WARM UP 1.Compare and contrast Lewis structures and structural formulas. 2.Draw a Lewis structure and a structural formula for CO 2.

Slides:



Advertisements
Similar presentations
Chemical Formulas and Equations
Advertisements

Unit 6 Covalent Bonding.
1 4.6 Covalent Compounds Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings Chapter 4 Forces Between Particles.
Bell Ringer Draw the Molecule & give the Formula for: – Carbon and 2 Sulfurs – Hydrogen, Oxygen, and Chlorine – Carbon, two Chlorines, 2 Fluorines – Phosphorus,
Molecular Geometry Notes. February 3, 2014 You will be able to describe the molecular geometry of a molecule. Correct HW 6B A note on nomenclature Notes.
Covalent Nomenclature Naming Molecular Compounds.
Chapter 7.1 Chemical Names & Formulas (p )
Nomenclature Continued Chapter 6 Sections 5 and 6.
Table of Contents Lecture/Lab/Activity Date Pg# 22. The Periodic Table9/24/ Periodic Def & Trends9/27/ Electron config practice10/4/10.
Covalent Compounds.
Prefixes for Naming Covalent Bonds. Prefixes Mono - 1 Di - 2 Tri - 3 Tetra - 4 Penta - 5 Hexa - 6 Hepta - 7 Octa - 8 Nona - 9 Deca - 10.
Naming Molecular Compounds CH 4 methane BCl 3 boron trichloride CO 2 Carbon dioxide All are formed from two or more nonmetals. Ionic compounds generally.
Compound Names and Formulas. Ionic Compounds CATIONS CATIONS Na = Sodium ionNa = Sodium ion Mg = Magnesium ionMg = Magnesium ion Anions Anions F = Fluoride.
C OVALENT C OMPOUNDS. 1. Usually soft and squishy 2. Not soluble in water 3. Does not conduct electricity 4. Low melting points 5. Low boiling points.
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 (a.k.a. Covalent Compounds)
Aim: How do chemists write and interpret chemical formulas? How are elements named? IUPAC- International Union of Pure and Applied Chemists Formulas use.
COS 3.0, 3.1 CONTRAST THE FORMATION OF IONIC AND COVALENT BONDS BASED ON THE TRANSFER OR SHARING OF VALENCE ELECTRONS. DEMOSTRATE THE FORMATION OF POSITIVE.
Chapter 9.3 Naming and Writing Formulas for Molecular Compounds
Ch Chemical Bonds III. Naming Molecular Compounds  Molecular Names  Molecular Formulas.
Chapter Naming & Formula Writing for Molecular Compounds.
COMPOUNDS part two: molecular compounds. += Na Cl NaCl Reminder: Ionic compounds involve a metal IONIC COMPOUNDS and a non-metal.
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. Outline  Molecular Compounds  Diatomic Molecules  Naming Molecular Compounds  Combining Capacity.
Chemical Bonds I. Why Atoms Combine  Chemical Formula  Chemical Bond  Stability.
Naming Molecular Compounds!. What are Molecular Compounds made of?  Nonmetals ONLY!!
Bonding. Why do atoms bond? Atoms bond to get 8 valence electrons! Octet Rule: atoms need 8 valence electrons to be stable. 2 ways to get 8 1. transfer.
Nomenclature Covalent Naming and Formula Writing.
Science 10. Covalent Compounds Covalent compounds are formed between non- metals only Nonmetals combine in more than one ratio therefore we must use prefixes.
Chemical Bonds I. Why Atoms Combine  Chemical Formulas  Chemical Bonds  Stability.
Molecular Compounds 3.3. Facts Molecular compounds occur when non metals combine to form a pure compound. These non-metals share electrons forming a molecular.
Molecular Compounds.  Held together by covalent bonds  Elements involved are nonmetals  Binary Compound: two nonmetals  Example: H 2 O Molecular Compounds.
Chapter 19 – Molecules and Compounds Bonding and Molecules Atoms react /combine with other atoms to form molecules. Chemical bonds hold them together.
Covalent compounds Sharing of electrons. Chemical Bonds Ionic Bond – Transfer of electron – Exist in a crystal lattice form Covalent Bond – Pairs of electrons.
Molecular Compounds (a.k.a. Covalent Compounds). Ionic Compounds Review Ionic compounds are the combination of ions. E.g. Na+ + Cl-  NaCl. This formula.
How Do We Make Compounds?
Naming Binary Molecular Compounds 2 elements covalent bond.
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 SNC2DI. Terms to Know A covalent bond is formed when elements share electrons to make a bond. A molecular compound is formed from.
NOMENCLATURE Binary Molecular Compounds Periodic Table.
Day 14 – Covalent bonds Sci 10Chemistry. Covalent Bonds Non-metal + non-metal.
How are Molecules Depicted? 6.2. Lewis Structures Valence e- = an e- in the outermost E level of an atom and determines the chemical properties Lewis.
Covalent Compound Notes Covalent Compounds – Electrons Prefixes Non-metal + Non-metal Stuck together in a molecule – Electrons are SHARED between elements.
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.
II. Molecular Compounds. Covalent Bonding A major type of atomic bonding occurs when atoms share electrons.atoms As opposed to ionic bonding in which.
Molecular Compounds and Covalent Bonds SNC2D. Terms to Know A covalent bond is formed when elements share electrons to make a bond. A molecular compound.
Objectives Determine the name of covalent compounds Determine the name of covalent compounds Determine the formulas of covalent compounds Determine the.
Properties of Covalent Compounds Formed between 2 non-metals Generally have much lower melting and boiling points than ionic compounds. Are soft and squishy.
WARM UP Do ACT Prep Passage 5 – Reducing Pollution 5 minutes Start when the bell rings.
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.
WARM UP “A ship in the harbor is safe, but that is not what ships are built for.” –William Shedd 1.What does this mean to you? 2.How can you apply this.
Naming Molecular Compounds Covalent Bonding. Names and Formulas Remember covalent bonding occurs between two non- metals There are three rule to naming.
 Name binary (compound made up of 2 elements) inorganic covalent compounds by using prefixes, roots, and suffixes.  Describe the process of naming an.
22.3 Notes Part D Covalent Formulas & Naming. Objectives Write formulas and names for covalent compounds.
Molecular Compounds.
Molecules EQ: How are the electrons arranged in a covalent bond?
Naming Ionic Compounds
Naming Molecular Compounds
Molecular Nomenclature
Covalent Nomenclature
III. Naming Molecular Compounds Molecular Names Molecular Formulas
Wednesday, November 12, 2014 Objective: Students will be able to write the formula for Type III Compounds. Warm-Up: Identify the following compounds as.
III. Naming Molecular Compounds Molecular Names Molecular Formulas
Molecular Nomenclature
Q/A How do you think Carbon would bond with Oxygen? What type of bond do you think this is ? There is actually many ways that Carbon can bond with Oxygen.
molecular compounds are compounds consisting of nonmetals
Covalent bond: Chemical bonding that results from the sharing of electrons between two atoms
Presentation transcript:

WARM UP 1.Compare and contrast Lewis structures and structural formulas. 2.Draw a Lewis structure and a structural formula for CO 2.

Naming Covalent Molecules

Empirical vs. Molecular Empirical formula –Reduced ratio Names don’t indicate # of atoms –Ionic Molecular formula –Actual number of atoms Names must indicate # of atoms –Covalent

Basic Naming First element –Same name Second element –Ending changed to –ide

Naming With Prefixes Put a prefix before each name –Indicates number of atoms in formula –Mono- before first atom is omitted 1=mono2=di3=tri 4=tetra5=penta6=hexa 7=hepta8=octa9=nona 10=deca

WRAP UP Write the formulas for: –Dihydrogen monoxide –Tetraphosphorus pentabromide –Sulfur hexafluoride

WARM UP 1.Name: -C 3 H 7 -PBr 5 -H 2 O -Si 4 Cl 6

WRAP UP Draw Lewis structures for the following molecules and name each of them: NH 3 CCl 4 H 2 OHBr

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2025 SlidePlayer.com. Inc. All rights reserved.