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Chemistry of s, p and d Block Elements Quiz

5 Questions

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Chemistry of s, p and d Block Elements Quiz

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Questions and Answers

What is the trend in metallic radius from Li to Cs?

First increases, then decreases

Decreases

Increases (correct)

Remains constant

How does the ionization energy change down Group 1 elements?

First decreases, then increases

Remains constant

Decreases (correct)

Increases

What effect does the increase in atomic radius have on ionization energy?

No effect

Decreases (correct)

Increases

First decreases, then increases

How does reactivity change as we move down Group 1 elements?

<p>Increases</p> Signup and view all the answers

What must always be considered when writing equations in inorganic chemistry?

<p>Balancing equations</p> Signup and view all the answers

Study Notes

Introduction to s, p, and d Block Elements

Describes physical and chemical properties of elements in s, p, and d blocks.
Aids in identifying trends and patterns in the periodic table.

Group 1 Elements

All Group 1 elements are metals; hydrogen is an exception as a nonmetal.
Exhibits low densities in comparison to most metals.
Valence shell electron configuration of ns1, leading to high reactivity.

Sodium and Potassium Salts

Sodium occurs naturally in salts like NaCl (rock salt) and Na2B4O7·10H2O (borax).
Potassium salts include KCl (sylvite) and KCl·MgCl2·6H2O (carnallite).

Group Trends in Alkali Metals

Alkali metals possess a lustrous appearance.
High electrical and thermal conductivity characterizes these metals.
Softness increases as one moves down the group.
Melting points decrease down the group.
Alkali metals consistently exhibit an oxidation number of +1 in compounds.
Most compounds formed are stable ionic solids.

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Description

Test your knowledge of the physical and chemical properties of s, p, and d block elements in the periodic table. Explore the trends and patterns among these elements and their valence shell electron configurations.