Periodic table electron division

The Periodic Table Elements within the same column of the periodic table have similar outer electron configurations and the same number of valence electrons (electrons in tire outermost principal shell), and tirerefore similar chemical properties. The periodic table is divisible into blocks (s block, p block, d block, and/block) in which particular sublevels are filled. As you move across a period to tire right in tire periodic table, atomic size decreases, ionization energy increases, and metallic character decreases. As you move down a column in the periodic table, atomic size increases, ionization energy decreases, and metallic character increases. 

The filling of the table described above leads to a natural division of the periodic table into blocks according to the outer electron configurations of atoms (see Fig. 2). Elements of the s block all have... 

Fig. 1.13 The modern periodic table in which the elements are arranged in numerical order according to the number of protons (and electrons) they possess. The division into groups places elements with the same number of valence electrons into vertical columns within the table. Under lUPAC recommendations, the groups are labelled from 1 to 18 (Arabic numbers). The vertical groups of three r/-block elements are called triads. Rows in the periodic table are called periods. The first period contains H and He, but the row from Li to Ne is sometimes referred to as the first period. Strictly, the lanthanoids include the 14 elements Ce-Lu, and the actinoids include Th-Lr however, common usage places La with the lanthanoids, and Ac with the actinoids (see Chapter 24).

The most basic division of the elements in the periodic table is into metals and non-metals. The most important chemical property of a metal atom is the tendency to give up one or more electrons to form a positive ion metals tend to have low ionization... 

Examine Figure 4.12, which shows the division of the periodic table into metals, nonmetals, and metalloids. Use what you know about electron configurations to explain these divisions. 96. Examine Figure 4.14, which shows the elements that form predictable ions. Use what you know about electron configurations to explain these trends. 

The long form of the periodic table is divided into four blocks the s-, p-, d- and f-blocks (Chapter 3). This division reflects the filling of the outermost orbitals with electrons (Figure 2.62). 

The fourth network component, the inert-pair effect, states that the valence ns electrons of main-group metallic elements, particularly those to the right of the second- and third-row transition metals, are less reactive than expected. These relatively inert ns pairs mean that elements such as In, Tl, Sn, Pb, Sb, Bi, and Po often form compounds where the oxidation state is 2 less than the expected group valence. The two major reasons for this effect are (1) larger-than-normal effective nuclear charges in these elements and (2) lower bond energies in their compounds. The fifth network component, the metal-nonmetal line, is just the division of the periodic table into metal, nonmetal, and metalloid regions. 

The most basic division of the elements in the periodic table is into metals and non-metals. The most important chemical property of a metal atom is the tendency to give up one or more electrons to form a positive ion metals tend to have low ionization energies. The metallic elements are found on the left side of the table, as shown in Fig. 7.35. The most chemically reactive metals are found on the lower left-hand portion of the table, where the ionization energies are smallest. The most distinctive chemical property of a nonmetal atom is the ability to gain one or more electrons to form an anion when reacting with a metal. Thus nonmetals are elements... 

Metal an element that gives up electrons relatively easily and is lustrous, malleable, and a good conductor of heat and electricity. (2.7) Metalloids (semimetals) elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties. (7.13 19.1)... 

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