Chapter 2: Problem 118
An atom has 2 electrons in \(\mathrm{K}\) -shell, 8 electrons in L-shell and 6 electrons in M-shell. The number of s-electrons present in the clement is (1) 10 (2) 7 (3) 6 (4) 4
Short Answer
Expert verified
6
Step by step solution
01
- Identify the shells' electron configuration
The electron configuration is given as 2 electrons in the \(\text{K}\)-shell, 8 electrons in the \(\text{L}\)-shell, and 6 electrons in the \(\text{M}\)-shell.
02
- Understand s-, p-, d- orbitals
Know that each shell can hold a different number of electrons in s-, p-, and d- orbitals. The K-shell (1st shell) has only s-orbitals, the L-shell (2nd shell) has s- and p-orbitals, and the M-shell (3rd shell) has s-, p-, and d-orbitals.
03
- Count s-electrons in each shell
In the K-shell, there are 2 electrons, all are in the 1s-orbital. In the L-shell, the first 2 electrons fill the 2s-orbital, and the remaining 6 electrons fill the 2p-orbital, contributing 2 s-electrons. In the M-shell, the first 2 electrons fill the 3s-orbital, giving another 2 s-electrons.
04
- Add up all s-electrons
Sum up all the s-electrons in each shell: \(\text{K-shell:}\text{ 2 s-electrons}\) + \(\text{L-shell: 2 s-electrons}\) + \(\text{M-shell: 2 s-electrons}\) = 6 s-electrons.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
s-electrons
In atomic structure, electrons reside in different orbitals around the nucleus. These orbitals are categorized as s-, p-, d-, and f-orbitals. The s-orbitals are unique because they can hold a maximum of two electrons and are spherical in shape. Each electron shell (or energy level) starts filling with s-electrons first. In the problem provided, we see how s-electrons are distributed in the K, L, and M shells:
- The K-shell (1st energy level) has 1s orbitals, which can hold 2 electrons.
- The L-shell (2nd energy level) has 2s and 2p orbitals, but the s-electrons occupy the 2s orbital first, also up to 2 electrons.
- The M-shell (3rd energy level) follows the same pattern, filling the 3s orbital with up to 2 electrons.
Understanding how s-electrons fill these orbitals is crucial because it tells us how the atom's electron configuration builds from the simplest to more complex shapes. In our example, we find 2 s-electrons in the K-shell, 2 in the L-shell, and 2 in the M-shell, adding up to 6 s-electrons.
- The K-shell (1st energy level) has 1s orbitals, which can hold 2 electrons.
- The L-shell (2nd energy level) has 2s and 2p orbitals, but the s-electrons occupy the 2s orbital first, also up to 2 electrons.
- The M-shell (3rd energy level) follows the same pattern, filling the 3s orbital with up to 2 electrons.
Understanding how s-electrons fill these orbitals is crucial because it tells us how the atom's electron configuration builds from the simplest to more complex shapes. In our example, we find 2 s-electrons in the K-shell, 2 in the L-shell, and 2 in the M-shell, adding up to 6 s-electrons.
atomic structure
Atomic structure is the arrangement of protons, neutrons, and electrons in an atom. The nucleus, made up of protons and neutrons, is at the center. Electrons orbit the nucleus in different energy levels or shells. Each electron shell can hold a specific maximum number of electrons.
The shells are denoted as K, L, M, etc., where the K-shell is closest to the nucleus. Electrons fill these shells starting from the innermost shell and moving outward:
- The K-shell can hold up to 2 electrons.
- The L-shell can hold up to 8 electrons.
- The M-shell can hold up to 18 electrons.
Understanding atomic structure helps us predict behaviors like chemical reactivity and bonding. When analyzing an atom with 2 electrons in the K-shell, 8 in the L-shell, and 6 in the M-shell, we see that its electron configuration adheres to these fundamental rules of atomic structure.
The shells are denoted as K, L, M, etc., where the K-shell is closest to the nucleus. Electrons fill these shells starting from the innermost shell and moving outward:
- The K-shell can hold up to 2 electrons.
- The L-shell can hold up to 8 electrons.
- The M-shell can hold up to 18 electrons.
Understanding atomic structure helps us predict behaviors like chemical reactivity and bonding. When analyzing an atom with 2 electrons in the K-shell, 8 in the L-shell, and 6 in the M-shell, we see that its electron configuration adheres to these fundamental rules of atomic structure.
electron shells
Electron shells, or energy levels, are layers where electrons orbit the nucleus. Each shell has a different energy level and capacity to hold electrons:
- The first shell (K-shell) has the lowest energy and can hold up to 2 electrons in its 1s orbital.
- The second shell (L-shell) has more energy than the K-shell. It includes a 2s orbital that can hold 2 electrons and three 2p orbitals that can hold a total of 6 electrons, making a total capacity of 8 electrons.
- The third shell (M-shell) contains 3s, 3p, and 3d orbitals, holding up to 18 electrons in total.
Electrons populate these shells according to the Aufbau principle, which states that electrons fill the lowest energy orbitals first. This principle helps explain the distribution seen in the exercise. The given atom's electron configuration of 2 electrons in K-shell, 8 in L-shell, and 6 in M-shell shows that the lower energy shells are filled up before moving to higher ones. Understanding the order and capacity of electron shells is fundamental to grasping atomic behavior and properties.
- The first shell (K-shell) has the lowest energy and can hold up to 2 electrons in its 1s orbital.
- The second shell (L-shell) has more energy than the K-shell. It includes a 2s orbital that can hold 2 electrons and three 2p orbitals that can hold a total of 6 electrons, making a total capacity of 8 electrons.
- The third shell (M-shell) contains 3s, 3p, and 3d orbitals, holding up to 18 electrons in total.
Electrons populate these shells according to the Aufbau principle, which states that electrons fill the lowest energy orbitals first. This principle helps explain the distribution seen in the exercise. The given atom's electron configuration of 2 electrons in K-shell, 8 in L-shell, and 6 in M-shell shows that the lower energy shells are filled up before moving to higher ones. Understanding the order and capacity of electron shells is fundamental to grasping atomic behavior and properties.