Chapter 6 Bonding

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

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

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

Covalent Bonding

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

Covalent Bonding

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

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

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

Covalent Bonding 6-11

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

Lewis Structures 6-13

Lewis Structures 6-14

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

Structural Formulas 6-16

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

Multiple Bonds Bond Distance H-H 0.075nm F-F 0.128nm Cl-Cl 0.198nm Br-Br 0.228nm I-I 0.266nm C-N 0.147nm C=N 0.138nm C≡N 0.116nm 6-18

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

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

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

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

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

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

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

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

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

Molecular Geometry ______________: Molecules have a triangular, bent shape. *_____________ molecules A central atom Ex. BCl3 bonded to 3 other atoms. 6-28

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

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

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

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

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

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

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

Hybrid Orbitals ~ sp

Hybrid Orbitals ~ sp2

Hybrid Orbitals ~ sp3

Hybrid Orbitals

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

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

Ch. 6 The End!