The number of protons in an atom is called the atomic number. For example, all atoms with 6 protons are of the chemical element carbon, and all atoms with 92 protons are of the element uranium. The number of neutrons in the nucleus does not have to be the same in every atom of an element. Atoms of the same element with different numbers of neutrons are called isotopes.
The number of protons in the nucleus causes its electric charge. This fixes the number of electrons in its normal (unionized) state. The electrons in their atomic orbitals determine the element's various chemical properties.
Elements are the basic building blocks for all types of substances. If a substance contains more than one type of atom, it is a compound or a mixture. The smallest particle of a compound is a molecule.
118 different chemical elements are known to modern chemistry. 92 of these elements can be found in nature, and the others can only be made in laboratories. The human body is made up of 26 elements. The last natural element discovered was uranium, in 1789. The first man-made element was technetium, in 1937.
Chemical elements are commonly arranged in the periodic table. Where the elements are in the table tells us about their properties relative to the other elements.
Chemical symbols[change | change source]
Chemical elements are given a unique chemical symbol. Chemical symbols are used all over the world. This means that, no matter which language is spoken, there is no confusion about what the symbol means. Chemical symbols of elements almost always come from their English or Latin names. For example, carbon has the chemical symbol 'C', and sodium has chemical symbol 'Na', after the Latin natrium. Tungsten is called 'W' after its German name, wolfram. 'Au' is the symbol for gold and it comes from the Latin word for gold, aurum. Another symbol which comes from Latin is 'Ag'. This is the element silver and it comes from the Latin argentum. Lead's symbol, 'Pb', comes from the Latin plumbum and the English word plumber derives from this as pipes used to be made out of lead. Some more recently discovered elements were named after famous people, like einsteinium, which was named after Albert Einstein.
Compounds[change | change source]
Elements can join (react) to form pure compounds (such as water, salts, oxides, and organic compounds). In many cases, these compounds have a fixed composition and their own structure and properties. The properties of the compound may be very different from the elements it is made from. Sodium is a metal that burns when put into water and chlorine is a poisonous gas. When they react together they make sodium chloride (salt) which is generally harmless in small quantities and edible.
Mixtures[change | change source]
Isotopes[change | change source]
Most elements in nature consist of atoms with different numbers of neutrons. An isotope is a form of an element with a certain number of neutrons. For example, carbon has two stable, naturally occurring isotopes: carbon-12 (6 neutrons) and carbon-13 (7 neutrons). Carbon-14 (8 neutrons) is a naturally occurring radioactive isotope of carbon. Of each element, except for Ununoctium, at least two isotopes are known.
Classification[change | change source]
However, a few elements have properties in between those of metals and non-metals. These elements are called semimetals (or metalloids).
Related pages[change | change source]
References[change | change source]
- Ryan, Lawrie (2001). Chemistry for You: National Curriculum Edition for GCSE (2 ed.). Nelson Thornes. ISBN 9780748762347.
- Brand, Ian; Grime, Richard (2002). Longman Chemistry 11-14. Pearson Education. ISBN 9780582447554.
- Devlin, Jacinta; Cochrane, Helen (2005). "1". Science Links 2. Coffey, Rhonda (VELS Edition ed.). Heinemann. p. 5. ISBN 1740815203.
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- "Periodic Table: Uranium". Chemical Elements.com. Retrieved 2011-03-22.
- "BBC Bitesize: Science: Chemical and material behaviour: Atoms and elements: Chemical symbols". BBC. p. 3. Retrieved 2011-03-23.
- Kidd, D. A. (2008). Collins Pocket Latin Dictionary. Collins. ISBN 9780007263745.
- Otter, Chris; Stephenson, Kay, eds. (2008). Salters Advanced Chemistry: Chemical Ideas (Third ed.). Heinemann. p. 17. ISBN 978-0-435631-49-9.