Electron configurations oxygen

Phosphoms shows a range of oxidation states from —3 to +5 by virtue of its electronic configuration. Elemental P is oxidized easily by nonmetals such as oxygen, sulfur, and halides to form compounds such as 2 5 2 5 reduced upon reaction with metals to generate phosphides. The... 

Give the ground-state electron configuration for each of the following elements (a) Oxygen (b) Silicon (c) Sulfur... 

Figure 2.14. The molecular orbitals of gas phase carbon monoxide, (a) Energy diagram indicating how the molecular orbitals arise from the combination of atomic orbitals of carbon (C) and oxygen (O). Conventional arrows are used to indicate the spin orientations of electrons in the occupied orbitals. Asterisks denote antibonding molecular orbitals, (b) Spatial distributions of key orbitals involved in the chemisorption of carbon monoxide. Barring indicates empty orbitals.5 (c) Electronic configurations of CO and NO in vacuum as compared to the density of states of a Pt(lll) cluster.11 Reprinted from ref. 11 with permission from Elsevier Science.

A biradical is a molecule with two unpaired electrons. The unpaired electrons are usually on different atoms, as depicted in (20). In that biradical, one unpaired electron is on one carbon atom of the chain and the second is on another carbon atom several bonds away. In some cases, though, both electrons are on the same atom. One of the most important examples is the oxygen atom itself. Its electron configuration is He]2s22/ x.22py12pzl and its Lewis symbol is -O. The O atom has two unpaired electrons, and so it can be regarded as a special type of biradical. 

The oxygen atom, with valence electron configuration 2s12px12pv 12p J, has two electrons with unpaired spins (its Lewis symbol is -O-, which we abbreviate to -0-). Two radicals are also produced when the oxygen atom attacks a hydrogen molecule ... 

Iron is the second most abundant metal on earth. It is a group 8 and period 4 element with [Ar] 3cf4s as electronic configuration. Iron as a metal is rarely found because it oxidizes readily in the presence of oxygen and moisture. Hence, it forms salts in its preferred oxidation state +2 and +3. 

The shared electrons in the water molecule fill the outer energy shell of both hydrogen and oxygen. The electron configuration of the molecule, including the two shared electrons, is shown in Figure 7.1. 

Give the electron configuration of oxygen, hydrogen, nitrogen, and carbon. 

On another sheet of paper, write out the electron configurations for carbon, hydrogen, nitrogen, oxygen, bromine, chlorine, and iodine. 

On the basis of the number of holes and the electron configurations, identify the different colored balls as carbon, hydrogen, nitrogen, and oxygen. Label them in Data Table 1. (The colors of bromine, chlorine, and iodine have already been recorded for you.)... 

Hydrogen and oxygen, for example, react to form water so that both elements have a stable electron configuration (which refers... 

Since each hydrogen atom has two electrons and the oxygen atom has eight electrons, the octet rule is satisfied. In H +, the atom would have no electrons, which is not the electronic configuration of a noble gas. 

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