Chemical bonds are the invisible forces that hold everything together...
Chemistry200 views·Updated 31 Aug 2026·4 pagesGCSE Chemistry: Chemical Bonding and Structures Notes
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Covalent Bonding Basics
Covalent bonds form when non-metal atoms decide to share electrons rather than fight over them. Think of it like flatmates sharing the electricity bill - everyone benefits and gets what they need.
The number of electron pairs shared depends on how many electrons each atom needs to fill its outer shell. A single bond shares one pair of electrons, whilst a double bond shares two pairs - like the difference between holding hands and bear-hugging.
There are three main types of covalent structures you need to know. Giant covalent structures like diamond contain billions of atoms all strongly bonded together. Small molecules like water contain just a few atoms bonded together, with different molecules held by much weaker forces.
Key Tip: Remember that covalent bonding only happens between non-metals - metals are too generous with their electrons to share nicely!
2
of 4
Large Molecules and Properties
Large molecules (like polymers) are basically small repeating units joined together in long chains - imagine a paper chain but with atoms. These chains are held together by intermolecular forces that are stronger than those in small molecules.
The structure of covalent compounds determines their properties completely. Giant covalent structures have incredibly high melting and boiling points because you'd need to break those strong covalent bonds - that takes massive amounts of energy.
Small molecules have low melting and boiling points since you only need to overcome weak intermolecular forces, not the actual bonds. They're usually gases or liquids at room temperature. Large molecules sit somewhere in the middle - stronger than small molecules but weaker than giant structures.
Exam Tip: If asked about melting points, always mention whether you're breaking covalent bonds (high energy) or just intermolecular forces (low energy).
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of 4
Ionic Bonding
Ionic bonding happens when metals and non-metals meet - and it's basically atomic robbery. Metal atoms lose electrons to become positive ions, whilst non-metal atoms gain these electrons to become negative ions.
These oppositely charged ions are attracted to each other by electrostatic forces - the same force that makes your hair stick to a balloon. Since this attraction works in all directions, millions of ions arrange themselves in a 3D structure called a giant ionic lattice.
Working out ionic formulae is straightforward once you know the charges. From a bonding diagram, just count how many of each ion you need. For example, magnesium fluoride needs one Mg²⁺ ion for every two F⁻ ions, giving the formula MgF₂.
Memory Trick: Think "opposite attracts" - positive and negative ions stick together like magnets, but atoms of the same charge push apart.
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of 4
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Chemistry200 views·Updated 31 Aug 2026·4 pagesGCSE Chemistry: Chemical Bonding and Structures Notes
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isaac@isaac_pcpe
Chemical bonds are the invisible forces that hold everything together - from the water you drink to the diamond in jewellery. Understanding how atoms share, steal, or pool electrons is key to mastering chemistry and explains why different materials have...
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Covalent Bonding Basics
Covalent bonds form when non-metal atoms decide to share electrons rather than fight over them. Think of it like flatmates sharing the electricity bill - everyone benefits and gets what they need.
The number of electron pairs shared depends on how many electrons each atom needs to fill its outer shell. A single bond shares one pair of electrons, whilst a double bond shares two pairs - like the difference between holding hands and bear-hugging.
There are three main types of covalent structures you need to know. Giant covalent structures like diamond contain billions of atoms all strongly bonded together. Small molecules like water contain just a few atoms bonded together, with different molecules held by much weaker forces.
Key Tip: Remember that covalent bonding only happens between non-metals - metals are too generous with their electrons to share nicely!
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Large Molecules and Properties
Large molecules (like polymers) are basically small repeating units joined together in long chains - imagine a paper chain but with atoms. These chains are held together by intermolecular forces that are stronger than those in small molecules.
The structure of covalent compounds determines their properties completely. Giant covalent structures have incredibly high melting and boiling points because you'd need to break those strong covalent bonds - that takes massive amounts of energy.
Small molecules have low melting and boiling points since you only need to overcome weak intermolecular forces, not the actual bonds. They're usually gases or liquids at room temperature. Large molecules sit somewhere in the middle - stronger than small molecules but weaker than giant structures.
Exam Tip: If asked about melting points, always mention whether you're breaking covalent bonds (high energy) or just intermolecular forces (low energy).
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Ionic Bonding
Ionic bonding happens when metals and non-metals meet - and it's basically atomic robbery. Metal atoms lose electrons to become positive ions, whilst non-metal atoms gain these electrons to become negative ions.
These oppositely charged ions are attracted to each other by electrostatic forces - the same force that makes your hair stick to a balloon. Since this attraction works in all directions, millions of ions arrange themselves in a 3D structure called a giant ionic lattice.
Working out ionic formulae is straightforward once you know the charges. From a bonding diagram, just count how many of each ion you need. For example, magnesium fluoride needs one Mg²⁺ ion for every two F⁻ ions, giving the formula MgF₂.
Memory Trick: Think "opposite attracts" - positive and negative ions stick together like magnets, but atoms of the same charge push apart.
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