Chapter 8
description
Transcript of Chapter 8
![Page 1: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/1.jpg)
1
Chapter 8
Covalent Bonding I
![Page 2: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/2.jpg)
2
Molecules and Molecular Cpds
noble gases (e.g. He and Ne) and most elements are monatomic.
![Page 3: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/3.jpg)
3
Molecules and Molecular Cpds
• Non-metals• e.g. [O2 ;not a cpd], CO2, C6H12O6
element
Covalent cpds• atoms held together by sharing e- are joined by
a covalent bond to form covalent cpds
![Page 4: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/4.jpg)
4
Molecules and Molecular Cpds
Covalent bonds• not so strong as Ionic bonds (electrostatic
attractions).
• Covalent cpds: made up of ALL nonmetals (how about ionic cpds?)
![Page 5: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/5.jpg)
5
Molecules and Molecular Cpds
Molecule • a neutral group of atoms (all nonmetals) joined
together by covalent bonds.
• may be a cpd (e.g. CO2) or an element (e.g. N2)
covalent cpds = molecular cpds
![Page 6: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/6.jpg)
6
Molecules and Molecular Cpds
• e.g. air contains oxygen molecules (O2) and nitrogen molecules (N2)---not cpds
A diatomic element consists of 2 atoms. e.g. 7 diatomic elements are H2, N2, O2,
F2, Cl2, Br2, I2
![Page 7: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/7.jpg)
7
Diatomic Molecules
Hydrogen Colorless gas H2
Nitrogen Colorless gas N2
Oxygen Pale blue gas O2
Fluorine Pale yellow gas F2
Chlorine Pale green gas Cl2
Bromine Reddish brown liquid Br2
Iodine Lustrous, dark purple solid
I2
![Page 8: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/8.jpg)
8
A Hydrogen Molecule
• 2 H atoms share a pair of e- in a covalent bond.
A covalent bond is formed by 2 shared e-.
![Page 9: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/9.jpg)
9
Covalent Bonds
• 2 of the same atoms form a covalent bond, e.g., when 2 F atoms form the F2 molecule.
• a pair of valence e- are shared---single covalent bond (2 shared e-).
• Form octets of for both atoms
Shared pair of e-
![Page 10: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/10.jpg)
10
Molecules and Molecular Cpds
Molecular cpd (covalent cpd):
- cpds composed of molecules
• e.g. H2O , CO2 , C6H12O6
![Page 11: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/11.jpg)
11
Molecules and Molecular Cpds
![Page 12: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/12.jpg)
12
Physical Properties Properties Ionic cpd Covalent cpd
Example NaCl CO 2
State at room temperature Crystalline solid Solid, liquid or gas
Melting point High Low
Conduct electricity in liquid state
Yes No
Water solubility High Low
Conduct electricity in aqueous solution
Yes poor
![Page 13: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/13.jpg)
13
Molecular Formulas
![Page 14: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/14.jpg)
14
Covalent Bonds
• All diatomic elements (F2, Cl2, Br2, I2, O2, N2, and H2) have covalent bonds.
• are molecules (not molecular cpds)• The other molecules are ALL cpds
• Most of the elemental diatomic molecules are gases at room temp—Cl2, F2, O2, N2, and H2.
![Page 15: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/15.jpg)
15
Modeling Water
• 2 covalent bonds.
• octet• duplet
![Page 16: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/16.jpg)
16
Lone (unshared) pair
Bonding (shared) pair
3 covalent bonds
![Page 17: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/17.jpg)
17
A Model for Ammonia
• Each H shares a pair of e- with the N.
• N’s remaining 2 e- form a lone pair.
• N has a complete octet of e-.
Lone pair
![Page 18: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/18.jpg)
18
double bond
• sharing 2 pairs of e- between 2 atoms.
Modeling Carbon Dioxide
![Page 19: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/19.jpg)
19
Double Bonds and Triple bonds
F−F
O=O
N≡N
O=C=O
![Page 20: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/20.jpg)
20
(1) Name the elements in the order listed in the formula.
(2) Use prefixes to indicate the # of each kind of atom.
9.3Naming Binary Molecular Cpds
![Page 21: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/21.jpg)
21
(3) Omit the prefix mono- when the formula contains only 1 atom of the 1st element in the name. e.g. CO2 (we don’t say monocarbon)
(4) The suffix of the name of the 2nd element is -ide.
9.3Naming Binary Molecular Cpds
![Page 22: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/22.jpg)
22
(5) Use the prefixes in the name to tell the subscript of each element in the formula.
(6) Then write the correct symbols for the 2 elements with the appropriate subscripts.
9.3Writing Formulas for Binary Mol. Cpds
![Page 23: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/23.jpg)
23
9.3Naming Binary Molecular Cpds
![Page 24: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/24.jpg)
24
Naming Binary Molecular Cpds
NF3 SF4
CO2 SbCl3
CO NH3
H2O CF4
CS2 P4S3
BCl3 SO2
IF7 SO3
PCl5 CCl4
C2O5 MgCl2
HCl SiCl4
![Page 25: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/25.jpg)
25
CST problem 1
(picture of a circuit) The above picture shows a light bulb connected to a battery with the circuit interrupted by a solution. When dissolved in the water to form a 1.0 molar solution, all of the following substances will complete a circuit allowing the bulb to light except
A hydrochloric acid
B sodium nitrate
C sucrose
D ammonium sulfate
![Page 26: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/26.jpg)
26
Name Hydrogen Chlorine Ammonia Methane
Molecular Formula
H2 Cl2 NH3 CH4
CST problem 2
What type of bond do all of the molecules in the table above have in common?
A covalent
B ionic
C metallic
D polar
Table of common molecules
![Page 27: Chapter 8](https://reader036.fdocuments.us/reader036/viewer/2022062322/56814ebe550346895dbc5e47/html5/thumbnails/27.jpg)
27
The End