Chapter 8 – Covalent Bonding

Slides:



Advertisements
Similar presentations
Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. In nature, only the noble gas elements, such as helium and neon, exist as.
Advertisements

Do Now 1.Define electronegativity. 2.What is a bond? 3.What are the THREE types of bonds? 4.What type of bond will form between… Na and Cl?? H and Cl??
Aim: What are molecular compounds? DO NOW: 1. COMPARE AND CONTRAST METALLIC BONDING AND IONIC BONDING. 2. WHAT WOULD BE THE IONIC CHARGE FOR AN ATOM WITH.
#1 How are the melting points and boiling points of molecular compounds usually different from ionic compounds. Covalent Compounds often have Low melting.
Investigating Matter Chapter 11 Fig. 9.3.
Ionic/Covalent Bonding Notes. Stable or Unstable? An atom is only stable if it has a full valence shell If an atom is stable, it will not bond If an atom.
Chapter 8 Covalent Bonding 8.1 Molecular Compounds
Chapter 3 Classification of Matter
COVALENT BONDS Chapter 5 Section 3.
Objectives  When you complete this presentation, you will be able to …  distinguish between the melting points and boiling points of molecular compounds.
Chemistry 8.1.
Get it? Explain it.. Unit 4: Bonding Lesson 1: Aim and Objectives Aim: Why do elements form bonds? Objectives: 1.Learn the benefit for atoms to join.
CHAPTER 8: COVALENT BONDING
Molecules and Molecular Compounds
CHEMISTRY 111/112 Chapter Eight: Covalent Bonding.
© Copyright Pearson Prentice Hall Molecular Compounds > Slide 1 of 18 Molecules and Molecular Compounds In nature, matter takes many forms. The noble gases,
8.1 Molecular Compounds > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 8 Covalent Bonding 8.1 Molecular Compounds.
Bonding Types and Properties 1. Identify compounds as ionic or molecular (covalent) based on ionic compounds being the combination of metals with nonmetals.
Chapter 7 and 8.  Valence electrons are responsible for the bonding between two atoms.
Covalent Bonding Ms. Cook. Covalent Bonds The electrons are shared between the atoms for each to reach an octet. A molecule is a neutral group of atoms.
8.1 Molecular Compounds > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 8 Covalent Bonding 8.1 Molecular Compounds.
Chemistry 8.1.
Properties of Ionic and Covalent Compounds
Chemical Stability Knowing this information about oxidation numbers, which elements are the most chemically stable elements? Noble gases - Are the most.
Molecular compound: neutral group of atoms joined by covalent bonds. covalent bond: formed by sharing e – ’s between atoms. (nonmetals only) Unit 6: Covalent.
Chapter 8 Covalent Bonding.
SECTION 1.2 PAGES 8-11 Types of Chemical Bonds. Ion Formation Ions are charged particles that form during chemical changes when one or more valence electrons.
Chapter 8 – Covalent Bonding. Review of Ions  We learned about electrons being transferred (“given up” or “stolen away”)  This type of “tug of war”
© Copyright Pearson Prentice Hall Molecular Compounds > Slide 1 of 18 Chemistry 10/21/2015 Covalent Bonds.
Aim: What are molecular compounds?. Ionic Compounds Review  In Ionic Bonding electrons are being transferred (“given up” or “stolen away”)  Occurs between.
8.1 Molecular Compounds > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 8 Covalent Bonding 8.1 Molecular Compounds.
Chemical Bonding Ionic, Covalent, and Metallic bonding.
Molecular Compounds. Objectives Distinguish between the melting points and boiling points of molecular compounds and ionic compounds Distinguish between.
CHEMISTRY 111/112 Chapter Eight: Covalent Bonding.
Chemical Bonding Just as the physical and chemical properties of elements are determined by their atomic structure, the properties of compounds are determined.
Chapter 6 Chemical Names and Formulas
Chapter 6 section 2 Covalent bonding Molecular compounds.
Chapter Eight: Covalent Bonding
Chemistry 8.1.
Ionic/Covalent Bonding Notes
Major Bond Types COVALENT e- are shared between 2 atoms
Covalent Bonds.
Covalent Bonding.
Chapter 8 Covalent Bonding 8.1 Molecular Compounds
Chapter 8 Covalent Bonding 8.1 Molecular Compounds
Unit 7: Covalent Bonding
Ionic/Covalent Bonding Notes
Unit 4 Compounds, Naming, Formula Writing
Covalent Bonds Chapter 5 Section 3.
Practice: True or False
Naming Ionic Compounds
Covalent Bonding.
Unit 3 Bonding & Chemical Rxns
Ionic/Covalent Bonding Notes
Ch. 15 Notes---Ionic Bonding & Ionic Compounds
Molecular compounds and covalent bonds
Molecular Compounds.
Molecular Compounds.
Substances’ properties depend on their bonds.
Unit 7: Bonding.
Covalent Bonding.
What is a molecular compound?
The Structure of Matter
Covalent Bonds 8-2.
Section 3 – Covalent Bonds Pg 192
Characteristics of Chemical Bonds
Covalent Bonds.
Chapters 7 and 8 – Bonding.
Section 4: Covalent bonding
Putting Atoms together
Presentation transcript:

Chapter 8 – Covalent Bonding

Section 8.1 – Molecular Compounds A covalent bond is formed between atoms held together by sharing electrons. A molecule is a group of atoms joined by covalent bonds. A diatomic molecule is 2 atoms bonded together.

Diatomic Elements There are 7 naturally existing diatomic elements. They are N2, O2, F2, Cl2, Br2, I2, and H2.

Properties of Molecular Compounds Molecular Compounds Ionic Compounds Low melting points high melting points Tend to be gases or liquids crystalline solids Made of nonmetals metal and nonmetal Made of covalent bonds ionic bonds Poor conductors conductor when molten or aqueous

Molecular Formulas A molecular formula is the chemical formula of a molecular compound. A molecular formula shows how many atoms of each element a molecule contains. A molecular formula shows the actual number of atoms while a formula unit shows the lowest whole-number ratio of ions.

Section 8.1 Assessment How are the melting points and boiling points of molecular compounds usually different from those of ionic compounds? What information does a molecular formula provide? What are the only elements that exist in nature as uncombined atoms? What term is used to describe such elements? Describe how the molecule whose formula is NO is different from the molecule whose formula is N2O. Give an example of a diatomic molecule found in Earth’s atmosphere.