Bonding Flashcards
Explain the Properties of Simple Covalent bonding
Relatively low melting point, soft and brittle, highly volatile
Why are double bonds more unreactive?
The double bonds will have a higher orbital overlap as more electrons are being shared. This causes the covalent bond to be stronger, therefore harder to break
What is a Polar substance?
A substance with high polarity in its bonds, causing a general dipole-dipole attraction throughout the structure
State the three intermollecular forces that can act on a covalent bond, in order from weakest to strongest
Van Der Waals Forces
Dipole-Dipole
Hydrogen Bonding
Describe Van der Waals Forces
An electron disparity causes a difference in electronegativity in the molecule. Instantaneous dipole created. This attracts another particle causing an induced dipole. Larger molecule = More electrons = Higher strength and longer lasting dipole meaning stronger VDW force
Describe Dipole-Dipole Forces
When bonds have a high difference in electronegativity, this causes a charge disparity to form throughout the molecules structure. The partially negative (𝛅⁻) dipole will be attracted to other partially positive (𝛅ᐩ) dipoles causing an intermollecular force throughout the polar material
Describe Hydrogen Bonding
A strong type of Dipole-Dipole attraction. Hydrogen that bonds to F,N,O.
What is Electronegativity?
The ability for an atom to pull electron density towards itself
Factors that affect the Electronegativity of an atom
Shielding - More shielding = less electronegative main level shells inbetween nucleus
Radius - Larger radius = less electronegative more space between nucleus
Nuclear Charge - Higher Charge = more electronegative stronger attraction
Explain the Properties of Ionic bonding
Brittle: any damage to the structure causes disruption of charges causing repulsions
Conducts: when molten or aqueous, ions become free to carry charge in the structure
Giant Ionic lattice formed: Electrostatic attraction between oppositely charged ions
Factors of Ionic molecules melting point
Higher charge difference between ions increases melting point
Smaller ions means stronger EM attraction increasing boiling point
Explain the Properties of Metallic bonding
Sea of delocalised electrons allow for electrical conduction
Malleable (easily molded) and Ductile (drawn into a wire) - atoms slide past each other easily
High melting point - Strong attraction between the positive ions and sea of delocalised electrons
Factors of Metallic bonding melting point
Higher Charge = Higher melting point due to more free electrons
Smaller Atomic Radius = Higher melting point due to less shielding
Explain Co-ordinate bonding
When both electrons in a covalent bond come from one atom instead of both atoms sharing one electron. Atoms in a co-ordinate bond behave the same as covalent bonds.
e.g in ammonium NH+
