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Chapter 10: Problem 11

One of the blocks described in Model 3 is often referred to as the "s-block" and one of the blocks is often referred to as the " \(p\) -block". Identify each of these "blocks" and explain the significance of their names in terms of electron configurations.

Short Answer

Expert verified
The 's-block' includes Group 1 and 2 in the periodic table as the s orbital can hold a maximum of two electrons. The 'p-block' includes Groups 13 to 18, as the p orbital can hold a maximum of six electrons. Their names s-block and p-block represent the type of atomic orbital in which their outermost electrons reside, which determines their atomic structure and chemical properties.

Step by step solution

01

Identifying Blocks

The 's-block' includes Group 1 (alkali metals) and Group 2 (alkaline earth metals) in the periodic table, and hydrogen and helium. The 'p-block' includes Groups 13 to 18, known as the main group elements.
02

Understanding Electron Configuration

Atoms in the 's-block' elements have their outermost, or valence, electrons in the s orbital. The s orbital can hold a maximum of two electrons. This is why there are two groups in the 's-block'. Atoms in the 'p-block' elements have their outermost electrons in the p orbital. The p orbital can hold a maximum of six electrons. This is why there are six groups in the 'p-block'.
03

Explaining the Significance

The names 's-block' and 'p-block' come from the type of orbital in which the outermost electrons reside. The 's' in 's-block' and 'p' in 'p-block' represent the type of atomic orbital. This shows the atomic structure and the chemical properties of the elements due to different electron configuration.

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Most popular questions from this chapter

In the photoelectron spectrum of Sc, the peak at \(0.63 \mathrm{MJ} / \mathrm{mole}\) is assigned to the \(4 s\) subshell. Why is the peak at \(0.77 \mathrm{MJ} / \mathrm{mole}\) in the \(\mathrm{Sc}\) spectrum assigned as a third subshell of \(n=3\) (named \(3 d\) ) as opposed to being a second subshell of \(n\) \(=4\) (that is, \(4 p)\) ?

\begin{aligned} &\text { Complete the following table: }\\\ &\begin{array}{|c|l|l|} \hline \text { Element } & n \text { for the valence shell } & \text { IE }_{1}(\mathrm{MJ} / \mathrm{mole}) \\ \hline \mathrm{N} & & \\ \hline \mathrm{Ar} & & \\ \hline \end{array} \end{aligned}

\text { Predict the electron configuration of Ga. }

What is the common feature of the electron configurations of the elements in a given column of the periodic table?

Based on the form of the periodic table, how many electrons is the \(3 d\) subshell capable of holding?
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