covalent bonding chapter 8. introduction the bonds that hold atoms of molecules together are...

Covalent Covalent BondingBonding

Chapter Chapter 88

Introduction

• The bonds that hold atoms of molecules together are fundamentally different from those of ionic compounds.

• The types of atoms that comprise molecules are more limited than ions.

• The properties of molecules are different from ionic compounds.

• These properties are a result of the interactions between molecules.

Molecular CompoundsMolecular CompoundsSection 8.1Section 8.1

• Molecules and Molecular Compounds

• Molecular Formula

Different Compounds Have Different Bonding Interactions

Noble gas:No interactions

Ionic compound:Ionic Bonds

Metal:Metallic Bonds

How about the following compounds?

What type ofinteractions hold these compounds together?

I.) Molecules and Molecular Compounds

Molecules: A neutral group of atoms joined together by covalent bonds.

Molecular Compound: A compound composed of molecules.

Water is a molecularcompound

Made up of many molecules of water.

Covalent Bonds

• No atoms give up their electrons completely, nor does any atoms take electrons.

• You can think of the bond as a “tug of war” between the atoms.

The sharing of electrons between two atoms.

The Covalent Bond

We can use Lewis dot structures to show the sharing of electrons.

Molecules Are Created from Covalently Bonded Atoms

Properties of Molecular Compounds

• All the molecules of a given molecular compound are the same.

• Low melting points and boiling points

• Gases or liquids at room temperature

• Composed of atoms of two or more non-metals.

II.) Molecular Formula

• A molecular formula shows how many atoms of each element a molecule contains.

• Subscripts after each symbol indicates the number of atoms of the element are in the molecule.

• The subscripts are not necessarily the lowest whole-number ratios.

• Does not give any information about the molecular compounds structure.

The chemical formula of a molecular compound.

Let’s look at some formulas for molecular compounds.

1. NO

2. NH3

3. CH4

4. H20

5. N2H2

How many atoms of each element are present in each molecular compound?

The Nature of The Nature of Covalent BondingCovalent Bonding

Section 8.2Section 8.2• The Octet Rule in

Covalent Bonding

• Single Covalent Bonds

• Double & Triple Covalent Bonds

• Bond Dissociation Energies

I.) The Octet Rule in Covalent Bonding• Atoms will strive to obtain the electron

configuration of noble gases, if they can.

ns2np6

• In covalent bonding, electron sharing usually occurs so that atoms attain the electron configuration of noble gases. There are exceptions, however.

• Metals & metalloids of Group 4A, 5A, 6A, and 7A will form covalent bonds to meet their octet.

Three Types of Covalent Bonds

• Single bonds, double bonds, and triple bonds.

• These different types of bonds are based on the number of electrons shared between to atoms.

• Each type of bond has different characteristics– Bond length, bond strength

II.) The Single Covalent Bond

• A single bond can be represented as two dots between two atoms or a single dashed line between them.

• We can use a structural formula to describe the bonding between atoms.

A covalent bond formed when two atoms share one pair of electrons.

Let’s see how hydrogen forms it’s bond.

Let’s see how water forms its bonds.

Let’s see how methane forms its bonds.

Sample Problem

Write the structural formulas for the following molecules.

1.F2

2.H2O2

3.Cl2

Class Problem

Write the structural formulas for the following molecules.

1.I2

2.PCl3(Class Problem #5)

What happened with the electrons that did not participate in bonding?

• These unshared electrons are known as lone pairs and are represented as two dots around the molecular compounds.

Let’s examine this with water.

III.) Double Bond and Triple Bonds

• Electrons are shared so that both atoms of the double bond can obtain a noble gas configuration.

Double Bond: A covalent bond formed when two atoms share two pairs of electrons.

Sample Problem

Try drawing the structural formulas for the following double bonded compounds.

1.Formaldehyde (CH2O)

2.Ethylene (C2H4)

• Again, the sharing occurs so that both atoms can obtain an octet in their outer-most (valence) energy level.

Triple Bond: A covalent bond formed when two atoms share three pairs of electrons.

Sample Problem

Try drawing the structural formulas for the following triple bonded compounds.

1.Hydrogen cyanide (CHN)

2.Ethyne (C2H2)

Class Problem

Write the structural formulas for the following molecules.

1.SO2

2.NO3

3.HCN

(Class Problem #6)

Coordinate Covalent BondsCoordinate Covalent Bonds

• The shared electron pair comes from one of the bonding atoms.

• Can show the donated pair in structural formula as arrows that point from the atom donating the pair to the atom receiving the pair.

• Once formed the this type of covalent bond is like any other.

A type of covalent bond in which one atom contributes both bonding electrons.

Sample Problem

Draw the structural formula for the following compounds.

1.Carbon monoxide (CO)

2.Ammonium ion (NH4+)

Polyatomic Ions

• The bonds holding polyatomic ions together are covalent and coordinate covalent bonds.

• Electrons are gained or lost to give the polyatomic ions their charges.

A tightly bound group of atoms that has a positive or negative charge and behaves as a unit.

Class Problem

Write the structural formulas for the following ion: SO3

2-

(Class Problem #7)

Examining Differences in the Examining Differences in the BondsBonds

IV.) Bond Dissociation Energy

The energy required to break the bond between two covalently bonded atom.

A large bond dissociation energy corresponds to a strong covalent bond.

ResonanceResonance

• The actual bonding in such a compound is a hybrid, or a mixture, of the extremes represented by the resonance structures.

A resonance structure occurs when itis possible to draw or more valid electron dot structures that have the same number of electron pairs for a molecule or ion.

Let’s draw the structure for ozone (O3)

Exceptions to the Octet RuleExceptions to the Octet Rule

• For some molecules and ions it is not possible to draw the structures to satisfy the octet rule.

• The octet rule cannot be satisfied for molecules and ions whose total number of valence electrons is an odd number.

• These molecules will have either more than or less than the required octet; many will have unpaired electrons.

Exceptions (cont.)Exceptions (cont.)

• Some molecules with an even number of valence electrons will also violate the octet rule.

• Some atoms expand the octet to include 10 or 12 electrons in their valence shell.

Let’s look at some exceptions.1. Nitrogen dioxide (NO2)

2. Boron trifluoride (BF3)

3. Phosphorus pentachloride (PCl5)

Polar Bonds and Polar Bonds and MoleculesMolecules

Section 8.4Section 8.4• Bond Polarity

• Polar Molecules

• Attractions Between Molecules

I.) Bond Polarity• Covalent bonds differ in the way the

electrons are shared.

• The character of the bonds depends on the kind and number of atoms joined together.

• The type of covalent bonding helps to determine the properties of a molecule.

• Covalent bonds can be polar or nonpolar.

Comparing Comparing Bond TypesBond Types

(Nonpolar)

Nonpolar Covalent Bonds

• Atoms of equal “strength” pull on the electrons.

• Identical atoms share electrons equally.

• H2, O2, N2 are examples.

Polar Covalent Bonds• A covalent bond in

which the electrons are not shared equally.

• The “stronger” atom will pull more of the electrons to itself.

Atom’s Strength = Electronegativity

The ability of an atom of an elementto attract electrons when the atom is in a compound. (Chapter 6)

Periodic Trend in Periodic Trend in ElectronegativityElectronegativity

Electronegativity Differences& Bond TypeElectronegativity

Difference Range

Most Probable Type of Bond

Example

0.0 – 0.3 Nonpolar covalent

H-H (0.0)

0.4 – 0.9 Moderately Polar Covalent

H-Cl (0.9)

1.0 – 1.9 Very Polar Covalent

H-F (1.9)

≥ 2.0 Ionic Na+Cl- (2.1)

Use the table to determine the type of bond each pair of atom will form.

1. H, N2. K, Cl3. C, Cl4. Cl,Cl

Sample Problem

Draw the electron dot structure for each

molecule. Identify polar covalent bonds by

assigning slightly positive and slightly

negative symbols to the appropriate atoms.

1. HOOH

2. BrCl

3. HBr

4. H2O

Class Problem

Identify the bonds between atoms of each pair of elements as nonpolar covalent, moderately polar covalent, very polar, or ionic.

a)H and Br

b)K and Cl

c)C and O

d)Br and Br

(Class Problem #8)

II.) Polar Molecules• One end is

slightly negative, the other slightly positive.

• Dipole: A molecule that has two poles.

III.) Attraction Between Molecules• These are the intermolecular forces.

• Intermolecular forces are weaker than ionic or covalent bonds.

• These interactions determines the physical state of molecular compounds at room temperature.

• Three types:– Dipole interactions– Dispersion forces– Hydrogen bonds

Comparing Intermolecular and Intramolecular Forces

Dipole Interactions• These forces occur

between polar molecules.

• The negative ends are attracted to the positive ends.

• These forces are similar to but much weaker than ionic interactions

Dispersion Forces• Weakest of all

interactions• Occurs between

nonpolar molecules.• Induced charges

hold these molecules together.

• Strength of this interaction increases with increasing # of electrons.

Hydrogen Bonds

These are interactions in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom.

• H-bonds are about 5% the strength of a covalent bond.

• These bonds are extremely important in determining the properties of water and many biological molecules.

Covalent Covalent BondingBonding

Chapter Chapter 88The EndThe End