Group numbers, periodic

Make a rough sketch of the periodic table for elements 1 through 18, including the following information group number, period number, atomic number, atomic symbol, and condensed electron configuration. 

You do not have a periodic table. You are told that the condensed electron configuration for strontium is [Kr]5s. Identify the group number, period number, and orbital block in which strontium appears on the periodic table. Show your reasoning. 

When the characteristic element is partially or wholly present in a lower oxidation state than corresponds to its Periodic Group number, oxidation numbers are used for example, [O2HP—O—P03H] , dihydrogendiphosphate(III,V)(2—). 

Periodic table. The group numbers stand above the columns. The numbers at the left of the rows are the period numbers. The black line separates the metals from the nonmetals. [Note A complete periodic table is given inside the front cover.)... 

These structures (without the circles) are referred to as Lewis structures. In writing Lewis structures, only the valence electrons written above are shown, because they are the ones that participate in covalent bonding. For the main-group elements, the only ones dealt with here, the number of valence electrons is equal to the last digit of the group number in the periodic table (Table 7.1). Notice that elements in a given main group all have the same number of valence electrons. This explains why such elements behave similarly when they react to form covalently bonded species. 

Magnesium, 543 Magnesium arsenate, 436 Main-group element An element in one of the groups numbered 1 to 2 or 13 to 18 of the periodic table, 31,153t, 165t... 

B.15 Name each of the following elements (a) Sc (b) Sr (c) S (d) Sb. List their group numbers in the periodic table. Identify each as a metal, a nonmetal, or a metalloid. 

FIGURE C.7 The typical monatomic anions formed by a selection of elements in the periodic table. Notice how the charge on each ion depends on its group number. Only the nonmetals form monatomic anions under common conditions. 

The transition metals lie in the d block, at the center of the periodic table, between the s-block metals and the elements in the p block, as Figure 20-1 shows. As we describe in Chapter 8, most transition metal atoms in the gas phase have valence electron configurations of, where x is the group number of the metal. Titanium, for... 

In books on inorganic chemistry, the marked increase in the stability of the lower oxidation state (by two units) of heavier elements descending the main groups of the periodic Table is often explained by the inert s-pair effect (see J. E. Huheey U)). For example, elements like In and Sn may use only 1 or 2 electrons for the formation of bonds instead of 3 or 4 (group number), leaving one electron pair in the outer valence shell inert . The electron pair is assumed to occupy an s-orbital. This classification does not very much contribute to the understanding of bonding first... 

The elements that form only one cation are the alkali metals (group IA), the alkaline earth metals (group IIA), zinc, cadmium, aluminum, and most often silver. The charge on the ions that these elements form in their compounds is always equal to their periodic table group number (or group number minus 10 in the newest labeling system in the periodic table). 

The charge on every monatomic anion is equal to the group number minus 8 (or 18, if the most modern periodic table group numbering system is used). 

Obviously, these definitions need clarification. Chemists commonly assume Ni =8, which allows (Nt — Xi) to be interpreted as the group number of A in the periodic system (fixed for each group) can then be interpreted as follows ... 

As a final comment on terminology, we note that elemental semiconductors are formed from a single element, e.g., Si or Ge, whereas compound semiconductors are formed from two binary), three ternary), four quaternary), or, rarely, more elements. Semiconductor alloys refer to solid solutions where either one anion or one cation can substitute for another, or possibly two or more such substitutions can occur for a binary semiconductor AB a simple alloy with C would be represented as Ai CjcB. Semiconductors are often classified by the group numbers in the periodic table. Thus, for example, I-VII semiconductors include Cul and AgBr, II-VI semiconductors include ZnS, CdTe, and HgTe, III-V semiconductors include GaAs, GaN, InP, and InSb, and IVx-VIv semiconductors include PbSe and Sn02. Fundamental physical properties are compiled in a recent handbook [22]. 

A We assume that atoms lose or gain relatively few electrons to become ions. Thus, elements that will form cations will be on the left-hand side of the periodic table, while elements that will form anions will be on the right-hand side. The number of electrons lost when a cation forms is the periodic group number the number of electrons added when an anion forms is eight minus the group number. 

Figure 3.19 illustrates the dependence of Asp on location in the periodic table for each of the first three elements of main groups 13-17. The promotion energy varies with group number in a manner similar to electronegativity (cf. Fig. 3.17). Although Asp is doubtless important, other factors (such as differences in orbital radii) appear to play a role in general spd hybridization.

Figure B.l depicts the periodic table of the elements in the current IUPAC-approved form, with US-style assignments of group numbers as used throughout this book. This standard textbook table (STT) provides an accepted common vocabulary for the row (period) and column (group) assignments of each chemical element, and is thus an asset to clear pedagogical communication.

Figure B. 1 The periodic table of the elements in IUPAC-approved standard textbook-table (STT) form, showing the US-style labeling of group number 1—18.

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