Molecular Compounds.

Slides:

Advertisements

Similar presentations

Unit 6 Covalent Bonding.

Advertisements

Table of Contents Lecture/Lab/Activity Date Pg# 22. The Periodic Table9/24/ Periodic Def & Trends9/27/ Electron config practice10/4/10.

Naming Covalent Bonds.  Write the names of both elements.  Change the final ending to -ide.  Add prefixes to indicate subscripts.  Only use mono-

Molecular Compounds. Types of Compounds Ionic Metal (or NH 4 + ) with a non-metal Transfer of electrons from metal  non-metal Have ionic bonds Molecular.

Naming Molecular Compounds

Molecular Compounds. Outline  Molecular Compounds  Diatomic Molecules  Naming Molecular Compounds  Combining Capacity.

Writing and Naming Binary Molecular Compounds Composed of two anions (binary) Check on periodic table to make sure! Name describes the type and number.

Covalent Bonding.  Atoms that share a pair of electrons are joined together by a covalent bond.  A neutral particle that is composed of atoms joined.

Covalent Bonding (Molecular Compounds) I. Characteristics of Molecular Compounds A. Compounds result from the sharing of electrons B. Lower melting points,

1.3: Covalent & Metallic Bonds Covalent Bonds –Form when atoms share 1 or more pairs of e- 2 nonmetals don’t transfer e- to fill the outer most energy.

Covalent compounds Sharing of electrons. Chemical Bonds Ionic Bond – Transfer of electron – Exist in a crystal lattice form Covalent Bond – Pairs of electrons.

Chapter 8 Covalent Bonding.

Naming Covalent (Molecular) Compounds

Molecular Compounds. A molecule forms when two or more non- metallic atoms bond together –It can be made up of atoms of different elements or of atoms.

MOLECULAR COMPOUNDS What are they and how to name them?

Molecular Compounds Held together by Covalent bonds. –Between two or more non-metal elements. –Sharing of electrons –Name using prefixes. Subscripts after.

CHEMISTRY PART 11 Covalent Compounds. Remember...  Metals want to lose electrons and non-metals want to gain them.  These are ionic bonds.

In this chapter you will learn about compounds and their names and formulas.

MOLECULAR COMPOUNDS. Bonding Atoms combine with each other in two general ways: 1. Ionic Compounds: transfer of electrons from one atom to another June.

Binary Molecular Compounds

and Chemical Nomenclature

Naming Covalent Compounds

Writing Chemical Formulas.

Unit 6: Covalent Bonding

PREFIXES FOR NON METALLIC COMPOUNDS

Binary Molecular Compounds

Covalent Bonding EQ: How are the chemical formulas and chemical names written for covalent molecules? How do you draw VSEPR diagrams for covalent compounds?

Chapter 8 Covalent bonding.

Covalent Molecules EQ: How are the chemical formulas and chemical names written for covalent molecules?

Molecules EQ: How are the electrons arranged in a covalent bond?

Naming Covalent Compounds

Molecular Compounds SNC2D.

Forming Molecular Bonds

II. Covalent Bonds.

Molecules and covalent compounds

Chapter 6 – Chemical Bonds

Covalent Bonding Day two

II. Molecular Compounds

Atoms strive for 8 valence, so they bond

Molecules and covalent compounds

Covalent Nomenclature

Naming Molecular Compounds

Covalent Nomenclature

Molecular Nomenclature

II. Molecular Compounds (p. 164 – 172, 211 – 213)

Covalent Nomenclature

4.2 Names and Formulas of Compounds

Molecular Compounds SNC2D.

Naming Binary Covalent Compounds

Binary Covalent Compounds

Topic 6: Chemical Compounds

Learning Objectives To understand the bonding that occurs in molecular compounds To compare and contrast ionic and molecular compounds.

Covalent Compounds Two non-metals.

Wednesday, November 12, 2014 Objective: Students will be able to write the formula for Type III Compounds. Warm-Up: Identify the following compounds as.

Chemical Formulas and Equations

II. Molecular Compounds

X=Nonmetal________ More than 2 elements in compound __________ XYZ2

Binary Covalent Compounds

DO NOW Pick up notes and handout

BINARY MOLECULAR COMPOUNDS

Molecular Nomenclature

Naming Binary Covalent Compounds

Matter & Bonding Lesson # 3

Chapter 6 Chemical bonding.

Chemistry Lesson # 4 Molecular Compounds.

Chemical Formulas and Equations

COVALENT MOLECULES.

molecular compounds are compounds consisting of nonmetals

COVALENT BONDING.

COVALENT COMPOUNDS.

Presentation transcript:

Molecular Compounds

Molecular Compounds Molecular compounds are formed when atoms of two or more different elements share electrons. Usually formed between 2 or more non-metals and are also called covalent compound. A covalent bond is formed when electrons are shared between atoms. For example, water (H2O)

Ionic vs. Molecular Ionic Compounds Molecular Compounds How atoms bond? Transfer of electron(s) Share of electrons What bonds with what? Metal to non-metals Non-metal to non-metal What do they form? Lattice structure (solids) Solid, liquid or gas

Diatomic Gases Elements that have two atoms joined by one or more covalent bonds to form a molecule The anagram is HOBrFINCl H2 O2 Br2 F2 I2 N2 Cl2

Draw Lewis Diagram H2 Br2 F2 I2 N2 Cl2

What is the difference between a molecular formula and structural formula? A molecular formula is a chemical formula – it shows the number of atoms of each element. A structural formula shows the arrangement of the atoms that make up a molecule.

Binary Molecular Compounds Binary molecular compounds are compounds composed of two non-metals joined by one or more covalent bonds.

Naming Binary Molecular Compounds Use a prefix to indicate the number of each atom present. Molecular Compounds Prefixes 1 Mono- 6 Hexa- 2 Di- 7 Hepta- 3 Tri- 8 Octa- 4 Tetra- 9 Nona- 5 Penta- 10 Deca- Example: Carbon dioxide tells us it is made of 1 carbon atom and 2 oxygen atoms Note: don’t use mono for the first non-metal in the chemical formula

Naming Binary Molecular Compounds Count the # of atoms of the first element. Write the prefix for this number followed by the name of the first element. If there is only one of the first element we leave out the prefix. Count the # of atoms of the second element. Write the prefix for this number followed by the name of the element using the suffix –ide Example: N2O4 Nitrogen atoms = 2  dinitrogen Oxygen atoms = 4  tetraoxide = tetroxide Full name = dinitrogen tetroxide Example: C2F6 Carbon atoms = 2  dicarbon Fluorine atoms = 6  hexafluoride Full name = dicarbon hexafluoride

Writing Chemical Formulas for Binary Molecular Compounds Write the symbol for the elements. Write the subscript for the number of atoms represented by the prefix. Notice – the ratio in the formula is not reduced to its simplest form like ionic compounds. Example: Sulfur trioxide SO3 Diphosphorus pentasulfide P2S5