Structures and bonding Flashcards
What is metallic bonding?
Due to the fact that metals give away electrons to another atom, there outer electrons become delocalised with the structure, leaving a fixed lattice of positive metal ions which a sea of electrons move in.
What are the characteristics of a metal (not transitional) and why?
-Soft (uniform layers can slide past each other)
-High melting and boiling points (due to the strong electrostatic forces)
-Conductors of electricity ( delocalised electrons)
What are electrostatic forces?
The forces that occur when a positive and negative charge are attracted to each other
What are covalent structures and what are their characteristics?
When two non-metals bond together by sharing electrons on their outer shell. They have high melting and boiling points as it takes a lot of energy to break these covalent bonds
What is the difference/ similarities between graphite and diamond?
Both are made of carbon atoms
Graphite is made when a carbon bonds with two other carbons making layers, this makes graphite slippery.
Diamond is when a carbon bonds with three other carbons making a 3D shape. This makes it harder to break.
Why do substances have different melting/boiling points?
Because their attractive forces vary.
Why do ionic compounds have high melting points?
When a non-metal and a metal react and form an ionic compound, they have a strong electrostatic force between them two, due to the charges they gain from reacting with each other. this means it requires more energy for the ions to be separated resulting in a high melting points as they can’t break away as easily.
What is a covalent bond?
When non-metals bond together by sharing electrons.
