Patterns in ionization energy

Neutral atoms

have an equal number of protons and electrons

Ionization energy

The energy required to remove an electron from a neutral atom

Ionization energy down the group

Ionization energy down the group decrease because atomic radius increases and shielding affect increases

Ionization energy across the period

Ionization energy increases because atomic size decreases and nuclear charge increases

the gas phase

To avoid the influence of nearby atoms, measurements of ionization energies are made on isolated atoms in the gas phase

Patterns in electronegativity

Electronegativity is a fundamental concept in chemistry that helps us understand how atoms interact with each other to form bonds. This presentation will explore the patterns and trends in electronegativity, providing insights into its impact on chemical behavior

electronegativity

Electronegativity is the ability of atoms to attract electrons within a chemical bond.​

Ionic bonds

Large electronegativity differences result in the transfer of electrons, forming ions and ionic bonds

covalent bonds

Similar electronegativity values lead to the sharing of electrons, creating covalent bonds

Polar covalent bond

Intermediate differences in electronegativity create unequal sharing, resulting in polar covalent bonds

Factors affecting electronegativity

Electronegativity is directly proportional to the nuclear charge and is inversely proportional to the atomic radius

down the group atomic radius

increase

down the group electronegativity

decrease

across the period electronegativity

increase

across the period nuclear energy

increase

across the period no of protons

increase

Atomic size and Electronegativity

As atomic size increases, the distance between the nucleus and valence electrons also increases.

Larger atoms experience a weaker attraction to electrons due to increased distance, resulting in lower electronegativity

atomic size and electronegativity exhibit an inverse relationship, with larger atoms having lower electronegativity

nonpolar covalent

If the electronegativity difference is less than 0.5

polar covalent​

If the ΔEN is between 0.5 and 1.6

Ionic bond

If the ΔEN is greater than 1.7