Electronegativity Periodic Trend - Using the Periodic Table to help determine electronegativity!

The video explains electronegativity, the tendency of an atom to attract electrons, using a tug-of-war analogy. It discusses trends in electronegativity on the periodic table, noting it increases from bottom to top and left to right. The video explains these trends using examples, highlighting the role of energy levels and proton count. It emphasizes that energy levels are more significant than nucleus strength when comparing elements. Examples include comparisons between aluminum and gallium, rubidium and iodine, and potassium and phosphorus.

What is electronegativity?

• The ability of an atom to lose electrons

• The tendency of an atom to attract electrons

• The size of an atom

• The number of protons in an atom

Why does electronegativity increase as you move up the periodic table?

• Atoms have larger sizes

• Atoms have more energy levels

• Atoms have more protons

• Atoms have fewer energy levels

Which element is likely to have a higher electronegativity, lithium or sodium?

• It depends on the number of protons

• Both have the same electronegativity

• Lithium

• Sodium

What factor primarily causes electronegativity to increase from left to right across a period?

• Increase in the number of protons

• Increase in energy levels

• Decrease in atomic size

• Decrease in the number of protons

Between rubidium and iodine, which has a higher electronegativity and why?

• Rubidium, because it is larger

• Iodine, because it has fewer energy levels

• Iodine, because it has more protons

• Rubidium, because it has more energy levels