Metals ionic compounds with

It has been known for more than a century, however, that transition metals also form a variety of ionic compounds with more complex formulas such as... 

The nature of a binary hydride is related to the characteristics of the element bonded to hydrogen (Fig. 14.8). Strongly electropositive metallic elements form ionic compounds with hydrogen in which the latter is present as a hydride ion, H. These ionic compounds are called saline hydrides (or saltlike hydrides). They are formed by all members of the s block, with the exception of beryllium, and are made by heating the metal in hydrogen ... 

The elements show increasing metallic character down the group (Table 14.6). Carbon has definite nonmetallic properties it forms covalent compounds with nonmetals and ionic compounds with metals. The oxides of carbon and silicon are acidic. Germanium is a typical metalloid in that it exhibits metallic or nonmetallic properties according to the other element present in the compound. Tin and, even more so, lead have definite metallic properties. However, even though tin is classified as a metal, it is not far from the metalloids in the periodic table, and it does have some amphoteric properties. For example, tin reacts with both hot concentrated hydrochloric acid and hot alkali ... 

Other metallic elements form ionic compounds with cation charges ranging from -F1 to + 3. Aluminum nitrate nonahydrate, A1 (N03)3 9 H2 O, is composed of cations, NO3 anions, and water molecules. Silver nitrate (AgNO ), which contains Ag cations, is a soluble silver salt that is used in silver plating. 

Q. Why do metals tend to form ionic compounds with nonmetals ... 

The elements show increasing metallic character down the group (Table 14.12). Carbon has definite nonmetallic properties it forms covalent compounds with nonmetals and ionic compounds with metals. The oxides of carbon and silicon are acidic. Germanium is a typical metalloid... 

In earlier chapters, we saw examples of how the metallic or nonmetallic character of an element affects its chemistry. Metals tend to form ionic compounds with nonmetals, whereas nonmetals tend to form covalent, molecular compounds with one another. Thus, binary metallic hydrides, such as NaH and CaH2, are ionic solids with high melting points, and binary nonmetallic hydrides, such as CH4, NH3, H20, and HF, are covalent, molecular compounds that exist at room temperature as gases or volatile liquids (Section 14.5). 

Because reactive metals, such as sodium, hold on to the element(s) they have combined with, they are usually difficult to extract. For example, sodium chloride (as rock salt) is an ionic compound with the Na+ and Cl ions strongly bonded to one another. The separation of these ions and the subsequent isolation of the sodium metal is therefore difficult. 

Metals form alloys with each other. They form ionic compounds with nonmetals. Nonmetals form only covalently bonded compounds with each other. As a result, metals become only positively (+) charged ions, whereas nonmetals become either negatively (-) or positively (+) charged ions. 

Table 12.1 shows some organometallic lithium compounds. It is seen from their formulas that these compounds are ionic. As discussed in Section 12.2, 1A metals have low electronegativities and form ionic compounds with hydrocarbon anions. Of these elements, lithium tends to form metal-carbon bonds with the most covalent character therefore, lithium compounds are more stable (though generally quite reactive) than other organometallic compounds of group 1A metals, most... 

A majority of halides and oxides have the structures expected for largely ionic compounds, with the metal in octahedral... 

Electrovalent bonds are formed between oppositely charged ions, and typically a metal donates electrons to a nonmetal. For example, sodium chloride (common salt, an important constituent of the body s fluids) is written as Na Cl. For sodium chloride only one electron is involved in the transfer and the molecular formula is written as NaCl. However, if sodium forms an ionic compound with oxygen, an oxygen atom needs two electrons to form an ion, so it will need to have two sodium atoms donating electrons ... 

From the discussion of Chapter I, it follows that metallic conduction is to be associated with partially filled bands of collective-electron states. Since the s-p bands of an ionic compound are either full or empty, metallic conduction implies partially filled d bands, and collective d electrons imply Rtt < Rc(n,d). From the requirement Rtt < Rc(n4) it is apparent that the metallic conduction in ionic compounds must be restricted either to transition element compounds in which the anions are relatively small or to compounds with a cation/anion ratio > 1. Also Rc(n,d) decreases, for a given n, with increasing atomic number, that is with increasing nuclear charge, and the presence of eQ electrons increases the effective size of an octahedral cation (627) (see Fig. 66) and similarly UQ electrons the size of a tetrahedral cation. It follows that If the cation/anion ratio < 1, MO d electrons are more probable in ionic compounds with octahedral-site cations if the cations contain three or less d electrons MO d electrons are more probable in ionic compounds with tetrahedral-site cations if the cations contain two or less d electrons. 

Metal oxides, the products of oxidation of metals are ionic compounds with the metal ions and oxide ions arranged in arrays in the crystal lattices. When the metal oxide contains excess metal ions in interstitial positions, they are known as n-type (or negative carrier type) oxides. When the metal oxides contain vacant sites (deficient in metal ions) in the lattice the oxides are known as p-type (positive carrier type). 

Type II binary ionic compounds with the metal possessing more than one type of cation... 

The sharp distinction between ionic and covalent solids is maintained in a rearrangement of the periodic table of elements made by Pantelides and Harrison (1975). In this table, the alkali metals and some of their neighbors are transferred to the right (see Fig. 2-7). The elements of the carbon column (column 4) and compounds made from elements to either side of that column (such as GaAs or CdS) are covalent solids with tetrahedral structures. Compounds made from elements to either side of the helium column of rare gases (such as KCl or CaO) are ionic compounds with characteristic ionic structures. A few ionic and covalent compounds do not fit this correlation notably, MgO, AgF, AgCl, and AgBr are... 

An operational description is that one reactant (the more ionic compound with the more electropositive metal) transfers alkyl anions to the other. Thus the four methyl groups in Li2BeMe4 form a distorted tetrahedron around the beryllium, with longer distances to the lithium ions. However, this description is oversimplified. The low-temperature nuclear magnetic resonance (NMR) spectrum of Li3MgMe5 has three different methyl resonances, suggesting structure (14), related to the MeLi tetramer. Ate complexes with zinc and aluminum compounds also form. Electron-deficient bridge-bonded structures, exemplified by the X-ray structure of... 

The bonding for oxygen atoms in heteratomic molecules is viewed as essentially covalent (see Covalent Bonds) (e.g. MeOH, Mc2C=0, MeCHO, and MeC(O)OOH) and similar to that for carbon, nitrogen, and chlorine atoms. In contrast, a Lewis acid base formahsm often is used for metal oxygen compounds with ionic interactions by dianionic 0x0 groups (e.g. [Ba2+ q2-], [Fe + (0 -) ] -, [Mn + (Q2-)4]-, and [(Cu+)20 ]). This results from the thermodynamic relations for ionic solution equihbria, and the inference that the combination of ions results in molecules and complexes held together by electrostatic interactions (equations 33 35). 

In the ionic compounds considered previously (Type I), the metal involved forms only a single type of cation. That is, sodium forms only Na+, calcium forms only Ca2+, and so on. However, as we will see in more detail later in the text, many metals can form more than one type of positive ion and thus form more than one type of ionic compound with a given anion. For... 

The formate ion, CH02, forms ionic compounds with many metal ions. Assume that 9.7416 g M(CH02)2 (where M represents the atomic symbol for a particular metal) is dissolved in water. When a solution of 0.200 M sodium sulfate is added, a white precipitate forms. The sodium sulfate solution is added until no more precipitate forms then a few milliliters are added in excess. The precipitate is filtered, dried, and weighed. It has a mass of 9.9392 g. The filtrate is saved for further use. 

O2" Peroxide 149 Forms ionic compounds with alkali metals, Ca, Sr, Ba strong oxidizing agent... 

There are general reactivity trends on the periodic table that are useful to know. Metals and nonmetals usually combine to form ionic compounds with the metal giving up an electron to become positively charged and the nonmetal element gaining an electron to become... 

B is correct. You should recognize this compound as ionic because alkaline earth metals like to form ionic compounds with halogens. 

Carbon forms covalent compounds with nonmetals and ionic compounds with metals. 

Halides of metals tend to be ionic unless the metal has an oxidation number greater than +2. For example, sodium chloride and copper(ll) chloride are ionic compounds with high melting points, whereas titanium(lV) chloride and iron(lll) chloride sublime as molecules. 

Form ionic compounds with metals and molecular (covalent) compounds with other nonmetals... 

Most metals react with most nonmetals to form binary ionic compounds. The Group lA metals combine with the Group VIIA nonmetals to form binary ionic compounds with the general formula MX (Section 7-2) ... 

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