Periodic Trends: Reactivity and Metallic Character

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How does reactivity change for metals down a group?
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For metals, reactivity increases down a group as it becomes easier to lose electrons.
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How does reactivity change for nonmetals across a period?
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For nonmetals, reactivity increases across a period as elements become more likely to gain electrons.
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Why does reactivity decrease for metals across a period?
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Reactivity decreases for metals across a period as increased nuclear charge makes it harder to lose electrons.
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Why is francium the most reactive metal?
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Francium is highly reactive due to its large atomic size and low ionization energy.
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Why do halogens have high reactivity?
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Halogens have high reactivity because they have high electronegativity and can easily gain electrons.
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How does metallic character change across a period?
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Metallic character decreases across a period as elements transition from metals to nonmetals.
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How does metallic character change down a group?
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Metallic character increases down a group as elements become more metallic in their properties.
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What is the relationship between metallic character and electrical conductivity?
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Metallic character is directly related to electrical conductivity, as metals are good conductors due to delocalized electrons.
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How does the position in the periodic table affect the reactivity of alkali metals?
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Alkali metals are more reactive down the group due to their increasing atomic size and lower ionization energies.
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What is the most reactive nonmetal and why?
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Fluorine is the most reactive nonmetal because it has a high electronegativity and a small atomic radius.
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How does reactivity of alkaline earth metals compare to alkali metals?
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Alkaline earth metals are less reactive than alkali metals because they have higher ionization energies.
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What predicts the type of oxidation states shown by transition metals?
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The type of oxidation states is influenced by their ability to lose different numbers of d or s electrons.
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What is the trend in the reducing ability of metals down a group?
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The reducing ability of metals increases down a group as they lose electrons more easily.
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How does the reactivity of halogens change down the group?
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Reactivity of halogens decreases down the group due to increased atomic size and a decrease in electronegativity.
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Why do some metals not react as expected based on their position?
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Transition metals may not follow expected trends due to their complex electron interactions and stable d-subshell configurations.
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