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Chapter 3: Problem 41

The number of d-electrons in \(\mathrm{Ni}\) (atomic number = 28) is equal to that of the a. d-electrons in \(\mathrm{Ni}^{2+}\) b. Total electrons in \(\mathrm{N}\) (atomic number \(=7\) ) c. s and p-electrons in \(\mathrm{F}^{-}\) d. p-electrons in Ar (atomic number \(=18\) )

Short Answer

Expert verified
The number of d-electrons in Ni is equal to the number of d-electrons in Ni虏鈦�.

Step by step solution

01

Determine d-electrons in Neutral Ni

Nickel (Ni) has an atomic number of 28. Its electron configuration is: \[ \text{Ni}: [\text{Ar}] \, 3d^8 \, 4s^2 \]. Therefore, it has 8 d-electrons.
02

Calculate d-electrons in Ni虏鈦�

In Ni虏鈦�, two electrons are removed, typically from the 4s orbital, giving: \[ \text{Ni}^{2+}: [\text{Ar}] \, 3d^8 \]. Hence, Ni虏鈦� also has 8 d-electrons.
03

Verify Total Electrons in N

For nitrogen (N), atomic number 7 means it has 7 total electrons: \[ \text{N}: 1s^2 \, 2s^2 \, 2p^3 \]. Thus, there are 7 total electrons.
04

Verify s and p-electrons in F鈦�

For fluoride ion \( \text{F}^- \) (atomic number 9, gained one electron): \[ \text{F}^-: 1s^2 \, 2s^2 \, 2p^6 \]. It has 8 electrons in the s and p orbitals total.
05

Verify p-electrons in Ar

Argon (Ar) has an atomic number of 18 with the electron configuration: \[ \text{Ar}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \]. It has 6 p-electrons.

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Key Concepts

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

d-electrons
Electrons residing in the d-orbital are called d-electrons. These are found in elements where the d-orbital is being filled.
  • d-electrons typically appear when you reach the transition metals in the periodic table.
  • The d-orbital can hold up to 10 electrons.
For example, in nickel (Ni) which has an atomic number of 28, the electron configuration is \[ [\text{Ar}] \, 3d^8 \, 4s^2 \].This means, out of the 28 electrons of nickel, 8 are d-electrons, located in the 3d orbital.The presence of d-electrons gives transition metals like nickel their characteristic properties like magnetism and complex ion formation.
Electron Configuration of Ions
The electron configuration of an ion involves adjusting the electron configuration of the neutral atom to account for the gain or loss of electrons.
  • Cations are formed by losing electrons, often from the outermost shell first.
  • Anions are formed by gaining electrons into the outermost shell.
For example, in the case of the nickel ion \( \text{Ni}^{2+} \), two electrons are typically removed from the 4s orbital, resulting in the configuration \[ [\text{Ar}] \, 3d^8 \].This shows that ions have different electron configurations than their corresponding neutral atoms, affecting their chemical behavior and reactivity.
Nickel
Nickel is a transition metal known for its hardness and resistance to corrosion. It is located in the fourth period and tenth group of the periodic table.
  • Atomic number: 28
  • Electron configuration: \[ [\text{Ar}] \, 3d^8 \, 4s^2 \]
  • Common oxidation state: +2
Nickel's electron configuration reflects its status as a transition metal with a partially filled d-orbital.Nickel commonly forms a \( \text{Ni}^{2+} \) ion, as seen in compounds like nickel chloride and nickel sulfate.The 3d orbital's occupation is crucial for the magnetic and catalytic properties of nickel.
Fluoride Ion
The fluoride ion \( \text{F}^- \) is formed when a fluorine atom gains one electron.This occurs because fluorine has a high affinity for electrons, seeking a full, stable outer shell.
  • Fluoride ion configuration: \[ 1s^2 \, 2s^2 \, 2p^6 \]
  • Total electrons: 10
  • Formed by gaining an electron: great for attaining noble gas configuration (Neon)
The electron configuration of \( \text{F}^- \) makes it highly stable, similar to neon, a noble gas.Its high electronegativity and stability make it reactive in the formation of ionic compounds, such as sodium fluoride (\( \text{NaF} \)).
p-electrons
p-electrons are those found in the p-orbitals of an atom, which have a higher energy level than s-electrons.Each set of p-orbitals can hold a maximum of 6 electrons since there are 3 p-orbitals, each accommodating 2 electrons.In atomic configurations, such as argon (Ar),
  • Argon has an electron configuration of \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \]
  • It has 6 p-electrons located in the 3p orbital.
These p-electrons contribute significantly to the bonding and chemical properties of an element, influencing aspects like polarizability and molecular formation.

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Most popular questions from this chapter

Match the following: Column I A. \(2 \mathrm{~s}\) B. \(2 \mathrm{p}\) C. \(3 \mathrm{~s}\) D. \(3 \mathrm{p}\) (p) Sum of \((\mathrm{n}+1)\) is 3 (q) total number nodes are two (r) only one node (s) no radial node

In the following questions, two statements (Assertion) \(\mathrm{A}\) and Reason (R) are given. Mark a. If \(\mathrm{A}\) and \(\mathrm{R}\) both are correct and \(\mathrm{R}\) is the correct explanation of \(\mathrm{A}\) b. If \(\mathrm{A}\) and \(\mathrm{R}\) both are correct but \(\mathrm{R}\) is not the correct explanation of A c. A is true but \(\mathrm{R}\) is false d. A is false but \(\mathrm{R}\) is true e. \(\mathrm{A}\) and \(\mathrm{R}\) both are false (A): \(3 \mathrm{~d} \mathrm{Z}^{2}\) orbital is spherically symmetrical. \((\mathrm{R}): 3 \mathrm{~d} Z^{2}\) orbital is the only \(\mathrm{d}\)-orbital which is spherical in shape.

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. \(\mathrm{A}_{2} \mathrm{~B}_{6}\)

Passing an electrical charge through argon gas contained in a partially evacuated vessel yields which of the following? a. A line spectrum b. A continuous spectrum c. No visible change d. White light

In the following questions, two statements (Assertion) \(\mathrm{A}\) and Reason (R) are given. Mark a. If \(\mathrm{A}\) and \(\mathrm{R}\) both are correct and \(\mathrm{R}\) is the correct explanation of \(\mathrm{A}\) b. If \(\mathrm{A}\) and \(\mathrm{R}\) both are correct but \(\mathrm{R}\) is not the correct explanation of A c. A is true but \(\mathrm{R}\) is false d. A is false but \(\mathrm{R}\) is true e. \(\mathrm{A}\) and \(\mathrm{R}\) both are false (A): The kinetic energy of the photo-electron ejected increases with increase in intensity of incident light. \((\mathbf{R}):\) Increase in intensity of incident light increases the rate of emission.
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