Periodicity in Properties-II

The video tutorial covers electron affinity and electronegativity, explaining their definitions, trends, and factors affecting them. Electron affinity can be positive or negative, with halogens having high negative values and noble gases showing positive values. Electronegativity is a measure of an atom's ability to attract electrons in a bond, influencing the type of bond formed. The tutorial discusses how these properties vary across periods and groups in the periodic table, influenced by atomic size, shielding effect, and nuclear charge.

What is the electron gain enthalpy of noble gases typically like?

• High and negative

• Zero

• Low and negative

• Positive

Which element shows a decrease in electron gain enthalpy as you move down Group 17?

• Fluorine

• Chlorine

• Bromine

• Iodine

What is the primary factor that causes the discrepancy in electron affinities across a period?

• Atomic size

• Valence shell electronic configuration

• Shielding effect

• Nuclear charge

What type of bond is formed when two atoms have nearly equal electronegativities?

• Non-polar covalent bond

• Metallic bond

• Polar covalent bond

• Ionic bond

How does electronegativity change as you move from left to right across a period?

• It remains constant

• It increases

• It decreases

• It fluctuates

Which factor does NOT affect the electronegativity of an element?

• Effective nuclear charge

• Atomic size

• Number of valence electrons

• Color of the element

What happens to electronegativity as you move down a group in the periodic table?

• It remains the same

• It decreases

• It increases

• It becomes zero