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Chapter 2 - Models Of Bonding & Structure

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Atom Symbol

Chapter 1 - Models Of The Particulate Nature Of Matter

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 Globe with Meridians

Chapter 3 - Classification Of Matter

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Fire

Chapter 4 - What Drives Chemical Reactions?

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Rocket

Chapter 5 - How Much, How Fast & How Far?

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Test Tube

Chapter 6 - What Are The Mechanisms Of Chemical Change?

Metallic bonds are like a glittering sea of electrons 🌊. Imagine a busy beach, where the sand particles are metal cations and the ocean is a pool of freely moving electrons - that&#39;s metallic bonding!

📍 Attraction Force: The stronger the attractions between the cations (sand particles) and delocalized electrons (the ocean waves), the stronger the bond.

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📍 Ionic Radius: Think of the ionic radius as the space a cation takes up on our beach. Bigger space? Weaker bond! Smaller space? Stronger bond!

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📍 Ionic Charge: Imagine if the sand particles had a superpower and attracted the ocean even more! The stronger their power (ionic charge), the stronger the bond.

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📍 Electron Density: Think of this as how packed our ocean (of electrons) is. A super crowded beach has stronger bonds because there are more electrons around.

✨ Group 1 Metals Showdown: Lithium vs. Sodium vs. Potassium!

<ul>
	<li>As you move down the group (from lithium to potassium), the melting and boiling points decrease.</li>
</ul>

🍉 Real-world example: Imagine a string of fairy lights. Closer bulbs light up brighter and faster. Lithium&#39;s atoms are closer (smaller ionic radius) so they bond stronger and have a higher melting point. As we go down, the bulbs (atoms) get further apart, making the bond weaker and decreasing the melting point.

<ul>
	<li>Across the period, melting and boiling points increase.</li>
</ul>

🔍 Why?

<ul>
	<li>Ionic Radius: The atoms get closer (smaller radius) as you move across. Remember our fairy lights? Closer bulbs light up brighter! So, stronger bonds.</li>
	<li>Ionic Charge: The attraction power of our sand particles gets stronger as you move across. More attraction? You guessed it, stronger bond!</li>
	<li>Number of Delocalized Electrons: Aluminium contributes three electrons to our ocean, while sodium adds just one. Imagine three waves hitting the shore versus one; which one&rsquo;s stronger?</li>
</ul>

🍪 Real-world example: Let&#39;s think of metallic bonding as a cookie recipe. Sodium is like adding one chocolate chip to the cookie dough, while aluminium is like adding three! More chips make for a richer, more satisfying cookie (or in this case, a stronger metallic bond)!

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Remember: Atoms are like the ultimate social butterflies of the chemical world. The way they interact and bond defines their properties. And just like us, their surroundings and &quot;friends&quot; (or electrons, in this case) impact how strong or weak their relationships are!

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🎉 Happy Chemistry-ing! 🎉

Unlock Metallic Bond Strength Secrets!

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Standard Level

Chemistry SL

Chapter 2 - Models Of Bonding & Structure

Unlock Metallic Bond Strength Secrets!

Table of content

Understanding metallic bonds🔗

What affects the strength of metallic bonds?

Unlock the Full Content!

Chapter 2 - Models Of Bonding & Structure

Unlock Metallic Bond Strength Secrets!

Table of content

Understanding metallic bonds🔗

What affects the strength of metallic bonds?

Unlock the Full Content!