Lecture Note - Chemical Reactivity

Lecture Note - Chemical Reactivity - Chemical Reactivity...

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Chemical Reactivity Hydrogen Unlike the rest of the Group 1A elements, which exist as metals, elemental hydrogen exists as gaseous H 2 molecules. Compounds formed between hydrogen and non-metals are molecular rather than ionic. ( i.e. , hydrogen forms covalent bonds with non-metals). For example, hydrogen reacts with halogens (Group VIIA) according to: H 2 (g) + X 2 → 2 HX (g) where X can be any halogen, such as F, Cl, Br, or I. Hydrogen in these compounds has an oxidation state of +1 while the halogens are -1. Similarly, hydrogen reacts to other elemental non-metals in a predictable fashion: 2 H 2 (g) + O 2(g) → 2 H 2 O (g) 8 H 2 (g) + S 8(s) → 8 H 2 S (g) 3 H 2 (g) + N 2(g) → 2 NH 3(g) Hydrogen can also form compunds with more active metals to form ionic hydrides . For example, lithium hydride is formed according to: 2 Li (s) + H 2 (g) → 2 LiH (s) The metal ( Li in this case) loses an electron to become a cation and H gains an electron to become H - (hydride anion), which has an charge of -1. Here's another example: Mg (s) + H 2 (g) → MgH 2(s) By gaining an electron, the hydride ion obtains the stable electron configuration of a closed
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This note was uploaded on 07/31/2008 for the course CHY 152 taught by Professor Foucher during the Winter '08 term at Ryerson.

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Lecture Note - Chemical Reactivity - Chemical Reactivity...

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