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Questions and Answers
What is the primary reason for the decrease in metallic character across a period?
What is the primary reason for the decrease in metallic character across a period?
Which of the following factors increases metallic character?
Which of the following factors increases metallic character?
What is the primary trend observed down a group in terms of metallic character?
What is the primary trend observed down a group in terms of metallic character?
What is the term for the ability of an element to exhibit metallic properties such as conductivity and malleability?
What is the term for the ability of an element to exhibit metallic properties such as conductivity and malleability?
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Which of the following is a key concept related to periodic trends?
Which of the following is a key concept related to periodic trends?
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What is the primary reason for the increase in atomic radius down a group?
What is the primary reason for the increase in atomic radius down a group?
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Which of the following is a trend in electronegativity across a period?
Which of the following is a trend in electronegativity across a period?
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What is the main factor that affects ionization energy?
What is the main factor that affects ionization energy?
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Which of the following is a characteristic of metals?
Which of the following is a characteristic of metals?
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What is the relationship between nuclear charge and atomic radius?
What is the relationship between nuclear charge and atomic radius?
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Which of the following is a trend in ionization energy down a group?
Which of the following is a trend in ionization energy down a group?
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Study Notes
Atomic Radius
- Definition: The distance from the nucleus to the outermost electron in an atom.
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Trends:
- Increases down a group (left to right) due to additional energy levels.
- Decreases across a period (top to bottom) due to increased nuclear charge.
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Factors affecting atomic radius:
- Shielding effect: Inner electrons shield outer electrons from nuclear charge, increasing radius.
- Effective nuclear charge: Increased nuclear charge decreases radius.
Electronegativity
- Definition: The ability of an atom to attract electrons in a covalent bond.
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Trends:
- Increases across a period (left to right) due to increased nuclear charge.
- Decreases down a group (top to bottom) due to increased shielding effect.
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Factors affecting electronegativity:
- Nuclear charge: Increased nuclear charge increases electronegativity.
- Shielding effect: Decreased shielding effect increases electronegativity.
Ionization Energy
- Definition: The energy required to remove an electron from an atom.
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Trends:
- Increases across a period (left to right) due to increased nuclear charge.
- Decreases down a group (top to bottom) due to increased shielding effect.
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Factors affecting ionization energy:
- Nuclear charge: Increased nuclear charge increases ionization energy.
- Shielding effect: Decreased shielding effect increases ionization energy.
Metallic Character
- Definition: The ability of an element to exhibit metallic properties (e.g., conductivity, malleability).
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Trends:
- Decreases across a period (left to right) due to increased nuclear charge.
- Increases down a group (top to bottom) due to increased shielding effect.
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Factors affecting metallic character:
- Electronegativity: Decreased electronegativity increases metallic character.
- Shielding effect: Increased shielding effect increases metallic character.
Periodic Trends
- Horizontal trends: Across a period, elements exhibit similar trends due to increased nuclear charge.
- Vertical trends: Down a group, elements exhibit similar trends due to increased shielding effect.
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Key concepts:
- Effective nuclear charge
- Shielding effect
- Electronegativity
- Ionization energy
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Description
Understand the concept of atomic radius, its trends, and factors affecting it, including shielding effect and effective nuclear charge.
