Ionic BONDING. Noble Gases Have complete outer shells that cannot accept anymore electrons Unreactive Will not combine (form bonds) with any other.

Slides:

Advertisements

Similar presentations

Ionic Bonding Chapter 13 Ionic Bonding

Advertisements

Chapter 7 Ionic Bonding.

MYP Chemistry Ionic Bonding and Ionic Compounds International College Spain.

Atom Stability * In order for atoms to be stable, they need to have their outer energy level completely filled. * In most cases, atoms need to have 8 valence.

BONDING. Bonds Between Atoms Covalent Ionic Molecules Network Metallic.

Warm-Up #22 A. 34 Copy and Answer 1.How many valence electrons does calcium have? 2.If calcium lost two electrons, what would be its charge? 3.How many.

Ionic Bonds and Properties of Ionic Compounds.  Recall that atoms lose or gain electrons to form ions.  Metals tend to lose electrons and form positively.

Valence Electrons l The electrons responsible for the chemical properties of atoms are those in the outer energy level. l Valence electrons - The electrons.

Ions and Ionic Compounds

Chemical Bonding.

Bonding INTRODUCTION FOR SCIENCE 10. Chemical Reactivity The reactivity of an element depends on the number of valence electrons. If the outer shell of.

Chapter 15 Ionic Bonding. Valence Electrons  Do the electron configuration for the following elements Li Be B O F Ne.

Ionic and Covalent Bonding. » Atoms bond when their valence electrons interact ˃Atoms with full outermost energy levels are not reactive (Noble Gases)

Chemical Bonding…. How Atoms Combine Bonding involve electrons in the outermost energy level Valence Electrons.

Ions & Compounds. Ions atoms that have lost or gained electrons do this to get a stable outer shell (8) they now have a charge.

Chemical Bonding. Ionic Bonds Ionic bonds are made between metal and non-metal atoms Electrons are transferred from the metal atom to the non-metal atom.

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

8.2 Ionic Bonding. Ionic Bonds Ionic bonds are made between metal and non-metal atoms Electrons are transferred from the metal atom to the non-metal atom.

Making Compounds. Chemical compounds form so that each atom has an octet of electrons in its valence level. This can occur by gaining, losing or sharing.

Chapter 4 Part 1 - Ionic Compounds Electron Review l Valence electrons - electrons in the outer energy level. l Core electrons -those in the energy levels.

metals: lose valence electrons –form cation –form cation (+ ion) non-metals: gain electrons anion –form anion (- ion)

Warm-Up #32 A. 34 Copy and Answer 1.How many valence electrons does calcium have? 2.If calcium lost two electrons, what would be its charge? 3.How many.

Number of ProtonsAtomic Number Number of NeutronsAtomic Mass – Atomic Number Number of ElectronsNumber of protons (Atomic Number)

Bonding Types and Properties 1. Identify compounds as ionic or molecular (covalent) based on ionic compounds being the combination of metals with nonmetals.

1. Identify which ions gained or lost electrons: Na + O What is the difference between cation and anion? Give an example of each. 3. Write the ions.

Unit 4 Bonding Notes.  All chemical compounds are held together by bonds  We will be learning about 3 types of bonds  Ionic, Covalent, and Metallic.

IONS. Neutral Atoms: Review Neutral Atoms have the same number of PROTONS and ELECTRONS. Protons have a POSITIVE charge. + Electrons have a NEGATIVE charge.

Chapter 7 “Ionic and Metallic Bonding”. Section 7.2 Ionic Bonds and Ionic Compounds l OBJECTIVES: –Explain the electrical charge of an ionic compound.

What are ionic bonds? Section 15-5.

 The goal of every atom is to become stable – most elements have partially filled outer shells and they must bond with another atom to become stable.

Bonding Why do atoms bond? The octet rule – all atoms bond so they have 8 electrons in their outer shell, so that it is FULL.

Ionic Bonds LEARNING TARGET: HOW DOES AN ION BECOME POSITIVELY OR NEGATIVELY CHARGED? HOW DOES AN IONIC BOND FORM?

Ionic Bonding What happens to the e-? Electron Dot diagrams l A way of keeping track of valence electrons. l How to write them l Write the symbol. l.

Ionic Compounds and Bonding SNC2D – Academic Science.

Chapter 8 Ionic and Metallic Bonding Keeping Track of Electrons l The electrons responsible for the chemical properties of atoms are those in the outer.

Atoms chemically bond in an attempt to feel stable like noble gases. They do this by either filling their valence shells or getting rid of the electrons.

BONDING. WHY ATOMS COMBINE -1 All atoms want a full outer shell Some atoms will lose electrons to empty their shells These become positively charged ions.

Science 10 Lesson 2 BOHR MODELS + IONIC BONDING. Student Review  Draw a model for sulfur atom.

TYPES OF CHEMICAL BONDS Chapter 5. CHEMICAL BONDS Atoms bond by gaining, losing, or sharing electrons in their outer rings. The way an atom fills its.

Unit 4 - Bonding Part 1 – Ionic Bonding & Metallic Bonding.

Chemical Formulas Uses chemical symbols to represent the atoms of the elements and their ratios in a chemical compound Example: CO 2.

Chemical Bonding: Ch. 7: Ionic Bonding. Chapter 7: Ionic Bonding First off – what you need to remember before getting into this chapter…

6.1 Ionic Bonding   HES Chemistry Unit: Ions and Ionic Bonds.

Bonds How does an ionic bond form? How does a covalent bond form?

IONIC BONDING. HOW DOES IT WORK? Ionic bonding takes place between metals and non-metals Metal atoms try to attain noble gas strucure (full outer shells)

Ionic substances C2.1/2 10-Jul-11. Metal + Non-metal Metal atoms Non-metal atoms + ions– ions electrons Ionic compound Atoms get full outer shells.

When an atom gains or loses electrons they become electrically charged particles called When an atom gains or loses electrons they become electrically.

Structure of Atom Nucleus  Proton –Positive Charge Neutron-No Charge

Ionic Compounds and Bonding

Forming Compounds.

Notes: Ionic Bonds 1. Key Concept: Ionic bonds form when electrons are

It’s time to talk about Bonds…

Introduction for Science 10

Chemical Bonding Chapter 11.

Chemical Bonding Chapter 13 Ionic Bonds Section 2

Chemical Bonding.

I. Why Atoms Combine Chemical Formulas Chemical Bonds Stability

Ionic Bonding Chapter 27.

Chemical Bonding Chapter 11.

Presentation transcript:

Ionic BONDING

Noble Gases

Have complete outer shells that cannot accept anymore electrons Unreactive Will not combine (form bonds) with any other element 2 2,8 2,8, 8 2,8, 8, 18

Metal atoms Metal atoms have incomplete outer shells Have 1, 2 or 3 electrons on their outer shell Metal atoms want to LOSE these extra electrons in order to have a full outer shell (like the noble gases)

Metal atoms Metal atoms lose electrons to form a CATION CATION: when a neutral metal atom loses one or more electrons to form a positively charged ion 2,8,1  2,8

Metal Cations Possible Metal Cations: Lose 1 electron = +1 eg. K + Lose 2 electrons = +2 eg. Ca 2+ Lose 3 electrons = +3 eg. Al 3+ Aluminum metal lost 3 electrons to become stable

Non-metal Atoms Non-metals have incomplete outer shells Have 5, 6, or 7 electrons on their outer shell Non-Metal atoms want to GAIN additional electrons in order to have a full outer shell (like the noble gases) 2, 8, 7 2, 6

Non-Metal atoms Non-Metal atoms gain electrons to form an ANION ANION: when a neutral non-metal atom gains one or more electrons to form a negatively charged ion 2,8,7  2,8,8

Non-Metal Anions Possible Non-Metal Anions: Gain 1 electron = -1 eg. F - Gain 2 electrons = -2 eg. O 2- Gain 3 electrons = -3 eg. N 3- Nitrogen non-metal atom gains 3 electrons to become stable

Ionic Bonds - results from the TRANSFER of electrons from a metal to a non-metal Lithium atom needs to lose 1e- where Fluorine atom needs to gain 1e- -What a perfect match! -They will form an ionic bond! -Cations Anions

Opposites Attract!!

Ions are held strongly by opposite charges in a 3D lattice

Properties 1. High melting points because of strong attractions between cations and anions 2. Soluble in water Soluble (lattice breaks apart into free ions)

3. Conducts electricity because of the charged ions freely moving in water (but not in solid state)

4. Brittle – similar ions can repel if they come into contact