Q. Silicon is classified as

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Q. The greater attractive force due to increasing positive nuclear charge pulls valence shell electrons closer to

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Q. Silicon is in the center of period 3 and has a structure of

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Q. Group 0 doesn't have a covalent radius as they do not form bonds with each other are the atoms of

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Q. Ions which are greater than their original atoms are

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Q. The atomic radius of silicon is

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Q. The conductivity of electric current increases across metals of period 3 from sodium to

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Q. The other measures of atomic radii are

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Q. At room temperature phosphorus and sulfur are

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Q. The melting point of chlorine is

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Q. Cations are much smaller than their

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Q. The elements present in right of silicon are

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Q. The metallic bonding in aluminum is stronger because of the large number of

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Q. Chlorine (Cl₂) is in gas form at

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Q. The distance between two nuclei of the same type of atom is called

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Q. Going across period the first ionization energy

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Q. Every atom of silicon (Si) is held together in a silicon molecule with strong

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Q. In case of electric conductivity, Silicon (Si) is a

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Q. Across the period, the nuclear charge

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Q. 1683 °C is the melting point of

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