An Introduction to Environmental Chemistry by Julian E. Andrews, Peter Brimblecombe, Tim D. Jickells,

By Julian E. Andrews, Peter Brimblecombe, Tim D. Jickells, Peter S. Liss, Brian Reid

This introductory textual content explains the basics of the chemistry of the usual atmosphere and the consequences of mankind's actions at the earth's chemical platforms. keeps an emphasis on describing how normal geochemical tactics function over various scales in time and house, and the way the results of human perturbation could be measured. subject matters diversity from popular worldwide matters equivalent to atmospheric pollutants and its impact on international warming and ozone destruction, to microbiological tactics that reason toxins of ingesting water deltas. includes sections and data packing containers that specify the elemental chemistry underpinning the topic coated. every one bankruptcy includes a checklist of extra analyzing at the topic region. up-to-date case stories. No past chemistry wisdom required. appropriate for introductory point classes.

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These pages have the advantage of many excellent colour illustrations and photographs. The information can be used to consolidate on material covered in this book, or as way of starting to explore a subject in more depth. To help you find material on the Internet, at the end of each chapter we have included a list of keywords or phrases as input for search engines. We use keywords rather than specific site addresses as website addresses change rapidly and would soon become dated in a book. The keyword lists are not intended to be complete, but are based on the main themes discussed in each chapter.

1), which break down the ionic crystal into a solution of separate charged ions: .. Na. + :Cl .. H 2O ª Na + .. ( aq ) + :Cl . : (aq ) eqn. ) Positively charged atoms like Na+ are known as cations, while negatively charged ions like Cl- are called anions. g. g. g. aluminium, Al3+) cations. g. g. g. nitrogen, N3-) anions. 1). The silicon ion Si4+ is an interesting exception. 2) are distorted. This produces an appreciable degree of covalency in the Si–O bond. 4 Using chemical equations The chemical principles discussed in this book are often illustrated using equations.

Those further away from the nucleus are less tightly held and may be used in ‘transactions’ with other atoms. These loosely held electrons are known as valence electrons. Electrons normally occupy spaces available in the lowest energy orbitals such that energy dictates the electron distribution around the nucleus. The valence electrons reside in the highest occupied energy levels and are thus the easiest to remove. For example, the element sodium (Na) has a Z number of 11. This means that sodium has 11 electrons, 10 of which are core electrons, and one valence electron.

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