Ionization energy of an atom

The ionization energy of an atom is a measure of its tendency to lose electrons the larger the ionization energy, the more difficult it is to remove an electron. There are several different ways of comparing the tendencies of different atoms to gain electrons. The most useful of these for our purposes is the dectronegativity, which measures the ability of an atom to attract to itsdf the electron pair forming a covalent bond. 

The first ionization energy of an atom is the minimum energy required to convert one mole of the gaseous atom (in its ground - lowest energy - electronic state) into one mole of its gaseous unipositive ion ... 

Why do the values of successive ionization energies of an atom always show an increasing trend ... 

The second ionization energy of an atom is the energy required to remove the second electron from the monopositive gaseous ion the third ionization... 

The ionization energy of an atom is defined as the minimum energy necessary to detach an electron from the neutral gaseous atom (see Section 3.3). It can be obtained directly from the photoelectron spectrum of an atomic gas. Appendix F lists measured ionization energies of the elements, and Figure 5.24 shows the periodic trends in first and second ionization energies with increasing atomic number. 

Two features of electron affinity to remember are (1) The electron affinity of an element is equal to the enthalpy change that accompanies the ionization process of its anion, and (2) a large positive electron affinity means that the negative ion is very stable (that is, the atom has a great tendency to accept an electron), just as a high ionization energy of an atom means that the atom is very stable. 

The first four ionization energies of an atom X are 403, 2633, 3900 and 5080kJmor. Suggest to what periodic group X belongs and give reasons for your choice. 

The ionization energy of an atom is fhe energy required to remove an electron from an individual atom in the gas phase ... 

Why do the successive ionization energies of an atom always increase Note the successive ionization energies for silicon given in Table 7.5. Would you expect to see any large jumps between successive ionization energies of silicon as you removed all the electrons, one by one, beyond those shown in the table ... 

The larger a core ionization energy of an atom in a molecule, the larger the sum of electronegativities of the atoms or groups bonded to this atom. 

Based on our previous examination of ionization energies, it is expected that the ionization energy of an atom would increase as the nuclear charge, Z, increases. In addition, the ionization energy of an atom should decrease if the electron being removed is moved farther from the nucleus (that is, if d increases). 

The first ionization energy of an atom is a measure of the energy change associated with removing an electron from the atom to form a cation. For example, the first ionization energy of Cl(g), 1251 kj/mol, is the energy change associated with the process... 

The ease with which electrons can be removed from an atom or ion has a major impact on chemical behavior. The ionization energy of an atom or ion is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion. We first encountered ionization in our discussion of the Bohr model of the hydrogen atom. CEO (Section 6.3) If the electron in an H atom is excited from n = 1 (the ground state) to = the electron is completely removed from the atom the atom is ionized. 

Why is it possible to measure the successive ionization energies of an atom until all the electrons are removed, but it becomes increasingly difficult and often impossible to measure the electron affinity of an atom beyond the first stage ... 

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