Ionization energy and atomic radius

Complete the concept map using the following terms electronegativity, electron configuration, periodic trends, ionic radius, atomic radius, ionization energy, and periodic table. 

Describe atomic radius, ionization energy, and electron affinity and their periodic trends explain patterns in successive ionization energies and identify which electrons are involved in ion formation (to yield a noble gas or pseudo-noble gas electron configuration) ( 8.4) (SPs 8.3-8.5) (EPs 8.33-8.46)... 

Several physical and chemical properties of the elements depend on effective nuclear charge. To understand the trends in these properties, it is helpful to visualize the electrons of an atom in shells. Recall that the value of the principal quantum number (n) increases as the distance from the nucleus increases Section 6.7]. If we take this statement literally, and picture all the electrons in a shell at the same distance from the nucleus, the result is a sphere of uniformly distributed negative charge, with its distance from the nucleus depending on the value of n. With this as a starting point, we will examine the periodic trends in atomic radius, ionization energy, and electron affinity. 

The relative size of sodium and potassium ions is an example of a periodic property one that is predictable based on an element s position within the periodic table. In this chapter, we examine several periodic properties of elements, including atomic radius, ionization energy, and electron affinity. We will see that these properties, as well as the overall arrangement of the periodic table, are explained by quantum-mechanical theory, which we examined in Chapter 7. The arrangement of elements in the periodic table— originally based on similarities in the properties of the elements— reflects how electrons fill quantum-mechanical orbitals. 

In this section we will consider how the periodic table can be used to correlate properties on an atomic scale. In particular, we will see how atomic radius, ionic radius, ionization energy, and electronegativity vary horizontally and vertically in the periodic table. 

All the elements in a main group have in common a characteristic valence electron configuration. The electron configuration controls the valence of the element (the number of bonds that it can form) and affects its chemical and physical properties. Five atomic properties are principally responsible for the characteristic properties of each element atomic radius, ionization energy, electron affinity, electronegativity, and polarizability. All five properties are related to trends in the effective nuclear charge experienced by the valence electrons and their distance from the nucleus. 

STEP 3 Unfold the sheet and draw lines along all fold lines. Label as follows Periodic Trends, Periods, and Groups in the first row, and Atomic Radius, Ionic Radius, Ionization Energy, and Electronegativity in the first column. 

Identify which trends in the diagrams below describe atomic radius, ionization energy, electron affinity, and electronegativity. 

The atomic properties that are responsible for the chemistry of an element are atomic radius, ionization energy, election affinity, and polarizability. The electronegativity of an atom is also an important consideration. Before we attempt to explain the chemistry of the elements in terms of atomic properties, it will be helpful to examine Figure 21-1, which summarizes the periodic... 

Boron forms perhaps the most extraordinary structures of all the elements. It has a high ionization energy and is a metalloid that forms covalent bonds, like its diagonal neighbor silicon. However, because it has only three electrons in its valence shell and has a small atomic radius, it tends to form compounds that have incomplete octets (Section 2.11) or are electron deficient (Section 3.8). These unusual bonding characteristics lead to the remarkable properties that have made boron an essential element of modern technology and, in particular, nan otechn ol ogy. 

Restatement How are ionization energy and atomic radius affected by the heat of reaction for... 

Here, let us examine some properties. These are electronegativity, metallic and nonmetallic properties, atomic and ionic radius, ionization energy, acidity and basicity. 

The trends for electron affinity, shown in Figure 2.19, are more irregular than the trends for ionization energy and atomic radius. Nevertheless, the following general trends can be observed ... 

Know the trends for electronegativity, ionization energy, and atomic radius across the periodic table. 

Does the information on alkali metals in Table 12.9 of the text confirm the general periodic trends in ionization energy and atomic radius Explain. 

The periodic structure of the elements is evident for many physical and chemical properties, including chemical valence, atomic radius, electronegativity, melting point, density, and hardness. Two classic prototypes for periodic behavior are the variations of the first ionization energy and the atomic radius with atomic number. These are plotted in Figs. 9.4 and 9.5. 

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