Catalyst (5 minutes) Draw electron dot structures for the following elements (find the number of valence electrons!) ON A SEPARATE SHEET OF PAPER (KEEP.

Slides:

Advertisements

Similar presentations

8 th Grade Science. Atomic Structure Atoms have a nucleus that contains Protons and Neutrons Electrons are contained in shells that surround the nucleus.

Advertisements

Covalent Bonding Bonding models for methane, CH4. Models are NOT reality. Each has its own strengths and limitations.

 Octet rule - __________________________________________ ____________________________  atoms tend to gain, lose or share electrons to try and have eight.

Most commonly missed questions

Take out your interactive notebook and set up an In, Out Through on your next two open pages.

Ionic and Covalent Bonding 1. Bonding Atoms with unfilled valence shells are considered unstable. Atoms will try to fill their outer shells by bonding.

Covalent bonding Grade 9 Chemistry Starter What ions do Chlorine form? Imagine you have 2 chlorine ions – how could they help EACH OTHER to reach a stable.

1 Covalent Bonding Ionic compounds form most commonly between a metal and non-metal. Now we look at compounds formed when 2 non-metals bond...

PART II. Covalent Bonds LET’S FIRST REVIEW IONIC BONDING.

Ions and Ionic bonding Chemistry. What’s in an atom? (review and new Info) Atoms are made up of 3 particles: 1.Protons -Located in the nucleus (center.

Multiple Bonds Chemistry 11 Ms. McGrath. Multiple Bonds A nonmetal with 4, 5 or 6 valence electrons have more than one unpaired electron. This results.

Cornell Notes 2/1/10. What we’ve learned so far…. Atoms lose/gain electrons to form cations and anions (8 valence electrons like a noble gas!) Charged.

PART II. LET’S FIRST REVIEW IONIC BONDING In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds. FK.

Lewis Diagrams For Ionic and Covalent Compounds. First, we’ll consider the ionic compound strontium fluoride.

Group 1 – The Alkali Metals Watch the demo. Write down your observations. Write down the chemical reactions (word and symbol)

Lewis Structure and Bonding. Lewis Dot Diagram of Atoms The chemical symbol for the atom is surrounded by a number of dots corresponding to the number.

Inorganic chemistry Assistance Lecturer Amjad Amjad Jumaa  Chemical bonds.  Ionic Bonds,  Covalent Bonds. 1.

Compounds and Bonding Putting 2 and 2 Together. Covalent Bonds.

 atoms that lose or gain electrons become ions  cations have + charge  anions have – charge  cations and anions are attracted to each other by elecrostatic.

Covalent Bonding & Polarity Chapter 6.2. Chemical Bonding  Ionic Bond – Force that holds cations and anions together and which involves the transfer.

Covalent Bonding Vocabulary covalent bond covalent bond single bond single bond double bond double bond triple bond triple bond molecule molecule structural.

Covalent Bonds.  Octet rule – all atoms want to have 8 electrons in their outer shell  Exception – helium (2)  Noble gases – very stable  Binary ionic.

Covalent Bonding Covalent bonding is the type of bonding that occurs between two non- metallic elements. Non-metallic elements do no form ions when they.

Making Bonding Models.

Bonding. A Chemical Bond The forces that hold groups of atoms together and make them function as a unit Bonding involves only the valence electrons There.

Chapter Sixteen: Compounds  16.1 Chemical Bonds and Electrons  16.2 Chemical Formulas  16.3 Molecules and Carbon Compounds.

CHEMICAL BONDING IONIC BONDS COVALENT BONDS IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both.

Bellringer: Ionic Bonds 1.What is the daily learning target? 2.In an ionic bond, explain what happens to the electrons? 3.In your own words, explain how.

Unit 6A: Ionic and Covalent Bonding. Ions Why do elements in the same group behave similarly? They have the same number of valence electrons. Valence.

Covalent Bonds.

Bonding SC.8.P.8.5: Recognize that there are a finite number of elements and that their atoms combine in a multitude of ways to produce compounds that.

IPC Notes Types of Bonds. Remember… Atoms combine by gaining, losing or sharing electrons in order to become chemically stable. Atoms become chemically.

The rules to. The TWO basic rules  Opposites ATTRACT and likes REPEL  Nature moves in the direction of the least resistance (lowest energy)

1 Types of CHEMICAL BONDS. 2 Essential Question: How does the number and arrangement of electrons affect the way that atoms bond?

Covalent bonds: Sharing is caring!

Ionic Bonds and Compounds. The Octet Rule The Octet rule states that elements gain or lose electrons to attain an electron configuration of the nearest.

Electron Dot Diagrams / Lewis Structures Atom and Covalent Compound diagramming.

Chapter Sixteen: Compounds  16.1 Chemical Bonds and Electrons  16.2 Chemical Formulas  16.3 Molecules and Carbon Compounds.

Bonding. Ionic Bonding Chemical bonding that results from the electrical attraction between cations and anions is called ionic bonding. Cations give up.

PART II. Covalent Bonds Ionic Bond = Metal – Non Metal Covalent Bond = Non-Non.

Bonding Chapter 8.

Ionic Bonds Chapter 14.

Chemical Bonding Ionic and Covalent.

BONDING PART II.

Covalent Bonding Bonding models for methane, CH4. Models are NOT reality. Each has its own strengths and limitations.

Section 16.1 – Chemical Bonds & Electrons pp

Why do atoms have a neutral (no) charge?

Electron Dot Diagrams / Lewis Structures

Bonding Basics Title the page: 10/29 Warm-Up: Bonding Basics

Chemical Bonds Section 2.3.

Formation of Ionic Compounds

Materials Science Lesson 5.

Brief biochemistry.

Daily Science Label the following as a molecule, atom, compound, or both (molecule and compound) H3 H2O Ca NaCl How many and what kind of atoms do you.

Chemical Bonding.

Section 16.1 – Chemical Bonds & Electrons pp

NC Standards Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic.

Lewis Dot Diagrams.

Covalent Bonds 2a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to.

What? Why? When? Which? Where? How? Mod.H U.3 L3&4

Lecture 8A - Formation of Covalent (Molecular) Compounds

NC Standards Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic.

Chapter Sixteen: Compounds

Covalent Bonding Bonding models for methane, CH4. Models are NOT reality. Each has its own strengths and limitations.

Chemical Bonding Sections 1-3.

Chemical Formulas & Compounds.

Chemical Bonding with Elements

Presentation transcript:

Catalyst (5 minutes) Draw electron dot structures for the following elements (find the number of valence electrons!) ON A SEPARATE SHEET OF PAPER (KEEP IT FOR THE WEEK): 1. Chlorine 2. Carbon 3. Oxygen 4. Nitrogen Cl CN O

What we’ve learned so far…. Atoms lose/gain electrons to form cations and anions (8 valence electrons like a noble gas!) Charged anions and cations form IONIC BONDS to make IONIC COMPOUNDS FK + -

What we’re learning today… Atoms can also SHARE electrons to form COVALENT BONDS! Why is this important?  Covalent bonds are important in many organic molecules (living creatures)  Examples:  Cell membranes are made of lipids (We’d be puddles of liquid without them!)  Proteins (We’d starve without them!)

Covalent Bond The chemical bond formed when two atoms SHARE electrons  Why do atoms form bonds? To gain the same number of valence electrons as a noble gas! Cl Full octet (8)! Bonding Pair

Types of Covalent Bonds Single Bond: ONE pair of shared electrons Double Bond (Pi Bond): TWO pairs of shared electrons Triple Bond: THREE pairs of shared electrons Cl OO NN

How many bonds can an atom form? # bonds formed = # of UNPAIRED electrons # electrons atoms keep = # electrons in PAIRS NN 3 unpaired electrons = 3 bonds! O 2 pairs = four electrons the atom keeps!

Example 1 How many bonds can Sulfur form? How many electrons will Sulfur keep to itself? S Two unpaired electrons! Four electrons will be kept by sulfur! S Two pairs of electrons! Two bonds can be formed!

Example 2 How many bonds can Carbon form? How many electrons will Carbon keep to itself? C Four unpaired electrons! Zero electrons will be kept by carbon! C No pairs of electrons! Four bonds can be formed!

Example 3 How many bonds can Neon form? How many electrons will Neon keep to itself? Ne Zero unpaired electrons! Eight electrons will be kept by neon! Ne Four pairs of electrons! Zero bonds can be formed!

Announcements Homework – Due Fri Feb 4 Read Sec 8.1, pp Define vocab on p 240 (7 words) Choose any 3 of the words and draw an illustration to show what they mean

Worksheet COMPLETE the worksheet