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Chapter 1: Problem 6

Which neutral atom of the following elements would have the most unpaired electrons? (A) Titanium (B) Manganese (C) Nickel (D) Zinc

Short Answer

Expert verified
The neutral atom with the most unpaired electrons among Titanium (Ti), Manganese (Mn), Nickel (Ni), and Zinc (Zn) is Manganese (Mn).

Step by step solution

01

Recall the Electron Configurations

Identify the electron configurations of Titanium (Ti), Manganese (Mn), Nickel (Ni), and Zinc (Zn). The configurations are: \nTi: [Ar] 4s2 3d2\nMn: [Ar] 4s2 3d5\nNi: [Ar] 4s2 3d8\nZn: [Ar] 4s2 3d10
02

Applying Hund's Rule

Apply Hund's Rule to the electron configurations. The rule states that, in a subshell, electrons occupy every orbital singly before they occupy orbitals doubly. Hence, unpaired electrons are counted.\nFor Ti: The number of unpaired electrons are 2 from the 3d shell. \nFor Mn: The number of unpaired electrons are 5 from the 3d shell. \nFor Ni: The number of unpaired electrons are 2 from the 3d shell, as 3d8 means 2 electrons are paired and 6 are unpaired. \nFor Zn: The number of unpaired electrons are 0 as all the electrons in the 3d shell are paired.
03

Compare the Number of Unpaired Electrons

From step 2, it's clear that the atom of Manganese (Mn) has the highest number of unpaired electrons, i.e., 5.

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Key Concepts

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

Hund's Rule
Hund's Rule is a fundamental principle used to determine the electron configuration of atoms, particularly within the same subshell. It emphasizes how electrons are distributed among orbitals when filling them up. According to this rule, every orbital in a subshell is singly occupied by electrons before any one orbital is doubly occupied. This is because electrons repel each other due to their like charges, and they prefer to be as far apart as possible within an atom.
Thus, applying Hund鈥檚 Rule helps predict the arrangement of electrons and the resulting magnetic properties of an atom.
  • Think of it like seats on a bus: each person fills an empty seat first before pairing up.
  • Ensures electrons maximize their total spin by occupying individual orbitals singly.
  • Helps determine the number of unpaired electrons within an atom.
Unpaired Electrons
Unpaired Electrons are key to understanding the magnetic properties of atoms. They are electrons that occupy an orbital singly rather than in pairs within the atom's electron configuration. The presence of unpaired electrons results in a magnetic moment, and atoms with unpaired electrons can exhibit paramagnetic behavior.
In contrast, atoms where all electrons are paired will display diamagnetic behavior and be repelled by a magnetic field.
  • These electrons play a crucial role in chemical bonding and reactions.
  • Counted using electron configurations and Hund's Rule.
  • Atoms with the highest number of unpaired electrons typically exhibit stronger magnetic properties.
Transition Metals
Transition Metals are a group of elements found in the d-block of the periodic table. These metals are characterized by having partially filled d-orbitals, which gives rise to their unique properties such as variable oxidation states, colored compounds, and catalytic behaviors.
  • They are defined by the filling of their d-electron shells.
  • Include elements like Titanium, Manganese, Nickel, and Zinc.
  • Exhibit a wide range of oxidation states compared to other elements.
  • Electron configuration closely influences their chemical and physical properties.
  • The number of unpaired electrons can affect their magnetic properties and reactivity.
Electron Shells
Electron Shells refer to the regions around the nucleus of an atom where electrons are likely to be found. Each shell can hold a specific number of electrons and is composed of subshells (s, p, d, f) that accommodate electrons.
  • Outermost shells often determine an element's chemical properties.
  • The arrangement of electrons in these shells is captured in an atom's electron configuration.
  • Understanding the distribution of electrons across these shells helps explain an atom's reactivity and bonding behavior.
  • Transition metals have their d-electrons "transition" between levels, affecting their arrangement and chemical characteristics.

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Most popular questions from this chapter

Use the following information to answer questions 29-31. Pennies are made primarily of zinc, which is coated with a thin layer of copper through electroplating, using a setup like the one above. The solution in the beaker is a strong acid (which produces H' ions), and the cell is wired so that the copper electrode is the anode and zinc penny is the cathode. Use the following reduction potentials to answer questions \(29-31 .\) $$\begin{array}{|l|l|}\hline \text { Half-Reaction } & {\text { Standard Reduction Potential }} \\ \hline \mathrm{Cu}^{2++2 e^{-} \rightarrow \mathrm{Cu}(s)} & {+0.34 \mathrm{V}} \\ \hline 2 \mathrm{H}^{++2 e^{-} \rightarrow \mathrm{H}_{2}(g)} & {0.00 \mathrm{V}} \\ \hline \mathrm{Ni}^{2++2 e^{-} \rightarrow \mathrm{Ni}(s)} & {-0.25 \mathrm{V}} \\\ \hline \mathrm{Zn}^{2++2 e^{-} \rightarrow \mathrm{Zn}(s)} & {-0.76 \mathrm{V}} \\ \hline\end{array}$$ What is the required voltage to make this cell function? (A) 0.34 V (B) 0.42 V (C) 0.76 V (D) 1.10 V

Which substance would have the highest boiling point? (A) Ethanol, because it is the most asymmetrical (B) Acetone, because of the double bond (C) Ethylene glycol, because it has the most hydrogen bonding (D) All three substances would have very similar boiling points because their molar masses are similar.

A mixture of helium and neon gases has a total pressure of 1.2 atm. If the mixture contains twice as many moles of helium as neon, what is the partial pressure due to neon? (A) 0.2 atm (B) 0.3 atm (C) 0.4 atm (D) 0.8 atm

Which of the substances would be soluble in water? (A) Ethylene glycol only, because it has the longest bond lengths (B) Acetone only, because it is the most symmetrical (C) Ethanol and ethylene glycol only, because of their hydroxyl (-OH) (D) All three substances would be soluble in water due to their permanent dipoles.

Directions: Questions 4-7 are short free-response questions that require about 9 minutes each to answer and are worth 4 points each. Write your response in the space provided following each question. Examples and equations may be included in your responses where appropriate. For calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive credit for your answer. Pay attention to significant figures. A stock solution of \(2.0 \mathrm{M} \mathrm{MgCl}_{2}\) is dissolved in water. (a) (i) In the beaker below, draw a particulate diagram that represents \(\mathrm{MgCl}_{2}\) dissolved in water. The approximate sizes of each atom/ion are provided for you. Your diagram should include at least four water molecules, which should be correctly oriented compared to the ions dissolved in solution. (DIAGRAM CANT COPY) (ii) Why are the chloride ions from (a)(i) larger than the magnesium (b) (i) A student wishes to make up 500 \(\mathrm{mL}\) of 0.50 \(M \mathrm{MgCl}_{2}\) for an experiment. Explain the best method of doing so utilizing a graduated cylinder and a volumetric flask. Assume \(\mathrm{MgCl}_{2}\) is fully soluble. (ii) What are the concentrations of the \(\mathrm{Mg}^{2+}\) and \(\mathrm{Cl}^{-}\) ions in the new solution?
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