Understanding chemical bonding is crucial for grasping how atoms stick...
Chemistry87 views·Updated 10 Sept 2026·3 pagesUnderstanding Bonding in NAT 5 Chemistry
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emily@emily_wncfw
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Covalent Bonding and Molecules
Ever wondered how water stays together or why oxygen gas exists as O₂? Covalent bonding happens when non-metal atoms share electrons to stick together. The shared electrons create an electrostatic attraction between the positive nuclei and the electron pair - think of it as atoms holding hands through their electrons.
Covalent molecules are small structures with strong bonds inside but weak attractions between different molecules. This explains why water boils at just 100°C - those weak intermolecular forces break easily. These molecules can't conduct electricity because there are no free-moving charged particles floating about.
The shape matters too! Molecules come in four main shapes: linear (like carbon dioxide), angular (like water), trigonal pyramidal (like ammonia), and tetrahedral (like methane). These shapes affect how molecules interact with each other.
Quick tip: Remember that covalent substances dissolve in other covalent solvents - "like dissolves like" is a handy rule!
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Covalent Networks and Ionic Bonding
Not all covalent substances are small molecules. Covalent networks like diamond and graphite are massive structures where strong covalent bonds extend throughout the entire material. This makes them incredibly tough with sky-high melting points - you'd need thousands of degrees to melt diamond!
Ionic bonding works completely differently. When metals meet non-metals, electrons transfer from one to the other, creating oppositely charged ions that attract each other. Picture sodium giving an electron to chlorine to make salt - the resulting ionic lattice is held together by powerful electrostatic forces.
Ionic compounds have high melting points because those electrostatic attractions are seriously strong. They're brilliant conductors when molten or dissolved because the ions can move freely, but they're hopeless as solids since the ions are locked in place.
Remember: Ionic compounds dissolve in water because water molecules can surround and separate the ions!
3
of 3
Metallic Bonding
Metals have their own special bonding trick that explains why they're so useful. Metallic bonding occurs when positive metal ions sit in a "sea" of delocalised electrons that can move freely throughout the structure. Think of it as electrons that don't belong to any particular atom but wander around helping everyone.
This electron mobility is why metals conduct electricity so well - those free electrons can carry current through the material. The strong attraction between positive ions and the electron sea also gives metals their high melting and boiling points.
Unlike ionic compounds, metals don't dissolve in water. The metallic bonding is too strong and doesn't interact well with water molecules, which is why your copper pipes don't dissolve when water flows through them!
Key insight: The "electron sea" model explains almost all metallic properties - conductivity, strength, and insolubility all come from those mobile electrons!
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Chemistry87 views·Updated 10 Sept 2026·3 pagesUnderstanding Bonding in NAT 5 Chemistry
E
emily@emily_wncfw
Understanding chemical bonding is crucial for grasping how atoms stick together to form everything around you. There are three main types of bonding - covalent, ionic, and metallic - each with unique properties that determine how substances behave in the...
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Covalent Bonding and Molecules
Ever wondered how water stays together or why oxygen gas exists as O₂? Covalent bonding happens when non-metal atoms share electrons to stick together. The shared electrons create an electrostatic attraction between the positive nuclei and the electron pair - think of it as atoms holding hands through their electrons.
Covalent molecules are small structures with strong bonds inside but weak attractions between different molecules. This explains why water boils at just 100°C - those weak intermolecular forces break easily. These molecules can't conduct electricity because there are no free-moving charged particles floating about.
The shape matters too! Molecules come in four main shapes: linear (like carbon dioxide), angular (like water), trigonal pyramidal (like ammonia), and tetrahedral (like methane). These shapes affect how molecules interact with each other.
Quick tip: Remember that covalent substances dissolve in other covalent solvents - "like dissolves like" is a handy rule!
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Covalent Networks and Ionic Bonding
Not all covalent substances are small molecules. Covalent networks like diamond and graphite are massive structures where strong covalent bonds extend throughout the entire material. This makes them incredibly tough with sky-high melting points - you'd need thousands of degrees to melt diamond!
Ionic bonding works completely differently. When metals meet non-metals, electrons transfer from one to the other, creating oppositely charged ions that attract each other. Picture sodium giving an electron to chlorine to make salt - the resulting ionic lattice is held together by powerful electrostatic forces.
Ionic compounds have high melting points because those electrostatic attractions are seriously strong. They're brilliant conductors when molten or dissolved because the ions can move freely, but they're hopeless as solids since the ions are locked in place.
Remember: Ionic compounds dissolve in water because water molecules can surround and separate the ions!
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Metallic Bonding
Metals have their own special bonding trick that explains why they're so useful. Metallic bonding occurs when positive metal ions sit in a "sea" of delocalised electrons that can move freely throughout the structure. Think of it as electrons that don't belong to any particular atom but wander around helping everyone.
This electron mobility is why metals conduct electricity so well - those free electrons can carry current through the material. The strong attraction between positive ions and the electron sea also gives metals their high melting and boiling points.
Unlike ionic compounds, metals don't dissolve in water. The metallic bonding is too strong and doesn't interact well with water molecules, which is why your copper pipes don't dissolve when water flows through them!
Key insight: The "electron sea" model explains almost all metallic properties - conductivity, strength, and insolubility all come from those mobile electrons!
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Our AI Companion is a student-focused AI tool that offers more than just answers. Built on millions of Knowunity resources, it provides relevant information, personalised study plans, quizzes, and content directly in the chat, adapting to your individual learning journey.
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