Structure, Bonding, Properties, Energy Changes Flashcards
What are ionic solids made of?
Metals and non-metals
What particles are found in ionic solids?
Ions (cations and anions)
What are the attractive forces in ionic solids?
Ionic / electrostatic bonds (transfer of electrons between atoms)
What are molecular solids made of?
Non-metals
What particles are found in molecular solids?
Molecules
What are the attractive forces in molecular solids?
Weak Intermolecular forces
What are covalent network solids made of?
Non-metals (diamond, graphite, silicon dioxide)
What particles are found in covalent network solids?
Atoms
What are the attractive forces in covalent network solids?
Covalent bonding (sharing of electrons)
What are metallic solids made of?
Metals
What particles are found in metallic solids?
Cations (positively charged ions) + delocalised electrons
Define metallic bonding
Attraction between loosely held valence electrons and cations (positively charged ions) in sea of delocalised electrons
Define ionic bonding
Electrostatic attraction between oppositely charged ions
Define covalent bonding
Bond in which one or more pairs of electrons are shared by two atoms. It’s intramolecular (between atoms within the molecule)
Define intermolecular bonding
Weak attraction between molecules
Explain hardness property
Indicates strong metallic, covalent, or ionic bond - much energy is needed to overcome attraction
Explain high melting point / boiling point
Indicates strong attraction between atoms or ions (metallic, covalent or ionic bond)
Explain brittle property
Indicates ionic bond (when directional forces causes like charged ions to line up, they repel)
Explain low melting point / boiling point
Soft, indicates weak attraction / weak intermolecular forces between molecules (molecular solid)
Explain malleable, ductile property
Indicates non-directional attraction/forces due to metallic bond. Layers of cations slide over one another.
Explain conducts electricity property
Has free moving charged particles (ions). Delocalised electrons in metals (graphite) or ions in molten or aqueous ionic substances. These are called conductors. (Solid ionic substances cannot conduct electricity due to their ions not being able to move freely, so these solids are called insulators)
Explain solubility property
Non-polar substances e.g. I2 dissolve in non-polar solvents e.g hexane due to their attraction being stronger than the weak intermolecular forces.
Polar covalent molecules and many iconic solids dissolve in polar solvents e.g H2O due to attraction between charged particles. Attraction between solvent-solute releases sufficient energy to overcome the solute-solute and solvent-solvent attractions. (Iconic solids are not polar)
Structure of ionic solids
Fixed 3-D lattice of alternating cations (positively charged ions) and anions (negatively charged ions)
Structure of metallic solids
3-D lattice of positively charged metal cations with delocalised electrons bonded to all the metal cations
Malleable meaning
Able to be shaped without breaking
Ductile meaning
Able to be drawn into a thin wire without breaking
Monatomic Structure type’s particles and which substances?
Atoms. Group 0 elements
Simple Molecular Structure type’s particles and which substances?
Molecules. Most non-metals, except group 0
Giant Covalent Structure type’s particles and which substances?
Atoms. Diamond, graphite, silicon, silicon dioxide
Ionic Structure type’s particles and which substances?
Ions. Metal + non-metal compounds (combined)
Metallic Structure type’s particles and which substances?
Ions & delocalised electrons. Metals
