Explain why the metallic bonds in some metals are stronger than bonds in other metals?

Answer 1

The physical properties of different metals may be rationalized on the basis of intrinsic nuclear charge and number of valence electrons.

The physical characteristics of metals, such as their malleability, ductility, electrical and thermal conductivity, and luster, are explained by metallic bonding.

Certain metals contribute more valence electrons to the metallic network than others. Low melting solids and liquids made of alkali metals only have one valence electron in the metallic lattice.

The #d#-block metals have more valence electrons to contribute, and thus the positive ions in a sea of electrons, become more positive (because they have lost more electrons), and there is a greater density of electron "sea". This is an area where simple chemical considerations lead on to band structure, which I am reluctant (and incompetent!) to discuss.

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Answer 2

Xavier Avery

Stronger metallic bonds are found in metals with more delocalized electrons, smaller atoms, and well-organized structures. Other factors that affect the strength of metallic bonds include the number of electrons available for bonding, the size of the metal atoms, and the arrangement of atoms in the crystal lattice.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.