Bonding in Chemistry. Chemical Bonds All chemical reactions involve breaking of some bonds and formation of new ones where new products are formed.
|
|
- Darleen Bennett
- 5 years ago
- Views:
Transcription
1 CHEMICAL BONDS Atoms or ions are held together in molecules or compounds by chemical bonds. The type and number of electrons in the outer electronic shells of atoms or ions are instrumental in how atoms react with each other to form stable chemical bonds. Over the last 150 years scientists developed several theories to explain why and how elements combine with each other. Bonding in Chemistry Central theme in chemistry: Why and How atoms attach together This will help us understand how to: 1. Predict the shapes of molecules. 2. Predict properties of substances. 3. Design and build molecules with particular sets of chemical and physical properties. CHEMICAL BONDS Two of the most common substance on our dining table are salt and granulated sugar Chemical Bonds All chemical reactions involve breaking of some bonds and formation of new ones where new products are formed. NaCl C 12 H 22 O 11 The properties of substances are determined in large part by the chemical bonds that hold their atoms together 1
2 Bonding Theories Lewis bond Theory Valence Bond Theory Molecular Orbital Theory Lewis Bonding Theory Atoms ONLY come together to produce a more stable electron configuration. Atoms bond together by either transferring or sharing electrons. Many of atoms like to have 8 electrons in their outer shell. Octet rule. There are some exceptions to this rule the key to remember is to try to get an electron configuration like a noble gas. Li and Be try to achieve the He electron arrangement. Lewis Symbols of Atoms Uses symbol of element to represent nucleus and inner electrons. Uses dots around the symbol to represent valence electrons. Puts one electron on each side first, then pair. Remember that elements in the same group have the same number of valence electrons; therefore, their Lewis dot symbols will look alike. Li Be B C N O: :F: :Ne: Valence electrons 2
3 Practice to write the Lewis symbol for Arsenic As is in group 15 (5), therefore it has 5 valence electrons. As Using Lewis Theory to Predict Chemical Formulas Compounds Predict the formula of the compound that forms between calcium and chlorine. Cl Draw the Lewis dot symbols of the elements. Transfer all the valance electrons from the metal to the nonmetal, adding more of each atom as you go, until all electrons are lost from the metal atoms and all nonmetal atoms have 8 electrons. Cl Ca Ca Ca 2+ Cl CaCl 2 Examples for Lewis representation of some chemical bonds F F F F F F H O H O H H O O O O O O Example: Write the Lewis structure of CO 2. Information: Given: CO 2 Find: Lewis structure Solution Map: formula skeletal electron distribution Lewis Total number of valence electrons = = 16 Actually 24 electrons needed for completing the octet of each atom Thus = 8 electrons are shared. Since two electrons make a bond, the molecule should have 4 bonds. The remaining 8 electrons are lone pair electrons O C O 3
4 Practice Draw Lewis Resonance Structures for CNO (C is Central with N and O Attached) C = 4 N = 5 O = 6 (-) = 1 N C O Total = 16 e - N C O Example NO 3 1. Write skeletal structure. N is central because it is the most metallic. 2. Count valence electrons. N = 5 O 3 = 3 x 6 = 18 (-) = 1 Total = 24 e - - TYPES OF CHEMICAL BONDS Ionic bonds Covalent bonds The three possible types of bonds. Metallic bonds 4
5 Ionic compounds consist of a cation and an anion the formula is always the same as the empirical formula the sum of the charges on the cation and anion in each formula unit must equal zero. Lewis bonding theory as able to explain ionic bonds very well. The ionic compound NaCl Ionic bonding Ionic substances are formed when an atom that loses electrons relatively easily react with an atom that has a high affinity for electrons. ex. metal-nonmetal compound Chemical Bonds Ionic bonds are formed by the attraction of oppositely charged ions. 5
6 Ionic Bonds Ions that pack as spheres in a very regular pattern form crystalline substances. Metal to nonmetal. Metal loses electrons to form cation. Nonmetal gains electrons to form anion. The electronegativity between the metal and the nonmetal must be > than 2. Ionic bond results from + to attraction. Larger charge = stronger attraction. Smaller ion = stronger attraction. Lewis theory allows us to predict the correct formulas of ionic compounds. Formation of an Ionic Solid 1. Sublimation of the solid metal M(s) M(g) [endothermic] 2. Ionization of the metal atoms M(g) M + (g) + e - [endothermic] 3. Dissociation of the nonmetal 1/2X 2 (g) X(g) [endothermic] 6
7 More Gains and Losses Can elements lose or gain more than one electron? The element magnesium, Mg, in Group 2 can lose two electron and element oxygen in Group 6 can gain two electrons to form stable Nobel gas configurations. The ions can come together to form a crystal structure. Relative sizes of some ions and their parent atoms. How about the bonds between atoms that have the same electronegativity (as in H-H) or when the electonegativuty difference is < 1.0 (as in C-H)? 7
8 Convalent Bonds Sharing Some atoms are unlikely to lose or gain electrons because the number of electrons in their outer levels makes this difficult. Consider the Lewis dot structure of carbon... C. C e - The alternative is sharing electrons. Covalent Bonds Often found between two nonmetals. Typical of molecular species. Atoms bonded together to form molecules. Strong attraction. Atoms share pairs of electrons to attain octets. Molecules generally weakly attracted to each other. Observed physical properties of molecular substance due to these attractions. Covalent Bonding Electron are shared by nuclei The Convalent Bond Shared electrons are attracted to the nuclei of both atoms. They move back and forth between the outer energy levels of each atom in the covalent bond. So, each atom has a stable outer energy level some of the time. 8
9 FORMATION OF H-H COVALENT BOND The formation of a bond between two atoms. An electron density plot for the H 2 molecule shows that the shared electrons occupy a volume equally distributed over BOTH Hydrogen atoms. Chemical Bonds Covalent bonds form when atoms share 2 or more valence electrons. Covalent bond strength depends on the number of electron pairs shared by the atoms. Electron Density for the H 2 molecule single bond double bond < < triple bond 9
10 Examples of Convalent Bond The neutral particle is formed when atoms share electrons is called a molecule Single Covalent Bonds Two atoms share one pair of electrons. 2 electrons. One atom may have more than one single bond. F F F F F F H O H O H H Double Covalent Bond Two atoms sharing two pairs of electrons. 4 electrons. Shorter and stronger than single bond. Chemical Bonds O O O O O O 10
11 Bond Polarity Bonding between unlike atoms results in unequal sharing of the electrons. One atom pulls the electrons in the bond closer to its side. One end of the bond has larger electron density than the other. The result is bond polarity. The end with the larger electron density gets a partial negative charge and the end that is electron deficient gets a partial positive charge. δ+ H Cl δ- Nonpolar and polar covalent bonds Probability representations of the electron sharing in HF. 11
12 Trends in electronegativity across a period and down a group Nature of bonds and electronegativity Electronegativity Bond difference ( ) > 2 Ionic 0.4 < < 2 Polar covalent < 0.4 Covalent 12
13 In practice no bond is totally ionic. There will always be a small amount of electron sharing. Percent ionic character of chemical bonds as a function of electronegativity difference Dipole Moment of HF Bond Polarity and Dipole Moments 1D= coulomb meter µ=( C)( m)= =4.4 D for fully ionic Measured dipole moment=1.83 D =δ( ) δ= Ionic character=1.83/4.4=41.6% Dipole Moment µ=qr Q: center of charge of magnitude R: distance 13
14 Bond Polarity Polar Molecules and Electric Field = = = 2.1 Pure Covalent Polar Ionic Electronegativity difference Polarized electron of HCl bond 14
15 Percent ionic character of chemical bonds as a function of electronegativity difference Dipole Moment of HF 1D= coulomb meter µ=( C)( m)= =4.4 D for fully ionic Measured dipole moment=1.83 D =δ( ) δ= Ionic character=1.83/4.4=41.6% Molecular Geometry Molecules are three-dimensional objects. We often describe the shape of a molecule with terms that relate to geometric figures. These geometric figures have characteristic corners that indicate the positions of the surrounding atoms with the central atom in the center of the figure. The geometric figures also have characteristic angles that we call bond angles. Valence Shell Electron Pair Repulsion (VSEPR Model) It is used to predict the geometries of molecules formed from nonmetals. Postulate: the structure around a given atom is determined principally by minimizing electron pair repulsion. The bonding and nonbonding pairs should be positioned as far apart as possible. 15
16 Predicting a VSEPR Structure Draw Lewis structure. Put pairs as far apart as possible. Determine positions of atoms from the way electron pairs are shared. Determine the name of molecular structure from positions of the atoms. For non-metals compounds, four pairs of electrons around a given atom prefer prior to form a tetrahedral geometry to minimize the electron repulsions. Draw the Lewis structure Count the pairs of electrons and arrange them to minimize repulsions Determine the positions of the atoms Name the molecular structure 16
17 The bonding pair is shared between two nuclei; and the electrons can be close to either nucleus. A lone pair is localized on only one nucleus, so both electrons are close to that nucleus only. Lone pairs require more space than bonding pair. The bonding pairs are increasingly squeezed together as the number of lone pairs increases. Molecular Geometries Molecular Geometries 17
18 Electron Pairs Practice drawing these shapes below Linear TP Tetra TBP Octa COMPOUND is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds Polarity of Molecules H 2 H 2 O NH 3 CH 4 A diatomic molecule contains only two atoms H 2, N 2, O 2, Br 2, HCl, CO A poly molecule contains more than two atoms In order for a molecule to be polar it must: 1. Have polar bonds. Electronegativity difference theory. Bond dipole moments measured. 2. Have an unsymmetrical shape. Vector addition. Polarity effects the intermolecular forces of attraction. O 3, H 2 O, NH 3, CH 4 18
19 Molecule Polarity The O C bond is polar. The bonding electrons are pulled equally toward both O ends of the molecule. The net result is a nonpolar molecule. Molecule Polarity The H O bond is polar. Both sets of bonding electrons are pulled toward the O end of the molecule. The net result is a polar molecule. 19
20 Water molecule behaves as if it had a positive and negative end. The Covalent Chemical Bond 20
21 Bond Energies Bond breaking requires energy (endothermic). Bond formation releases energy (exothermic). DH = SD(bonds broken) - SD(bonds formed) energy required energy released 21
22 Bond Energies Covalent Bond Energies and Chemical Reactions H 2 +F 2 2HF ΔH=ΣD (bonds broken)-σd (bonds formed) ΔH=D H-H +D F-F -2D H-F = =-544 kj Bond Energy of CH 4 Experimental result : 1652 kj/mol C(g)+4H(g) CH 4 (g) kj/mol An average C-H bond energy per mole of C-H bond: 1652/4=413 (kj/mol) Metallic Bonding The model of metallic bonding can be used to explain the properties of metals. The luster, malleability, ductility, and electrical and thermal conductivity are all related to the mobility of the electrons in the solid. The strength of the metallic bond varies, depending on the charge and size of the cations, so the melting points and DH fusion of metals vary as well. 22
23 10/04/2014 IONIC COMPOUNDS vs METALS SLIP PLANES BREAKING INORGANIC MATERIAL ALLOY vs PURE METAL 23
Chapter 9. Chemical Bonding I: The Lewis Model. HIV-Protease. Lecture Presentation
Lecture Presentation Chapter 9 Chemical Bonding I: The Lewis Model HIV-Protease HIV-protease is a protein synthesized by the human immunodeficiency virus (HIV). This particular protein is crucial to the
More informationChapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
More informationChapter 7 Chemical Bonding
Chapter 7 Chemical Bonding 7.1 Ionic Bonding Octet rule: In forming compounds atoms lose, gain or share electrons to attain a noble gas configuration with 8 electrons in their outer shell (s 2 p 6 ), except
More informationIntroductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 12 Chemical Bonding Structure
More informationChapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective
Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry 11.1 Periodic Trends in Atomic Properties Discuss the atomic trends Metals are located on the left side of the periodic
More informationChapter 8: Concepts of Chemical Bonding
Chapter 8: Concepts of Chemical Bonding Learning Outcomes: Write Lewis symbols for atoms and ions. Define lattice energy and be able to arrange compounds in order of increasing lattice energy based on
More informationIts Bonding Time. Chemical Bonds CH 12
Its Bonding Time Chemical Bonds CH 12 What is a chemical bond? Octet Rule: Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its
More informationChemistry: The Central Science
Chemistry: The Central Science Fourteenth Edition Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds Three basic types of bonds Ionic Electrostatic attraction between ions Covalent Sharing of
More informationCHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Problems: 1-26, 27c, 28, 33-34, 35b, 36(a-c), 37(a,b,d), 38a, 39-40, 41-42(a,c), 43-58, 67-74 12.1 THE CHEMICAL BOND CONCEPT chemical bond: what holds atoms or ions together
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationChapter 6 Chemical Bonding
Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between
More informationOften times we represent atoms and their electrons with Lewis Dot Structures.
They are trying to get their number of valence electrons to either 0 or 8. Group 1: 1 valence electron Group 2: 2 valence electrons Group 13: 3 valence electrons Group 14: 4 valence electrons Group 15:
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.3 Bond Polarity and Dipole Moments 8.5 Energy Effects in Binary Ionic Compounds 8.6 Partial Ionic Character
More informationNOTES: UNIT 6: Bonding
Name: Regents Chemistry: Mr. Palermo NOTES: UNIT 6: Bonding www.mrpalermo.com Name: Key Ideas Compounds can be differentiated by their chemical and physical properties. (3.1dd) Two major categories of
More informationbond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction
bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction ionic compound- a metal reacts with a nonmetal Ionic bonds form when an atom that
More informationCovalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B
Covalent Bonding 1. Obtain the number of valence electrons for each of the following atoms from its group number and draw the correct Electron Dot Notation (a.k.a. Lewis Dot Structures). a. K b. N c. Cl
More informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
More informationChapter 6. Table of Contents. Section 1 Covalent Bonds. Section 2 Drawing and Naming Molecules. Section 3 Molecular Shapes. Covalent Compounds
Covalent Compounds Table of Contents Section 1 Covalent Bonds Section 2 Drawing and Naming Molecules Section 3 Molecular Shapes Section 1 Covalent Bonds Bellringer Make a list of the elements that form
More informationCHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM)
CHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM) Associate Degree in Engineering Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore Community College
More informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and
More informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8. Basic Concepts of Chemical Bonding 8.1 Lewis Symbols and the Octet Rule When atoms or ions are strongly attracted to one another, we say that there is a chemical bond between them. In chemical
More informationIonic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding. Ionic Bonding. Attraction that holds atoms together
BONDING Chemical Bond Attraction that holds atoms together Types include IONIC, METALLIC, or COVALENT Differences in electronegativity determine the bond type Ionic Bond TRANSFER of electrons between atoms
More informationChapter 8 Covalent Boding
Chapter 8 Covalent Boding Molecules & Molecular Compounds In nature, matter takes many forms. The noble gases exist as atoms. They are monatomic; monatomic they consist of single atoms. Hydrogen chloride
More informationUnit 3 - Chemical Bonding and Molecular Structure
Unit 3 - Chemical Bonding and Molecular Structure Chemical bond - A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together 6-1 Introduction
More informationIB Chemistry. Chapter 4.1
IB Chemistry Chapter 4.1 Chemical Bonds Atoms or ions that are strongly attached to one another Chemical bonds will form if potential energy decreases (becomes more stable) 2 Valence Electrons Valence
More informationChapter 8. Ions and the Noble Gas. Chapter Electron transfer leads to the formation of ionic compounds
Chapter 8 Chemical Bonding: General Concepts 1 8.1 Electron transfer leads to the formation of ionic compounds Ionic compounds form when metals and nonmetals react The attraction between positive and negative
More informationNa Cl Wants to lose ONE electron! Na Cl Ionic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding.
BONDING Chemical Bond Attraction that holds atoms together Types include IONIC, METALLIC, or COVALENT Differences in electronegativity determine the bond type Ionic Bond TRANSFER of electrons between atoms
More informationName AP CHEM / / Chapter 8 Outline Bonding: General Concepts
Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Types of Chemical Bonds Information about the strength of a bonding interaction is obtained by measuring the bond energy, which is the energy
More informationBonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationWhat is Bonding? The Octet Rule. Getting an Octet. Chemical Bonding and Molecular Shapes. (Chapter Three, Part Two)
Chemical Bonding and Molecular Shapes (Chapter Three, Part Two) What is Bonding? Bonding describes how atoms interact with each other in an attractive sense. There are three types of bonding: Ionic bonding
More informationUNIT 5.1. Types of bonds
UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence
More informationBonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
More informationBonds can bend and stretch without breaking (bond lengths are averages)
The Structure of Matter What are compounds? Two or more different elements bonded together by VALENCE ELECTRONS o The force that holds two atoms together The ability to write a formula, such as H2O, indicates
More informationCHEMISTRY Matter and Change Section 8.1 The Covalent Bond
CHEMISTRY Matter and Change Section Chapter 8: Covalent Bonding CHAPTER 8 Table Of Contents Section 8.2 Section 8.3 Section 8.4 Section 8.5 Naming Molecules Molecular Structures Molecular Shapes Electronegativity
More informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds An attractive force that holds two atoms together in a more complex unit Three basic types of bonds Ionic Electrons are transferred from one
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationChapter 6. Chemical Bonding
Chapter 6 Chemical Bonding Section 6.1 Intro to Chemical Bonding 6.1 Objectives Define chemical bond. Explain why most atoms form chemical bonds. Describe ionic and covalent bonding. Explain why most chemical
More informationCartoon courtesy of NearingZero.net. Unit 3: Chemical Bonding and Molecular Structure
Cartoon courtesy of NearingZero.net Unit 3: Chemical Bonding and Molecular Structure Bonds Forces that hold groups of atoms together and make them function as a unit. Ionic bonds transfer of electrons
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE The Ionic Bond Formation of Ions The
More informationTypes of Bonding : Ionic Compounds. Types of Bonding : Ionic Compounds
Types of Bonding : Ionic Compounds Ionic bonding involves the complete TRANSFER of electrons from one atom to another. Usually observed when a metal bonds to a nonmetal. - - - - - - + + + + + + + + + +
More informationScientists learned that elements in same group on PT react in a similar way. Why?
Unit 5: Bonding Scientists learned that elements in same group on PT react in a similar way Why? They all have the same number of valence electrons.which are electrons in the highest occupied energy level
More informationChapter 8 Notes. Covalent Bonding
Chapter 8 Notes Covalent Bonding Molecules and Molecular Compounds Helium and Neon are monoatomic, meaning they exist as single atoms Some compounds exist as crystalline solids, such as NaCl Others exist
More informationCHEMICAL BONDS. Electrical forces. Reflect a balance in the attractive and repulsive forces between electrically charged particles
CHEMICAL BONDS Chemical Bonds: Electrical forces. Reflect a balance in the attractive and repulsive forces between electrically charged particles Lewis Theory of Bonding: Electrons play a fundamental role
More informationChemical Bonding AP Chemistry Ms. Grobsky
Chemical Bonding AP Chemistry Ms. Grobsky What Determines the Type of Bonding in Any Substance? Why do Atoms Bond? The key to answering the first question are found in the electronic structure of the atoms
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Questions to Consider What is meant by the term chemical bond? Why do atoms bond with each other to form compounds? How do atoms bond with each other to form
More informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
More informationChemical Bonding I: Covalent Bonding. How are atoms held together in compounds?
I: Covalent Bonding How are atoms held together in compounds? IONIC or COVALENT bonds or forces For most atoms, a filled outer shell contains 8 electrons ----- an octet Atoms want to form octets when they
More informationChapter 6. Preview. Objectives. Molecular Compounds
Section 2 Covalent Bonding and Molecular Compounds Preview Objectives Molecular Compounds Formation of a Covalent Bond Characteristics of the Covalent Bond The Octet Rule Electron-Dot Notation Lewis Structures
More informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More informationAP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
More informationUnit Six --- Ionic and Covalent Bonds
Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples
More informationChapter 7: Chemical Bonding and Molecular Structure
Chapter 7: Chemical Bonding and Molecular Structure Ionic Bond Covalent Bond Electronegativity and Bond Polarity Lewis Structures Orbital Overlap Hybrid Orbitals The Shapes of Molecules (VSEPR Model) Molecular
More informationChapter 8 The Concept of the Chemical Bond
Chapter 8 The Concept of the Chemical Bond Three basic types of bonds: Ionic - Electrostatic attraction between ions (NaCl) Metallic - Metal atoms bonded to each other Covalent - Sharing of electrons Ionic
More informationChemical Bonding Chapter 8
Chemical Bonding Chapter 8 Get your Clicker, 2 magnets, goggles and your handouts Nov 15 6:15 PM Recall that: Ionic-Involves the transfer of electrons - forms between a metal and a nonmetal Covalent-Involves
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 12 Chemical Bonding by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 12 1 Chemical Bond Concept
More informationCHAPTER 12 CHEMICAL BONDING
CHAPTER 12 CHEMICAL BONDING Core electrons are found close to the nucleus, whereas valence electrons are found in the most distant s and p energy subshells. The valence electrons are responsible for holding
More informationChpt 8 Chemical Bonding Forces holding atoms together = Chemical Bonds
Chpt 8 Chemical Bonding Forces holding atoms together = Chemical Bonds Kinds of chemical bonds: 1. Ionic 2. Covalent 3. Metallic Useful guideline: Octet rule Atoms tend to gain, lose, or share e - to achieve
More informationCh. 12 Section 1: Introduction to Chemical Bonding
Name Period Date Chemical Bonding & Intermolecular Forces (Chapter 12, 13 &14) Fill-in the blanks during the PowerPoint presentation in class. Ch. 12 Section 1: Introduction to Chemical Bonding Chemical
More informationChemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds
Chemical Bonding Table of Contents Section 1 Introduction to Chemical Bonding Section 2 Covalent Bonding and Molecular Compounds Section 3 Ionic Bonding and Ionic Compounds Section 4 Metallic Bonding Section
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.2 Electronegativity 8.3 Bond Polarity and Dipole Moments 8.4 Ions: Electron Configurations and Sizes 8.5 Energy
More informationCHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING
CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING 6.1 Introduction to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different
More informationSection 8.1 The Covalent Bond
Section 8.1 The Covalent Bond Apply the octet rule to atoms that form covalent bonds. Describe the formation of single, double, and triple covalent bonds. Contrast sigma and pi bonds. Relate the strength
More informationChapter Nine. Chemical Bonding I
Chapter Nine Chemical Bonding I 1 The Ionic Bond and Lattice Energies 2 Lewis Dot Symbols Consists of atomic symbol surrounded by 1 dot for each valence electron in the atom Only used for main group elements
More informationIonic and Covalent Bonding
1. Define the following terms: a) valence electrons Ionic and Covalent Bonding the electrons in the highest occupied energy level always electrons in the s and p orbitals maximum of 8 valence electrons
More informationChapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
More informationChemical Bonding Basic Concepts
Chemical Bonding Basic Concepts Valence electrons are the outer shell electrons of an atom. The valence electrons are the electrons that particpate in chemical bonding. Group e - configuration # of valence
More informationCHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS
CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence
More informationCovalent Bonding bonding that results from the sharing of electron pairs.
Unit 5 Notes Covalent Bonding, Covalent Compounds, and Intermolecular Forces Chemical Bond a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms
More informationCHEMICAL BONDS. Determining Percentage Composition, Empirical, and Molecular Formulas for Compounds:
CHEMICAL BONDS Chemical Bonds: The strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds (EU 2.C). Reflect a balance in the attractive and repulsive forces
More informationAtoms have the ability to do two things in order to become isoelectronic with a Noble Gas.
CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when
More informationChemistry Chapter 6 Test Review
Chemistry Chapter 6 Test Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A mutual electrical attraction between the nuclei and valence electrons
More informationMolecular Compounds Compounds that are bonded covalently (like in water, or carbon dioxide) are called molecular compounds
Chapter 8: Covalent Bonding Section 1: Molecular Compounds Bonds are Forces that hold groups of atoms together and make them function as a unit. Two types: Ionic bonds transfer of electrons (gained or
More informationChemistry Review Unit 4 Chemical Bonding
Chemistry Review The Nature of Chemical Bonding, Directional Nature of Covalent Bonds, Intermolecular Forces Bonding 1. Chemical compounds are formed when atoms are bonded together. Breaking a chemical
More informationAtoms with a complete outer shell do not react with other atoms. The outer shell is called the valence shell. Its electrons are valence electrons.
Bonding and the Outer Shell Use this table for reference: http://www.dreamwv.com/primer/page/s_pertab.html Atoms with incomplete shells react with others in a way that allows it to complete the outer shell.
More informationName Date Class MOLECULAR COMPOUNDS. Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides
8.1 MOLECULAR COMPOUNDS Section Review Objectives Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides Vocabulary covalent bond molecule diatomic molecule
More informationChapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More informationBig Idea: Ionic Bonds: Ionic Bonds: Metals: Nonmetals: Covalent Bonds: Ionic Solids: What ions do atoms form? Electron Electron
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More informationWhat is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds?
Chapter 8 What is a Bond? A force that holds atoms together. Why? We will look at it in terms of energy. Bond energy- the energy required to break a bond. Why are compounds formed? Because it gives the
More informationCovalent Molecules and Lewis Structures Time required: two 50-minute periods
Mega Molecules, LLC!!!!! Name: Hands-On Science with Molecular Models!! Date:!!!!!!!! Hour: Introduction Covalent Molecules and Lewis Structures Time required: two 50-minute periods To study covalent molecules,
More informationChem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept
Chem 1075 Chapter 12 Chemical Bonding Lecture Outline Slide 2 Chemical Bond Concept Recall that an atom has and electrons. Core electrons are found to the nucleus. Valence electrons are found in the s
More informationElectrons responsible for the chemical properties of atoms Electrons in the outer energy level Valence electrons are the s and p electrons in the
Electrons responsible for the chemical properties of atoms Electrons in the outer energy level Valence electrons are the s and p electrons in the outermost, or highest energy level The number of Valence
More informationChapter 8. Chemical Bonding I: Basic Concepts
Chapter 8 Chemical Bonding I: Basic Concepts Topics Lewis Dot Symbols Ionic Bonding Covalent Bonding Electronegativity and Polarity Drawing Lewis Structures Lewis Structures and Formal Charge Resonance
More informationChapter 6. Preview. Lesson Starter Objectives Chemical Bond
Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in
More informationChemical Bonding -- Lewis Theory (Chapter 9)
Chemical Bonding -- Lewis Theory (Chapter 9) Ionic Bonding 1. Ionic Bond Electrostatic attraction of positive (cation) and negative (anion) ions Neutral Atoms e - transfer (IE and EA) cation + anion Ionic
More informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationCh 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules
Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES
More informationCh 9 Liquids & Solids (IMF) Masterson & Hurley
Ch 9 Liquids & Solids (IMF) Masterson & Hurley Intra- and Intermolecular AP Questions: 2005 Q. 7, 2005 (Form B) Q. 8, 2006 Q. 6, 2007 Q. 2 (d) and (c), Periodic Trends AP Questions: 2001 Q. 8, 2002 Q.
More informationCHEMISTRY. Chapter 9 The Basics of Chemical Bonding. The Molecular Nature of Matter. Jespersen Brady Hyslop SIXTH EDITION
CEMISTRY The Molecular Nature of Matter SIXT EDITIN Jespersen Brady yslop Chapter 9 The Basics of Chemical Bonding Copyright 2012 by John Wiley & Sons, Inc. Chemical Bonds Attractive forces that hold atoms
More informationConcepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds. David A. Katz Pima Community College Tucson, AZ
Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds David A. Katz Pima Community College Tucson, AZ Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction
More informationChapter 6. Preview. Lesson Starter Objectives Chemical Bond
Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in
More information4/6/2015. Formed between metals and non-metals Opposite sides of the periodic table CHEMICAL BOND IONIC VS. COVALENT BONDS CHEMICAL BONDING BOND TYPES
CEMICAL BOND CEMICAL BONDING BOND TYPES IONIC VS. COVALENT BONDS Ionic Bond bonding between a metal (cation) & a non metal (anion) that involves the transfer of electrons from cation to anion (forms compounds)
More informationChapter 9 Ionic and Covalent Bonding
Chem 1045 Prof George W.J. Kenney, Jr General Chemistry by Ebbing and Gammon, 8th Edition Last Update: 06-April-2009 Chapter 9 Ionic and Covalent Bonding These Notes are to SUPPLIMENT the Text, They do
More informationSection 6.2 1/13/2014. Most Chemical Compounds. Molecular (or Covalent) Compound. Covalent Bonding and Molecular Compounds
Section 6.2 Covalent Bonding and Molecular Compounds Most Chemical Compounds Are molecules, a neutral group of atoms that are held together by covalent bonds. It is a single unit capable of existing on
More informationWorksheet 5 - Chemical Bonding
Worksheet 5 - Chemical Bonding The concept of electron configurations allowed chemists to explain why chemical molecules are formed from the elements. In 1916 the American chemist Gilbert Lewis proposed
More informationChemical Bonding I: Basic Concepts
Chapter 8 Chemical Bonding I: Basic Concepts Dr. A. Al-Saadi 1 Chapter 8 Preview Ionic Bonding vs. covalent bonding. Electronegativity and dipole moment. Bond polarity. Lewis structure: ow to draw a Lewis
More informationIntroduction to Chemical Bonding
Chemical Bonding Introduction to Chemical Bonding Chemical bond! is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together Why are most
More informationChemical Bonding I: Basic Concepts
Chemical Bonding I: Basic Concepts Chapter 9 Valence electrons are the outer shell electrons of an atom. The valence electrons are the electrons that participate in chemical bonding. Group e - configuration
More informationChapter 8 Concepts of Chemical. Bonding
Chapter 8 Concepts of 8.1 Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms. Electrons are free
More informationCHEMICAL BONDING COVALENT BONDS IONIC BONDS METALLIC BONDS
CHEMICAL BONDING COVALENT BONDS IONIC BONDS METALLIC BONDS Metallic Bonds How atoms are held together in solid metals. Metals hold onto their valence electrons very weakly. Think of them as positive ions
More information