Covalent Radius
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Covalent Radius

• Half the distance between two identical atoms bonded together by a single covalent bond. Nobel gases do not have a covalent radius because they do not form covalent bonds.

Trends:

• Across a period, covalent radius decreases because effective nuclear charge increases (due to an increase in no. of protons and little increase in shielding) therefore shells are pulled closer towards the nucleus.

• Covalent radius increases down a group due to the constant effective nuclear charge and increase in no. of shells at increasing distances from the nucleus.

• Covalent radius is constant across the first row of transition metals because despite an increase in no. of protons across the period, electrons enter the inner 3D subshell, therefore the increase in nuclear charge is shielded so all the transition metals feel the same effective nuclear charge.

Other Notes in this Category

1. Acid Base Character of Period 3 Oxides
2. Acid-Base Character of Group 4 Oxides
3. Covalent Radius
4. Defintions: Electrophile, nucleophile, radical
5. Equations of reactions of period 3 elements with oxygen and chlorine.
6. Ionization Energy and Electron Affinity
7. Ionization Energy and Electron Affinity 2
8. Thermal Stability of gp1 and 2 carbonates.

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