Bondings Flashcards
How does metallic bonding have attraction?
the electrostatic attraction between the positive ions in a giant metallic lattice and a “sea” of delocalised electrons
Give me 4 properties of metallically bonded material
-They have good electric conductivity (because of the delocalised electrons)
-High meting and boiling points (because of strong bonds)
-Malleability (the ability to bend and be shaped by hammering)
-The Ductility (The possibility to be drawn into wires)
Give me a minimum of 5 properties of Giant Covalent Structures.(Diamond)
-Each carbon atom is attracted by 4 other carbon atoms
-High melting and boiling points
-No delocalised electrons
-Is scratch resistant
-Normally transparent or translucent
-Cannot conduct electricity
-Hard Structure
-It has a “giant lattice’ structure
-Can be used to make cutting tools
Give me a minimum of 5 properties of Giant covalent structures (Graphite)
-Each carbon atom is joined with three other carbon atoms
-High Melting and Boiling Points - Strong covalent bonds within the layers (but the layers are attracted to each other by weak intermolecular forces)
-Contains Delocalised/Free Moving Electrons
-It can be scratched easily
-Opaque/Black
-Can conduct electricity due to free-moving electrons
-Soft - Layers can slide easily
-Layers of hexagonal rings held by weak intermolecular forces
-Uses are for lubricant and electrode in Electrolysis
Give me a minimum of 3 properties of giant covalent structures (Silicon (IV))
-The structure of Silicon (IV) Oxide is similar/resemblance to that of a diamond.
-Hard Structure
-High melting and boiling point - More energy to overcome
-Rigid Tetrahedral Structure
-Does not conduct electricity
What are covalent bonds? And why do they happen?
Covalent bonding is a type of chemical bonding that involves the sharing of electron pairs between atoms. This sharing of electrons allows atoms to achieve a more stable electron configuration, typically by filling their outer electron shells. Covalent bonds occur when atoms have similar electronegativities and are able to share electrons in order to achieve a more stable state. This type of bonding is typically seen in nonmetallic elements.
Covalent compounds properties do list thee shall atleast 1
-The intermolecular forces in covalent compounds (the gap in the are weak but have strong covalent bonds.
-Covalent Compounds have low melting and boiling point. They require less energy to break the weak intermolecular forces (same as attractive forces).
-Poor Electrical Conductivity - No free electrons or ions present to carry an electrical current
Give me the properties of ionic compounds atleast 3
-High Boiling and Melting Point: A lot of energy is needed to overcome the strong electrostatic forces between oppositely charged ions
-Good Electrical Conductivity when molten or aqueous:
-As the charges flow, ions can move freely in an aqueous/molten state.
- Ions are not free to move when in a solid state, as the charges cannot flow.
-Brittle (Easily breaksdown and turns into a powder like state)
-Low Volatility (The substance easily evaporates in low tempretures)
When states change from solid to gas,and gas to solid what do we call them?
Solid to Gas:Sublimation
Gas to Solid:Deposition
