Ionic Compounds & Covalent Bonding

Slides:



Advertisements
Similar presentations
Ionic Bonding.  Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form.
Advertisements

Ionic Bonds Chapter 4 Ionic Compounds What are Chemical Bonds Force that holds 2 atoms together Attraction between + nucleus and – electron Attraction.
Ionic Bonding.
Introduction to Chemical Bonding
Ionic Compounds and Metals
Chapter 7 Ionic Compounds and Metals
Ch 7 Notes. Atoms ‘building blocks’ Element ‘one kind of atom’ Compounds ‘different kinds of atoms’ Shown w/ Symbols Shown w/ Formulas Molecule two or.
Ionic Compounds Chapter 8. Forming Chemical Bonds Chemical Bond: The force that holds two atoms together. Valence Electrons Opposite forces attract Octet.
Chapter 8: Ionic Compounds.
Ionic Bonding. CA Standards  Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons.
Introduction to Chemical Bonding Bond Formation Ionic Bonds Covalent Bonds.
Ionic bond.
Objectives Know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.
Chemical Bonding.
Ionic Compounds Atoms are rarely found in nature in their pure state. Most often they are combined with other elements in compounds. Two major types of.
Ionic and Covalent Bonding. » Atoms bond when their valence electrons interact ˃Atoms with full outermost energy levels are not reactive (Noble Gases)
 Chapter 7.  What is a chemical bond? o The force that holds two atoms together.  Bond formation o attraction between the positive nucleus of one atom.
Chapter 7 Ionic and Metallic Bonding Section 7.1 Ions.
Chapters 8 and 9 Ionic and Covalent Bonding. A chemical bond is a force that holds two atoms together. Chemical bonds may form by the attraction between.
Chemical Bonding Chemical bond – The attractive force between the protons of one atom for the electrons of another atom Determined by electronegativity.
Bonding Ionic Valence Electrons The number of valence electrons in an atom of an element determines the many properties of that element, including the.
Chapter 6 Chemical Bonds.
Ionic Compounds and Metals
CHEMICAL BONDING IONIC BONDS COVALENT BONDS METALLIC BONDS.
Ionic and Covalent Bonding
BONDING OF ELEMENTS Predict Why do elements bond? Why are valence electrons so important?
Chemistry Chapter 8 Notes 3. Review Compounds Can all be represented by chemical formulas Are connected by chemical bonds Ionic Metallic Covalent Compounds.
Ionic Bonding. Stable Electron Configuration When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely.
Chemical Bonding Chapter 12. Objectives O SPI Identify the common outcome of all chemical changes O SPI Use the periodic table to determine.
Chapter 6 Chemical Bonds. Why Bond? An atom’s goal is to be stable This means that the highest occupied energy level is filled with electrons For most.
Module 4 Lesson 1 Ionic and Metallic Bonding. Have you ever wondered why… Metals can be easily formed into sheets? Metallic bonding.
Chapter 1 Chemical Bonding. All matter is made up of atoms. Atoms are the basic building blocks of all the substances in the universe.
Chapter 6 Chemical Bonds.
Chemical Bonding Review All atoms have valence electrons
PAP Chapter 6 CHEMICAL BONDING Cocaine. Chemical Bonding  A chemical bond is a mutual electrical attraction between the nuclei and valence electrons.
Ionic Compounds Chapter 8 I will define a chemical bond I will describe how ions form I will identify ionic bonding and the characteristics of ionic compounds.
Chapter 8 IONIC COMPOUNDS.
Chapter 8 Ionic Compounds. I. Chemical Bonds The force that holds two atoms together Valence electrons are involved in the formation of chemical bonds.
Ionic Bonding. CA Standards  Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons.
Flashcards for Ionic & Metallic Bonding. What particle is transferred in ionic bonding? Electron.
WHY DO ATOMS BOND TOGETHER? ATOMS WANT TO ACHIEVE A STABLE ELECTRON CONFIGURATION (OR FULL OUTER SHELL OF VALENCE ELECTRONS).
CHAPTER 5: CHEMICAL BONDING Name:Prachayanee Chueamsuwanna Date: Oct. 19,2015.
Chapter 7 Ionic compounds and metals. 7.1 Ion Formation Ions are formed when atoms gain or lose valence electrons to achieve a stable octet electron configuration.
Warm-Up: Put on Page 14 l Write the electron configuration, orbital diagram, and electron dot diagram for the following elements: 1.Iron 2.Sulfur.
Chapter 6: Chemical Bonds When the highest occupied energy level of an atom is filled with e, the atom is stable and not likely to react. In other words,
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.
1 Ionic and Metallic Bonding Ch Review What is a valence electron? –Electrons in the highest (outermost) occupied energy level Related to the group.
Draw an orbital diagram for Al. Electrons and Ions Which electrons are responsible for chemical properties? Valence electrons Core electrons.
Review Game Unit 5 Element Bonding. When the highest occupied energy level of an atom is filled with electrons, the atom is _______ and not likely to.
Chemical Bonding Ionic, Covalent, and Metallic bonding.
Bonding. Think of some properties of salt Forms crystals Brittle Hard Solid High melting and boiling point Forms an electrolyte (conducts electricity.
Ionic, Covalent, Metallic and Hydrogen Bonds Chemical Bonding.
Ionic Compounds. An element’s atoms need to acquire 8 valence electrons in order to be stable like a noble gas. (except for hydrogen and helium which.
The 8 valance electrons in the noble gases make them chemically stable All other Elements “want” their valence electron structure to look like a noble.
Chapters 8 and 9 Ionic and Covalent Bonding. Forming Chemical Bonds Chemical Bond  Force that holds 2 atoms together  Attraction between + nucleus and.
Ionic Bonding.
Ionic Compounds and Metals
Comparison of Properties Ionic Compounds Covalent Compounds Metals
Chapter 6 – Chemical Bonds
Structure of Atom Nucleus  Proton –Positive Charge Neutron-No Charge
Unit 3 Bonding & Chemical Rxns
Binary Ionic Compounds
Ionic Compounds and Metals
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.
Flashcards for Ionic & Metallic Bonding
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.
Ionic Bonding.
Ionic Bonding.
Ionic Bonding.
Chapters 7 and 8 – Bonding.
Presentation transcript:

Ionic Compounds & Covalent Bonding

Forming Chemical Bonds Chemical Bond: the force that holds atoms together. May form by the attraction between a positive nucleus and negative electrons, which result in positive and negative ions. This is because of valence electrons, which are the electrons in the outer shell of the electron cloud that are involved in bonding. Group 1: 1 valence electron Group 2: 2 valence electrons Group 13: 3 valence electrons Group 14: 4 valence electrons Group 15: 5 valence electrons Group 16: 6 valence electrons Group 17: 7 valence electrons Group 18: 8 valence electrons (maximum amount allowed)

Formation of Ions Ion: an atom with a charge (gain or loss of electrons). Cation – positive ion (lost electrons) Anion – negative ion (gained electrons) Atoms gain or lose valence electrons to obtain a complete outer energy shell. (lose to get to 0 / gain to get to 8) Group 1: +1 (loses its 1 valence electron to have zero) Group 2: +2 (loses its 2 valence electrons to have zero) Group 13: +3 (loses its 3 valance electrons to have zero) Group 15: -3 (gains 3 valence electrons to have eight) Group 16: -2 (gains 2 valence electrons to have eight) Group 17: -1 (gains 1 valence electron to have eight)

Ionic Compounds Contain Ions (basically you are adding positives and negatives and balancing to equal 0) Net charge of a compound must be ZERO. Total positive charge = Total negative charge If the positive ion does not equal negative ion, *subscripts* are used to help balance total charges. Symbols, Charges, Switch and Reduce. Example: Sodium, Na, group 1, will lose 1 valence electron (electrons are negative, gives it a +1 charge) Chlorine is group 17, will gain 1 more electron to get to 18 and be like a noble gas, giving it -1 charge (gains 1 negative electron). Together, +1 and -1 are 0, so the compound for Sodium and chlorine is NaCl, named Sodium chloride.

More examples of ionic compounds A compound with Calcium and chlorine forms like this: Calcium is group 2, so loses 2 electrons, +2 charge Chlorine, group 17, gains 1 electron, -1 charge. Symbols: Ca+2 Cl-1 Symbols, charges, switch, reduce (by switch, we mean switch the charges to the opposite atom, make it a subscript, drop the charge) Ca+2 Cl-1 So the formula is Ca1Cl2. There should be 2 Chlorines with 1 Calcium to make this compound neutral. You can drop the ‘1’ as a subscript. CaCl2 Calcium chloride

Properties of Ionic Compounds and hints for naming/writing: Ionic Compounds (Ionic Bonding): Bonding between positive & negative ions. The *metal (groups 1,2, Al and B in 13, and the transition metals) will LOSE ELECTRONS TO BECOME POSITIVE. The *nonmetals (groups 15, 16, 17) will GAIN ELECTRONS TO BECOME NEGATIVE (group 14 shares) Positive ions transfer their electrons to negative ions. Between a metal cation and a non-metal anion. Most called salts, or oxides if the non-metal is oxygen. Strong attractive forces that result in crystal lattice structures. High melting points, high boiling points, hard-rigid-brittle solids.

Binary Compounds with Polyatomic ions Compounds containing more than 2 elements Polyatomic ions (PAI) These are groups of atoms covalently bonded but have one charge, and as a group behave as one substance, example: sulfate ion is SO4-2. In this PAI, there is one Sulfur, 4 Oxygens, together they have a charge of -2. If you remember from your Lewis structures and studies of valence electrons, this means there are 2 extra electrons in the bonding process.

Binary with Polyatomic Ions, cont’d The PAI acts as one unit, and then can bond with a metal or oppositely charged ion to form an ionic bond. The bonding between the atoms IN the PAI is covalent, the bonding between the PAI (polyatomic ion) is *ionic Example: Sodium sulfate, a product found in soaps and shampoos, is Na2SO4 You have a chart with polyatomic ions, *learn it!

Types of Compounds Covalent Compounds (Covalent Bonding) Bonding in which valence electrons are shared. Between only non-metals A molecule is formed when two or more atoms bond covalently. Most elements when found uncombined in nature are monatomic, which means there is one individual atom. A few exceptions include atoms that must exist diatomically, these molecules contain 2 atoms. These are bound covalently, and include: Hydrogen H2 Nitrogen N2 Oxygen O2 Fluorine F2 Chlorine Cl2 Bromine Br2 Iodine I2

Metallic Bonding Transition metals, groups 3-12, or the d block, form metallic bonds with each other, which are strong lattice structures where the positive nuclei are rigid and the electrons travel in the spaces between: They do not share valence electrons with neighboring atoms nor do they lose electrons to form ions when bonding with other transition metals. The outer energy levels of the metals atoms overlap. Electron Sea Model: all metal atoms in a metallic solid contribute their valence electrons to a sea of electrons (called delocalized electrons- because they are free to move and form a metal cation). Metallic Bond: the attraction of a metallic cation for delocalized electrons.

Metallic compound properties Properties: physical properties of metals can be explained by metallic bonding. High Melting Point High Boiling Point Malleable Ductile (they can be drawn into wires) Durable Conductors of heat and electricity

Metallic compounds cont’d Alloy: a mixture of elements that has metallic properties. Alloy’s properties are different than the individual metals in the alloy. Examples include: stainless steel, brass, and bronze which are all mixtures of different transition metals