Oxygen is rarely the central atom in a structure and can never bond with more than 4 elements due to its small size and its inability to create an expanded valence shell. When oxygen has an oxidation state of -1/2, as in \(O_2^-\), the compound is called a superoxide. Examples of this type of compound include \(Na_2O_2\) and \(BaO_2\). Nonmetal oxides, which form covalent bonds, are simple molecules with low melting and boiling points.Ĭompounds with oxygen in an oxidation state of -1 are referred to as peroxides. These can dissolve in water and react to form hydroxides they are therefore called basic anhydrides or basic oxides. When oxygen reacts with metals, it forms oxides that are mostly ionic in nature. Typically, compounds with oxygen in this oxidation state are called oxides. Oxygen's primary oxidation states are -2, -1, 0, and -1/2 (in O 2 -), but -2 is the most common. Ozone at very high altitudes in the atmosphere is responsible for protecting the Earth's surface from ultraviolet radiation however, at lower altitudes it becomes a major component of smog. However, because of its unstable nature it disappears and leaves the water unprotected from bacteria. It is a very good oxidizing agent, stronger than dioxygen, and can be used as a substitute for chlorine in purifying drinking water without giving the water an odd taste. The latter allotrope, ozone, is a pale-blue poisonous gas with a strong odor. However, compounds that contain oxygen are considered to be more thermodynamically stable than O 2. The O 2 bond is very strong, and oxygen can also form strong bonds with other elements. In general, O 2 (or dioxygen) is the form referred to when talking about the elemental or molecular form because it is the most common form of the element. It is also used in water treatment, as an oxidizer in rocket fuel, for medicinal purposes, and in petroleum refining. It is used in the manufacture of iron, steel, and other chemicals. There are many commercial uses for oxygen gas, which is typically obtained through fractional distillation. It is second to nitrogen as the most abundant element in the atmosphere. ![]() It is the most abundant element by mass in both the Earth's crust and the human body. Oxygen is a gas at room temperature and 1 atm, and is colorless, odorless, and tasteless. Overall, the periodic table with charges is useful to help determine the nature of the chemical element in its ionic form, i.e., whether it loses or gains electrons to achieve the nearest inert gas configuration.\): Select properties of Group 16 elements For example, helium (with atomic number 2) has a complete first shell, while in case of neon with atomic number 10, 2 electrons fill the first shell and the remaining 8 occupy the second shell, thus making the element inert. In case of inert gases or noble gases (the helium group), the electrons fill up the shell completely and their charge is zero. So, to achieve a complete shell (nearest inert gas, neon like configuration), it donates its 1 electron, thus having a charge +1 (represented as Na 1+). ![]() Over here, the electronic configuration is 2 electrons in the S shell, 8 in the P shell, and remaining 1 in the outer D shell. Let’s take an example of sodium (Na) that has atomic number 11. Thus, according to this method, 2 electrons are allotted in the first shell, 8 electrons in the second shell, and 18 electrons in the third shell. In order to find out the charge, first examine the configuration of electrons in the orbitals or shells (S, P, D, and F shells) as per the 2n 2 rule (where ‘n’ is the number of shells). Briefly speaking, the charge of an element in its ionic form refers to the actual number of electrons that it loses or gains to achieve the nearest noble gas configuration. And a periodic table with atomic mass and charges interprets both the charges and atomic mass. Likewise, the periodic table with charges illustrates elements with the probable charges, when they are in the ionic form. You may also come across periodic table with atomic mass that gives a simplified view of the elements with their respective mass numbers (total number of protons and neutrons). This labeled periodic table of element with names and their atomic number helps in easy interpretation of the properties of elements. Thus, instead of sorting elements as per their mass number (which is so in Mendeleev periodic table), elements are arranged from left to right, according to increasing order of the atomic number. ![]() The modern periodic table of elements, or just periodic table, is a tabular representation of the identified elements (as of date 118) along with their respective symbolic name and atomic number.
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