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Chapter 11: Problem 111

Write the electron configuration for each of the following atoms. (Chapter 5) \begin{equation} \begin{array}{ll}{\text { a. fluorine }} & {\text { c. titanium }} \\ {\text { b. aluminum }} & {\text { d. radon }}\end{array} \end{equation}

Short Answer

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Fluorine: 1s虏 2s虏 2p鈦�; Aluminum: 1s虏 2s虏 2p鈦� 3s虏 3p鹿; Titanium: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d虏; Radon: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 4f鹿鈦� 5d鹿鈦� 6p鈦�.

Step by step solution

01

Understand the Periodic Table Position

Identify the electron shell and number of electrons for each atom based on their position in the periodic table. Fluorine is atomic number 9, aluminum is 13, titanium is 22, and radon is 86.
02

Determine Electron Configuration Order

Recall the order of electron filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p. Electrons fill lower energy orbitals first.
03

Write Electron Configuration for Fluorine

Fluorine has 9 electrons. Its configuration is 1s虏 2s虏 2p鈦�. Fill the orbitals in order until all electrons are used.
04

Write Electron Configuration for Aluminum

Aluminum has 13 electrons. Begin with 1s虏 2s虏 2p鈦� 3s虏 3p鹿. Continue adding electrons to each orbital until they are all included.
05

Write Electron Configuration for Titanium

Titanium has 22 electrons. The configuration is 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d虏. Notice the transition to 3d after 4s is filled.
06

Write Electron Configuration for Radon

Radon has 86 electrons. Continue the sequence to form the configuration: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 4f鹿鈦� 5d鹿鈦� 6p鈦�.

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Key Concepts

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

Periodic Table
The periodic table is a tool used by chemists to organize the elements based on their properties. It groups elements into rows and columns, which helps us understand their chemical behavior. Each row is called a period, and elements in the same column belong to a group or family. The layout of the periodic table reflects the recurring or periodic nature of chemical properties.

  • Elements are ordered by increasing atomic number鈥攖he number of protons in an atom鈥檚 nucleus.
  • The position of an element can tell us about its electron configuration.
  • Elements in the same group often have similar electron configurations and chemical properties.
The periodic table is divided into blocks based on electron subshells: s-block, p-block, d-block, and f-block. Understanding these blocks helps predict an element's behavior and write its electron configuration efficiently.
Electron Filling Order
Electron filling order, also known as the Aufbau principle, governs the sequence in which electrons occupy orbitals in an atom. According to this principle, electrons will fill the lowest energy orbitals first. This order is vital for determining the electron configuration of an element.

To correctly fill electrons, follow this sequence:
  • 1s, 2s, 2p, 3s, 3p
  • 4s before 3d
  • 4d and 5p after 5s
  • 6p comes after 5d and so on
  • F-block (4f and 5f) fits into the 6th and 7th periods but after 6s and 7s respectively
This sequence helps to understand how electrons populate energy levels. By using this order, we determine the distribution of electrons in an atom's electron shells and subshells.
Atomic Number
An element's atomic number is a fundamental property that defines it. It is equal to the number of protons in an atom's nucleus, which also equals the number of electrons in a neutral atom. Each element on the periodic table has a unique atomic number, distinguishing it from other elements.

  • For example, fluorine has an atomic number of 9, indicating 9 protons and, in a neutral state, 9 electrons.
  • The atomic number increases sequentially from left to right across the periodic table.
  • Knowing the atomic number helps to write the electron configuration as it tells us the total number of electrons present.
Understanding the atomic number is crucial as it not only categorizes elements but also lays the foundation for assessing many of their chemical and physical properties.
Orbitals
Orbitals are regions in an atom where electrons are likely to be found. Each orbital can hold a certain number of electrons and is part of an electron shell. The shape and orientation of orbitals are determined by quantum numbers and influence the chemical bonding of elements.

There are different types of orbitals:
  • s orbitals: Spherical in shape and can hold 2 electrons.
  • p orbitals: Dumbbell-shaped and each can hold 6 electrons across 3 orientations (px, py, pz).
  • d orbitals: More complex shapes with the ability to hold 10 electrons across 5 orientations.
  • f orbitals: Even more complex, these can hold 14 electrons across 7 orientations.
Orbitals help us describe where electrons reside and also explain an element鈥檚 reactivity and positions within the periodic table. Understanding orbitals allows chemists to predict and explain chemical reactions and bonding patterns.

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Most popular questions from this chapter

Nickel-Iron Battery In 1901 , Thomas Edison invented the nickel-iron battery. The following reaction takes place in the battery. \begin{equation} \mathrm{Fe}(\mathrm{s})+2 \mathrm{NiO}(\mathrm{OH})(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \end{equation} \begin{equation} \quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\mathrm{Fe}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{Ni}(\mathrm{OH})_{2}(\mathrm{aq}) How many mol of \(\mathrm{Fe}(\mathrm{OH})_{2}\) is produced when 5.00 \(\mathrm{mol}\) of Fe and 8.00 \(\mathrm{mol}\) of \(\mathrm{NiO}(\mathrm{OH})\) react? \end{equation}

List several reasons why the actual yield from a chemical reaction is not usually equal to the theoretical yield.

Analyze Tetraphosphorus trisulphide \(\left(P_{4} S_{3}\right)\) is used in the match heads of some matches. It is produced in the reaction \(8 \mathrm{P}_{4}+3 \mathrm{S}_{8} \rightarrow 8 \mathrm{P}_{4} \mathrm{S}_{3}\) . Determine which of the following statements are incorrect, and rewrite the incorrect statements to make them correct. \begin{equation} \begin{array}{l}{\text { a. } 4 \text { mol } P_{4} \text { reacts with } 1.5 \text { mol } S_{8} \text { to form } 4 \text { mol } P_{4} S_{3} \text { . }} \\\ {\text { b. Sulfur is the limiting reactant when } 4 \text { mol } P_{4} \text { and } 4 \text { mol } S_{8} \text { react. }} \\ {\text { c. } 6 \text { mol } P_{4} \text { reacts with } 6 \text { mol } S_{8} \text { forming } 1320 \text { g } P_{4} S_{3} \text { . }}\end{array} \end{equation}

Iron Production Iron is obtained commercially by the reaction of hematite \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)\) with carbon monoxide. How many grams of iron is produced when 25.0 \(\mathrm{mol}\) of hematite reacts with 30.0 \(\mathrm{mol}\) of carbon monoxide? \begin{equation} \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g}) \rightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{g}) \end{equation}

Electrolysis Determine the theoretical and percent yield of hydrogen gas if 36.0 g of water undergoes electrolysis to produce hydrogen and oxygen and 3.80 g of hydrogen is collected.
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