Use your knowledge of electronegativities, but do not refer to tables or figures in the text, to

Use your knowledge of electronegativities, but do not refer...

Key Concepts

Ionic Character

Ionic character describes the extent to which a bond behaves like an ionic bond rather than a covalent bond. When the electronegativity difference between the bonded atoms is high, the electron density is unevenly distributed, resulting in a bond that has a significant ionic character.

Electronegativity

This is a fundamental property of an atom that indicates its ability to attract electrons towards itself when forming a chemical bond. It is essential in understanding how electrons are shared or transferred between atoms in molecule formation.

Electronegativity Difference

This concept refers to the difference in electronegativity between two bonded atoms. A large difference typically results in uneven electron sharing, where one atom pulls electrons away from the other, leading to increased bond polarity and a greater ionic character.

Periodic Trends

Periodic trends, such as changes in electronegativity across periods and groups, play a crucial role in predicting the behavior of atoms in chemical bonds. These trends help in estimating the relative ionic or covalent nature of bonds by giving insights into how electron affinity shifts between different elements.

Transcript

00:01 We're given five different bonds, so ch, f -h, nacl, v -r -h, and kf, and we're trying to figure out which of those have the highest ionic character, largest ionic character.

00:13 So we're going to organize them from least, i -a -c -karacter, i'm just going to call this ic, but no other i'm just talking about i -nic character, to greatest ionic character, right? because we are not allowed to use values, i kind of drew a layout of a periodic table, and just the values that i need, right? we know that the least ionic character is going to be given to us by non -polar covaling compounds.

00:44 And then somewhere in the middle, you're going to have polar covalent.

00:49 And here, you're going to have ionic compounds with a large metallic characteristic.

00:57 So before we even start, i like to draw out or in my periodic table the trends that i know.

01:05 So i know this way, electron negativity increases.

01:12 And that's important, right? i know this way, election negativity decreases.

01:23 I also know that as we go down, mectatic character increases instead of zionization energy, right? so those metals are most likely to give up those electrons, right? in transfer electrons, which will make them ionic, which will make the ionic character really good.

01:52 The ionic character is going to be the ability to transfer elections instead of sharing electrons, right? and very highly electric negative is going to be non -metals, right, are going to be somewhere in here.

02:05 So the first thing you should do, it helps, is to figure out what's going to be ionic and what's going to be covalent.

02:10 So i know that ionic on this side, i have to have an acl and i have to do this.

02:17 Have kf.

02:18 Now we're going to have to switch tomorrow maybe once we figure out.

02:21 So right now i'm just kind of placing them around and then i'm not doing order yet.

02:27 And then on this side i'm going to do covalin.

02:29 So those three are covalent.

02:30 So i have c -h, f -h, and then b -r -h.

02:37 Right.

02:38 So those three and then those two is what i'm comparing.

02:41 Comparing those two to each other and those three to each other because i know zionic, so they're going to be on this side.

02:47 Great is i character and then i know our covalence are going to be on this side with the least ionic character.

02:53 Remember, i .c.

02:54 In this case, it's short for ionic character.

02:58 So we can start with nacl and kf...

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