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Chapter 8: Problem 15

The electron configurations of ions derived from representative elements follow a common pattern. What is the pattern, and how does it relate to the stability of these ions?

Short Answer

Expert verified
The common pattern in electron configurations of ions derived from representative elements is that they try to achieve a noble gas configuration, meaning having a full set (octet) of electrons in the outermost shell. This pattern directly relates to the stability of ions as having a noble gas configuration is the most stable. Ions achieving this configuration are highly stable because they have a complete set of electrons in their outer shell.

Step by step solution

01

Identify the pattern in electron configuration

Ions originating from representative elements often try to achieve a noble gas electron configuration. This pattern is typically the filling of the s and p sub-levels, making a total of 8 valence electrons, which is known as octet rule.
02

Illustrate how stability is achieved

The stability of these ions is achieved by attaining a full electron configuration similar to that of a noble gas. Atoms gain, lose or share electrons to fulfill the octet rule and thus become stable. For instance, a sodium atom loses one electron to form a positive ion with the electron configuration of Neon (a noble gas), while a chlorine atom gains one electron to form a negative ion with the electron configuration of Argon (also a noble gas). The charged ions formed are more stable than their parent atoms.
03

Summary of the correlation between the pattern and stability

The pattern, therefore, is atoms adjusting their electrons to reach a noble gas configuration, which is a complete and stable electron configuration, by filling their outermost energy level with up to eight electrons (octet). The correlation between this pattern and the stability of ions is that a noble gas configuration is the most stable, and ions mimic this configuration to increase their stability.

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Which oxide is more basic, \(\mathrm{MgO}\) or \(\mathrm{BaO}\) ? Why?

Define ionization energy. Ionization energy measurements are usually made when atoms are in the gaseous state. Why? Why is the second ionization energy always greater than the first ionization energy for any element?

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