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Chemistry15 views·Updated 18 Sept 2026·2 pagesUnderstanding Electronegativity Made Simple
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Understanding Electronegativity
Think of electronegativity as a measure of how greedy an atom is for electrons when it's bonded to another atom. Some atoms are proper electron hogs, whilst others are more generous with sharing.
The pattern is quite straightforward: electronegativity increases across periods (left to right on the periodic table) and decreases down groups (top to bottom). This means fluorine is the greediest element of all!
When two atoms have identical electronegativity values, like in H-H bonds, they share electrons equally. This creates a non-polar covalent bond where neither atom gets preferential treatment. However, when there's a difference in electronegativity, one atom pulls the electrons closer, creating a polar covalent bond with slight positive and negative charges.
Key insight: The greater the electronegativity difference, the more polar the bond becomes. Once the difference exceeds 1.8, the bond becomes ionic rather than covalent!
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Polar Molecules and Molecular Shape
Just because a molecule contains polar bonds doesn't automatically make it a polar molecule - this is where molecular geometry becomes crucial. The key is whether the individual bond dipoles cancel each other out or create a net dipole.
Symmetrical molecules tend to be non-polar because their dipoles cancel out perfectly. Think of it like a tug-of-war where both teams are equally strong. Asymmetrical molecules, however, are typically polar because there's an uneven pull in one direction.
Molecules become asymmetrical when the central atom has lone pairs of electrons or when the terminal atoms are different. Water is a perfect example - its bent shape (caused by lone pairs on oxygen) means the dipoles don't cancel out, making it a polar molecule.
Exam tip: When explaining why water is polar, mention both its asymmetrical shape due to lone pairs AND that the dipoles don't cancel out. This covers both marking points!
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Chemistry15 views·Updated 18 Sept 2026·2 pagesUnderstanding Electronegativity Made Simple
A
Alaine@alaine_uiem
Ever wondered why oil and water don't mix? It's all about electronegativity- how atoms compete for electrons in chemical bonds. Understanding this concept will help you predict how molecules behave and why some substances are attracted to each other...
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Understanding Electronegativity
Think of electronegativity as a measure of how greedy an atom is for electrons when it's bonded to another atom. Some atoms are proper electron hogs, whilst others are more generous with sharing.
The pattern is quite straightforward: electronegativity increases across periods (left to right on the periodic table) and decreases down groups (top to bottom). This means fluorine is the greediest element of all!
When two atoms have identical electronegativity values, like in H-H bonds, they share electrons equally. This creates a non-polar covalent bond where neither atom gets preferential treatment. However, when there's a difference in electronegativity, one atom pulls the electrons closer, creating a polar covalent bond with slight positive and negative charges.
Key insight: The greater the electronegativity difference, the more polar the bond becomes. Once the difference exceeds 1.8, the bond becomes ionic rather than covalent!
2
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Polar Molecules and Molecular Shape
Just because a molecule contains polar bonds doesn't automatically make it a polar molecule - this is where molecular geometry becomes crucial. The key is whether the individual bond dipoles cancel each other out or create a net dipole.
Symmetrical molecules tend to be non-polar because their dipoles cancel out perfectly. Think of it like a tug-of-war where both teams are equally strong. Asymmetrical molecules, however, are typically polar because there's an uneven pull in one direction.
Molecules become asymmetrical when the central atom has lone pairs of electrons or when the terminal atoms are different. Water is a perfect example - its bent shape (caused by lone pairs on oxygen) means the dipoles don't cancel out, making it a polar molecule.
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