Problem 35
Question
An element has 2 electrons in its \(\mathrm{K}\) shell, 8 electrons in L shell, 13 electrons in \(\mathrm{M}\) shell and one electron in \(\mathrm{N}\) shell. The element is (a) \(\mathrm{Cr}\) (b) \(\mathrm{Fe}\) (c) \(\mathrm{V}\) (d) Ti
Step-by-Step Solution
Verified Answer
The element is Chromium (Cr), option (a).
1Step 1: Understand Electron Shells
Elements are organized by their electron configurations, consisting of different shells: K, L, M, N, etc. Each shell can hold a specific number of electrons. The K-shell holds up to 2 electrons, L-shell holds up to 8, M-shell up to 18, and the N-shell can start filling after M reaches 8.
2Step 2: Analyze Given Electron Configuration
The problem states there are 2 electrons in the K shell, 8 in the L shell, 13 in the M shell, and 1 in the N shell. Summing these up gives the total electrons: 2 + 8 + 13 + 1 = 24.
3Step 3: Identify the Element by Atomic Number
The atomic number of an element is equal to the number of protons, which is also the same as the number of electrons in a neutral atom. The atomic number 24 corresponds to the element Chromium (Cr) on the periodic table.
4Step 4: Verify and Choose Correct Option
Among the options given (Cr, Fe, V, Ti), Chromium (Cr) is the element with atomic number 24. Therefore, option (a) is the correct choice.
Key Concepts
Understanding Atomic StructureExploring Electron ShellsPeriodic Table Elements and Identification
Understanding Atomic Structure
The atomic structure of an element is the blueprint that defines its identity and properties. At the heart of this structure is the nucleus, containing protons and neutrons, while electrons orbit around the nucleus in defined spaces called orbitals or shells. The number of protons defines the atomic number, which is unique to each element. In a neutral atom, the number of electrons equals the number of protons.
Understanding this structure helps us determine the electron configuration, which describes how electrons are distributed among the different shells. These shells, denoted as K, L, M, N, and so on, accommodate varied numbers of electrons. The arrangement and number of these electrons influence the chemical behavior and reactivity of the element.
Overall, the atomic structure provides the framework to understand not only the physical aspects of the elements but also their chemical interactions and relationships with other elements.
Understanding this structure helps us determine the electron configuration, which describes how electrons are distributed among the different shells. These shells, denoted as K, L, M, N, and so on, accommodate varied numbers of electrons. The arrangement and number of these electrons influence the chemical behavior and reactivity of the element.
Overall, the atomic structure provides the framework to understand not only the physical aspects of the elements but also their chemical interactions and relationships with other elements.
Exploring Electron Shells
Electron shells, also known as energy levels, are critical in understanding how electrons are distributed in an atom. Each shell can hold a set maximum number of electrons: the K-shell can accommodate up to 2, the L-shell up to 8, the M-shell up to 18, and so on. The shells fill in a specific order, starting from the innermost shell (K) outward.
As we move to higher shells, they can hold more electrons due to increased distance from the nucleus. The Pauli Exclusion Principle and Hund's Rule explain the filling order and arrangement of electrons within these shells. These principles help predict how an element will interact chemically.
For instance, when a shell is filled or nearly filled, an element may become stable or inert, while others with unfilled shells tend to be more reactive. This concept divides elements into what we commonly refer to as metals, non-metals, and noble gases.
As we move to higher shells, they can hold more electrons due to increased distance from the nucleus. The Pauli Exclusion Principle and Hund's Rule explain the filling order and arrangement of electrons within these shells. These principles help predict how an element will interact chemically.
For instance, when a shell is filled or nearly filled, an element may become stable or inert, while others with unfilled shells tend to be more reactive. This concept divides elements into what we commonly refer to as metals, non-metals, and noble gases.
Periodic Table Elements and Identification
The periodic table is a comprehensive map of elements based on increasing atomic number, which corresponds to their electron configuration. Each element on the table is defined by its atomic number, which represents the total number of protons—and in a neutral atom, electrons.
- The periodic table is organized into rows (periods) and columns (groups or families) that indicate recurring chemical properties.
- Elements are arranged so that those with similar electron configurations or properties line up in columns. This arrangement allows scientists and students alike to predict behaviors and interactions among different elements.
- Element identification, such as in the exercise, involves pinpointing the number of electrons in different shells to determine the atomic number. This becomes incredibly useful in identifying unknown elements or verifying the properties of existing ones.
Other exercises in this chapter
Problem 33
The atomic number of an element is 17 . The number of orbitals electron pairs in its valence shell is (a) 3 (b) 4 (c) 6 (d) 8
View solution Problem 34
The correct representation for d orbital is (a) \((\mathrm{n}-1) \mathrm{d}^{1-9} \mathrm{~ns}^{1}\) (b) \((\mathrm{n}-1) \mathrm{d}^{1-10} \mathrm{~ns}^{1-2}\)
View solution Problem 36
Effective magnetic moment of \(\mathrm{Sc}^{3+}\) ion is (a) 0 (b) \(1.73\) (c) \(2.83\) (d) \(3.87\)
View solution Problem 37
Which of the following is not possible? (a) \(\mathrm{n}=2, l=1, \mathrm{~m}=0\) (b) \(\mathrm{n}=2, l=0, \mathrm{~m}=-1\) (c) \(\mathrm{n}=3, l=0, \mathrm{~m}=
View solution