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Chapter 9: Problem 42

Write the electron configurations of \(\mathrm{Sn}\) and \(\mathrm{Sn}^{2+}\).

Short Answer

Expert verified
Sn: [Kr] 4d^{10} 5s^2 5p^2; Sn^{2+}: [Kr] 4d^{10} 5s^2.

Step by step solution

01

Determine Atomic Number

First, we need to find the atomic number of Tin (Sn). From the periodic table, we know that the atomic number of Sn is 50.
02

Write Electron Configuration for Neutral Sn

The electron configuration of an element describes the distribution of its electrons among the orbitals. Starting from 1s, we fill up according to the Aufbau principle:\[\text{Sn: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6 \, 5s^2 \, 4d^{10} \, 5p^2\]Sn has a total of 50 electrons, and this is how they fill the orbitals.
03

Remove Electrons for Sn虏鈦� Ion

To find the electron configuration for Sn虏鈦�, we need to remove two electrons from the neutral Sn configuration. Electrons are removed from the outermost shell first, which is the 5p orbitals in this case:\[\text{Sn}^{2+}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6 \, 5s^2 \, 4d^{10}\]Thus, Sn虏鈦� has two fewer electrons than neutral Sn.

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Key Concepts

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

Understanding the Atomic Number
The atomic number is like an ID for elements on the periodic table. It tells us how many protons are in an atom of the element. For Tin (Sn), this number is 50. The atomic number is crucial because it also equals the number of electrons in a neutral atom, balancing the positive charges from protons. This knowledge forms the basis for determining an element's electron configuration, which is how we study the structure of atoms and predict chemical behavior.
Exploring the Aufbau Principle
The Aufbau principle is like following a rule book for filling up spots at a concert. It dictates the order in which electrons fill various atomic orbitals: from the lowest energy level to the highest. Think of it as filling seats in a theater row by row, from the front to the back.
  • Electrons always begin filling from the 1s orbital, the lowest energy level.
  • As they move to higher levels, they fill the 2s, 2p, 3s, and so forth.
This principle helps us write the electron configuration for Tin, ensuring each electron finds its precise spot according to energy levels, helping us visualize the atomic structure.
Diving into Orbitals
Orbitals are like specific seats in an atomic bus where electrons sit. Each orbital type ( s, p, d, f) has a different shape and capacity:
  • The s orbitals can hold 2 electrons.
  • The p orbitals can have 6.
  • The d orbitals accommodate 10.
  • The f orbitals pack up to 14 electrons.
In the case of Tin, 50 electrons spread over these orbitals, starting from 1s through 5p, as dictated by their energy levels. Understanding orbitals helps us comprehend how electrons occupy space and interact with other atoms.
Electron Removal and Ion Formation
When forming ions, electrons are lost from the outermost orbitals. For Sn^{2+}, we remove two electrons from the 5p orbital, the outermost shell. This reduces the electron count, altering the atom's charge, shape, and reactivity. The ion's electron configuration becomes shorter, as electrons from the highest energy level are gone. This process underscores the idea that chemical reactions often involve gaining or losing electrons, modifying the atom's electronic environment.

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Most popular questions from this chapter

For each of the following, use formal charges to choose the Lewis formula that gives the best description of the electron distribution: a. \(\mathrm{SOF}_{2}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{3}\) c. \(\mathrm{HClO}_{2}\)

Write resonance descriptions for the following: a. \(\mathrm{HNO}_{3}\) b. \(\mathrm{SO}_{3}\)

You land on a distant planet in another universe and find that the \(n=1\) level can hold a maximum of 4 electrons, the \(n=2\) level can hold a maximum of 5 electrons, and the \(n=3\) level can hold a maximum of 3 electrons. Like our universe, protons have a charge of \(+1\), electrons have a charge of \(-1\), and opposite charges attract. Also, a filled shell results in greater stability of an atom, so the atom tends to gain or lose electrons to give a filled shell. Predict the formula of a compound that results from the reaction of a neutral metal atom \(\mathrm{X}\), which has 7 electrons, and a neutral nonmetal atom \(\mathrm{Y}\), which has 3 electrons.

Phosphorous acid, \(\mathrm{H}_{3} \mathrm{PO}_{3}\), has the structure (HO) \(_{2}\) PHO, in which one \(\mathrm{H}\) atom is bonded to the \(\mathrm{P}\) atom, and two \(\mathrm{H}\) atoms are bonded to \(O\) atoms. For each bond to an \(H\) atom, decide whether it is polar or nonpolar. Assume that only polar-bonded \(\mathrm{H}\) atoms are acidic. Write the balanced equation for the complete neutralization of phosphorous acid with sodium hydroxide. A \(200.0-\mathrm{mL}\) sample of \(\mathrm{H}_{3} \mathrm{PO}_{3}\) requires \(22.50 \mathrm{~mL}\) of \(0.1250 \mathrm{M}\) \(\mathrm{NaOH}\) for complete neutralization. What is the molarity of the \(\mathrm{H}_{3} \mathrm{PO}_{3}\) solution?

What is the relationship between bond order and bond length? Use an example to illustrate it.
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