Define the term metallic bonding.
Sign in and upgrade to Premium to write and mark your own answer.
the strong electrostatic attraction; between positive metal ions and the sea of delocalised electrons
Metallic Bonding
Explain why magnesium has a higher melting temperature than sodium.
Sign in and upgrade to Premium to write and mark your own answer.
magnesium ions (Mg²⁺) have a higher charge than sodium ions (Na⁺) magnesium releases two delocalised electrons per atom while sodium releases only one the electrostatic attraction between Mg²⁺ ions and delocalised electrons is stronger, so more energy is needed to overcome the metallic bonding
Explain why metals conduct electricity in the solid state.
Sign in and upgrade to Premium to write and mark your own answer.
metals contain delocalised electrons that are free to move throughout the lattice; when a potential difference is applied, these electrons drift/carry charge through the metal
Describe the structure of a solid metal, referring to the particles present and how they are arranged.
Sign in and upgrade to Premium to write and mark your own answer.
a giant lattice of positive metal ions arranged in a regular repeating pattern; surrounded by a sea of delocalised electrons; the delocalised electrons come from the outer shell of each metal atom
A student claims that metals melt at high temperatures because “the bonds between atoms are very strong”. Discuss whether this statement is scientifically accurate, and give a more precise explanation using the metallic bonding model. In your answer you should: identify what is imprecise about the student’s statement; describe the correct particles present in a metallic lattice; explain why metals have high melting temperatures using the correct model.
Sign in and upgrade to Premium to write and mark your own answer.
the statement is imprecise because metals do not contain individual atoms bonded in pairs; they contain a giant lattice of positive metal ions, not neutral atoms the term “bonds between atoms” is misleading because metallic bonding is not localised between two atoms like a covalent bond a metal consists of a giant lattice of positive metal ions surrounded by a sea of delocalised electrons metallic bonding is the strong electrostatic attraction between the positive metal ions and the delocalised electrons this attraction acts throughout the entire lattice in all directions a large amount of energy is required to overcome these many strong electrostatic attractions, so metals have high melting temperatures