Electronegativity is an element's ability to attract bonding electron pairs in a covalent bond. It depends on an element's atomic radius and number of protons - larger atomic radius and fewer protons result in lower electronegativity as electrons are farther from the nucleus and protons have less attraction. However, full electron shells provide shielding that reduces the effect of more protons on electronegativity.
✔Here is an introduction to the Chemistry of Life, where you will learn about Ionic, Covalent and Metallic bonds. This presentation touches briefly, but it covers the definition of three major types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form due to the transfer of an electron from one atom to another. Covalent bonds involve the sharing of electrons between two atoms. Metallic bonds are formed by the attraction between metal ions and delocalized, or "free" electrons.✔
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✔Here is an introduction to the Chemistry of Life, where you will learn about Ionic, Covalent and Metallic bonds. This presentation touches briefly, but it covers the definition of three major types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form due to the transfer of an electron from one atom to another. Covalent bonds involve the sharing of electrons between two atoms. Metallic bonds are formed by the attraction between metal ions and delocalized, or "free" electrons.✔
Here is a YouTube of this presentation:
➡➡➡https://www.youtube.com/watch?v=8cRQjClbeas&feature=youtu.be
Check out more interesting posts on LabGirl:
➡➡➡ https://www.facebook.com/labgirldzd
Thank you! :)
2. The chemical Bond: Electronic concept of valency. Different types of chemical bond e.g. ionic, covalent, coordinate covalent metallic, dipole, hydrogen bond etc. Theories of covalent bonding and hybridization.
1. Moving down a group, the electronegativity decreases due to the l.pdfsudhinjv
1. Moving down a group, the electronegativity decreases due to the longer distance between the
nucleus and the valence electron shell, thereby decreasing the attraction, making the atom have
less of an attraction for electrons or protons. 2.Trend-wise, as one moves from left to right across
a period in the periodic table, the electronegativity increases due to the stronger attraction that
the atoms obtain as the nuclear charge increases.
Solution
1. Moving down a group, the electronegativity decreases due to the longer distance between the
nucleus and the valence electron shell, thereby decreasing the attraction, making the atom have
less of an attraction for electrons or protons. 2.Trend-wise, as one moves from left to right across
a period in the periodic table, the electronegativity increases due to the stronger attraction that
the atoms obtain as the nuclear charge increases..
2. What is electronegativity?
In a covalent bond between two different elements, the electron density is not
shared equally.
3. What is electronegativity?
In a covalent bond between two different elements, the electron density is not
shared equally.
This is because different elements have differing abilities to attract the bonding
electron pair. This ability is called an element’s electronegativity.
4. What is electronegativity?
In a covalent bond between two different elements, the electron density is not
shared equally.
This is because different elements have differing abilities to attract the bonding
electron pair. This ability is called an element’s electronegativity.
Electronegativity values
for some common
elements. Values given
here are measured on
the Pauling scale.
6. Electronegativity and atomic radius
The electronegativity of an element depends on a combination of two factors:
1. Atomic radius
As radius of an atom increases, the bonding pair of electrons become
further from the nucleus. They are therefore less attracted to the positive
charge of the nucleus, resulting in a lower electronegativity.
7. Electronegativity and atomic radius
The electronegativity of an element depends on a combination of two factors:
1. Atomic radius
As radius of an atom increases, the bonding pair of electrons become
further from the nucleus. They are therefore less attracted to the positive
charge of the nucleus, resulting in a lower electronegativity.
higher electronegativity lower electronegativity
8. Electronegativity, protons and shielding
2. The number of unshielded protons
The greater the number of protons in a nucleus, the greater the
attraction to the electrons in the covalent bond, resulting in higher
electronegativity.
9. Electronegativity, protons and shielding
2. The number of unshielded protons
The greater the number of protons in a nucleus, the greater the
attraction to the electrons in the covalent bond, resulting in higher
electronegativity.
However, full energy levels of electrons shield the electrons in the bond
from the increased attraction of the greater nuclear charge, thus reducing
electronegativity.
10. Electronegativity, protons and shielding
2. The number of unshielded protons
The greater the number of protons in a nucleus, the greater the
attraction to the electrons in the covalent bond, resulting in higher
electronegativity.
However, full energy levels of electrons shield the electrons in the bond
from the increased attraction of the greater nuclear charge, thus reducing
electronegativity.
11. Electronegativity, protons and shielding
2. The number of unshielded protons
The greater the number of protons in a nucleus, the greater the
attraction to the electrons in the covalent bond, resulting in higher
electronegativity.
However, full energy levels of electrons shield the electrons in the bond
from the increased attraction of the greater nuclear charge, thus reducing
electronegativity.
greater nuclear charge
increases
electronegativity…
…but extra shell of
electrons increases
shielding.