Questions and Answers
Which hybridization results in the highest electronegativity in carbon?
What role do ionization energies and electron affinities play in determining electronegativity?
In which of the following molecules would carbon exhibit the lowest electronegativity?
How does electronegativity change as you move down a group in the periodic table?
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Which factor contributes to higher electronegativity in a molecule?
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Which of the following is a key characteristic of halogens regarding electronegativity?
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What is the effect of substituents on electronegativity in compounds like CH4 and CF4?
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Which of the following statements is true regarding inert gases and electron affinity?
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What is the electron affinity value for inert gases?
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Which atomic property primarily indicates the capacity of an atom to attract electrons in a molecule?
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How does the charge on an atom influence its electronegativity?
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Which of the following elements is likely to have practically zero electron affinity?
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What property of an atom in a molecule is MOST affected by the oxidation state?
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Which of the following factors does NOT influence electronegativity?
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What effect does hybridization have on electronegativity?
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Which of the following configurations contributes to an element having high electron affinity?
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What happens to electron affinity as you move down a group in the periodic table?
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Which of the following elements is expected to have the highest electron affinity?
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What is the primary reason for the low electron affinity of fluorine compared to chlorine?
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Which of the following statements about electron affinity is correct?
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Which group of elements typically has the least electron affinity?
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Electron affinity tends to increase across a period due to:
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Which of the following describes why non-metals typically have higher electron affinities than metals?
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How does atomic size affect electron affinity within a group?
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Study Notes
Hybridisation and Electronegativity
- Electrons' penetrating power increases from s to p to d to f orbitals.
- S electrons face more nuclear attraction due to proximity to the nucleus.
- In sp hybridization (50% s character), atoms experience greater nuclear charge, leading to higher electronegativity, making sp hybridized carbons (like in acetylene) more electronegative than sp2 (ethylene) and sp3 (ethane).
Factors Influencing Electronegativity
- Electronegativity varies based on substituents; for instance, carbon in CF4 is more positive (and thus more electronegative) than in CH4 due to the nature of substituents.
- A higher average of electron affinity and ionization energy correlates to greater electronegativity.
- Effective nuclear charge directly affects an atom's electron-attracting power; increased nuclear charge results in increased electronegativity.
Variation in the Periodic Table
- Electronegativity trends show a decrease down a group and an increase across a period, influenced by electron density.
- Inert gases have zero electron affinities due to a stable electronic configuration, limiting their ability to gain electrons.
- Certain elements (Be, Mg, Ca, N) exhibit almost zero electron affinity due to their half-filled or fully filled configurations.
Charge Effects on Electronegativity
- Cations (positively charged atoms) are more electronegative than anions (negatively charged atoms). Increased positive charge enhances electronegativity.
- For example, chlorine in HClO3 (+5 oxidation state) is more electronegative than in HClO (+1 oxidation state).
Electron Affinity
- Electron affinity (EA) measures energy released when an atom gains an electron, expressed in eV/atom or kJ/mol; it indicates the ease of anion formation.
- Greater EA is associated with greater energy release during electron gain, reflecting stronger attraction for additional electrons.
- Electron affinity generally decreases down a group and increases across a period due to changes in atomic size and effective nuclear charge.
Electronegativity of Elements
- Halogens exhibit maximum electron affinity due to their drive for a stable electronic configuration.
- Electron affinity decreases from Cl to I in the group, but fluorine shows a lower electron affinity due to high electron-electron repulsion from added electrons in its compact structure.
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Description
Explore the fascinating world of hybridization in chemistry with this quiz. Understand the relationships between nuclear attraction, electronegativity, and hybridization types such as sp, sp2, and sp3. This quiz will help you grasp key concepts that influence molecular structure and reactivity.
