Covalent bond: Difference between revisions
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A covalent bond is a bond in which at least two | A covalent bond is a bond in which at least two [[Electrons|electrons]] are shared between [[Atom|atoms]]. A pair of electrons may be donated from one atom to another forming a [[dative bond|dative covalent bond]]. A covalent bond holds atoms together as it is the attraction of the negatively charged electrons to the positively charged nucleus of both atoms<ref>Structure and Bonding, Jack Barrett, 2001, Chapter 3, page 35, 3.1- Ionic, Covalent and Coordinate (or Dative) Bonding.</ref>. | ||
=== | === <br>Properties of Covalently Bonded Molecules === | ||
<references /> | <br>Covalently bonded molecules have relatively low melting points despite the high strength of the bond due to the weak intermolecular forces holding the solids together. The intermolecular forces can be strengthened when there is a difference in [[Electronegativity|electronegativity]] between the atoms making the bond polar. They don’t usually conduct electricity as the electrons are locked in the bond and aren’t free to flow.<ref>Single Bonds Jim Clark 2000 https://www.chemguide.co.uk/atoms/bonding/covalent.html#top (modified January 2014)</ref> | ||
=== <br>Types of Covalent Bond === | |||
=== <br>Single Bonds === | |||
[[Single_bond|<br>Single bonds]] are formed from the ‘head on’ overlap of [[Orbitals|orbitals]] in the outer shell of the atom in a process called [[hybridisation|hybridisation]] which forms a [[Sigma_bonding|sigma bond]]. Usually one electron is given from each atom but sometimes a pair will be donated from one atom to another with an empty outer orbital. This is called a dative covalent bond. Single bonds are free to rotate. <ref>Single Bonds Jim Clark 2000 https://www.chemguide.co.uk/atoms/bonding/covalent.html#top (modified January 2014)</ref><br> | |||
=== Double Bonds === | |||
<br>Double bonds are formed from the overlap of p-orbitals which overlap sideways. The [[Pi-bonding|pi bonds]] are weaker than sigma bonds but are used together to from the double bond. When the sigma bonds form the p-oribitals are pulled closer together and practically touch<ref>1. Double Bonds Jim Clark 2000 https://www.chemguide.co.uk/atoms/bonding/doublebonds.html (modified September 2012)</ref>. | |||
=== References === | |||
<references /> | |||
How do i add images? Also can the title be changed? | |||
Revision as of 16:06, 17 November 2017
A covalent bond is a bond in which at least two electrons are shared between atoms. A pair of electrons may be donated from one atom to another forming a dative covalent bond. A covalent bond holds atoms together as it is the attraction of the negatively charged electrons to the positively charged nucleus of both atoms[1].
Properties of Covalently Bonded Molecules
Covalently bonded molecules have relatively low melting points despite the high strength of the bond due to the weak intermolecular forces holding the solids together. The intermolecular forces can be strengthened when there is a difference in electronegativity between the atoms making the bond polar. They don’t usually conduct electricity as the electrons are locked in the bond and aren’t free to flow.[2]
Types of Covalent Bond
Single Bonds
Single bonds are formed from the ‘head on’ overlap of orbitals in the outer shell of the atom in a process called hybridisation which forms a sigma bond. Usually one electron is given from each atom but sometimes a pair will be donated from one atom to another with an empty outer orbital. This is called a dative covalent bond. Single bonds are free to rotate. [3]
Double Bonds
Double bonds are formed from the overlap of p-orbitals which overlap sideways. The pi bonds are weaker than sigma bonds but are used together to from the double bond. When the sigma bonds form the p-oribitals are pulled closer together and practically touch[4].
References
- ↑ Structure and Bonding, Jack Barrett, 2001, Chapter 3, page 35, 3.1- Ionic, Covalent and Coordinate (or Dative) Bonding.
- ↑ Single Bonds Jim Clark 2000 https://www.chemguide.co.uk/atoms/bonding/covalent.html#top (modified January 2014)
- ↑ Single Bonds Jim Clark 2000 https://www.chemguide.co.uk/atoms/bonding/covalent.html#top (modified January 2014)
- ↑ 1. Double Bonds Jim Clark 2000 https://www.chemguide.co.uk/atoms/bonding/doublebonds.html (modified September 2012)
How do i add images? Also can the title be changed?