Q.What is the basic difference between the terms 'electron gain enthalpy' and 'electronegativity'?

Fluorine is the most electronegative element.

Electronegativity increases across a period and decreases down a group, so it is greatest at the top-right (excluding noble gases). Fluorine, being small and highly effective at attracting bonding electro …

Fluorine has the highest Pauling electronegativity (4.0).

Electronegativity increases across a period and decreases down a group, so it is greatest at the top-right of the periodic table (excluding noble gases). Fluorine, being small with a high nuclear charge, attracts b …

Diagonal relationship is the close similarity in properties between certain second-period elements and the element diagonally placed to them in the third period.

On moving from left to right in a period atomic size decreases and electronegativity/ionic character changes, while moving down a group has the opposite effect. These two opposing trends partly cancel along a diagonal, so an element of period 2 and the element diagonally below-right of it in period 3 end up with a similar charge-to-size ratio (similar polarising power) and hence similar properties. …

Carbon is the most electronegative of the Group 14 elements listed.

Carbon, silicon, tin and lead all belong to Group 14. Electronegativity decreases down a group because atomic size increases and the valence electrons are farther from, and more shielded from, the nucleus. Carbon, being at the top of the gro …

Fluorine is the most electronegative element in the periodic table.

Electronegativity generally increases across a period (left to right) and decreases down a group, because atoms get smaller and hold their valence electrons — and any shared electrons — more tightly as effective nuclear charge increases and atomic radius decreases. Fluorine sits at the top-right of the main periodic table (excluding noble gases, which normally don't form bonds), giving it the smallest atomic radius among electronegativity-forming elements and the strongest pull on bonding electrons, with …

Fluorine is the most electronegative element.

Electronegativity is the tendency of an atom to attract shared electrons. It increases across a period (rising nuclear charge, smaller size) and decreases down a group. The maximum is reached at the top-right of the periodic table (excluding noble gases), at fluorine, which has a Pauling electronegativity of about 4.0 - higher …

Electronegativity rises across Period 2 as nuclear charge increases and atomic radius shrinks, so carbon (the rightmost element of the four listed) is the most electronegative.

Electronegativity is the tendency of an atom in a molecule to attract the shared pair of bonding electrons towards itself. Within a period, as we move left to right, the nuclear charge increases while the number of shells stays the same, so the outer electrons are held more tightly and electronegativity increases.

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On the Pauling scale, fluorine is assigned electronegativity 4.0, the maximum value used as the reference point for the whole scale.

Electronegativity measures an atom's tendency to attract the shared pair of electrons in a covalent bond toward itself. On the Pauling scale (the most commonly used scale, based on bond energy differences), values range roughly from about 0.7 (for caesium, the least electronegative common element) up to 4.0 for fluorine, the most electronegative element of all.

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