Covalent Bonding In Carbon Dioxide | Properties of Matter | Chemistry | FuseSchool
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- čas přidán 7. 06. 2017
- Carbon dioxide is a product of one of the most important chemical reactions in the world: combustion.
Combustion is how a lot of people in the world heat their homes and power their cars. It also unfortunately contributes to the greenhouse effect and global warming. The carbon dioxide molecule is formed from one carbon atom and two oxygens. As an element, carbon only has 4 outer shell electrons and oxygen 6.
Double covalent bonds form between the atoms, where two electrons from each atom are shared making 4 bonding electrons in total. The two groups of bonding electrons in carbon dioxide repel each other and this keeps the oxygen atoms as far away from each other as possible. Carbon dioxide is less reactive than water because it has two bonds with each oxygen. This means you need a lot more energy to break the atoms apart. Carbon dioxide's strong double bonds make it very stable and so whenever there are stray carbon and oxygen atoms flying about, they love to get together and form carbon dioxide.
Like water, the bonds in carbon dioxide are POLAR COVALENT, making the carbon atom delta positive and the oxygens delta negative. Although, unlike water, carbon dioxide is not a polar molecule overall.
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Helped my daughter alot in chemistry
thank you. Explained a lot simply
great.
@ 1:07, the two electrons positions in the two Oxygen atoms are incorrectly located. They suggest that the electrons of Oxygen and Carbon are attracting each other which is wrong in my opinion.
The two electrons should be at the bottom of the circle representing outer shell of Oxygen.
Over all, a very good presentation though.
Thank you for your feedback 😉
thank you!
Good video
Thanks😁
helped thx
How do you break the bond of CO2? I know that photosynthesis does, but could something as simple as Hydrogen break the bonds if you gave enough of it?
please tall it clearly
no
tnx u
How much energy, per mole, would it take to remove CO2 from the atmosphere? Where are you going to get all that energy at the rate you need to stop CO2's effect on the climate? What is the efficiency given the concentration of CO2 in the atmosphere? What percent of the energy spent performs the work of bonding CO2 to remove it from the atmosphere?
Aren't unsaturated bonds more reactive?
thats what i thought
who else is considering drowning themselves in the ocean rn over chemistry? :D