IB DP Chemistry: SL复习笔记3.1.5 Periodic Trends: Physical - Electronegativity

• Electronegativity is the ability of an atom to attract a pair of electrons towards itself in a covalent bond
• This phenomenon arises from the positive nucleus’s ability to attract the negatively charged electrons, in the outer shells, towards itself
• The Pauling scale is used to assign a value of electronegativity for each atom

First three rows of the periodic table showing electronegativity values

• Fluorine is the most electronegative atom on the Periodic Table, with a value of 4.0 on the Pauling Scale
• It is best at attracting electron density towards itself when covalently bonded to another atom

Electron distribution in the C-F bond of fluoromethane

Nuclear charge

• Attraction exists between the positively charged protons in the nucleus and negatively charged electrons found in the energy levels of an atom
• An increase in the number of protons leads to an increase in nuclear attraction for the electrons in the outer shells
• Therefore, an increased nuclear charge results in an increased electronegativity

As the nuclear charge increases, the electronegativity of an element increases as well

Atomic radius

• The atomic radius is the distance between the nucleus and electrons in the outermost shell
• Electrons closer to the nucleus are more strongly attracted towards its positive nucleus
• Those electrons further away from the nucleus are less strongly attracted towards the nucleus
• Therefore, an increased atomic radius results in a decreased electronegativity

As the atomic radius increases, the nucleus has less of an attraction for the bonding electrons causing atom A to have a higher electronegativity than atom B

• Electronegativity varies across periods and down the groups of the periodic table

Down a group

• There is a decrease in electronegativity going down the group
• The nuclear charge increases as more protons are being added to the nucleus
• However, each element has an extra filled electron shell, which increases shielding
• The addition of the extra shells increases the distance between the nucleus and the outer electrons resulting in larger atomic radii
• Overall, there is decrease in attraction between the nucleus and outer bonding electrons
• We say the effective nuclear charge has decreased down the group

Electronegativity decreases going down the groups of the periodic table

Across a period

• Electronegativity increases across a period
• The nuclear charge increases with the addition of protons to the nucleus
• Shielding remains the same across the period as no new shells are being added to the atoms
• The nucleus has an increasingly strong attraction for the bonding pair of electrons of atoms across the period
• This results in smaller atomic radii

Electronegativity increases going across the periods of the periodic table

Trends down a Group & across a Period Table