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Questions and Answers
Which of the following factors contributes to the decrease in ionization energy as you move down a group in the periodic table?
Which of the following factors contributes to the decrease in ionization energy as you move down a group in the periodic table?
Boron has a higher ionization enthalpy than Beryllium.
Boron has a higher ionization enthalpy than Beryllium.
False (B)
What is the definition of ionization enthalpy?
What is the definition of ionization enthalpy?
The amount of energy required to remove one electron from an isolated gaseous atom in its gaseous state.
The [BLANK] effect increases as the number of shells increases, resulting in a decrease in ionization energy.
The [BLANK] effect increases as the number of shells increases, resulting in a decrease in ionization energy.
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Match the following terms with their definitions:
Match the following terms with their definitions:
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The amount of energy required to remove an electron from an isolated gaseous atom in its ground state is called the ______ enthalpy.
The amount of energy required to remove an electron from an isolated gaseous atom in its ground state is called the ______ enthalpy.
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The ionization enthalpy of an element always increases as you move from left to right across a period in the periodic table.
The ionization enthalpy of an element always increases as you move from left to right across a period in the periodic table.
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What are the two main factors that influence ionization enthalpy?
What are the two main factors that influence ionization enthalpy?
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Which of these statements accurately describes the relationship between penetration power and ionization enthalpy?
Which of these statements accurately describes the relationship between penetration power and ionization enthalpy?
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Match the following properties with their impact on ionization enthalpy:
Match the following properties with their impact on ionization enthalpy:
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The ______ effect describes how inner electrons reduce the attraction between the nucleus and outer electrons.
The ______ effect describes how inner electrons reduce the attraction between the nucleus and outer electrons.
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Why does beryllium have a higher ionization enthalpy than boron, despite boron being located to the right of beryllium in the periodic table?
Why does beryllium have a higher ionization enthalpy than boron, despite boron being located to the right of beryllium in the periodic table?
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Explain why elements with half-filled or fully filled orbitals generally have higher ionization energies.
Explain why elements with half-filled or fully filled orbitals generally have higher ionization energies.
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Flashcards
Ionization Enthalpy
Ionization Enthalpy
The energy required to remove an electron from an isolated gaseous atom.
Trend in Ionization Energy
Trend in Ionization Energy
Ionization energy decreases down a group in the periodic table.
Effective Nuclear Charge
Effective Nuclear Charge
The net positive charge experienced by outer electrons in an atom.
Beryllium vs Boron Ionization
Beryllium vs Boron Ionization
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Shielding Effect
Shielding Effect
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Penetration Effect
Penetration Effect
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Trends Across a Period
Trends Across a Period
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Stable Electronic Configurations
Stable Electronic Configurations
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Ionization Energy Discrepancy
Ionization Energy Discrepancy
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Radial Probability Distribution
Radial Probability Distribution
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Study Notes
Ionization Enthalpy
- Ionization enthalpy is the energy needed to remove an electron from an isolated gaseous atom in its ground state.
- Factors affecting ionization enthalpy include: penetration and shielding effects.
- Penetration refers to the electron's proximity to the nucleus. s orbitals penetrate more than p or d orbitals. (e.g., 2s > 2p > 3s > 3p > 4s > 3d).
- Shielding is the effect of inner electrons shielding outer electrons from the full nuclear charge. This decreases the effective nuclear charge felt by outer electrons.
- Elements with half-filled or full electron orbitals are more stable and require more energy to remove an electron, thus having higher ionization enthalpy.
Trends in the Periodic Table
- Across a Period: Ionization enthalpy generally increases from left to right across a period due to decreasing atomic radius and increasing effective nuclear charge.
- Exception: The ionization enthalpy of boron is less than that of beryllium, despite the general trend. This is due to the combination of two factors. Beryllium’s stable electron configuration (fully filled subshells) and the greater penetration power of the 2s electron compared to the 2p electron in boron.
- Down a Group: Ionization enthalpy generally decreases down a group due to increasing atomic size and decreasing effective nuclear charge. Outer electrons are further from the nucleus resulting in a weaker effective nuclear pull. Increased shielding also contributes to this decrease.
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Description
This quiz covers the concept of ionization enthalpy, including factors such as penetration and shielding effects. It also explores trends in the periodic table, particularly how ionization enthalpy changes across a period. Test your understanding of these fundamental concepts in chemistry.
