C2 Bomding Structure And Properties Of Matter Flashcards
What is an ionic bond, where does it occur and what particles are involved
What it is: An ionic bond is the electrostatic attraction between oppositely charged ions.
Where it occurs: It forms between metals and non-metals.
Particles involved: Positive ions (cations) and negative ions (anions).
What is a covalent bond, where does it occur and what particles are involved
2 non metals
Sharing a pair or pairs of electrons to form a molecule
What is a metallic bond? Where does it occur? What are the particles involved?
What it is: A metallic bond is the attraction between a lattice of positive metal ions and a ‘sea’ of delocalized electrons.
Where it occurs: It occurs within metals.
Particles involved: Positive metal ions and delocalized electrons.
Describe the formation of an ionic bond in terms of electron transfer.
Metal atom loses its electrons. Forming a positive ion.
Non metal gain the electrons forming a negative ion
Electrostatic force of attraction due to opposite charges causes them to form an ionic bond
Describe the structure of a giant ionic lattice
Each positive ion (cation) is surrounded by negative ions (anions), and each negative ion is surrounded by positive ions.
Held together by strong electrostatic forces
Limitations of dots and cross diagrams for an ionic structure
They do not represent the repeating nature of giant ionic lattices
Describe a covalent bond in terms of electron sharing.
A covalent bond is formed when two non-metal atoms share pairs of electrons to achieve a full outer shell of electrons, making them more stable.
The shared electrons are attracted to the nuclei of both atoms, which holds the atoms together, forming a covalent bond.
Describe the structure of a metallic lattice, with reference to positive ions and electrons.
positive metal ions surrounded by a sea of delocalized electrons.
Describe metallic bonding with reference to electrons.
Metal atoms lose their outer shell electrons and become positive ions (cations).
These positive ions are arranged in a closely packed, regular lattice structure.
Delocalized Electrons:
The outer electrons that the metal atoms lose become delocalized, meaning they are free to move throughout the entire structure.
These delocalized electrons are not bound to any specific atom, but instead move around the lattice of positive ions.
Describe the Melting and boiling points of ionic bonds with reference to forces, particles, bonding and structure.
Melting and Boiling Points: Ionic compounds have high melting and boiling points because a large amount of energy is needed to overcome the strong electrostatic forces that hold the lattice together.
what is generally the melting and boiling point of simple molecular structures and why
Simple molecular substances typically have low melting and boiling points because less energy is needed to overcome the weak intermolecular forces between the molecules,
What is the melting and boiling point generally of giant covalent structures and why
The melting and boiling points of giant covalent structures is really high because of the covalent bonds that hold the atoms together.
What is generally the melting and boiling point of metallic structures and why?
Most metals have high melting and boiling points because a lot of energy is required to overcome the strong attraction between the metal ions and the delocalized electrons.
What is generally the melting and boiling point of metallic structures and why?
Most metals have high melting and boiling points because a lot of energy is required to overcome the strong attraction between the metal ions and the delocalized electrons.
What do polymers consist of?
long chains of repeating units called monomers.
