Topic 2. Bonding, Structure and Properties of Matter Flashcards
What are Ions?
Ions are charged particles formed when atoms lose or gain electrons.
What are Cations (Ions)?
Positively charged ions formed when an atom loses electrons (e.g. Na⁺).
What are Anions (Ions)?
Negatively charged ions formed when an atom gains electrons (e.g., Cl⁻).
How are Ionic compounds formed?
Ionic compounds form when cations and anions bond through electrostatic forces.
What are properties of Ionic compounds?
High melting and boiling points due to strong ionic bonds.
Generally soluble in water.
Conduct electricity when molten or dissolved in water, as ions are free to move.
How does Covalent bonding work?
Covalent bonding involves the sharing of electron pairs between non-metal atoms.
What is a single bond?
One pair of shared electrons (e.g., H₂).
What is a double bond?
Two pairs of shared electrons (e.g., O₂).
What is a triple bond?
Three pairs of shared electrons (e.g., N₂).
What are the properties of Molecular Compounds and how are they formed?
They are formed from covalent bonds; typically have lower melting and boiling points compared to ionic compounds.
What are Polymers?
Large molecules made up of repeating units called monomers, linked by covalent bonds.
What are the general properties of Polymers?
Vary widely based on the structure of the polymer. Generally, they can be flexible, durable, and resistant to chemicals.
What is a giant covalent structure?
An extensive networks of atoms connected by covalent bonds.
Give two examples of giant covalent structures.
Diamond and Graphite
What are the properties of giant covalent structures?
High melting and boiling points, brittle, poor conductors of electricity, three-dimensional and insoluble in water.
Name Allotropes of carbon.
Diamond, Graphite, Fullerenes, Graphene, Carbon nanotubes and Buckyballs.
What are Allotropes of carbon?
Allotropes of carbon are different structural forms of carbon.
What is Metallic Bonding?
The attraction between positively charged metal ions and delocalised electrons.
What are the properties of Metallic Bonding?
Conductor of electricity and heat due to free-moving electrons.
Malleable and ductile because layers of atoms can slide over each other without breaking the metallic bond.
High melting and boiling points
What are the three states of matter?
Solid, Liquid and Gas
What is a Solid?
Definite shape and volume; particles are closely packed in a fixed arrangement and vibrate in place.
What is a liquid?
Definite volume but takes the shape of the container; particles are close but can move past one another.
What is a gas?
No definite shape or volume; particles are far apart and move freely.
What is the change caused by melting?
Solid to Liquid
What is the change caused by freezing?
Liquid to Solid
What is the change caused by evaporation?
Liquid to Gas
What is the change caused by Condensation?
Gas to Liquid
What is the change caused by sublimation?
Solid to Gas directly (without passing through the liquid state)
What is Ionic bonding?
The attraction between a positively charged metal ion and a negatively charged non-metal ion.
What are the properties of a diamond?
Hard, transparent, high melting point and does not conduct electricity.
What are the properties of graphite?
Soft, non-transparent and a conductor of electricity due to delocalised electrons.
What are the properties of graphene?
Very strong, light, flexible, high resistance and excellent conductor of electricity.
What are Fullerenes?
Molecules composed entirely of carbon, arranged in a hollow sphere or tube (e.g., C₆₀ or buckyballs).
