Periodic table forms

Atoms that are dose to a noble gas (Group 18) in the periodic table form ions that contain the same number of electrons as the neighboring noble-gas atom. [Pg.38]

Several metals that are farther removed from the noble gases in the periodic table form positive ions. These include the transition metals in Groups 3 to 12 and the post-transition metals in Groups 13 to 15. The cations formed by these metals typically have charges of +1, +2, or +3 and ordinarily do not have noble-gas structures. We will postpone to Chapter 4 a general discussion of the specific charges of cations formed by these metals. [Pg.38]

Polyatomic ions, as you have seen (Table 2.2), are given special names. Certain non-metals in Groups 15 to 17 of the periodic table form more than one polyatomic ion containing oxygen (oxoanions). The names of several such oxoanions are shown in Table 2.3. From the entries in the table, you should be able to deduce the following rules ... [Pg.40]

As pointed out in Chapter 2, elements close to a noble gas in the periodic table form ions that have the same number of electrons as the noble-gas atom. This means that these ions have noble-gas electron configurations. Thus the three elements preceding neon (N, O, and F) and the three elements following neon (Na, Mg, and Al) all form ions with the neon configuration, is22s22p6. The three nonmetal atoms achieve this structure by gaining electrons to form anions ... [Pg.150]

Several elements in row 3 of the periodic table form itt bonds to oxygen through side-by-side overlap of 3 cf and 2 p orbitals. An example is the sulfate anion, whose Lewis structure appears in Figure 10-48. The steric number... [Pg.722]

After a consideration of optical transitions in which MMCT plays a role, and after a characterization of the excited states involved, a short review of mixed-valence compounds and their spectroscopy is in order. For more extended reviews we refer to Refs. [60,97], At least 40 elements of the periodic table form mixed-valence species which are of importance in solid state physics and chemistry, inorganic chemistry, materials science, geology and bioinorganic chemistry. It is usually their colors which are their most striking property (see also above), but they have more intriguing properties, for example electrical and magnetic properties. [Pg.175]

The Periodic Table forms one of the most remarkable, concise, and valuable tabulations of data in science. Its power lies in the regularities that it reveals, thus, in some respects, it has the same role as the SOM. Construct a SOM in which the input consists of a few properties of some elements, such as electronegativity, atomic mass, atomic radius, and electron affinity. Does the completed map show the kind of clustering of elements that you would expect What is the effect of varying the weight given to the different molecular properties that you are using ... [Pg.93]

Elements in the first column (Group 1) of the periodic table form ions with a +1 charge. [Pg.54]

A memorization aid the ele-/ V I ments below hydrogen in the periodic table form an upside-down T on the periodic table ... [Pg.132]

More than 90% of the natural metallic elements of the periodic table form perovskites the wide range of cations, the possibility of partial substitution of A or B cation sites, and the remarkable capacity to accommodate a multitude of different kinds of defects result in a wealth of properties of these solids leading to applications ranging from superconductors (33) to oxidation catalysts (34). [Pg.272]

Metals in groups 1A and 2A on the periodic table form cations with the same positive charge as their group numbers (1A = 1+ and 2A = 2+). [Pg.225]

IV. Ions of metals in the middle of the periodic table form more covalent character bonds with anions than do ions of metals in the first two or three groups of the periodic table (e.g., CdS > CaS). [Pg.118]

Except for helium, neon, and argon, all the elements in the Periodic Table form halides, often in several oxidation states, and halides generally are among the most important and common compounds. The ionic and covalent radii of the halogens are shown in Table 13-1. [Pg.553]

How, though, do elements in the middle of the periodic table form bonds Look at methane, CH4, the main constituent of natural gas, for example. The bonding in methane is not ionic because it would be energetically difficult for carbon (Is 2p ) to either gain or lose four electrons to achieve a noble-... [Pg.10]

Hypothesizing Look at the locations of potassinm and calcium on the periodic table. Form a hypothesis as to why the melting point of calcinm is considerably higher than the melting point of potassinm. [Pg.238]

Although magnesium and the alkaline-earth metals situated below it in the periodic table form ionic chlorides, beryllium chloride (BeCl2) is a covalent compound. [Pg.112]

The transition metals in the center of the periodic table form cations with charges from 1 + to 3+, but not in any particular easy-to-remember way. Several form ions with two different charges, like iron, Fe2+ and Fe3+, copper, Cu+ and Cuz+, and mercury, Hg22+ and Hg2+. (Note that Hg22+ is a diatomic cation, two Hg+ ions bonded together acting as a single unit, Hg+—Hg+.)... [Pg.86]

The alkaline earth group as a whole stands in marked contrast to transition metals and post-transition metals. For example, most of the metals in the periodic table form insoluble precipitates with the sulfide ion (S2), with the result that sulfide ores of transition and post-transition metals are very common in Earths crust. Common examples of metal sulfides include galena (lead sulfide), cinnabar (mercury sulfide), gree-nockite (cadmium sulfide), acanthite (silver sulfide), cobaltite (cobalt arsenic sulfide), sphalerite (ZnS), stibnite (antimony sulfide), several copper sulfides, orpiment and realgar (both forms of arsenic sulfide), and pyrite (iron sulfide). None of the alkaline earths, however, are found as sulfides. [Pg.90]

Atoms of the second-period elements cannot have more than eight valence electrons around the central atom, bnt atoms of elements in and beyond the third period of the periodic table form some compounds in which more than eight electrons snrronnd the central atom. In addition to the 3s and 3p orbitals, elements in the third period also have 3d orbitals that can be nsed in bonding. These orbitals allow an atom to form an expanded octet. One componnd in which there is an expanded octet is snlfnr hexafluoride, a very stable compound. The electron configuration of snlfnr is [Ne]3x 3p". In SFg, each of snlfnr s six valence electrons forms a covalent bond with a flnorine atom, so there are twelve electrons around the central sulfur atom ... [Pg.351]

Why ruthenium and osmium These elements lie in a relatively centered position within the Periodic Table, forming stable compounds in a wide range of oxidation states. For example, Os( n2-C2Ph2)(CO)(P Pr3)2 (d ) and OsH6(P Pr2Ph)2 (d ) are known and sufficiently stable to be characterized, even by X-ray [2] and neutron diffraction [3] techniques, respectively. This allows, with only two elements, to have a first forecast about the behavior of a wide range of metallic ions, from the point of view of the Scheme 1. [Pg.191]

Elements in the same vertical column in the periodic table form a group (or family) and generally have similar properties. [Pg.56]

All metals in the periodic table form nitrates, M(N03) c. Nitrate is a common anion. Many nitrates occur in nature. These are widely used in industry, and many are common laboratory reagents. Nitrates are salts of nitric acid. Their hazardous properties vary widely. The toxicity of nitrates depends exclusively on the metal cation part of the molecule. [Pg.712]

The elements in Groups 1 and 2 on the periodic table form 1+ and 2+ cations, respectively. Group 7 atoms can gain one electron to form 1 ions. Group 6 atoms form 2 ions. [Pg.105]

When atoms form covalent bonds, they try to attain a valence-electron configuration similar to that of the following noble gas element. When the elements in the first few horizontal rows of the periodic table form covalent bonds, they attempt to achieve the configurations of the noble gases helium (two valence electrons, duet mle) and neon and argon (eight valence electrons, octet mle). [Pg.677]

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