Electron configuration, of boron

Explain the magnitudes in terms of the electron configurations of boron and deduce the number of valence electrons of boron. 

Create a board game called Orbital Orientation. Draw and cut out a two-dimensional representation of the x, y, and z p orbital orientations superimposed over each other in the center of your board. (See Figure 7.2.) Place a spinner in the center of the orbitals. Each player takes a turn and spins the spinner. When a player lands on or near a particular orbital, that player can place an electron into that orbital. It is assumed that the Is and 2s orbitals are filled, each with two electrons. The purpose of the game is to attain the electron configurations of boron, carbon, nitrogen, oxygen, fluorine, and neon. The first player to do so wins. (Remember Pauli s exclusion principle No atomic orbital can contain more than two electrons.) Also, each p orbital must contain one electron before a second electron can be added to a p orbital. 

Write down the ground state electronic configuration of boron, and give a set of quantum numbers that uniquely defines each electron. 

Boron is the only group 3A element that can be considered nonmetaHic and thus is our final element in this chapter. The element has an extended network structure with a melting point (2300 C) that is intermediate between the melting points of carbon (3550 °C) and silicon (1410 °C). The electron configuration of boron is [He]2s 2p. ... 

Elements in Group 3A, particularly boron and aluminum, also tend to form compounds in which they are surrounded by fewer than eight electrons. Because the electron configuration of boron is l/2s p, it has a total of three valence electrons. Boron reacts with the halogens to form a class of compounds having the general formula BX3, where X is a halogen atom. Thus, in boron trifluoride there are only six electrons around the boron atom ... 

Table 12.1 Electronic Configuration of Boron, Nitrogen, Silicon, and Aluminum...

Boron is the first member of Group 13 elements. It is a non-metal and forms only covalent compounds. It exhibits an oxidation state +3 in all its compounds. The electron configuration of boron is ns np and boron is said to form three covalent bonds using sp hybrid orbitals. The compounds of boron are electron deficient and accept a pair of electrons (Lewis acids). The bonding in certain boron compounds is of considerable theoretical interest. 

Electronic configuration of boron atom (excited state)... 

With both the I5 and the 2s orbitals filled to capacity, the next electron, which is needed for the electron configuration of boron, must reside in the 2p subshell. Because all three 2p oibitals are of equal energy, or degenerate, the electron can occupy any one of them. By convention, we nsually show the first electron to occupy the p subshell in the first empty box in the oibital diagram... 

Qualitative and quantitative aspects of the Lewis theory of acids and bases, and practical applications of Lewis acids, are discussed in a series of monographs [1,4-6,30-46] and reviews [47-49], The following aspects are taken into account (a) electronic configuration of acceptors (A = M MX are generally metal and boron salts), (b) nature of anions (usually halides), (c) peculiarities of thin structure of donors (B are generally the compounds containing N, P, As, Sb O, S, Se, Te F, Cl, Br, I atoms) their electronic structure, spatial accessibility, and mutual position of donor centers. Moreover, the nature of X, order of binding of A and B in formation of adducts of type AB , nature of solvents, and evaluation of AH or AG of the processes (1.1)—(1.5) [31,48] should also be considered. 

B.]—Boron, with an electron configuration of Is2 2s2, can be represented by the orbital notation shown in answer B. 

Nonmetallic elements include hydrogen and the upper right-hand portion of the p block (see Topic B2. Fig. 7). Covalent bonding is characteristic of the elements, and of the compounds they form with other nonmetals. The bonding possibilities depend on the electron configurations of the atoms (see Topics A4 and Cl). Hydrogen (Topic F2) is unique and normally can form only one covalent bond. Boron (Topic F3) is also unusual as compounds such as BF3 have an incomplete octet. Electron... 

An additional hindrance to relating the reactivity of R M types to the electronic configuration of the metal involved is the tendency for extensive intermolecular associations of organometallic compounds. The extent to which alkyls of the boron family dimerize is a function of both the size and electric field of the metal atom. The reactivity of monomeric triethylborane versus that of dimeric triethylaluminum is therefore less readily analyzed into electronic effects. 

The element belongs to the large group of transition elements or d block. The position within the Periodic Table of the elements is below zinc and above mercury. The zinc group has a filled d ° orbital and is transitional between the d block and the p block elements of boron and others. The outer electronic configuration of the zinc group is d S and the common oxidation state is -i- II. 

Problem 2.22. The electron configuration of element 5, boron, is ls 2s 2p. To form the next element, carbon, an additional electron must be added to the 2p subshell to give the configuration ls 2s 2p. Does it go into the same or a different p orbital ... 

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