Type of Bonds for CO2 (Carbon dioxide)
For CO2 (Carbon dioxide) the type of bonds between atoms are considered covalent (molecular). This occurs when two non-metal atoms bond and electron pairs are shared between atoms. For single bonds one pair of electrons are shared, for double bonds two pairs, and for triple bonds, three pairs are shared. Carbon dioxide has a double bond with each Oxygen atom. Resources for determining type of bonds: CO2 Lewis Structure: https://youtu.be/dD0Xl4acUFg Metals & Non-metals: https://youtu.be/OoooStZQHdA Finding Valence Electrons (element): https://youtu.be/x1gdfkvkPTk How to Draw Lewis Structures: https://youtu.be/1ZlnzyHahvo For CO2 the bonds between the C and O will be polar due to the difference in electronegativity values for C and O. However, because the CO2 molecule is linear and each O atom is on opposite sides, the dipole will cancel and the net dipole for CO2 will be zero. Therefore, the Carbon dioxide molecule will be non-polar.
For CO2 (Carbon dioxide) the type of bonds between atoms are considered covalent (molecular). This occurs when two non-metal atoms bond and electron pairs are shared between atoms. For single bonds one pair of electrons are shared, for double bonds two pairs, and for triple bonds, three pairs are shared. Carbon dioxide has a double bond with each Oxygen atom. Resources for determining type of bonds: CO2 Lewis Structure: https://youtu.be/dD0Xl4acUFg Metals & Non-metals: https://youtu.be/OoooStZQHdA Finding Valence Electrons (element): https://youtu.be/x1gdfkvkPTk How to Draw Lewis Structures: https://youtu.be/1ZlnzyHahvo For CO2 the bonds between the C and O will be polar due to the difference in electronegativity values for C and O. However, because the CO2 molecule is linear and each O atom is on opposite sides, the dipole will cancel and the net dipole for CO2 will be zero. Therefore, the Carbon dioxide molecule will be non-polar.