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Questions and Answers
What is the trend observed for atomic radii as you move down a group in the periodic table?
What does Coulomb's Law primarily describe?
Effective nuclear charge increases as the number of electron shielding increases.
False
As you move down a group in the periodic table, the atomic radius tends to ______.
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What term is used to describe the outermost electrons that are involved in bonding?
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Match the following concepts to their descriptions:
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Study Notes
Periodic Trends
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Atomic Radius: Increases down a group and decreases across a period.
- The more electron shells an atom has, the larger its atomic radius.
- As you move across a period, the number of protons increases, pulling the electrons in tighter, resulting in a smaller atomic radius.
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Ionization Energy: The energy needed to remove an electron from a gaseous atom.
- Increases across a period and decreases down a group.
- The higher the ionization energy, the more difficult it is to remove an electron.
- Electrons in smaller atoms are held more tightly by the nucleus, requiring more energy to be removed.
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Electron Affinity: The change in energy when an electron is added to a gaseous atom.
- Generally increases across a period.
- Decreases down a group.
- The higher the electron affinity, the more stable the resulting anion.
- Atoms with a strong attraction for electrons tend to gain electrons more easily.
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Metallic Character: The tendency of an element to lose electrons and form positive ions (cations).
- Increases down a group and decreases across a period.
- Elements with low ionization energy and high electron affinity tend to be more metallic.
- Trend Summary: The periodic trends of atomic radius, ionization energy, electron affinity, and metallic character reflect the interplay between nuclear charge, electron shielding, and the distance between the nucleus and outer electrons.
Coulomb's Law
- Describes the electrostatic force between charged particles
- Force is directly proportional to the product of the charges
- Force is inversely proportional to the square of the distance between them
Nuclear Charge, Shielding Effect & Effective Nuclear Charge
- Nuclear Charge: The positive charge of an atom's nucleus, equal to the number of protons
- Shielding Effect: The reduction in the attraction between the nucleus and an electron due to the presence of inner-shell electrons
- Effective Nuclear Charge (Zeff): The net positive charge experienced by an electron in an atom, taking into account shielding.
How to Calculate the Effective Nuclear Charge?
- Zeff = Z - S
- Z: Atomic Number (number of protons)
- S: Number of core electrons (electrons in inner shells)
Conceptual Connection 8.4
- Relates to the understanding of Coulomb's Law and its implications for the periodic trends observed in the periodic table.
Problems by Topic Questions 57 & 58
- These questions focus on applying the concepts of nuclear charge, shielding effect, and effective nuclear charge to specific elements and their properties.
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Description
Test your understanding of ionization energy and the properties of elements with this chemistry quiz. You'll be challenged to arrange elements based on their ionization energies and metallic character, helping you grasp these fundamental concepts in chemistry.
