Write the Lewis structure for nitrosyl fluoride, FNO. Using only a periodic table, identify: (a)

step 1 We're drawing the compound nitrousil fluoride, FNO. Now, nitrousil means N -O, and then the fluo

Write the Lewis structure for nitrosyl fluoride, FNO. Using...

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the valence electrons of atoms within a molecule. They depict bonds as lines and lone pairs as dots, helping to visualize the connectivity, electron distribution, and formal charges in the molecule. This tool is essential for predicting molecular geometry and bonding behavior.

Bond Order

Bond order refers to the number of chemical bonds between a pair of atoms. Higher bond orders generally indicate a greater number of shared electrons, which typically results in shorter and stronger bonds. Understanding bond order helps in comparing bond lengths and strengths within molecules.

Electronegativity

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The differences in electronegativity between atoms determine the polarity of a bond; a greater difference usually leads to a more polar bond, which affects the molecule’s reactivity and interactions.

Bond Length and Strength

Bond length is the distance between the nuclei of two bonded atoms, and bond strength is the energy required to break a bond. Generally, bonds with higher orders are shorter and stronger, while single bonds are longer and weaker. This concept is used to predict the relative stability of bonds within a molecule.

Periodic Table Application in Bonding

The periodic table provides crucial information such as atomic size, valence electrons, and electronegativity, which are all used to predict bonding patterns and molecular structures. Using periodic trends, one can infer properties like bond strength, bond length, and bond polarity when analyzing molecules.

Transcript

00:01 We're drawing the compound nitrousil fluoride, fno.

00:06 Now, nitrousil means n -o, and then the fluoride is a fluorine attached to that.

00:13 And the element that's generally in the middle of this is the n, which i believe is the reason that they wrote it f -n -o, is to tell you that that's literally the connection.

00:23 F -n.

00:26 All right.

00:27 Now, to draw out, we're going to need to add up the valence electrons.

00:30 We've got a periodic table already labeled by.

00:32 Column.

00:34 So fluorine has seven valence electrons, nitrogen has five, and oxygen has six.

00:47 So we're working with a total of 14 electrons, or 18, i'm sorry, 18.

00:57 Now we already have our base structure drawn and there's two bonds in that.

01:02 Each bond has two electrons in it.

01:05 So right now we're down to subtract 4 because there's two bonds, two electrons each, we're down to 14.

01:14 We'll fill in the outer valence electrons before we worry about inner ones.

01:19 So the fluorine needs six more, as does the oxygen.

01:26 That takes off 12.

01:27 We've got two left.

01:28 We'll put them on the nitrogen.

01:32 Now, we've used up all our electrons.

01:35 However, nitrogen still doesn't have enough.

01:39 It only has six.

01:40 So we're going to have to do a double bond.

01:42 And we have a couple options.

01:45 We can take a lone pair from the oxygen and move it, or we could take a lone pair from the fluorine and move it.

01:54 One of them will give us this structure, and the other will give us this one.

02:13 And we've got to decide which one it's going to be.

02:17 To do that, we're going to use formal charge.

02:20 We'll take the formal charges of each atom, and then the one that has the best numbers, ideally all zeros or numbers as close to zeros as possible would be the more stable form.

02:30 So it would be the dominant resonant structure.

02:34 Reminder that formal charge equals how many valence electrons the atom would have started with its number from the periodic table minus half of its bonding electrons and all of its non -bonding.

02:55 Whoa.

02:57 Hit the scroll bar.

02:58 Go back.

03:00 There we go.

03:01 Non -bonding.

03:05 That's non -bonding.

03:07 Electrons.

03:08 Okay.

03:09 An easier way to remember it is that formal charge equals the valence minus the sticks, minus the dots for that element.

03:20 All right, so we'll start with our structure on the left.

03:22 First, we'll look at flooring.

03:26 Floring begins its life with seven valence electrons based on its column in the periodic table.

03:32 The same number that we used to add up the valence electrons to begin with.

03:36 Now we're going to subtract off how many sticks or how many bonds are attached to that flooring.

03:41 There are two.

03:44 And then how many dots are on the fluorine? and there are four.

03:49 7 minus 2 minus 4 is plus 1.

03:52 I can tell you right off the bat, this is going to be an awful looastroctor, or awful option.

03:58 Because fluorine is the most electronegative atom there.

04:02 Remember, electronegativity increases as you go up into the right.

04:06 The most electronegatom has the ability to hog electrons.

04:10 There's no way it's going to be positive.

04:13 That would mean it lost electrons.

04:16 But we'll keep going anyway.

04:18 The nitrogen starts its life with five valence.

04:22 It's got three sticks attached to it, and it's got two electrons on it for a zero.

04:29 And then we have oxygen...

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