Electronic configurations abbreviation

Element Atomic Number Orbital Diagram Abbreviated Orbital Diagram Electron Configuration Abbreviated Electron Configuration... 

Often, to save space, electron configurations are shortened the abbreviated electron configuration starts with the preceding noble gas. For the elements sulfur and nickel,... 

Strategy To obtain the electron configuration, use Figure 6.9. Go across each period in succession, noting the sublevels occupied, until you get to iodine. To find the abbreviated configuration, start with the preceding noble gas, krypton. 

Write electron configurations, full or abbreviated, for atoms or ions. 

Write the abbreviated ground state electron configuration for... 

Write the symbol and the abbreviated electron configuration of the element described. 

To illustrate these rules, consider the Fe2+ ion. Because the atomic number of iron is 26, this +2 ion must contain 26 — 2 = 24e. Of these electrons, the first 18 have the argon structure the remaining six are located in the 3d sublevel The abbreviated electron configuration is I... 

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 ... 

Instead of writing out the entire electron configuration of an atom, especially an atom with many electrons, we sometimes abbreviate the configuration by using the configuration of the previous noble gas and represent the rest of the electrons explicitly. For example, the full configuration of iron can be given as... 

The possible states of electrons are called orbitals. These are indicated by what is known as the principal quantum number and by a letter—s, p, or d. The orbitals are filled one by one as the number of electrons increases. Each orbital can hold a maximum of two electrons, which must have oppositely directed spins. Fig. A shows the distribution of the electrons among the orbitals for each of the elements. For example, the six electrons of carbon (B1) occupy the Is orbital, the 2s orbital, and two 2p orbitals. A filled Is orbital has the same electron configuration as the noble gas helium (He). This region of the electron shell of carbon is therefore abbreviated as He in Fig. A. Below this, the numbers of electrons in each of the other filled orbitals (2s and 2p in the case of carbon) are shown on the right margin. For example, the electron shell of chlorine (B2) consists of that of neon (Ne) and seven additional electrons in 3s and 3p orbitals. In iron (B3), a transition metal of the first series, electrons occupy the 4s orbital even though the 3d orbitals are still partly empty. Many reactions of the transition metals involve empty d orbitals—e.g., redox reactions or the formation of complexes with bases. 

The chemical properties of atoms and the types of bond they form with each other are determined by their electron shells. The electron configurations of the elements are therefore also shown in Fig. A. Fig. B explains the symbols and abbreviations used. More de-... 

An abbreviated way of presenting electron configuration is to write the principal quantum number and letter of each occupied orbital and then use a superscript to indicate the number of electrons in each orbital. The orbitals of each atom are then written in order of increasing energy levels. For the group 1 elements, this notation is... 

Write the electron configuration for uranium, U (atomic number 92), in abbreviated notation. 

Using the abbreviated notation, give the electron configuration for strontium, Sr (atomic number 38). 

Chemisorption and Physisorption. One classification of adsorption phenomena is based on the adsorption energy the energy of the adsorbate-surface interaction. In this classification there are two basic types of adsorption chemisorption (an abbreviation of chemical adsorption) and physisorption (an abbreviation of physical adsorption). In chemisorption the chemical attractive forces of adsorption are acting between surface and adsorbate (usually covalent bonds). Thus, there is a chemical combination between the substrate and the adsorbate where electrons are shared and/or transferred. New electronic configurations are formed by this sharing of electrons. In physisorption the physical forces of adsorption, van der Waals or pure electrostatic forces, operate between the surface and the adsorbate there is no electron transfer and no electron sharing. 

All beryllium nuclei contain four protons and therefore +4 electronic units, so that four electrons orbit the nucleus of the neutral atom. Its electronic configuration is is2 2s2. This can be abbreviated as an inner core of inert helium (a noble gas) plus two s-wave electrons in the second radial s state (He)2S2. This locates Be at the top of Group IIA (Mg, Ca, Sr, Ba) of the periodic table. Beryllium therefore has valence +2. 

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