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Chapter 2: Problem 9

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

Short Answer

Expert verified
Answer: The common feature in the electron configurations of Group VIIA elements is that they all have seven electrons in their outermost (valence) energy level with a "p^5" configuration. This explains their similar chemical properties, as they tend to gain one electron to achieve a stable electron configuration (a full octet).

Step by step solution

01

Identify the elements in Group VIIA

Group VIIA elements are: Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), and Astatine (At).
02

Write the electron configurations for each element

To understand the commonality in Group VIIA elements, let's write down their electron configurations: - Fluorine (F): 1s^2 2s^2 2p^5 - Chlorine (Cl): 1s^2 2s^2 2p^6 3s^2 3p^5 - Bromine (Br): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5 - Iodine (I): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^5 - Astatine (At): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^5
03

Identify the common feature in electron configurations

By examining the electron configurations of Group VIIA elements, we can see that they all have seven electrons in their outermost (valence) energy level. The electron configuration of their valence shell ends with "p^5": - Fluorine (F): 2p^5 - Chlorine (Cl): 3p^5 - Bromine (Br): 4p^5 - Iodine (I): 5p^5 - Astatine (At): 6p^5 This "p^5" configuration is the common feature that all elements in Group VIIA share, which explains their similar chemical properties as they tend to gain one electron to achieve a stable electron configuration (a full octet).

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Most popular questions from this chapter

Chromium has four naturally occurring isotopes: \(4.34 \%\) of \({ }^{50} \mathrm{Cr}\), with an atomic weight of \(49.9460\) amu; \(83.79 \%\) of \({ }^{52} \mathrm{Cr}\), with an atomic weight of \(51.9405 \mathrm{amu} ; 9.50 \%\) of \({ }^{53} \mathrm{Cr}\), with an atomic weight of \(52.9407 \mathrm{amu} ;\) and \(2.37 \%\) of \({ }^{54} \mathrm{Cr}\), with an atomic weight of \(53.9389\) amu. On the basis of these data, confirm that the average atomic weight of \(\mathrm{Cr}\) is \(51.9963 \mathrm{amu}\)

(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?

The net potential energy \(E_{N}\) between two adjacent ions is sometimes represented by the expression $$ E_{N}=-\frac{C}{r}+D \exp \left(-\frac{r}{\rho}\right) $$ in which \(r\) is the interionic separation and \(C\), \(D\), and \(\rho\) are constants whose values depend on the specific material. (a) Derive an expression for the bonding energy \(E_{0}\) in terms of the equilibrium interionic separation \(r_{0}\) and the constants \(D\) and \(\rho\) using the following procedure: 1\. Differentiate \(E_{N}\) with respect to \(r\) and set the resulting expression equal to zero. 2\. Solve for \(C\) in terms of \(D, \rho\), and \(r_{0}\) - 3\. Determine the expression for \(E_{0}\) by substitution for \(C\) in Equation \(2.12\). (b) Derive another expression for \(E_{0}\) in terms of \(r_{0}, C\), and \(\rho\) using a procedure analogous to the one outlined in part (a).

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

Calculate the force of attraction between a \(\mathrm{K}^{+}\) and an \(\mathrm{O}^{2-}\) ion whose centers are separated by a distance of \(1.5 \mathrm{~nm}\).
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