Covalent bond,** with one atom adopting a partial negative charge $$\delta -$$, and hydrogen adopting a positive charge $$\delta +$$.  

Separation of charges between two non-idential bonded atoms is called the **dipole moment.**  This moment is represented through a vector along the bond.  

<figure><img src="https://1345459981-files.gitbook.io/~/files/v0/b/gitbook-x-prod.appspot.com/o/spaces%2FU8XLVR7CYYLRlgazrP2A%2Fuploads%2F26MycUmwSumPewTPWrwP%2Fimage.png?alt=media&#x26;token=8350b9dc-60f0-4be2-8c6a-ae25389666f5" alt=""><figcaption></figcaption></figure>

The vector starts as a plus sign at the less electronegative side and points to the more electronegative atom in the bond.