Ionic, Covalent, Metallic Bonding Flashcards
(25 cards)
What is ionic bonding?
Bonding between a metal and a non-metal involving transfer of electrons.
What particles are involved in ionic bonding?
Positive metal ions and negative non-metal ions.
What holds ions together in ionic bonding?
Strong electrostatic forces between oppositely charged ions.
What is covalent bonding?
Bonding between non-metals involving the sharing of electron pairs.
What is a molecule?
A group of atoms bonded together by covalent bonds.
What are examples of covalent molecules?
Water (H₂O), oxygen (O₂), carbon dioxide (CO₂).
What are properties of covalent molecules?
Low melting and boiling points, do not conduct electricity.
What is a giant covalent structure?
A network of atoms all joined by covalent bonds (e.g., diamond, graphite).
What is metallic bonding?
Bonding between metal atoms involving a ‘sea’ of delocalised electrons.
What holds metallic bonds together?
Electrostatic attraction between positive metal ions and delocalised electrons.
Why do metals conduct electricity?
Because delocalised electrons can move and carry current.
Why are metals malleable?
Layers of atoms can slide over each other.
What is the structure of a metal?
A giant lattice of positive ions surrounded by delocalised electrons.
What is the boiling point of substances with ionic bonds?
High, due to strong electrostatic forces.
Do simple covalent molecules conduct electricity?
No, because they have no free electrons or ions.
What type of elements form covalent bonds?
Non-metals.
What is the difference between a single and a double covalent bond?
A single bond shares one pair of electrons, a double shares two pairs.
What are lone pairs in covalent bonding?
Pairs of electrons not involved in bonding.
What is an example of a giant ionic structure?
Sodium chloride (NaCl).
Why are ionic compounds brittle?
Shifting layers bring like charges together, causing repulsion and shattering.
Why do covalent substances have low melting points?
Weak intermolecular forces between molecules.
Why are alloys harder than pure metals?
Different-sized atoms distort layers, making sliding more difficult.
What is the bonding in graphite?
Covalent bonds within layers and delocalised electrons between layers.
What are some properties of metallic substances?
High melting points, good conductivity, malleability.
