metallic bonding

• Metallic bonding is the topic of discussion in this video.
• In a metal, there is a giant lattice of positive ions and delocalized electrons, which hold the particles together through metallic bonding.
• Metals are good conductors of heat and electricity due to their physical properties.
• All the atoms in a metal are in rows, regularly arranged and close together, allowing energy to be transferred through the metal.
• The free electrons in metals can whizz around and carry energy through the metal, making them good conductors of heat.
• Electrons are negatively charged and when they move through the metal, it creates an electrical current, making metals good conductors of electricity.
• Group one elements in the periodic table, such as lithium, sodium, potassium, rubidium, cesium, have a higher melting point than group two elements.
• Group two elements have two delocalized electrons for every atom, while group one elements have one delocalized electron for every atom, contributing to a higher melting point in group two.
• Group two metals have a higher melting point compared to group one elements because the metal ions have more positive charge and there are more free electrons.
• Metallic bonding is the topic of discussion in this video.
• In a metal, there is a giant lattice of positive ions and delocalized electrons, or free electrons, swimming around doing what they want.
• The structure of a metal can be sketched and labeled.
• Metallic bonding holds the ions and particles in a metal together.
• Metals are good conductors of heat and electricity because all the atoms are in rows, regularly arranged, and close together.
• The free electrons in metals can whizz around and carry energy through the metal.
• Electrons are negatively charged and when they move through the metal, it creates an electrical current.
• Metals are malleable and ductile because the layers of atoms can slide over each other.
• Group one elements in the periodic table include lithium, sodium, potassium, rubidium, cesium, and their melting points are decreasing as we go down the group because the atoms are bigger and the distance between the nucleus and the delocalized electrons is bigger.
• Group two elements in the periodic table have two delocalized electrons for every atom and their melting points are higher compared to group one elements because the metallic bonding is stronger.
• Magnesium has one more proton than sodium, so it has a bigger positive charge, which makes the metallic bonding stronger and the melting point higher.