1. 6.2 Covalent Bonds
A covalent bond is a chemical bond in which two nonmetal atoms share a pair of valence electrons
How are atoms held together in a covalent bond?
The attractions between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond.

2. COVALENT BOND: the FORCE that holds two nonmetal atoms together as a MOLECULE while they SHARE a PAIR of VALENCE electrons (e-).
Held together by attraction between protons (p+) and shared electrons (e-).
MOLECULE: NEUTRAL group of ATOMS that are JOINED together by ONE OR MORE COVALENT BONDS.

3. Covalent Bonds
Sharing Electrons
A hydrogen atom has one electron.
Two hydrogen atoms become stable by sharing their electrons and forming a covalent bond.
When two atoms share one pair of electrons, the bond is called a single bond.

4. There are several ways to show a covalent bond.
Covalent Bonds
There are several ways to show a covalent bond.
Electron dot model - bond is shown by a pair of dots in the space between the symbols for the hydrogen atoms.
Structural formula - pair of dots is replaced by a line.
Electron cloud and the space-filling models show orbitals of atoms overlap when a covalent bond forms.

5. Covalent Bonds
Molecules of Elements
Two hydrogen atoms bonded together form a unit called a molecule.
Molecule is a neutral group of atoms that are joined together by one or more covalent bonds.

6. Covalent Bonds
The hydrogen molecule is neutral because it contains two protons (one from each atom) and two electrons (one from each atom).
A chemical formula can be used to describe the molecules of an element as well as a compound The element hydrogen as a molecule has the chemical formula H2.
The compound that makes a water molecule has the chemical formula H2O.

7. Covalent Bonds
Many nonmetal elements exist as diatomic molecules.
Diatomic means “two atoms.”

8. Multiple Covalent Bonds
When two atoms share three pairs of electrons, the bond is called a triple bond.
Nitrogen has five valence electrons.
In a nitrogen molecule (N2) atoms share three pairs of electrons,
each atom in N2 has eight valence electrons.
Each pair of shared electrons is represented by a long dash in the structural formula NN.

9. Unequal Sharing of Electrons
What happens when atoms don’t share electrons equally?
What factors determine whether a molecule is polar?

10. Unequal Sharing of Electrons
When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial negative charge. The other atom has a partial positive charge.
The type of atoms in a molecule and its shape are factors that determine whether a molecule is polar or nonpolar.

11. Unequal Sharing of Electrons
Except for noble gases, elements on the right of the periodic table tend to have a greater attraction for electrons than elements on the left.
Elements at the top of a group tend to have a greater attraction for electrons than elements at the bottom of a group have.

12. Unequal Sharing of Electrons
Polar Covalent Bonds
In a molecule of an element, the atoms that form covalent bonds have the same ability to attract an electron.
Shared electrons are attracted equally to the nuclei of both atoms.
In a molecule of a compound, electrons may not be shared unequally.

13. Unequal Sharing of Electrons
A covalent compound forms when hydrogen reacts with chlorine.
Chlorine atom has a greater attraction for electrons than a hydrogen atom does.
In hydrogen chloride molecule - shared electrons spend more time near the chlorine atom than near the hydrogen.
A covalent bond in which electrons are not shared equally is called a polar covalent bond.

14. Unequal Sharing of Electrons
Shared electrons in a hydrogen chloride molecule spend less time near the hydrogen atom than near the chlorine atom.

15. Unequal Sharing of Electrons
Polar and Nonpolar Molecules
Can you assume that a molecule that contains a polar covalent bond is polar?
When a molecule has only two atoms, it will be polar.
When molecules have more than two atoms, the answer is not obvious.

16. Unequal Sharing of Electrons
In a carbon dioxide (CO2) molecule, the polar bonds between the carbon atom and the oxygen atoms cancel out because the molecule is linear.

17. Unequal Sharing of Electrons
In a carbon dioxide (CO2) molecule, the polar bonds between the carbon atom and the oxygen atoms cancel out because the molecule is linear.
In a water (H2O) molecule, the polar bonds between the oxygen atom and the hydrogen atoms do not cancel out because the molecule is bent.

18. Unequal Sharing of Electrons
In carbon dioxide, there are double bonds between each oxygen atom and the central carbon atom.
Oxygen has a greater attraction for electrons than carbon, so each double bond is polar.
The carbon-oxygen double bonds are directly opposite each other.
The pulls on the electrons from opposite directions are equal.
The pulls cancel out and the molecule as a whole is nonpolar.

19. Unequal Sharing of Electrons
In a water molecule, there are two single bonds between oxygen and hydrogen.
The bonds are polar because oxygen has a greater attraction for electrons than hydrogen.
The water molecule is bent, the polar bonds do not cancel.
The oxygen side of the molecule has a partial negative charge. The hydrogen side has a partial positive charge.

20. Attraction Between Molecules
How do attractions between polar molecules compare to attractions between nonpolar molecules?
Attractions between polar molecules are stronger than attractions between nonpolar molecules.

21. Attraction Between Molecules
In a molecular compound, forces of attraction between molecules hold them together in liquid or solid form
Attractions are not as strong chemical bonds
But still determine solid/liquid properties
Water boils at much higher temperature (100°C) vs –161.5°C for methane because water molecules are polar molecule while methane is not

22. Attraction Between Molecules
Dashed lines represent attractions between partially positive hydrogen atoms and partially negative oxygen atoms. The symbols – and + are used to indicate a partial charge.

23. Attraction Between Molecules
Attractions among nonpolar molecules are weaker than attractions among polar molecules, but they do exist.
Attractions among nonpolar molecules explain why carbon dioxide can exist as dry ice and why nitrogen can be stored as a liquid at low temperatures and high pressures.

24. What attractions hold two atoms in a molecule together?
Assessment Questions
What attractions hold two atoms in a molecule together?
attraction between ions with opposite charges
attraction between the nuclei of the atoms and shared electrons
attraction between each nucleus and the electrons of the other atom
attraction between the molecule and other molecules

25. What attractions hold two atoms in a molecule together?
Assessment Questions
What attractions hold two atoms in a molecule together?
attraction between ions with opposite charges
attraction between the nuclei of the atoms and shared electrons
attraction between each nucleus and the electrons of the other atom
attraction between the molecule and other molecules ANS: B

26. What determines whether a molecule is polar?
Assessment Questions
What determines whether a molecule is polar?
type of atoms and shape of molecule
mass of atoms and number of valence electrons
type and mass of atoms
ionization energy and number of covalent bonds

27. What determines whether a molecule is polar?
Assessment Questions
What determines whether a molecule is polar?
type of atoms and shape of molecule
mass of atoms and number of valence electrons
type and mass of atoms
ionization energy and number of covalent bonds ANS: A

28. Why does water have a much higher boiling point than methane?
Assessment Questions
Why does water have a much higher boiling point than methane?
Methane molecules are more polar, so its molecules have stronger attractive forces.
Partial charges on the polar water molecules increase attractive forces between molecules.
A water molecule has much more mass than a methane molecule, so water has a higher boiling point.
Water has a higher boiling point because its molecules do not contain carbon atoms.

29. Why does water have a much higher boiling point than methane?
Assessment Questions
Why does water have a much higher boiling point than methane?
Methane molecules are more polar, so its molecules have stronger attractive forces.
Partial charges on the polar water molecules increase attractive forces between molecules.
A water molecule has much more mass than a methane molecule, so water has a higher boiling point.
Water has a higher boiling point because its molecules do not contain carbon atoms. ANS: B