bonding Flashcards
What type of elements form ionic bonds?
A metal and a non-metal
What happens to electrons in ionic bonding?
electrons are transferred from the metal to the non-metal
What do non-metals become in ionic bonding?
Negative ions (anions) because the gain more electrons
What do metals become in ionic bonding?
Positive ions (cations) because they loose elsectorn
What holds ionic compounds together?
Strong electrostatic attraction between oppositely charged ions
Do ionic compounds conduct electricity?
only when melted or dissolved, because ions can move
What type of structure do ionic compounds form?
Giant ionic lattice
What type of elements form covalent bonds?
Two non-metals
Do ionic compounds have high or low melting points?
Do ionic compounds have high or low melting points?
What happens to electrons in covalent bonding?
Electrons are shared between atoms
What is a molecule?
A group of atoms joined by covalent bonds
Do simple covalent molecules conduct electricity?
No, because they have no free electrons or ions
Do simple covalent molecules have high or low melting points?
Low melting points
Give an example of a covalent molecule.
Water (H₂O), Oxygen (O₂), Methane (CH₄)
Why is diamond hard?
Each carbon makes 4 strong covalent bonds
What is a giant covalent structure?
A large 3D structure with many covalent bonds, like diamond or graphite
Why does graphite conduct electricity?
It has free (delocalised) electrons between layers
: What type of elements form metallic bonds?
Metals
What happens to electrons in metallic bonding?
Outer electrons are delocalised (free to move)
Do metals conduct electricity?
Yes, because delocalised electrons can move through the structure
What holds metallic bonds together?
Strong attraction between positive metal ions and delocalised electrons
Why are metals malleable (can be shaped)?
Layers of atoms can slide over each other
Do metals have high or low melting points?
High melting points
Why are metals good conductors of heat?
Delocalised electrons transfer energy quickly
What are the three types of bonding?
ionic, covalent, and metallic
What is a delocalised electron?
A free-moving electron not attached to one atom
What is an ion?
A charged atom that has gained or lost electrons
What is the force called that holds ionic bonds together?
Electrostatic attraction
: What type of bonding is in diamond, graphite, graphene, and silicon dioxide?
Giant covalent bonding
How many covalent bonds does each carbon atom make in diamond?
4
Why is diamond hard?
it has a rigid structure with 4 strong covalent bonds per carbon atom
How many covalent bonds does each carbon atom make in graphite?
3
Why can graphite conduct electricity?
It has delocalised electrons that can move between layers
Why is graphite soft and slippery?
Layers can slide over each other due to weak forces between them
What is graphene?
A single layer of graphite (one atom thick)
Name one use of graphene.
Electronics, flexible screens, strong materials
What is silicon dioxide made from?
Silicon and oxygen atoms
Why does silicon dioxide have a high melting point?
it has a giant covalent structure with strong bonds
What is buckminsterfullerene?
Buckminsterfullerene (C₆₀) is a molecule made of 60 carbon atoms arranged in a spherical shape.
How are the carbon atoms arranged in buckminsterfullerene?
The carbon atoms are arranged in hexagons and pentagons.
What is the shape of a buckminsterfullerene molecule?
It has a spherical shape
What are fullerenes?
Fullerenes are molecules made entirely of carbon atoms, and they can have various shapes, such as spheres (buckminsterfullerene) and cylinders (carbon nanotubes).
What is the chemical formula of buckminsterfullerene?
C₆₀ (60 carbon atoms)
What are the main uses of buckminsterfullerene?
t has potential applications in medicine, electronics, and nanotechnology (e.g., drug delivery, light storage).
Does buckminsterfullerene conduct electricity?
No, buckminsterfullerene does not conduct electricity as it is not a metallic substance,
