Why carbon dioxide is a gas at room temperature in terms of bonding and structure?

Carbon dioxide is made of one carbon atom that is sandwhiched in between two oxygen atoms. The carbon atom is in between each of the two oxygen atoms and there is a double bond between each carbon-oxygen bond (O=C=O). Thus, carbon dioxide is symmetrical. Oxygen is more electronegative than carbon. Therefore, the oxygens pull the electrons towards themselves with the same force on either side of the carbon atom. The symmetry of carbon dioxide and equal pulling...

Carbon dioxide is made of one carbon atom that is sandwhiched in between two oxygen atoms. The carbon atom is in between each of the two oxygen atoms and there is a double bond between each carbon-oxygen bond (O=C=O). Thus, carbon dioxide is symmetrical. Oxygen is more electronegative than carbon. Therefore, the oxygens pull the electrons towards themselves with the same force on either side of the carbon atom. The symmetry of carbon dioxide and equal pulling of oxygen on either side of the carbon results in little to no intermolecular existing within carbon dioxide other than London (dispersion) forces and Van Der Waals. These are very weak intermolecular forces that are overcome at room temperature. Thus, carbon dioxide molecules are able to move freely as a gas.