Ionic vs. Covalent Bonds

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#ChemicalBonds #IonicBonds #CovalentBonds
SCIENCE ANIMATION TRANSCRIPT: In this video, we will compare ionic and covalent bonds. In order to understand ionic bonds, we need to talk about ions first. Atoms are electrically neutral because they have equal numbers of both positively charged protons and negatively charged electrons. However, an atom can become a charged particle called an ion if it gains or loses electrons. If an atom gains electrons, it acquires more negative charge. As a result, it becomes a negatively charged ion. Conversely, if an atom loses electrons, it loses some of its negative charge and becomes a positively charged ion. The only way to get a positively charged ion is to lose negatively charged electrons. Remember, you can't just add a proton to make a positive ion because changing the number of protons would change it into a different element. Now, let's talk about ionic bonds. Notice that this term contains the word ion. That's because ionic bonds create ions out of electrically neutral atoms by the transfer of one or more valence electrons from one atom to another. Further, electrically neutral atoms of elements whose outer shell is less than half filled with valence electrons tend to donate electrons, while atoms whose outer shell is more than half filled tend to attract electrons. For example, sodium and chlorine atoms are electrically neutral. Chlorine, which only needs one electron to fill its outer shell, strongly attracts sodium's single valence electron. So, these elements react to form a chemical bond, creating sodium chloride. Sodium chloride, otherwise known as table salt, is an example of an ionically bonded compound. This is because the electrically neutral sodium atom became a positively charged ion by losing its valence electron. And chlorine became a negatively charged ion by gaining this electron from sodium. So, how do covalent bonds occur? The simplest substance that contains a covalent bond is a molecule of hydrogen gas also known as H2. A hydrogen atom has only one electron in its outer shell, which for this atom is also the shell nearest the nucleus. This shell can hold a maximum of two electrons. So, atoms of hydrogen tend to pair up and share their electrons so that both atoms have their outer shell filled. As you can see, covalent bonds occur when atoms share pairs of electrons. In this molecule, the hydrogen atoms form a single covalent bond. Another example of a covalently bonded molecule is carbon dioxide, or CO2. From its chemical formula, you know that carbon dioxide contains one carbon atom and two oxygen atoms. Carbon has four valence electrons, and both oxygen atoms have six valence electrons. But all three atoms would need eight electrons to fill their outer shells. So, each oxygen atom shares a pair of electrons with the pair of electrons in carbon. This results in two double covalent bonds where two pairs of electrons are shared between each atom. To summarize, the two main types of chemical bonds are ionic bonds and covalent bonds. In ionic bonds, one or more electrons are transferred from one atom to another. In covalent bonds, one or more pairs of electrons are shared between atoms. [music]
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[@80lala08]

note, for me:
the electrons circle around the nucleus which is why electrons in covalent bonds move around freely in both atoms

[@jhittiwakeeampai8623]

Thank you for video. It's easiest to understand.

[@Nih-Shabd]

Nice info 👍

[@maggiemurph]

Thank you so much for video! It deserves a much more subscribers .

[@harlensmichell1463]

Honestly, where were these video all my life? This is the easiest i've ever understood this; (this my 4th go around on biology lol)

[@syedabuhuraira9022]

Splendid

[@prem5864]

2:26 one electron to fill its outer shell ?? but 3rd ring maximum capacity is 18, right ? So what do u mean by to fill it’s outer shell ?

[@user-gu3gm5de7v]

Probably too late for this answer but here it is anyway. The outer shell he is referring to is the M-shell bcos the 17th electron is occupied in the 3p orbital(which is part of the M-shell) if you follow Hund's rule. 1s2, 2s2, 2p6,3s2, 3p5 = 2+2+6+2+5=17. So, Chlorine is more than half filled and thus attracts electron. It needs only one more electron to complete the 3p orbital and thus the "outer shell". It has this tendency bcos it reduces the overall energy of the atom, but you don't need to know this as it requires QM treatment. Anyway, that is your answer, hope it helps. If it doesn't and you are still sceptical then reading a bit about the QM treatment of Hydrogen atoms and subsequently about the quantum numbers n,l,m_l and m_s should help you bridge the gap between Physics and Chemistry, at least on the atomic scale. If you can differentiate between shells and orbitals then that would also help you answer this question but then again, the fundamentals lie in the quantum numbers.

[@prem5864]

@@user-gu3gm5de7v nice

[@preciseloki1556]

Which bond has a greater bond energy Ionic or covalent

[@4b25yeungyuenho5]

Covalent