Chemical Bonding Flashcards
What are ionic bonds?
They are strong electrostatic forces of attraction between oppositely charged ions.
State what is lattice energy.
It is the heat involved when one mole of a solid ionic compound is formed from its constituent gaseous ions under standard conditions of 298K and 1 atm.
What are metallic bonds?
They are electrostatic forces of attraction between metal cations and the sea of delocalised electrons.
What do you know by covalent bonds?
It is the electrostatic forces of attraction between the localised shared electrons and the positive nuclei.
What is a dative (co-ordinate) bond?
It is a covalent bond in which the shared pair of electrons is provided by only one of the bonded atoms.
How does covalent bond arise from π and** σ** bonds?
Covalent bonding arises from orbital overlap.
σ-bond is formed when valence orbitals overlap head-on with one another.
π-bond is formed when parallel valence orbitals overlap sideways with one another.
What is bond length?
It is the distance between two nuclei in a covalent bond.
What is bond energy?
It is the average energy required to break one mole of covalent bond in the gas phase under standard conditions.
What is electronegativity?
It refers to ability of an atom in a molecule to attract electrons to itself in a bond.
Briefly explain VSEPR (Valence Shell Electron Pair Repulsion) Theory.
Electron pairs (lone and bond pairs) will arrange themselves as far apart as possible so as to minimise repulsion and maximise stability.
Multiple bond is considered to be a single bond.
Lone pair - lone pair repulsion is greatest while bond pair - bond pair repulstion is the least.
Central atom that is more electronegative will give rise to larger electronic repulsion between two bond pairs.
Describe hydrogen bonding.
