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Chapter 3: Problem 93

The atomic numbers of elements \(\mathrm{X}, \mathrm{Y}, \mathrm{Z}\) are 19,21 and 25 respectively. The number of electrons present in the 'M' shells of these elements follow the order a. \(Z>Y>X\) b. \(X>Y>Z\) c. \(Z>X>Y\) d. \(\mathrm{Y}>\mathrm{Z}>\mathrm{X}\)

Short Answer

Expert verified
The order is a. \(Z > Y > X\).

Step by step solution

01

Understanding Electronic Configuration

The electronic configuration of an element is determined by distributing its electrons into different energy levels (shells), represented by 'K', 'L', 'M', etc. The shell capacities follow the rule: 2 electrons for K, 8 for L, and 18 for M.
02

Finding M shell electrons for Element X

Element X has an atomic number of 19. Its electronic configuration is 2 (K), 8 (L), and 9 (M). So, the M shell for X has 9 electrons.
03

Finding M shell electrons for Element Y

Element Y has an atomic number of 21. Its electronic configuration is 2 (K), 8 (L), and 11 (M). Therefore, the M shell for Y holds 11 electrons.
04

Finding M shell electrons for Element Z

Element Z has an atomic number of 25. Its electronic configuration is 2 (K), 8 (L), and 15 (M). Thus, the M shell for Z contains 15 electrons.
05

Comparing Number of Electrons in M shell

Now, compare the number of electrons in the M shells: Z has 15, Y has 11, and X has 9. This follows the order Z > Y > X.

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Key Concepts

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

Atomic Number
The atomic number of an element represents the number of protons found in the nucleus of its atom. It is also equal to the number of electrons in a neutral atom, which helps define its chemical properties and placement on the periodic table. For the elements mentioned, the atomic numbers are:
  • Element X: 19
  • Element Y: 21
  • Element Z: 25
These numbers are crucial because they determine the unique identity of each element. As the atomic number increases, so does the complexity of its electronic configuration.
Understanding atomic numbers assists in predicting how an element will behave chemically and helps explain why different elements have specific electron distributions.
Energy Levels
In an atom, electrons are arranged in energy levels or shells surrounding the nucleus. These shells are labeled as K, L, M, and so forth, each capable of holding a certain number of electrons. For example:
  • The K shell can hold up to 2 electrons.
  • The L shell is full with 8 electrons.
  • The M shell has a capacity of up to 18 electrons.
Electrons fill these shells starting from the lowest energy level (K) to higher ones (L, M, etc.), according to the energy minimization principle. This order is crucial in determining the electron distribution for an atom. For elements X, Y, and Z, the distribution into these shells dictates their respective chemical characteristics and reactivity.
Electron Distribution
Electron distribution refers to how electrons are organized in an atom's shells based on their atomic number and energy levels. It's a fundamental concept in determining an element's chemical behavior. The distribution follows the rule of filling from low to high energy:
  • For Element X with atomic number 19, the distribution is 2 (K), 8 (L), and 9 (M).
  • For Element Y with atomic number 21, it's 2 (K), 8 (L), and 11 (M).
  • For Element Z with atomic number 25, the distribution is 2 (K), 8 (L), and 15 (M).
This determines not only a stable baseline for the element's reactivity but also helps in predicting the type of chemical bonds it can form. Analyzing electron distribution allows for deeper insights into patterns of the periodic table and trends like reactivity and bonding capabilities.

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Most popular questions from this chapter

An atom A has the electronic configuration of \(1 \mathrm{~s}^{2}\) \(2 \mathrm{~s}^{2} 2 \mathrm{p}^{1}\). Atom B has the electronic configuration of \(1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{3} .\) The empirical formula of the compound obtained from the reaction of \(\mathrm{A}\) and \(\mathrm{B}\) is a. \(\mathrm{AB}\) b. \(\mathrm{AB}_{3}\) c. \(\mathrm{A}_{3} \mathrm{~B}_{3}\) d. \(\mathrm{A}_{2} \mathrm{~B}_{6}\)

In the Bohr's orbit, what is the ratio of total kinetic energy and the total energy of the electron? a. \(+1\) b. \(+2\) c. \(-2\) d. \(-1\)

How many moles of electrons weigh one kilogram? (mass of electron \(=9.108 \times 10^{-31} \mathrm{~kg}\), Avogadro number \(=6.023 \times 10^{23}\) ) a. \(6.023 \times 10^{23}\) b. \(1 / 9.108 \times 10^{31}\) c. \(\frac{6.023}{9.108} \times 10^{54}\) d. \(\frac{1}{9.108 \times 6.023} \times 10^{8}\)

In Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which one of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen? a. \(3 \rightarrow 2\) b. \(5 \rightarrow 2\) c. \(4 \rightarrow 1\) d. \(2 \rightarrow 5\)

A beam of protons is accelerated through a potential drop of 200 volts. The same experiment is done with a beam of deuterons. After acceleration each beam is bent by the same magnetic field in a directions perpendicular to that of the beam. Which beam will exhibit the greater curvature? a. The same curvature for both b. The beam with the larger velocity will exhibits the smaller curvature c. The proton beam d. The deuteron beam
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