Periodic table metals, nonmetals, and metalloids

The Periodic Table Metals, Nonmetals, and Metalloids 4-2 Aqueous Solutions An Introduction... 

TEIE PERIODIC TABLE METALS, NONMETALS, AND METALLOIDS... 

The elements can be divided into categories metals, nonmetals, and metalloids. Examples of each appear in Figure U. Except for hydrogen, all the elements in the left and central regions of the periodic table are metals. Metals display several characteristic properties. For example, they are good conductors of heat and electricity and usually appear shiny. Metals are malleable, meaning that they can be hammered into thin sheets, and ductile, meaning that they can be drawn into wires. Except for mercury, which is a liquid, all metals are solids at room temperature. 

Ion formation is only one pattern of chemical behavior. Many other chemical trends can be traced ultimately to valence electron configurations, but we need the description of chemical bonding that appears in Chapters 9 and 10 to explain such periodic properties. Nevertheless, we can relate important patterns in chemical behavior to the ability of some elements to form ions. One example is the subdivision of the periodic table into metals, nonmetals, and metalloids, first introduced in Chapter 1. 

Know the properties of metals, nonmetals, and metalloids and which elements on the periodic table belong to each group. 

Another way to look at the periodic table is to divide the elements into metals, nonmetals, and metalloids. Most of the elements in the table are metals. Metals are usually shiny and can be bent, hammered, or pulled into many different shapes without breaking into pieces. Metals are also good conductors, which means that heat and electricity can pass through them easily. Metals tend to give up electrons when they react with other elements. From this information, one could guess that most metals are found on the left side of the table, where the valence electron shells are mostly empty. 

The first step in being able to use the information contained in the periodic table is to understand how it is arranged. Most periodic tables are similar to one another but to lessen confusion the periodic table shown in Figure 1 will be used. One of the first things that stands out is that the table is composed of metals, nonmetals, and metalloids. 

You can use comparing and contrasting to help you classify objects or properties, differentiate between similar concepts, and speculate about new relationships. For example, as you read Chapters 1 and 2 you might begin to make a table in which you compare and contrast metals, nonmetals, and metalloids. As you continue to learn about these substances in the chapter on the Periodic Table, you can add to your table, giving you a better understanding of the similarities and differences among elements. 

Sketch a simplified version of the periodic table and indicate the location of groups, periods, metals, nonmetals, and metalloids. 

Most properties of metals, nonmetals, and metalloids are determined by their valence electron configurations. The number of valence electrons that a metal has varies with its position in the periodic table. Valence electrons in metal atoms tend to be loosely held. Nonmetals have four or more tightly held electrons, and metalloids have three to seven valence electrons. 

Figure 9.1 A general comparison of metals and nonmetals. A, The positions of metals, nonmetals, and metalloids within the periodic table. B, The relative magnitudes of some key atomic properties vary from left to right within a period and correlate with whether an element is metallic or nonmetallic.

Ss was menrioncd in Section 2.2, the periodic table is a listing of all die known elements. There is so much more to this table, however. Most notably, the elements arc organized in the table based on their physical and chemical properties. One of the most apparent examples is how the elements are grouped as metals, nonmetals, and metalloids. 

The more an element exhibits the physical and chemical properties of metals, the greater its metallic character. As indicated in Figure 7.12, metallic character generally increases as we proceed down a group of the periodic table and decreases as we proceed right across a period. Let s now examine the close relationships that exist between electron configurations and the properties of metals, nonmetals, and metalloids. 

Draw a rough sketch of a periodic table (no details are required). Indicate regions where metals, nonmetals, and metalloids are located. 

Section 7.6 The elements can be categorized as metals, nonmetals, and metalloids. Most elements are metals titey occupy the left side and the middle of the periodic table. Nonmetals appear in the upper-right section of the table. Metalloids occupy a narrow band between the metals and nonmetals. The tendency of an element to exhibit the properties of metals, called the metallic character, increases as we proceed down a column and decreases as we proceed from left to right across a row. 

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 elements in the periodic table can be classified even more broadly as metals, nonmetals, and metalloids, as shown in Figure 3-17. Metals tend toward... 

In Section 4.2, we identified elements as metals, nonmetals, and metalloids. An element that has metallic character is an element that loses valence electrons easily. Metallic character is more prevalent in the elements (metals) on the left side of the periodic table and decreases going from left to right across a period. The elements (nonmetals) on the right side of the periodic table do not easily lose electrons, which means they are less metallic. Most of the metalloids between the metals and nonmetals tend to lose electrons, but not as easily as the metals. Thus, in Period 3, sodium, which loses electrons most easily, would be the most metallic. Going across from left to right in Period 3, metallic character decreases to argon, which has the least metallic character. 

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 main-group descriptive section of this book (Part III, Chapters 9 to 19) systematically constructs a network of interconnected ideas for understanding the periodic table. The foundation for this network is introduced in Chapter 9 that describes the first five ideas (1) the periodic law, (2) the uniqueness principle, (3) the diagonal effect, (4) the inert-pair effect, and (5) the metal, nonmetal, and metalloid regions. 

Simply stated, inorganic chemistry deals with the 117 elements in the periodic table other than carbon. The elements in the periodic table are broadly grouped into three classifications metals, nonmetals, and metalloids (or semimetals). Inorganic chemists describe the physical and chemical properties of the elements themselves, as well as all of the chemical compounds the elements can form, both in nature and in the laboratory. 

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