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Chapter 2: Problem 9

With regard to electron configuration, what do all the elements in Group IIA of the periodic table have in common?

Short Answer

Expert verified
Answer: The similarity in the electron configuration of elements in Group IIA is that they all have two s-orbital electrons in their outermost shell. These two electrons are also known as valence electrons and play a crucial role in the chemical bonding and reactivity of these elements.

Step by step solution

01

Group IIA Elements

In the periodic table, Group IIA elements are also known as alkaline earth metals. These elements include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).
02

Electron Configuration

To determine the electron configuration of the elements, we can follow the Aufbau principle, filling up the orbitals according to their energy levels. Below are the electron configurations for each Group IIA elements: Beryllium (Be): 1s², 2s² Magnesium (Mg): 1s², 2s², 2p⁶, 3s² Calcium (Ca): 1s², 2s², 2p⁶, 3s², 3p⁶, 4s² Strontium (Sr): 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 5s² Barium (Ba): 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 4d¹⁰, 5s², 5p⁶, 6s² Radium (Ra): 1s², 2s², 2p⁶, 3s², 3p⁶, 3d¹⁰, 4s², 4p⁶, 4d¹⁰, 4f¹⁴, 5s², 5p⁶, 5d¹⁰, 6s², 6p⁶, 7s²
03

Common Electron Configuration Feature

All elements in Group IIA have their outermost shell (the highest energy level) containing two s-orbital electrons. This is a characteristic electron configuration within the group. These two s-orbital electrons are also referred to as valence electrons, which are responsible for chemical bonding and reactivity of these elements.

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Most popular questions from this chapter

(a) Cite two important quantum-mechanical concepts associated with the Bohr model of the atom. (b) Cite two important additional refinements that resulted from the wave- mechanical atomic model.

(a) What electron subshell is being filled for the rare earth series of elements on the periodic table? (b) What electron subshell is being filled for the actinide series?

Potassium iodide (KI) exhibits predominantly ionic bonding. The \(\mathrm{K}^{+}\) and \(\mathrm{I}^{-}\) ions have electron structures that are identical to which two inert gases?

Explain why hydrogen fluoride (HF) has a higher boiling temperature than hydrogen chloride (HCl) (19.4 vs. \(-85^{\circ} \mathrm{C}\) ), even though HF has a lower molecular weight.

Compute the percentage ionic character of the interatomic bond for each of the following compounds: \(\mathrm{MgO}, \mathrm{GaP}, \mathrm{CsF}, \mathrm{CdS},\) and \(\mathrm{FeO}\)
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