Chemical Reactivity - + S 8(s) → 8 H 2 S (g) 3 H 2 (g) +...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
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)
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: + 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 n=1 shell, that is, the noble gas configuration of He....
View Full Document

This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

Ask a homework question - tutors are online