covalent bonding ● covalent bond bonds between two nonmetals. electrons are shared, rather than...
DESCRIPTION
Types of Covalent Bonding Triple Covalent Bond – three pairs of electrons are shared between two nonmetals. – Ex: Nitrogen bonding with NitrogenTRANSCRIPT
Covalent Bonding●Covalent bond – Bonds between two nonmetals. Electrons are shared, rather than transferred.
●Electronegativities are not strong enough to pull electrons away completely, therefore, a covalent bond is formed from sharing electrons
•Molecules – chemical compounds made from covalent bonds • Molecules tend to be soft or brittle• Low melting points• Poor conductors of heat & electricity
Example: Chlorine atoms bonding to form Cl2Cl + Cl → Cl2
Lewis-Dot diagrams for covalent bonds are different than ionic bondsA dash is used to represent a pair of “shared” electrons
Types of Covalent BondingSingle Covalent Bond – One pair of electrons are shared between two nonmetals.
– Ex: Hydrogen bonding with Hydrogen
Double Covalent Bond – Two pairs of electrons are shared between two nonmetals.
– Ex: Oxygen bonding with Oxygen
Types of Covalent BondingTriple Covalent Bond – three pairs of electrons are shared between two nonmetals.
– Ex: Nitrogen bonding with Nitrogen
Quick Tips For BondingGroup 17 Halogens and Hydrogen only form one covalent bond
- one pair of electrons is shared to make a complete octet
Group 15 Nonmetals form three covalent bonds
- one triple bond, or a combination of double and single bonds.
Carbon can form up to four covalent bonds.
- any combination of single, double, or triple bonds
Group 16 Nonmetals form two covalent bonds• A double bond with another non-metal• 2 single covalent bonds
Bond PolarityNonpolar Covalent Bond – The bond created from an equal sharing of electrons.Atoms of the same element have the same electronegativity and produce nonpolar bondsEx. Br2, I2, N2, Cl2, H2, O2, F2Look familiar?
Polar Covalent Bond – Electrons are not shared equally.
- Between two different nonmetals, one will have a higher electronegativity
- the higher electronegativity produces a partial negative charge
- the lower electronegativity has a partial positive charge
- δ-- and δ+ are used to show a partial negative and partial positive charge
ElectronegativityHydrogen: 2.2Fluorine: 4.0