Periodic Trends: Reactivity and Metallic Character

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How does reactivity change for metals down a group?

For metals, reactivity increases down a group as it becomes easier to lose electrons.

How does reactivity change for nonmetals across a period?

For nonmetals, reactivity increases across a period as elements become more likely to gain electrons.

Why does reactivity decrease for metals across a period?

Reactivity decreases for metals across a period as increased nuclear charge makes it harder to lose electrons.

Why is francium the most reactive metal?

Francium is highly reactive due to its large atomic size and low ionization energy.

Why do halogens have high reactivity?

Halogens have high reactivity because they have high electronegativity and can easily gain electrons.

How does metallic character change across a period?

Metallic character decreases across a period as elements transition from metals to nonmetals.

How does metallic character change down a group?

Metallic character increases down a group as elements become more metallic in their properties.

What is the relationship between metallic character and electrical conductivity?

Metallic character is directly related to electrical conductivity, as metals are good conductors due to delocalized electrons.

How does the position in the periodic table affect the reactivity of alkali metals?

Alkali metals are more reactive down the group due to their increasing atomic size and lower ionization energies.

What is the most reactive nonmetal and why?

Fluorine is the most reactive nonmetal because it has a high electronegativity and a small atomic radius.

How does reactivity of alkaline earth metals compare to alkali metals?

Alkaline earth metals are less reactive than alkali metals because they have higher ionization energies.

What predicts the type of oxidation states shown by transition metals?

The type of oxidation states is influenced by their ability to lose different numbers of d or s electrons.

What is the trend in the reducing ability of metals down a group?

The reducing ability of metals increases down a group as they lose electrons more easily.

How does the reactivity of halogens change down the group?

Reactivity of halogens decreases down the group due to increased atomic size and a decrease in electronegativity.

Why do some metals not react as expected based on their position?

Transition metals may not follow expected trends due to their complex electron interactions and stable d-subshell configurations.