* +1 Oxidation State: Hydrogen typically has an oxidation number of +1 when bonded to nonmetals. This is because it tends to lose its single electron to achieve a stable noble gas configuration. Examples:
* HCl: Hydrogen is +1, chlorine is -1.
* H₂O: Hydrogen is +1, oxygen is -2.
* -1 Oxidation State: Hydrogen can also have an oxidation number of -1 when bonded to metals. In these cases, hydrogen gains an electron to achieve a stable configuration. Examples:
* NaH: Sodium is +1, hydrogen is -1.
* LiH: Lithium is +1, hydrogen is -1.
Key Points to Remember:
* Electronegativity: The oxidation state of hydrogen is determined by the relative electronegativity of the element it is bonded to. Nonmetals are more electronegative than hydrogen, so hydrogen becomes +1. Metals are less electronegative than hydrogen, so hydrogen becomes -1.
* Exceptions: There are some exceptions to these general rules, particularly in cases involving covalent bonds with elements similar in electronegativity to hydrogen.
