WebA) Graphite has delocalized pi-electrons over the entire sheet. This delocalization lowers the energy of the system, leading to greater thermodynamic stability. B) In diamond each carbon atom undergoes sp 3 hybridisation and linked to four other carbon atoms by using hybridised orbitals in tetrahedral manner. WebGraphite is smooth slippery and a good conductor of electricity because Each carbon atom is bonded to three other carbon atoms One of the bonds connecting. Grade. …

Why is graphite brittle? - Chemistry Stack Exchange

WebBecause it is electrically conductive, graphite can promote galvanic corrosion. In an oxidative atmosphere, graphite is effective at high temperatures up to 450 °C continuously and can withstand much higher temperature peaks. Graphite is characterized by two main groups: natural and synthetic. WebSep 28, 2024 · Graphite is soft and slippery because its carbon atoms are bound together by weak bonds known as Van der Waal forces. The bonds that connect the carbon … how to show wifi password windows10

What Are The Main Properties of Graphite? - Engineering Choice

WebJan 15, 2009 · Graphite is a good lubricant because of its giant covalent structure that makes it very slippery because layer of carbon atoms can slide over each other. … WebThe answer is friction. Why Friction Occurs Friction occurs because no surface is perfectly smooth. Even surfaces that look smooth to the unaided eye make look rough or bumpy when viewed under a microscope. Look at the metal surfaces in the Figure below. The aluminum foil is so smooth that it's shiny. WebWhy is Graphite soft and Diamond hard if both are pure carbon? Carbon alone forms the familiar substances graphite and diamond. Both graphite and diamond are made only of carbon atoms. Graphite is very soft and slippery. Diamond is the hardest substance known to man. If both are made only of carbon what gives them different properties? how to show willingness to learn