Textbook Question
Which of the following charts shows the general periodic trends for the electronegativities of the representative elements? [Section 8.4]
10. Periodic Properties of the Elements
Periodic Trend: Electronegativity
Multiple Choice
Why is oxygen considered highly electronegative compared to other elements?
A
Oxygen has a high atomic mass and a low number of valence electrons.
B
Oxygen has a large atomic radius and a low effective nuclear charge.
C
Oxygen has a small atomic radius and a high effective nuclear charge.
D
Oxygen has a low atomic mass and a high number of valence electrons.
Verified step by step guidance1
Electronegativity is the ability of an atom to attract electrons in a chemical bond. It is influenced by atomic size and effective nuclear charge.
Oxygen is highly electronegative because it has a small atomic radius, which means the valence electrons are closer to the nucleus, allowing for a stronger attraction.
The effective nuclear charge is the net positive charge experienced by valence electrons. Oxygen has a high effective nuclear charge due to its relatively high number of protons compared to its electron shielding.
A high effective nuclear charge increases the attraction between the nucleus and the valence electrons, enhancing oxygen's ability to attract electrons from other atoms.
Therefore, the combination of a small atomic radius and a high effective nuclear charge makes oxygen highly electronegative compared to many other elements.
Related Videos
Related Practice
