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Questions and Answers
What occurs to electron affinity as one progresses from left to right across a period?
What occurs to electron affinity as one progresses from left to right across a period?
How does electronegativity change as you move down a group?
How does electronegativity change as you move down a group?
Which of the following is NOT a metallic property?
Which of the following is NOT a metallic property?
What effect does atomic radius have on electron affinity when moving down a group?
What effect does atomic radius have on electron affinity when moving down a group?
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The ability of an atom to attract pairs of electrons in a chemical bond is known as what?
The ability of an atom to attract pairs of electrons in a chemical bond is known as what?
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What role does nuclear charge play in the attraction of electrons to the nucleus?
What role does nuclear charge play in the attraction of electrons to the nucleus?
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Which factor is primarily responsible for the different sizes of atoms in the periodic table?
Which factor is primarily responsible for the different sizes of atoms in the periodic table?
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What is the effect of electron shielding on the electrons in an atom?
What is the effect of electron shielding on the electrons in an atom?
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How does quantum theory contribute to our understanding of electron arrangement?
How does quantum theory contribute to our understanding of electron arrangement?
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What consequence does increased electron repulsion have within the same energy level?
What consequence does increased electron repulsion have within the same energy level?
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Which element has a greater atomic radius?
Which element has a greater atomic radius?
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What trend is observed in atomic radii as you move across a period from left to right?
What trend is observed in atomic radii as you move across a period from left to right?
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Why do atomic radii increase down a group?
Why do atomic radii increase down a group?
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Which statement is true about the reactivity of non-metals compared to metals?
Which statement is true about the reactivity of non-metals compared to metals?
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What factor contributes to the atomic radius changes across a period?
What factor contributes to the atomic radius changes across a period?
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Which of the following elements would likely have the largest atomic radius?
Which of the following elements would likely have the largest atomic radius?
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What describes the reactivity of noble gases?
What describes the reactivity of noble gases?
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In periodic trends, how does the strength of attraction between the nucleus and valence electrons change across a period?
In periodic trends, how does the strength of attraction between the nucleus and valence electrons change across a period?
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How does the shielding effect influence the atomic radius?
How does the shielding effect influence the atomic radius?
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What happens to the ionic radius when a neutral atom forms a positive ion?
What happens to the ionic radius when a neutral atom forms a positive ion?
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Why does ionic radius increase down a group?
Why does ionic radius increase down a group?
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What trend is observed in ionic radii for positive ions as one moves across a period?
What trend is observed in ionic radii for positive ions as one moves across a period?
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What defines the first ionization energy?
What defines the first ionization energy?
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How do ionization energies change across a period and why?
How do ionization energies change across a period and why?
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What effect does gaining an electron have on an atom?
What effect does gaining an electron have on an atom?
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What trend is observed regarding ionization energy as you move down a group?
What trend is observed regarding ionization energy as you move down a group?
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Study Notes
Trends in the Periodic Table
- Three factors contribute to periodic trends: quantum theory, nuclear charge, and electron shielding.
Quantum Theory
- Bohr's atomic model suggests electrons orbit the nucleus at specific energy levels and distances.
- This results in varying sizes and electrostatic forces between electrons and the nucleus.
- Electrons are positioned at a specific distance from the nucleus.
Nuclear Charge
- As more protons are added to the nucleus, the electrostatic attraction between the nucleus and the orbiting electrons increases.
- The increased nuclear charge leads to stronger attraction of electrons within the same energy level.
- This pulls electrons closer to the nucleus.
Electron Shielding
- Electrons experience repelling forces from other electrons.
- Electrons in lower energy levels shield those in higher levels, pushing them further from the nucleus.
- Increased electron population within energy levels enhances repulsion, further pushing electrons away from the nucleus.
Reactivity
- Reactivity is dependent on atomic structure.
- The noble gases are largely non-reactive.
- Reactivity in non-metals increases to the right.
- Reactivity in metals increases down.
Atomic Radius (Across a Period)
- Atomic radii generally decrease from left to right across a period.
- The attraction between the nucleus and valence electrons increases as protons are added, pulling the electrons closer.
- The number of filled inner energy levels remains the same.
Atomic Radius (Down a Group)
- Atomic radii generally increase down a group.
- The more inner energy levels, the more shielded the valence electrons become, and less pulled towards the nucleus, leading to an increase in atomic radius.
Ionic Radius (Positive Ions)
- Removal of electrons forms cations.
- Cations have a smaller radius than the original neutral atom.
- Ionic radii increase down a group, due to the outermost occupied electron energy level being further from the nucleus.
- Ionic radii decrease across a period as nuclear attraction to electrons increases.
Ionic Radius (Negative Ions)
- Gaining electrons forms anions.
- Anions have a larger radius than the original atom.
- Anions have increased repulsion of electrons leading to a larger radius.
Ionization Energy
- Ionization energy is needed to remove an electron from an atom or ion in the gaseous state.
- It is not consistent, as the electron being removed varies.
- First ionization energy is the energy to remove the least bound electron.
- Second ionization energy is removing an electron from the positively charged ion.
- Ionization energies increase across a period and generally decrease down a group.
Electron Affinity
- Electron affinity is the energy change when an electron is added to an atom.
- It is a measure of how strongly an atom attracts electrons.
- This results in the formation of an anion if the added electron produces a stable atom.
- Electron affinities generally increase across a period and decrease down a group.
Electronegativity
- Electronegativity measures an atom's ability to attract electrons in a chemical bond.
- Bond type is largely dictated by electronegativity differences between atoms.
- Electronegativity increases across a period and decreases down a group.
Metallic Properties
- Metallic properties result from the element's ability to lose electrons.
- Cations form, hydrogen is displaced in acids, basic oxides form, and ionic chlorides form, etc.
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Description
This quiz covers the key factors influencing periodic trends in the periodic table, including quantum theory, nuclear charge, and electron shielding. Understand how these concepts affect atomic structure and electron behavior. Test your knowledge on these fundamental principles of chemistry!
