Chemistry SM-1131 Week 15 Lesson 1

Chemistry SM-1131Week 15 Lesson 1

Dr. Jesse ReichAssistant Professor of Chemistry

Massachusetts Maritime AcademyFall 2008

Class Today• Poem• Review Chapter 10• Test Wednesday• Class on Friday- student evals and test returned• I’ll try to make some review sheets, but you should

make your own in case I don’t• Final is on Thursday. Check the schedule to find out

where you are supposed to meet and be.

Poem• “Follow your true north.”

Bonding theories• How bonding works. What hold molecules

together.• Ionic bonding- metal and a non-metal- one

element loses an electron, gains a positive charge, and the other gains an electron and a negative charge. They then become “electrostatically attracted.”

• Covalent- two non-metals- share electrons to obey the octet rule. Form a “chemical bond.”

Lewis Theory• Valence electrons are dots• Every main group element wants 0 or 8

valence electrons around it to be more like a noble gas. (except H which wants 0 or 2 and He which wants 2).

Figuring out Valence• Count up all the S and P electrons in the

highest shell.• Or, look at group number IA=1, IIA=2, IIIA=3,

IVA=4, VA=5, VIA=6, VIIA=7, VIIIA=8

Lewis Dot Theory

Adding electron dots• Normally, I want you to fill out the pattern like

we did above going around in a clockwise or counterclockwise fashion.

• When it’s time to pair electron pair them away from other atoms.

• If you have a central atom and only two side atoms. On the sides pair one up on top and the other on bottom.

Ions• So Lithium has 1 valence Electron. If it loses

that electron it has a +1 charge and 0 valence electrons. We’d write it like this: Li+ and the Lewis Dot would be this:

Li

Ions• Oxygen has 6 valence electrons. It wants

eight. So, typically it gains two electrons. We’ll write it like O2-, and it’s dot structure would be the following.

O

Ionic CompoundsLi +1 O -2

Li2O

Li O Li

What happens if the two Li each lose 1 electron?How many VE will each Li have? The O?Is the Octet Rule satisfied?

Li2O

Li O Li

Ionic Compounds• MgO• Mg+2O-2

• Mg2O2

• MgO

Mg OMg has 0 VE and O has 8 VE. Octet Rule!Don’t draw the arrows!

Ionic Bonding• Notice in all those cases it was between a

metal and a non-metal. The metals lost electrons. The non-metals gained them. Charges were formed. Oppositely charged particle were attracted to each other. That’s how ionic bonding works!

Covalent Bonding• Now, these example are two non-metals.

They will share electrons to fulfill the octet rule. When we draw the line by connecting the dots it’s called a covalent bond. It just means two elements are sharing electrons.

H2• H has 1 valence electron. It wants either 0 or

2. So far, we’ve seen it give or take an electron to get to 0 or 2 valence electrons. This time it’s going to do something different. It’s going to share.

H H we draw it this like: H H

I2• I has 7 valence electrons. It wants either 0 or

8. It’s going to share.

I I we draw it this like: I – I I - I

Bonds have 2 electrons• Because they share electrons when we count

how many electrons each one has we say both get the benefit of the two electrons in the bond.

• H-H each one has 2 electrons• I-I each one has 8 electrons, each I has 3 lone

pairs for 6 electrons, and then we say each one has 2 electrons from the shared bond

Multiple Bonds• O2 has a double bond.• N2 has a triple bond.• I’ll show you why on the board.

Dot Placing Exceptions• Every now and again you hit an exception.• SO2, which was on your packet was an exception.

I had forgotten.• If you fill out dots like normal you end up with an

unpaired electron on both oxygen atoms. You’d think there should be a way to make a bond somehow.

• If you think something should work, but it didn’t, try pairing dots on the central atom facing one of the adjacent elements.

Lewis Dot exceptions• PF5 (P has 10 Ve), SF6 (S has 12 Ve), BF3 (B has

Ve), SO4-2 (S has 12 Ve). PO4-3(P has 10 ve), NO (N has 7 Ve)

• You don’t have to memorize these, but if you see them or anything like them you have to know why it’s an exception to the octet rule.

Resonance• Sometimes molecules have 2 or more ways to

write the exact same thing, but now a double bond is on the left rather than the right and so on.

• These structures are called resonance structures.

• Sometimes a molecule exists as one, then the other, and sometimes it’s in between.

• Electron sloshing.

VSEPR• Linear- straight line• Trigonal Planer- connect outside atoms to

make a triangle• Tetrahedral- 4 corners of a cube- 2 in the

plane and 2 out of the plane• Trigonal pyramidal- looks like a pyramid• Bent- Lewis looks straight, but lone pair(s)

make these bent.

VSEPR• Linear (central atom with a triple bond or 2 double

bonds) • Trigonal planer (three terminal atoms, no lone

pairs, this is the only one where the atom isn’t trying to look tetrahedral)

• Tetrahedral (four terminal atoms)• Trigonal pryamidal (three terminal atoms and one

lone pair)• Bent (1 double bond, a single bond, 1 terminal

atom or 2 single bonds and two lone pairs)

3D• When you draw atoms in the plane of the

paper just use normal lines for bonds.• If you want to draw something coming

towards you draw a wedge as a bond• If you want to draw something going away

from you draw a hashed line as a bond.

Electronegativity• Many of you boneheads didn’t graph this• You won’t know the trends as well• I’ll probably ask for this on the test• It relates back to shielding, atomic radius, and

ionization energy (all of which you should have graphed.

Shielding• As you go across the period the charge

increase, but the shielding does not.• The nucleus is getting more and more positive,

and therefore electrons are getting drawn closer and closer to it.

• That is until the next period is reached, and then the next electron is pushed much further out by a whole new set of elements shielding it from the nucleus.

Atomic Radius• Radius shrinks as you go from left to right

because the effective nuclear charge (how much the electron actually feels a pull towards the center) increases

• As you go down the periodic table each new period gets a new set of shielding and therefore the electrons are further away from the nucleus and the radius expands.

Ionization energy• To ionize means to make an ion. We typically mean

ripping out an electron.• The electron that is the mostly weakly bound is the

one on the far left. If feels the weakest force holding it in place. That atom is easy to let go.

• Across the period the effective nuclear charge is increasing and its pulling electrons closer into it. As you move right it’s harder to dislodge an electron.

• As you go down there is more shielding in the way making it easier to rip out an electron.

Electronegativity• In the top right (F) you have a very strong

nucleus with very little shielding. You have a very strong pull towards F. So strong it can pull neighboring atom’s electrons towards it.

• In the bottom left you have an atom with an enormous amount of shielding and very little effective nuclear charge making it to the valence electron. There is very little pull towards the nucleus.

Tug of War• Electronegativity is like two atoms playing tug

of war in the playground. In general the big kid wins and the little kid goes home crying.

• The big kids are in the top right with the very positive nucleus and little shielding.

• Everyone to the left is a littler kid then the ones on the right.

• For covalent bonds, it’s still sharing, but it’s not an equal sharing.

Dipole moment• When the more electronegative element

starts pulling the electron closer to it we say it kinda gets a negative charge. When the less electronegative element holds onto its electron less we say it kinda gets a positive charge. These aren’t full charges, just partial.

• The electronegative elements get a partial negative, the electropositive gets a partial positive. We call the + and – a dipole.

BF3• F is the most electronegative element. B is

not. F steals electron density from B. Each F has a partial negative charge. The B has a partial positive.

CCl4• Cl is one of the most electronegative

elements. C is not. Watch what happens.

Water

Calculating Bond Type• You can calculate bond types by subtracting a

less electronegative element from the more electronegative element.

• If EN-EP= 0-.4 then it’s a non-polar bond where everything is shared equally (Cl-Cl)

• If EN-EP=.4-2.0 then it’s polar and one is the big kid and one is the little kid (HF, CO2)

• If EN-EP = 2.0+ then it’s ionic. It’s not shared, the EP gave its electron(s) to EN.

A difference• One of those three is not like the other.• BF3, it looks like all the arrows are pulling in

symetrically opposite directions.• CCl4, it looks like all the arrows are pulling in

symetrically oppsotive driections.• H2O, it looks like the H electrons are pulled up• All three have polar bonds, but because H

electrons are only going up and aren’t balanced out the molecule is uneven.

Polarity• Molecules that have polar bonds and are

overall will be asymetrical polar molecules.

Polar vs. Non-Polar• Polar molecules will dissolve in water• Non-Polar will not• Polar Molecules will dissolve salts• Non-Polar will not• Polar Molecules will be more dense and

harder to boil then similar looking non-polar molecules

THE END• Study for test on Wednesday• Get test, posted grades, student eval on Friday• Final on Thursday (I think 2:45pm)• It’s been fun and I’m proud of those of you

who worked your butts off.