Which atom has the least attraction for the electrons in a bond between that atom and an atom of hydrogen?
(1) carbon
(2)nitrogen
(3)oxygen
(4) fluorine

(1) Carbon

Explanation:

Then we are looking for attraction of electrons in a bond towards one element, we are looking at polar covalent bonds and electronegativity of the compound elements.

Polar Covalent Bonds - A pair of electrons that are bonded and are unequally shared between the 2 elements. It's bond value is from 0.4 < x < 1.7.

Electronegativity - The ability of an atom in a molecule to attract shared electrons to itself. The general trend of increasing Electronegativity is up and to the right of the Periodic Table.

Carbon is Element 6 in Period 2 Group 14.

Nitrogen is Element 7 in Period 2 Group 15.

Oxygen is Element 8 in Period 2 Group 16.

Fluorine is Element 9 in Period 2 Group 17.

Remember our trend for Electronegativity. If that is the case, the Fluorine would be the most electronegative, meaning it would attract shared electrons and hold on to them very strongly. Therefore, it would have a very strong attraction for Hydrogen's lone electron, as Fluorine wants to fill it's valence electron shell fully, from 7 to  8.

Therefore, the least attraction and the least electronegative element in the list is Carbon.

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

your answer is c) plasma

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