Bondings

• Covalent bonding is the sharing of electrons between two atoms.
• Ionic bonding occurs when one atom loses an electron to another, resulting in positively charged cations and negatively charged anions that attract each other.
• Metallic bonding involves metal atoms losing their outermost electrons and forming a sea of delocalized electrons held together by electrostatic attraction.
• Ionic bonding occurs when one atom loses an electron to another atom, resulting in positively charged cations (metals) and negatively charged anions (non-metals).
• Metallic bonding involves the attraction between positive metal ions and delocalized electrons.
• Metallic bonding involves metal atoms losing their outermost shell electrons and forming positive ions held together by electrostatic attraction.
• The strength of ionic bonds depends on the size of the ions involved and the distance between them.
• Diatomic includes : O2 N2 Cl2 I2 Br2
• Ionic bonding have higher melting point and boiling point than covalent bonding
• Ionic bonding is non-volatile
• Covalent bond is volatile
• Ionic bonding is soluble in water, insoluble in organic solvent
• Covalent bond is soluble in organic solvent, insoluble in water
• Metallic bonding are conductive to electricity and heat
• Allotropy is the existence of an element in two or more different forms in the same physical state.
• Graphite and diamond have high melting and boiling point. Because a lot of energy is needed to break the bonds.
• Diamond has higher density than graphite because it's tightly packed together while graphite is loosely packed together.
• Graphite is a dark grey, shiny solid
• Graphite conduct electricity  Because it has free electrons
• Graphite is soft because layers are held together by weak forces
• Graphite is parallel flat layers of carbon atoms bonded strongly in hexagonal arrangements.
• Graphite is bonded with weak van der waal's forces
• In graphite each carbon atom is bonded with another 3 carbon in the hexagonal ring
• Uses of graphite : Lubricant, electrodes, pencils
• Diamond is a colourless transparent crystal which sparkles in light
• Diamond does not conduct electricity, because it does not have free electrons
• Diamond is hard because bond are strong
• Diamond is denser than graphite because carbon atoms are packed closer
• In Diamond each carbon is bonded with another 4 carbon atoms in a tetrahedral arrangement
• Diamond is use for cutting tools, jewellery, drill bits
• Silicon dioxide is a giant molecular each silicon is joined by four oxygen atoms. Each atoms joined to two silicon atoms in a tetrahedral arrangement
• Silicon dioxide have high melting point and boiling point. Colourless crystalline. Non conductor of electricity.
• Silicon dioxide insoluble in water
• Silicon dioxide react with alkali so it is acidic
• Metal consist of giant lattice of metal ions in a sea of delocalized electrons
• Metals are malleable and ductile because layers of atoms in metals can slide over each other
• Metals have high melting and boiling points because bonds between metals are very strong