Electronegativity, metallic and non-metallic character

Electronegativity

Electronegativity is the ability of an atom to attract shared electrons in a chemical bond.
Measured on the Pauling scale, where fluorine has the highest value (4.0).
Electronegativity increases across a period from left to right due to increasing nuclear charge and a smaller atomic radius.
Electronegativity decreases down a group as atomic size increases, reducing the pull on shared electrons.
Non-metals like oxygen, nitrogen, and fluorine have high electronegativity values.
Metals like sodium and potassium have low electronegativity values.
Electronegativity differences between two bonded atoms determine the type of bonding (ionic, polar covalent, or non-polar covalent).
It is not defined for noble gases due to their inert nature (except for compounds like XeF₂).
High electronegativity indicates a strong tendency to attract electrons, making an element a strong oxidizing agent.
Electronegativity trends help explain the reactivity and properties of elements in compounds.

Metallic character refers to the tendency of an atom to lose electrons and form positive ions.
It is associated with metals, which are good conductors of electricity and heat.
Metallic character decreases across a period from left to right as ionization energy increases.
Metallic character increases down a group because ionization energy decreases, making it easier to lose electrons.
Elements in Group 1 (alkali metals) and Group 2 (alkaline earth metals) exhibit the highest metallic character.
Transition metals like iron, copper, and zinc have moderate metallic character.
Highly metallic elements are reactive with water and acids, forming hydrogen gas and metal hydroxides.
The metallic nature of elements is directly related to their low electronegativity and ionization energy.
Metallic character is important in determining an element's conductivity and malleability.

Non-metallic character is the tendency of an atom to gain electrons and form negative ions.
It is associated with non-metals, which are poor conductors of electricity and heat.
Non-metallic character increases across a period from left to right due to higher electronegativity and ionization energy.
Non-metallic character decreases down a group as atomic size increases and electron affinity decreases.
Group 17 (halogens) exhibits the highest non-metallic character, with fluorine being the most non-metallic element.
Non-metals like oxygen, sulfur, and phosphorus readily form covalent bonds by sharing electrons.
The non-metallic nature of an element is inversely related to its metallic character.
Non-metallic elements are often found in molecular compounds and exhibit acidic oxides.
Non-metallic character determines an element's oxidizing ability and reactivity with metals.

Electronegativity: Increases across a period, decreases down a group.
Metallic character: Decreases across a period, increases down a group.
Non-metallic character: Increases across a period, decreases down a group.
These trends are inversely related; as metallic character increases, non-metallic character decreases.

Electronegativity trends explain bond polarity and molecular properties.
Metallic and non-metallic characters determine the reactivity of elements in reactions.
Understanding these trends aids in predicting the physical and chemical behavior of elements.
Plays a crucial role in determining the suitability of elements for industrial and technological applications.
Periodic trends are essential for understanding the formation of compounds and their properties.

Electronegativity is highest for fluorine and lowest for cesium.
Metallic character is highest for Group 1 elements like francium.
Non-metallic character is highest for halogens, particularly fluorine.
Understanding these trends is vital for solving questions related to bonding, reactivity, and periodic properties.