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Chapter 2: Problem 2

Give the number of valence electrons for each of the following elements: (a) Br; (b) Rh; (c) Nb; (d) Te.

Short Answer

Expert verified
Br has 7, Rh has 9, Nb has 5, and Te has 6 valence electrons.

Step by step solution

01

Identify the Group Number for Bromine (Br)

To find the number of valence electrons for Bromine (Br), look for its position in the periodic table. Bromine is in Group 17 (also known as Group VIIA), which means it has 7 valence electrons.
02

Identify the Group Number for Rhodium (Rh)

Rhodium (Rh) is a transition metal in the 5th period and is part of the group of elements known as the 'd' block. For transition metals, the number of valence electrons includes the 'd' subshell and is typically 1 or 2. Since Rh is in Group 9, it has 1 electron in the 's' subshell and 8 in the 'd' subshell for a total of 9.
03

Identify the Group Number for Niobium (Nb)

Niobium (Nb) is also a transition metal, in the 5th period and part of Group 5. It has 1 electron in the 's' subshell and 4 in the 'd' subshell for a total of 5 valence electrons.
04

Identify the Group Number for Tellurium (Te)

Tellurium (Te) is in Group 16 (also known as Group VIA), which means it has 6 valence electrons.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding the Periodic Table
The periodic table is a remarkable chart that organizes all known elements according to their atomic number and properties. It's structured into rows called periods and columns known as groups or families.

Each group shares similar chemical properties, largely due to the number of valence electrons present in the atoms of the elements. Valence electrons are the outermost electrons and are vital for determining how an element reacts chemically. For instance, Group 17 elements, like Bromine (Br), typically have 7 valence electrons, which makes them very reactive and known as halogens.
Transition Metals Complexities
Transition metals, found in the central block of the periodic table (Groups 3 to 12), have unique and complex electron configurations. Unlike the elements in groups 1, 2, and 13 to 18, transition metals fill their 'd' subshells alongside the 's' subshell of their outermost energy level.

For example, Rhodium (Rh), a Group 9 transition metal, has a combination of 1 electron in its 's' subshell and 8 in its 'd' subshell, adding up to 9 valence electrons. This mix contributes to transition metals' ability to form a variety of different ions and compounds.
Chemical Principles in Action
Chemical principles explain the behavior of elements based on their atomic structure. One such principle is the octet rule, which states that atoms tend to gain, lose, or share electrons to have 8 in their valence shell, achieving stability similar to noble gases.

However, this rule primarily applies to main-group elements and less to transition metals like Rhodium (Rh) or Niobium (Nb), which deviate due to their 'd' subshell participation. Valence electrons facilitate chemical bonding, which is the crux of interactions that lead to compound formation.
Deciphering Electron Configuration
Electron configuration lays out the arrangement of electrons in an atom. Electrons inhabit energy levels or shells, and within each level, they fill subshells in a specific order: 's', 'p', 'd', then 'f'.

The valence electrons are the last to be added in the configuration. For instance, Tellurium (Te) has 6 valence electrons, filling up the 'p' subshell after the 's' subshell in its outer energy level. Understanding an element's electron configuration is crucial for grasping its chemical behavior and bonding potential.

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Most popular questions from this chapter

Write the Lewis structure for each of the following compounds: (a) methanethiol, \(\mathrm{CH}_{3} \mathrm{SH}\), one of the compounds found in bad breath and some cheeses; (b) carbon disulfide, \(\mathrm{CS}_{2}\), which is used to make rayon; (c) dichloromethane, \(\mathrm{CH}_{2} \mathrm{Cl}_{2}, \mathrm{a}\) common solvent.

The following species have the same number of electrons: Cd, \(\mathrm{In}^{+}\), and \(\mathrm{Sn}^{2+}\). (a) Write the electron configurations for each species. Are they the same or different? Explain. (b) How many unpaired electrons, if any, are present in each species? (c) What neutral atom, if any, has the same electron configuration as that of \(\operatorname{In}^{3+}\) ?

Give the ground-state electron configuration and number of unpaired electrons expected for each of the following ions: (a) \(\mathrm{Sb}^{3+}\); (b) \(\mathrm{Sn}^{4+}\); (c) \(\mathrm{W}^{2+}\); (d) \(\mathrm{Br}^{-}\); (c) \(\mathrm{Ni}^{2+}\).

Show how resonance can occur in the following organic ions: (a) acetate ion, \(\mathrm{CH}_{3} \mathrm{CO}_{2}{ }^{-}\); (b) enolate ion, \(\mathrm{CH}_{2} \mathrm{COCH}_{3}{ }^{-}\), which has one resonance structure with a \(\mathrm{C}=\mathrm{C}\) double bond and an \(-\mathrm{O}^{-}\)group on the central carbon atom; (c) allyl cation, \(\mathrm{CH}_{2} \mathrm{CHCH}_{2}^{+}\); (d) amidate ion, \(\mathrm{CH}_{3} \mathrm{CONH}^{-}\)(the \(\mathrm{O}\) and the \(\mathrm{N}\) atoms are both bonded to the second \(\mathrm{C}\) atom).

Chlorine can exist in both positive and negative oxidation states. What is the maximum (a) positive and (b) negative oxidation number that chlorine can have? (c) Write the electron configuration for each of these states. (d) Explain how you arrived at these values.
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