Which of the following has the greatest electronegativity difference between the bonded atoms? A) A strong acid made of hydrogen and a halogen, such as HCl
B) A diatomic gas, such as nitrogen (N2)
C) Cartoon bonded to a group 6A (16) nonmetal chalcogen, such as in Co
D) A group 1 alkali metal bonded to chloride, such as RbCl

D) A group 1 alkali metal bonded to chloride, such as RbCl

Explanation:

Which of the following has the greatest electronegativity difference between the bonded atoms?

A) A strong acid made of hydrogen and a halogen, such as HCl

The electronegativity difference between H and Cl is:

ΔEN = |EN(H)-EN(Cl)| = |2.1-3.0| = 0.9

B) A diatomic gas, such as nitrogen (N₂)

The electronegativity difference between N and N is:

ΔEN = |EN(N)-EN(N)| = |3.0-3.0| = 0.0

C) Carbon bonded to a Group 6A (16) nonmetal chalcogen, such as in CO

The electronegativity difference between C and O is:

ΔEN = |EN(C)-EN(O)| = |2.5-3.5| = 1.0

D) A group 1 alkali metal bonded to chloride, such as RbCl

The electronegativity difference between Rb and Cl is:

ΔEN = |EN(Rb)-EN(Cl)| = |0.8-3.0| = 2.2

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

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