<span>Out of the possible answers for this question, fluorine in the second period is correct. Of the four elements fluorine, chlorine, bromine and iodine, fluorine has the largest first ionization energy, with a Enthalpy number of 1681.0. Of all the elements, helium has the highest first ionization energy figure.</span>
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Answer: A group 1 alkali metal bonded to fluoride, such as LiF.
Explanation:
Electronegativity is defined as the property of an element to attract a shared pair of electron towards itself. The size of an atom increases as we move down the group because a new shell is added and electron gets added up.
1. A strong acid made of hydrogen and a halogen, such as HCl : A polar covalent bond is defined as the bond which is formed when there is a difference of electronegativities between the atoms. Electronegativity difference = electronegativity of chlorine - electronegativity of hydrogen = 3-2.1= 0.9
2. A group 1 alkali metal bonded to fluoride, such as LiF: Ionic bond is formed when there is complete transfer of electron from a highly electropositive metal to a highly electronegative non metal.
Electronegativity difference = electronegativity of fluorine - electronegativity of lithium= 4-1= 3
3. Carbon bonded to a group 6A (16) nonmetal chalcogen, such as in CO: A polar covalent bond is defined as the bond which is formed when there is a difference of electronegativities between the atoms.
Electronegativity difference = electronegativity of oxygen - electronegativity of carbon= 3.5-2.5= 1.0
4. A diatomic gas, such as nitrogen
: Non-polar covalent bond is defined as the bond which is formed when there is no difference of electronegativities between the atoms.
Electronegativity difference = 0
Thus the greatest electronegativity difference between the bonded atoms is in LiF.