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Periodic Properties
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A chemist is analyzing a new element discovered in Group 1 of the periodic table. They note its high reactivity, especially with water, and predict its metallic character. Given the trends of periodic properties, which of the following statements best explains the expected behavior of this element compared to elements in Group 17 (halogens)?

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A

The new element will have a higher ionization energy than halogens.

B

The new element will have a lower electronegativity than halogens.

C

The new element will exhibit non-metallic character like halogens.

D

The new element will have a larger atomic radius than halogens.

Understanding the Answer

Let's break down why this is correct

Alkali metals are very easy to lose one electron. Other options are incorrect because Misconception: people think heavier elements always need more energy to remove an electron; Misconception: thinking alkali metals look like non‑metals.

Key Concepts

Periodic Properties
Reactivity of Elements
Electronegativity
Topic

Periodic Properties

Difficulty

medium level question

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Deep Dive: Periodic Properties

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Definition
Definition

Periodic properties describe the trends in atomic size, ionization potential, electron affinity, electronegativity, metallic character, and non-metallic character across periods and groups. These properties help in understanding the reactivity and behavior of elements within the Periodic Table.

Topic Definition

Periodic properties describe the trends in atomic size, ionization potential, electron affinity, electronegativity, metallic character, and non-metallic character across periods and groups. These properties help in understanding the reactivity and behavior of elements within the Periodic Table.

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