Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN: 9781337399425
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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**7. Explain the trend as you move across a row of the periodic table for each of the following atomic properties using your understanding of effective nuclear charge.**

   a. **Atomic radius**
   
   b. **Ionization energy/electronegativity**

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### Explanation

When discussing the trends in atomic properties across a row of the periodic table, it is essential to understand the concept of effective nuclear charge (Z_eff). Effective nuclear charge is the net positive charge experienced by valence electrons in an atom.

#### a. **Atomic Radius**

As you move from left to right across a period of the periodic table, the atomic radius generally decreases. This trend occurs because:

1. **Increasing Protons:** The number of protons in the nucleus increases, which results in a higher positive charge.
2. **Higher Effective Nuclear Charge:** The increased positive charge pulls the electrons closer to the nucleus.
3. **Same Energy Level:** Electrons are added to the same principal energy level, ensuring they do not shield each other effectively from the nucleus's increasing pull.

Thus, atoms become smaller as the effective nuclear charge increases across a period.

#### b. **Ionization Energy/Electronegativity**

Ionization energy and electronegativity both generally increase as you move from left to right across a period. This trend can be explained by considering the following points:

- **Ionization Energy:** The energy required to remove an electron from an atom in its gaseous state. As you move across the period, the effective nuclear charge increases, making it more difficult to remove an electron due to the stronger attraction between the electrons and the nucleus.
  
- **Electronegativity:** The tendency of an atom to attract electrons towards itself in a chemical bond. With an increasing effective nuclear charge, atoms more strongly attract bonding electrons.

By understanding these trends, one can predict and rationalize the chemical behavior of different elements in the periodic table.
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Transcribed Image Text:Here is the transcribed text from the image, formatted for use on an educational website: --- **7. Explain the trend as you move across a row of the periodic table for each of the following atomic properties using your understanding of effective nuclear charge.** a. **Atomic radius** b. **Ionization energy/electronegativity** --- ### Explanation When discussing the trends in atomic properties across a row of the periodic table, it is essential to understand the concept of effective nuclear charge (Z_eff). Effective nuclear charge is the net positive charge experienced by valence electrons in an atom. #### a. **Atomic Radius** As you move from left to right across a period of the periodic table, the atomic radius generally decreases. This trend occurs because: 1. **Increasing Protons:** The number of protons in the nucleus increases, which results in a higher positive charge. 2. **Higher Effective Nuclear Charge:** The increased positive charge pulls the electrons closer to the nucleus. 3. **Same Energy Level:** Electrons are added to the same principal energy level, ensuring they do not shield each other effectively from the nucleus's increasing pull. Thus, atoms become smaller as the effective nuclear charge increases across a period. #### b. **Ionization Energy/Electronegativity** Ionization energy and electronegativity both generally increase as you move from left to right across a period. This trend can be explained by considering the following points: - **Ionization Energy:** The energy required to remove an electron from an atom in its gaseous state. As you move across the period, the effective nuclear charge increases, making it more difficult to remove an electron due to the stronger attraction between the electrons and the nucleus. - **Electronegativity:** The tendency of an atom to attract electrons towards itself in a chemical bond. With an increasing effective nuclear charge, atoms more strongly attract bonding electrons. By understanding these trends, one can predict and rationalize the chemical behavior of different elements in the periodic table.
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