| The atomic radius of an element may be considered to be half the interatomic distance between two adjacent atoms. |
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| In the typical metals the atomic radius decreases as electrons are added to the same shell because of increased electrostatic attraction. |
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| We can define an atomic radius based on the distances separating the nuclei of atoms when they are chemically bonded to one another. |
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| One of the many periodic properties of the elements that can be explained by electron configurations is size, or atomic radius. |
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| When we must be even more specific, we define the size of an atom in terms of its atomic radius, which is one-half the distance between the two nuclei in two adjacent metal atoms. |
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| The forces between an atom and its neighbours may be different in different directions, and thus we may find that no effective value of atomic radius can be found. |
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| As a result, lithium has the smallest atomic radius and francium has the largest. |
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| We could describe their size in terms of their waist measurement, but it is more usual to gauge their size by their atomic radius. |
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| The lattice spacing expanded in the a-direction and shrank in the c-direction by adding Ti and Cr atoms with larger atomic radius into AlN structure, respectively. |
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| The noble gas atoms, like atoms in most groups, increase steadily in atomic radius from one period to the next due to the increasing number of electrons. |
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| Al and V atoms had an atomic radius different from Ti atom. |
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