What Determines Atomic Bonding: Ionic, Covalent, or Polar Covalent?

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In summary, ionic bonding involves the transfer of electrons between atoms, covalent bonding involves the sharing of electrons, and polar covalent bonding involves unequal sharing of electrons due to differences in electronegativity. The type of bonding depends on the difference in electronegativity between atoms. The size of atoms can affect atomic bonding, with smaller atoms having stronger bonds and larger atoms having weaker bonds. Examples of compounds with different types of bonding include sodium chloride (ionic), water (covalent), and hydrogen fluoride (polar covalent). The strength of the bond differs between ionic, covalent, and polar covalent compounds, with ionic bonds being the strongest and polar covalent bonds being stronger than
  • #1
kasse
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Is there any rule that I can use to determine if an atom will consist of ionic bondings, covalent bondings or polar covalent bondings? I'm thinking of difference in electronegativity on the Pauling scale.
 
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  • #2
you mean a compound?!

the electronegativity difference should be more than 1.7 for the compound to be ionic.
 
  • #3
also, when there is an ion of high charge density(e.g. in AlCl3), covalency may occur.
 

What is the difference between ionic, covalent, and polar covalent bonding?

Ionic bonding involves the transfer of electrons from one atom to another, creating cations and anions that are held together by electrostatic forces. Covalent bonding involves the sharing of electrons between atoms, resulting in the formation of molecules. Polar covalent bonding is a type of covalent bonding where the shared electrons are not equally shared due to differences in electronegativity, resulting in a slightly positive and slightly negative end to the molecule.

What determines the type of bonding that occurs between two atoms?

The type of bonding that occurs between two atoms is determined by the difference in electronegativity between the atoms. If the difference is large, ionic bonding will occur. If the difference is small, covalent bonding will occur. If the difference is intermediate, polar covalent bonding will occur.

How does the size of atoms affect atomic bonding?

The size of atoms can affect atomic bonding in several ways. Smaller atoms tend to have stronger bonds due to their smaller atomic radius and increased nuclear charge, making it easier for them to attract and hold onto electrons. Larger atoms, on the other hand, have weaker bonds due to their larger atomic radius and decreased nuclear charge.

What are some examples of compounds with ionic, covalent, and polar covalent bonding?

Examples of compounds with ionic bonding include sodium chloride (NaCl) and magnesium oxide (MgO). Examples of compounds with covalent bonding include water (H2O) and methane (CH4). Examples of compounds with polar covalent bonding include hydrogen fluoride (HF) and ammonia (NH3).

How does the strength of the bond differ between ionic, covalent, and polar covalent compounds?

The strength of the bond differs between ionic, covalent, and polar covalent compounds. Ionic bonds are generally stronger than covalent bonds, as the electrostatic forces between oppositely charged ions are stronger than the shared electrons in covalent bonds. Polar covalent bonds are stronger than nonpolar covalent bonds, as the slight charge separation in polar covalent bonds creates stronger electrostatic interactions.

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