By means of Lewis structures, represent bonding between the following pairs of elements: (a) Cs

By means of Lewis structures, represent bonding between the...

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the valence electrons of atoms within a molecule. By using dots to indicate electrons and lines to represent bonds, these diagrams help visualize how atoms share or transfer electrons when forming chemical bonds. They are a fundamental tool for predicting the arrangement of electrons, which in turn influences the molecular structure and reactivity.

Ionic Bonding

Ionic bonding occurs when one atom donates one or more electrons to another atom, resulting in the formation of oppositely charged ions. This electrostatic attraction between ions with opposite charges holds them together. Typically, this type of bonding is observed between metals and non-metals, where the difference in electronegativity is large.

Covalent Bonding

Covalent bonding involves the sharing of electron pairs between atoms, allowing each atom to attain a more stable electron configuration. This type of bond is characteristic of interactions between non-metal elements, where atoms have similar electronegativities, leading to shared electron density rather than complete electron transfer.

Electronegativity

Electronegativity is a measure of how strongly an atom attracts electrons in a bond. Differences in electronegativity between bonding atoms determine whether a bond will be more ionic or covalent. A large difference typically leads to ionic bonding due to complete electron transfer, whereas a smaller difference favors covalent bonding through electron sharing.

Octet Rule

The octet rule is a principle stating that atoms tend to form bonds in such a way that each atom has eight electrons in its valence shell, achieving a noble gas configuration. This rule guides the formation of both ionic and covalent bonds as atoms gain, lose, or share electrons to fill their outermost electron shell, thereby gaining chemical stability.

Transcript

00:01 We are given different sets of elements and we're going to combine them together to draw the lewis that structure.

00:06 So the first thing you should do is figure out if the lewis structure is going to be for a nionic compound or for a covalent compound.

00:14 Because for an ionic compound is going to look very different than for a covalent compound.

00:18 For an ionic compound, you're going to have to show a transfer of electrons.

00:23 And then for a covalent compound, you're going to have to show a sharing of electrons.

00:27 So the first thing is cesium and bromine and this is going to be metal and non -metal.

00:34 So it's going to be ionic.

00:35 Another ways to do this is to look at the electronic activity difference and then use that chart with the values to figure out if it's going to be ionic or covalent.

00:46 This one is going to be covalent.

00:49 This is a non -metal with a semi -metal and most of my metals will form covalent -lis dot -like structures.

00:57 That says borne and chlorine is going to be covalent.

01:02 Seism and chlorine is going to be ionic.

01:05 Lithium and oxygen, ionic.

01:07 A good easy way to tell is metal and non -metal.

01:10 Now you have to be careful because i'm like beryllium.

01:13 Barrelium is a metal, but it can form covalent compounds because of the election at 2d difference with some non -metal.

01:19 So you have to be really careful.

01:21 But usually group 1 will form ionic compounds with non -metals.

01:26 That's what it most likely will form.

01:27 Especially how easy it is to remove elections from it.

01:31 And then chlorine and iodine are going to form covalent complex.

01:35 So again, it helps if you look at the lecture negativity difference, and then you can also do it that way.

01:40 All right, but if you're just doing it quick, just look metal, non -metal, metal, metal, non -metal, two non -metals, two non -metal, non -metal and semi -metal, and then metal and non -metal.

01:52 It will work about 90 % of the time.

01:54 So just be careful with something you like barely, or something that is really close together in the correct table.

02:00 Those are very far apart.

02:01 Those are very far apart.

02:03 So with ianic, you have to look at the charges or the number of valence elections.

02:10 So ccm has one valence election.

02:13 Bromene has seven.

02:15 One, two, three, four, five, six, seven.

02:18 Because this is ionic, it means that elections are going to be transferred.

02:21 So election is going to transfer from here to here.

02:24 And when we draw our lose that structure, we have to show that transfer, right? the arrow is not always really easy to show it, so we can draw it like this.

02:34 Cetium will have a positive charge showing that it lost an electron, and then bromine will have a negative charge with a full set of eight electrons to show that it gained an electron...

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