Bonding and physical properties Flashcards
What are the three intermolecular bonds?
Hydrogen bonds
Dipole-dipole
Van der Waals
What is the strongest intermolecular bond?
Hydrogen bond
What are the properties of graphite?
Brittle (arranged in sheets/layers)
Can conduct electricity (each C releases 1 electron into a delocalised sea of electrons)
High melting points (lots of strong covalent bonds therefore lots of energy required to break them)
What are the properties of diamond?
High melting point (higher than graphite. Lots of energy required to break all the bonds)
Cannot conduct electricity (due to no free electrons. Carbon has 4 covalent bonds)
What are the properties of ice?
Low melting point (only Hydrogen bonds need to be broken)
Low density as it freezes (Hydrogen bonds force water molecules apart, decreasing density)
Name 4 giant covalent compounds.
Graphite
Diamond
Silicon dioxide
Ice
What is an ionic bond?
Electrostatic attraction between the oppositely charged ions.
Describe the properties of giant ionic compounds.
High melting points - lots of electrostatic attraction between oppositely charged ions so lots of energy needed to break bonds.
Conducts electricity when dissolved or as a liquid - the ions are free to move and carry a charge
What type of atoms (metal/non metal) is involved in metallic, ionic, covalent bonds?
Metallic bonding - between 2 or more metals
Ionic bonding - between metal and non metals
Covalent bonding - between 2 non metals
What are the properties of metallic substances?
Positive ions surrounded by a sea of delocalised electrons.
Can conduct electricity
They are malleable due to layers
High melting points due to lots of electrostatic attractions.
What are the properties of simple molecular compounds? (Like CO2)
1) Low melting/boiling points.
2) Cannot conduct electricity (due to no free electrons/ions)
