Periodic table of elements
Summary
An element is a fundamental classification of atomic matter where differentiation of particles is based on the number of protons found in their nucleus. So far 118 elements are known to exist either by producing them artificially or finding them naturally in the environment. In the Periodic Table of the Elements elements are sorted in ascending order of proton number (Atomic number). The state of matter they exist in at Standard Temperature and Pressure (STP) is usually also provided.
A link to the table is given here
Elements by periodical table Group (vertical columns)
Elements in one group behave in a similar way and show the same overall general properties. The number of electrons in the outer shells of the electron orbitals is the same in every group, only the quantum number describing the orbitals increase. For instance the right column is that of the noble gasses. Because they have an outer shell of electrons that is completely filled they behave inert. See for an explanation Atoms and Molecules. On the utmost left there is a group of metals, called the alkali metals. They all are characterized by having one single electron in their outer valance orbital. Going down from Li, Na, K to Fr the reactivity lowers but these metals easily react with for instance water in a very exothermic way. The reason for this lowered reactivity is based upon the atomic weight. As the mass of the nucleus increases with each neutron and proton so increases the number of electrons (to balance the electric charge). Because these electrons are all at a larger distance from the nucleus the energy gained from removing one electron reduces according to the proportionality of r-2. The one free electron in the outer valence shell is in a so-called s-orbit. In all these metals there is only one free electron and these ball-shaped orbits are denoted by 1s1, 2s1, 3s1 etc all with an increasing average radius from the nucleus. For all the subsequent groups characterizations can be formulated based upon similarities in reactivity, the way they do react, how many electrons can be shared, etc. As a result, the likelihood of reactants to be able to react together can be determined from the Periodic Table of Elements. The way the element at the top of a column reacts, and the way it produces new chemicals gives a clue in how other elements in that same row will react. For instance carbon and hydrogen|(H2) react to methane. The bonds of the carbon|(C) take a tetraeder or pyramid shape. Silicium or Si responds in the same way and the carbon-chemistry is to most extent the same as silicium-chemistry.
Elements by periodical table Row
Elements in a row show different periodicities, such as electronegativities, increasing atomic mass, increasing number or protons and neutrons. The stability of these elements diminish however with an increasing number or nucleotides (protons and neutrons). These instabilities lead to radio-active decay as is evident from the Actinides and Lanthanides, the groups of the rare earths. They contain elements such as Plutonium, Radon and Urane, and notorious since the poison schandal in the UK Polonium.
The ratio of protons to neutrons is important in determining the stability of elements. If the ratio is over 1 the chance of a radioactive unstable element, or isotope of an element, becomes larger. The larger the ratio the larger that chance the element will be radioactive.
Other properties vary differently from the colum wise view of the periodic table of elements. Going down the reactivity decreases. Going in a row from left to right the reactivity increases, and properties such as electronegativity increases as well. For the latter reason the tendency to lose an electron to form a covalent bond decreases and turns into the tendency of needing one or more electrons to form a stable covalent bond, producing a more stable chemical substance or molecule. The alkalimetals are the most eager to loose an electron (they have the lowest electronegativity in the row) making them very reactive with water. The halogenides are for the opposite reason reactive, they need to attract that electron to obtain a more stable electron-configuration. HydrogenFluoride is among the strongest acids known to mankind, where Sodium Hydroxide is one of the strongest bases - as an example. Electronegativity also is the source for the occurrence of electric polarity in substances. In every molecule of water (H2O, the hydrogen is less inclined to keep its electron tightly bound, oxygen on the other hand, being more electronegative likes to share electrons to create a more stable electron configuration. This results in the protons being slightly more positively charged ∆+, where as oxygen is slightly more negatively charged 2∆-. This results in water being a highly polar fluid with the capability to facilitate hydrogen bonding in solutions and it somewhat non standard behaviour.
Elements classified alphabetically
- See Elements
Note
This article is not intended to delve into the past but is to provide a reasonable stepping stone into developing further articles for the individual elements. The history and development of the periodic table of elements may be included in version 1.1