1. Chapter 6
Bonding

2. Types of Bonding
_______________: a mutual ________ ______________ between the nuclei and valence electrons of different atoms that ________ the atoms together.
___________: chemical bonding that results from the _____________ between cations and anions. Electonegativity difference of _________.
______________: sharing of electron pairs between atoms.
6-2

3. Types of Bonding
The degree to which bonding between atoms is ionic or covalent can be estimated by calculating the difference in the electronegativity of the bonding atoms.
6-3

4. Covalent Bonding
_____________________: a covalent bond in which the bonding electrons are _________________ by the bonded atoms, resulting in a _______________ of electrical charge. Electronegativity difference is _________.
6-4

5. Covalent Bonding

6. Electronegativity difference is
Covalent Bonding
_______________: a covalent bond in which the bonded atoms have an _______________ for the shared electrons. Polar bonds result in a _____________ charge around the ________ _______________ atom (δ-) and a _________________ charge around the _________electronegative atom (δ+).
Electronegativity difference is
between ____________.
6-6

7. Covalent Bonding

8. Practice 1) What type of bond would form between the following atoms?
a) O-H___________________
b) C-H___________________
c) Cl-Cl__________________

9. Covalent Bonding
__________: a neutral group of atoms that are held together by ____________.
_________________: a chemical compound whose simplest units are ____________.
________________: indicates the relative numbers of atoms of each kind in a chemical compound using ________________ and _______________.
_______________: shows the type and numbers of atoms combined in a single molecule of a molecular compound.
6-9

10. Covalent Bonding
_____________: the energy required to _________ a chemical bond and form ___________ isolated atoms
_________: the average _____________ between two bonded atoms.
_______________: only __________ e- of an atom of a particular element are shown, indicated by ______ placed around the _________.
6-10

11. Covalent Bonding
6-11

12. Covalent Bonding
________________: formulas in which atomic symbols represent ______________, dot-pairs or dashes between two atomic symbols represent ____________ in _____________ and dots adjacent to only one atomic symbol represent ____________electrons.
______________: indicates the kind, number, arrangement and bonds but not the _______________ of the atoms in a molecule.
6-12

13. Lewis Structures
6-13

14. Lewis Structures
6-14

15. Practice 2) Draw the Lewis structure for the following molecules:
a) PF3
b) O2
c) CH2Cl2
6-15

16. Structural Formulas
6-16

17. Multiple Bonds
___________: a covalent bond in which ____________ of electrons is __________between two atoms.
____________: two shared pairs (4 e-)
___________: three shared pairs (6 e-)

18. Multiple Bonds Bond Distance H-H 0.075nm F-F 0.128nm Cl-Cl 0.198nm
Br-Br nm
I-I nm
C-N nm
C=N nm
C≡N nm
6-18

19. Resonance Structures
______________: bonding in molecules or ions that cannot be correctly represented by a single Lewis structure.
6-19

20. Ionic Bonding
________________: composed of positive and negative ions that are combined so that the __________ of positive and negative charges ___________.
_____________: the ________ collection of atoms from which an _______ compounds __________ can be established.
6-20

21. Ionic Bonding
______________: composed of ________ and __________ ions that are combined so that the _________ of positive and negative charges are ________.
___________: the _________ collection of atoms from which an ionic compounds formula can be established.
6-21

22. Ionic Bonding
____________: the ______________ of ions in an ionic compound.
_____________: the ____________ when one mole of an ionic compound is formed from ____________.
6-22

23. Bonding Comparison
____________ compounds tend to have ______, ______ and are not as _______ as ionic compounds. Many are __________ at room temp.
_________ compounds tend to have _______, ________ and are ____________. Ionic solutions are _______________ of electricity.
6-23

24. Polyatomic Ions
_______________: a charged group of covalently bonded atoms.

25. Metallic Bonding
_______________: the chemical bonding that results from the attraction between ___________ and the surrounding sea of _______________.

26. Molecular Geometry
________________: whether a molecule is polar or not is determined by the _____________________ and the _________ of the molecule.
_________: _______________________________ states that repulsion between sets of valence-level electrons surrounding an atom causes these sets to be oriented _____________ possible.
6-26

27. Common Molecular Shapes
Molecular Geometry
Common Molecular Shapes
__________: The atoms of a linear molecule are connected in a ________line. *__________ atom molecules!
All 2 atom molecules are linear (O2, HCl). Many 3 atom molecules are also linear. (CO2)
6-26

28. Molecular Geometry
______________: Molecules have a triangular, bent shape.
*_____________ molecules
A central atom Ex. BCl bonded to other atoms.
6-28

29. Molecular Geometry __________: A shape that has four surfaces.
*_________ molecules.
Tripod shaped.
Ex. CH4 All four sides are
identical.
6-29

30. Molecular Geometry _________________:
__________ molecules, no unshared pairs on the central atom.
6-30

31. Molecular Geometry
__________________: _________ molecules, no unshared pairs on the central atom.
6-31

32. Molecular Geometry
______________: The molecule has a central atom that is bonded to three other atoms and has an __________ of valence electrons.
*_________ molecules
Ex. NH3

33. Molecular Geometry
______________: ____________ result in a slightly smaller bond angle, due to an even greater repulsion force.
*___________ molecules
Ex. H2O

34. Practice
3) What shape would the following molecules have and would they be polar or nonpolar:
CH4:
SF6:
NH3:
6-34

35. Hybrid Orbitals
________________________: the mixing of ______________ atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of ________________.
6-35

36. Hybrid Orbitals ~ sp

37. Hybrid Orbitals ~ sp2

38. Hybrid Orbitals ~ sp3

39. Hybrid Orbitals

40. Intermolecular Forces
________________________: forces of _____________ between molecules. The _________________ are between polar molecules.
_________________: is created by ______ but ___________ charges that are separated by a short distance.
6-40

41. Intermolecular Forces
_________________: an intermolecular force in which a hydrogen atom that is bonded to a __________________ atom is attracted to an _________________ of electrons of an ______________ atom in a nearby molecule.
____________________: the intermolecular attractions resulting from the ____________ of electrons and the creation of __________________________.
6-41

42. Ch. 6
The
End!