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Chapter 8: Problem 83

Find the electron configuration of the element with \(Z=23 .\) From this, give its group and period in the periodic table. Classify the element as a main- group, a \(d\) -block transition, or an \(f\) -block transition element.

Short Answer

Expert verified
Vanadium (V) has electron configuration \([Ar] \, 3d^3 \, 4s^2\), is in Group 5, Period 4, and is a \(d\)-block transition metal.

Step by step solution

01

Identify the Element

The atomic number \( Z \) of the element is given as 23. Look up the periodic table to find the element with atomic number 23, which is Vanadium (V).
02

Determine Electron Configuration

Vanadium (V), with \( Z = 23 \), has 23 electrons. We'll fill the electron shells in order: \(1s^2\), \(2s^2\), \(2p^6\), \(3s^2\), \(3p^6\), \(4s^2\), \(3d^3\). Thus, the electron configuration is: \[1s^2 \,2s^2 \,2p^6 \,3s^2 \,3p^6 \,4s^2 \,3d^3.\]
03

Identify Group and Period

Vanadium is located in Period 4 of the periodic table because it has electrons in the fourth energy level (4s). It is in Group 5 of the periodic table, which includes transition metals.
04

Classify the Element

Vanadium is a \(d\)-block element because its last electron enters the \(3d\) subshell. \(d\)-block elements are also known as transition elements.

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Key Concepts

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

Periodic Table
The periodic table is a comprehensive chart that organizes all known elements by increasing atomic number, which is represented as \( Z \). Each element has a unique atomic number that defines its position on the periodic table.
It is divided into several sections:
  • The main-group elements, which include the s-block and p-block,
  • The d-block, known as the transition metals,
  • And the f-block, which includes the lanthanides and actinides.
Each row in the table is called a period, and each column is known as a group. Elements in the same group often share similar chemical properties.
Transition Metals
Transition metals are elements found in the d-block of the periodic table. They are characterized by having partially filled d-subshells, which give them unique properties such as the ability to form colorful compounds and multiple oxidation states.
These metals are located in groups 3 through 12 and are known for their:
  • High melting and boiling points,
  • Great strength and durability,
  • Efficient conductors of heat and electricity.
Common examples include iron, copper, and zinc. The transition metals play crucial roles in biological systems and industrial processes.
D-Block Elements
The d-block, also known as the transition block, is made up of elements where the d-orbitals are progressively filled. These blocks span groups 3 to 12 in the periodic table and include elements with electron configurations that end in d.
  • The d-block elements exhibit unique properties such as forming complex ions,
  • Showing catalytic behavior,
  • And having distinctive magnetic properties.
The electron configuration for these elements typically starts with the filling of the 4s orbital before moving to the 3d, which is why vanadium (V) has the configuration \(1s^2 \,2s^2 \,2p^6 \,3s^2 \,3p^6 \,4s^2 \,3d^3,\) placing it squarely in this category.

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Most popular questions from this chapter

Two elements are in the same group, one following the other. One is a metalloid; the other is a metal. Both form oxides of the formula \(\mathrm{RO}_{2}\). The first is acidic; the next is amphoteric. Identify the two elements.

Write the valence orbital diagram corresponding to the ground state of \(\mathrm{Nb}\), whose configuration is \([\mathrm{Kr}] 4 d^{4} 5 s^{1}\).

Theelectron affinity of the lutetium atom (element 71\()\) was measured using the technique of photoelectron spectroscopy with an infrared laser (the essay on p. 310 describes this instrumental method, using \(X\) rays). In this experiment, a beam of lutetium negative ions, \(\mathrm{Lu}^{-},\) was prepared and irradiated with a laser beam having a wavelength at \(1064 \mathrm{nm}\). The energy supplied by a photon in this laser beam removes an electron from a negative ion, leaving the neutral atom. The energy needed to remove the electron from the negative ion to give the neutral atom (both in their ground states) is the electron affinity of lutetium. Any excess energy of the photon shows up as kinetic energy of the emitted electron. If the emitted electron in this experiment has a kinetic energy of \(0.825 \mathrm{eV}\), what is the electron affinity of lutetium?

How much energy would be required to ionize \(5.00 \mathrm{mg}\) of \(\mathrm{Na}(g)\) atoms to \(\mathrm{Na}^{+}(g)\) ions? The first ionization energy of \(\mathrm{Na}\) atoms is \(496 \mathrm{~kJ} / \mathrm{mol}\).

The ground-state electron configuration of an atom is \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}\). What is the valence-shell configuration of the atom in the same group, but in Period 5 ?
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