QQuestionChemistry
QuestionChemistry
Why does the reactivity of metals increase but that of non-metals decrease as we go down a group in the periodic table?
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Answer
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Step 1:I'll solve this problem by explaining the periodic trends for metal and non-metal reactivity.
Step 2:: Understanding Atomic Structure
The reactivity of elements is fundamentally linked to their atomic structure, specifically: - Electron configuration - Valence electrons - Atomic radius - Ionization energy
Step 3:: Metals - Increasing Reactivity Down a Group
\text{Atomic Radius} \uparrow \implies \text{Electron Loss} \downarrow
For metals, reactivity increases down a group due to: - Increasing atomic radius - Decreasing ionization energy - Easier electron loss Explanation: - As you move down a group, electrons are added to new electron shells - Outer electrons are further from the nucleus - Less energy is required to remove these electrons - This makes metals more reactive because they can more easily form positive ions
Step 4:: Non-Metals - Decreasing Reactivity Down a Group
\text{Atomic Radius} \uparrow \implies \text{Electron Gain} \downarrow
For non-metals, reactivity decreases down a group because: - Increasing atomic radius - Decreasing electron affinity - More difficulty in gaining electrons Explanation: - Larger atomic size makes it harder for outer electrons to be attracted - Valence electrons are less tightly held - Less tendency to form negative ions
Final Answer
Metals become more reactive down a group due to easier electron loss, while non-metals become less reactive due to decreased electron-gaining capability, primarily caused by changes in atomic structure and electron configuration.
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