Unit Six --- Ionic and Covalent Bonds

Size: px
Start display at page:

Download "Unit Six --- Ionic and Covalent Bonds"

Transcription

1 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 Mg: 1s 2 2s 2 2p 6 3s 2 2 valence e - in level 3 Br: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 7 valence e - in level 4 Identification of group number gives valence electrons for the representative elements Group 1A elements (i.e., hydrogen, lithium, etc.) have 1 valence electron Group 6A elements (i.e., oxygen, sulfur, etc.) have 6 valence electrons Usually the only electrons used in chemical bonds Only electrons shown in the electron dot structures Electron Dot Structures Oxygen Nitrogen Sodium Calcium (6 valence e - ) (5 valence e - ) (1 valence e) (2 valence e - )

2 Electron Configurations for Ions Ions strive to become like noble gases Octet rule Atoms tend to achieve the electron configuration of a noble gas Ions strive to have 8 valence electrons Metals will lose electrons to go back to a noble gas configuration in the greatest energy level of their electron configurations Nonmetals will gain electrons to go to a noble gas configuration in the greatest energy level of their electron configurations Transition metals will go to a pseudo-noble gas configuration in their electron configurations Electron Configurations for Cations 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 + e - 8 valence electrons in the highest energy level Electron Configurations for Cations Electron Configurations for Cations 1s 2 2s 2 2p 6 3s 2 1s 2 2s 2 2p 6 + 2e - 8 valence electrons in the highest energy level 1s 2 2s 2 2p 6 3s 2 3p 1 1s 2 2s 2 2p 6 + 3e - 8 valence electrons in the highest energy level

3 Electron Configurations for Cations (Transition Metals) Ideally, transition metals would have to lose their d orbital electrons to achieve a noble gas configuration. Example: Cobalt (1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7 ) would have to lose nine electrons to get back to a noble gas configuration. Transition metals can have pseudo-noble gas electron configurations by typically losing the s orbital electrons. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7 1s 2 2s 2 2p 6 3s 2 3p 6 3d 7 15 electrons in the outer energy level Still a pseudo-noble gas configuration because of the s and p orbitals being filled Electron Configurations for Anions 1s 2 2s 2 2p 3 + 3e - 1s 2 2s 2 2p 6 8 valence electrons in the highest energy level Electron Configurations for Anions Electron Configurations for Anions 1s 2 2s 2 2p 4 + 2e - 1s 2 2s 2 2p 6 8 valence electrons in the highest energy level 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 + 1e - 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 8 valence electrons in the highest energy level

4 -- Ionic Bonds -- Ionic Bonds Forces of attraction that bind oppositely charged ions Examples Sodium chloride Na + attracted to a Cl - Aluminum bromide Al 3+ attracted to 3 Br - Electromagnetic attraction Transfer (NOT sharing) of electron(s) from one neutral atom to another neutral atom to create ions Each ion will have an octet in the outer shell Exceptions: transition metals -- Ionic Bonds -- Formation of Ionic Bonds 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 3s 2 3p 5 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 Transfer of the 3s 1 electron of the Na to the p orbital of the Cl Both ions now have octets -- Ionic Bonds -- Formation of Ionic Bonds -- Ionic Bonds -- Aragonite (CaCO 3 ) Barite (BaSO 4 ) Calcite (CaCO 3 ) 1s 2 2s 2 2p 6 3s 2 1s 2 2s 2 2p 4 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 Transfer of the 3s 2 electrons of the Mg to the p orbital of the O Both ions now have octets Hematite (Fe 2 O 3 ) Pyrite (FeS 2 ) Crystalline solids result from structured arrangements of ionic bonds.

5 -- Ionic Bonds -- Properties of Ionic Most ionic compounds are crystalline solids. Ions are arranged in repeating, three-dimensional patterns. Fourteen kinds of arrangements Coordination number Number of ions of opposite charge that surround the ion in a crystal -- Ionic Bonds -- Properties of Ionic Sodium chloride (NaCl) -- Ionic Bonds -- Properties of Ionic Cesium chloride (CsCl) Face-centered cubic structure Coordination number of 6 (6 Cl - ions around each Na + ion) Simple cubic structure Coordination number of 8 (8 Cl - ions around each Cs + ion)

6 -- Bonding in Metals -- Metallic Bonds and Metallic Properties Metallic Bonds Consist of the attraction of free-floating valence electrons for positivelycharged metal ions What hold the metal together Allow for malleability (ability to reshape and bend) Allow for conductivity Alloys Mixtures of two or more elements, at least one of which is a metal Generally made by melting a mixture of the elements and then cooling the mixture Properties are often superior to lone metals Steels The Nature of Covalent Bonds Bonding Theories Polar Bonds and Molecules Unit Six: Covalent Bonding Single Covalent Bonds Two atoms share one pair of electrons Each atom ideally achieves an octet in a covalent bond so that they resemble the electron configuration of a noble gas The Nature of Covalent Bonds Structural formula is a chemical formula showing the arrangment of atoms in a molecule

7 Array of sodium ions and chloride ions: Collection of water molecules: Formula unit of sodium chloride: Molecule of water: Na + Cl - H O H Chemical formula: NaCl Chemical formula: H 2 O Single Covalent Bonds Covalent bonds result from combinations of nonmetals (I.e., group 4A, 5A, 6A, and 7A elements) Single Covalent Bonds - Halogens Unshared pairs Also known as lone pairs Pairs of valence electrons that are not shared between atoms of a molecule Unshared pairs do not change form in a structural formula

8 Single Covalent Bonds Larger Molecules Single Covalent Bonds Larger Molecules Single Covalent Bonds Larger Molecules Spreading out the electrons More stability Less energy required Preferred arrangements Double Covalent Bonds Bonds that involve two shared pairs of electrons Used to attain stable noble-gas configurations

9 Double Covalent Bonds Double Covalent Bonds -- Exceptions Oxygen gas (O 2 ) Expectation: formation of a double-bond to achieve octets Evidence: formation of a single-bond with two electrons in the gas being unpaired Triple Covalent Bonds Bonds that involve three shared pairs of electrons Used to attain stable noble-gas configurations Coordinate Covalent Bonds Covalent bond in which an atom contributes both bonding electrons Structural formulas of coordinate covalent bonds show the bonds as arrows that point from the atom donating the pair of electrons to the atom receiving them Examples Carbon monoxide (CO) Ammonium ion (NH 4+ ) Sulfur dioxide (SO 2 )

10 Coordinate Covalent Bonds Carbon Monoxide (CO) Coordinate Covalent Bonds Ammonium Ion (NH 4+ ) An octet has been achieved for each molecule, but nitrogen contributes the electrons needed. An octet has been achieved for each molecule, but oxygen contributes the electrons needed. Bond Dissociation Energies Total energy required to sever the bond between two covalently bonded atoms High in carbon compounds, resulting in high stability of carbon compounds Table 16.3, page 448 Resonance Example: H H kj H + H This means that it would require 435 kj of energy to break the bond between the two atoms in a hydrogen gas molecule (H 2 ). Structures that occur when it is possible to write two or more valid Lewis dot structures that have the same number of electron pairs for a molecule or ion Structures are in constant resonance NOTE: Single bonds are longer than double bonds; double bonds are longer than triple bonds

11 Exceptions to the Octet Rule Impossibilities occur where using the octet rule does not work. Examples: Nitrogen dioxide (NO 2 ) Oxygen gas (O 2 ) Phosphorus pentachloride (PCl 5 ) Sulfur hexafluoride (SF 6 ) Exceptions to the Octet Rule Nitrogen Dioxide (NO 2 ) Exceptions to the Octet Rule Phosphorus Pentachloride (PCl 5 ) Exceptions to the Octet Rule Sulfur Hexafluoride (SF 6 )

12 Exceptions to the Octet Rule Cases for exceptions More than 8 valence electrons Less than 8 valence electrons How to draw Typically, the central atom will be the first one listed in the formula. Hydrogens and halogens will typically surround the central atom. Diamagnetic Substance weakly repelled by a magnetic field Paramagnetic Substance strongly attracted to a magnetic field These substances have molecules containing two or more unpaired electrons. Not to be confused with ferromagnetism (as with magnets) Mass if offset in a magnetic field Unit Six: Covalent Bonding Bonding Theories Molecular Orbitals Covalent bonding occurs as a result of an imbalance between the attractions and the repulsions of the nuclei and the electrons of the atoms. If two atoms don t bond, the repulsion between nuclei of two atoms and the atoms electrons is greater than the attractions of the electrons to the opposing nuclei. If two atoms do bond, the attractions of the electrons to the opposing nuclei is greater than the repulsion between nuclei of the two atoms and the atoms electrons. Pi bonds ( ) and sigma bonds ( ) are responsible for covalent bonding. Overlapping of orbitals cause bonds. Sharing of electrons from overlapping Symmetrical bonding VSEPR Theory Valence Shell Electron Pair Repulsion Theory Electron pairs around atoms tend to be as far apart as possible. Similar charges (I.e., negative charges from electrons) tend to repel each other and want to be spaced apart at maximum angles. Used to predict molecular geometries Bond angles Angles between bonds Spacing apart as far as possible Lone pairs of electrons will repel bonded atoms a bit more than expected toward each other around the central atom

13 Species type: AX 3 Geometry: Trigonal planar Predicted bond angle(s): 120 Species type: AX 4 Geometry: Tetrahedral Predicted bond angle(s): Example of geometry: CO 3 2- : Example of geometry: CH 4 : Species type: AX 5 Geometry: Trigonal bipyramidal Predicted bond angle(s): 90, 120, 180 Species type: AX 6 Geometry: Octahedral Predicted bond angle(s): 90, 180 Example of geometry: PCl 5 : Example of geometry: SF 6 :

14 Species type: AX 2 E 2 (E: lone electron pair around the central atom) Geometry: Bent Predicted bond angle(s): H 2 O: Species type: AX 2 E 3 (E: lone electron pair around the central atom) Geometry: Linear Predicted bond angle(s): 180 Example of geometry: XeF 2 : Species type: AX 3 E 2 (E: lone electron pair around the central atom) Geometry: T-shaped Predicted bond angle(s): 90, 180 Example of geometry: F 3 : Species type: AX 4 E (E: lone electron pair around the central atom) Geometry: See-saw Predicted bond angle(s): 90, 120, 180 Example of geometry: SeCl 4 :

15 Species type: AX 4 E 2 (E: lone electron pair around the central atom) Geometry: Square planar Predicted bond angle(s): 90, 180 Example of geometry: XeF 4 : Species type: AX 5 E (E: lone electron pair around the central atom) Geometry: Square pyramidal Predicted bond angle(s): 90, 180 Example of geometry: ClF 5 : Hybrid Orbitals Hybridization Atomic orbitals mix to form the same total number of equivalent hybrid orbitals Number of hybrid orbitals is equal to the number of atomic orbitals that are mixed Classifications sp: One s orbital is mixed with one p orbital sp 2 : One s orbital is mixed with two p orbitals sp 3 : One s orbital is mixed with three p orbitals Explains why atoms that should not be able to bond covalently can bond Based on the number of electrons pairs Unshared as well as shared electron pairs can be located in hybrid orbitals sp 3 hybridization : hydrogen electrons bonding with carbon electrons Carbon should only be able to bond with two other electron orbitals normally, but it can bond with four when its orbitals are hybridized.

16 Number of electron pairs Hybrid Orbitals and Their Geometries Atomic Orbitals Hybrid Orbitals Geometry Examples 2 s, one p sp Linear BeF 2, CO 2 Unit Six: Covalent Bonding Polar Bonds and Molecules 3 s, two p sp 2 Trigonal planar 4 s, three p sp 3 Tetrahedron BF 3, CO 3 2-, SO 3 CH 4, NH 3, H 2 O -- Polar Bonds and Molecules -- Bond Polarity The Tug of War The pairs of electrons that are bonds between atoms are pulled between the nuclei of the atoms in a bond. The electronegativities of the atoms determine the winner. Classifications for Bonds Nonpolar covalent When atoms pull the bond equally Happens with two atoms of equal electronegativity, most often using the same atoms Examples: H 2, O 2, N 2 Polar covalent When atoms pull the bond unequally Happens with two atoms of different electronegativities Example: HCl, HF, NH -- Polar Bonds and Molecules -- Bond Polarity Ionic When atoms pull the bond equally in an ionic compound Happens with two atoms of different electronegativities, most often using a metal and a nonmetal Examples: NaCl, KBr In a polar molecule, one end of the molecule is slightly more electronegative than the other atom, resulting in one atom being slightly negative ( -) because of higher electronegativitiy, and the other atom being slightly positive ( +) because of lower electronegativity. is known as a partial charge since it is much less than 1+ or 1- charge.

17 -- Polar Bonds and Molecules -- Bond Polarity Electronegativities and Bond Types See page 405, Table 14.2 for electronegativities. H: 2.1 Cl: 3.0 Since hydrogen is less, it will have the positive partial charge while chlorine has the negative partial charge = 0.9 HCl is polar covalent difference Nonpolar covalent bond H H (0.0 difference) difference difference Moderately covalent bond Very polar covalent bond H Cl (0.9 difference) H F (1.9 difference) -- Polar Bonds and Molecules -- Polar Molecules Dipole Molecule that has two poles Example: HCl from the previous page Polar vs. Nonpolar Water will be polar (charge goes from bottom to top even though the two cancel out sideways) Carbon dioxide will be nonpolar because the charges cancel out in all directions difference Ionic bond Na + Cl - (2.1 difference) -- Polar Bonds and Molecules -- Intermolecular Attractions van der Waals forces Two types: dispersion forces and dipole interactions Dispersion forces Weakest of all molecular interactions Caused by movement of electrons Strength increases as number of electrons in the molecule increases Examples: Br-Br, F-F, etc. Dipole interactions Occurs when polar molecules are attracted to one another Partial charge ( +) of one polar molecule is attracted to the opposite partial charge ( -) of another molecule -- Polar Bonds and Molecules -- Attractions Between Molecules Hydrogen bonding Hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom Example: water

18 Characteristics of Ionic and Covalent Characteristic Ionic Compound Covalent Compound Representative unit Formula unit Molecule Bond formation Transfer of electrons Sharing of electrons Types of elements Metals and nonmetals Nonmetals Physical state at room temperature Solid Solid, liquid, gas Melting point High (> 300 C) Low (< 300 C) Solubility in water Usually high High to low Electrical conductivity of aqueous solution Good conductor Poor conductor or doesn t conduct at all

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons

Covalent 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 information

Ch 6 Chemical Bonding

Ch 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 information

Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals

Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals 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 Mg: 1s 2 2s 2 2p 6 3s 2 2 valence e

More information

Chapter 8 Covalent Boding

Chapter 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 information

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons

Covalent 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 information

Molecular Compounds Compounds that are bonded covalently (like in water, or carbon dioxide) are called molecular compounds

Molecular 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 information

Na Cl Wants to lose ONE electron! Na Cl Ionic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding.

Na 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 information

Ionic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding. Ionic Bonding. Attraction that holds atoms together

Ionic 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 information

CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS

CHEMICAL 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 information

Bonding. Honors Chemistry 412 Chapter 6

Bonding. 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 information

Introduction to Chemical Bonding

Introduction 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 information

Chapter 16 Covalent Bonding

Chapter 16 Covalent Bonding Chemistry/ PEP Name: Date: Chapter 16 Covalent Bonding Chapter 16: 1 26; 28, 30, 31, 35-37, 40, 43-46, Extra Credit: 50-53, 55, 56, 58, 59, 62-67 Section 16.1 The Nature of Covalent Bonding Practice Problems

More information

Ionic and Covalent Bonding

Ionic 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 information

Bonding: 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. (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 information

Name Date Class MOLECULAR COMPOUNDS. Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides

Name 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 information

Bonding: 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. (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 information

Bonding. Polar Vs. Nonpolar Covalent Bonds. Ionic or Covalent? Identifying Bond Types. Solutions + -

Bonding. Polar Vs. Nonpolar Covalent Bonds. Ionic or Covalent? Identifying Bond Types. Solutions + - Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Bonding onors Chemistry 412 Chapter 6 Types of Bonds Ionic Bonds Force of attraction

More information

Chapter 12. Chemical Bonding

Chapter 12. Chemical Bonding Chapter 12 Chemical Bonding Chapter 12 Introduction to Chemical Bonding Chemical Bonding Valence electrons are the electrons in the outer shell (highest energy level) of an atom. A chemical bond is a mutual

More information

Chapter 8 : Covalent Bonding. Section 8.1: Molecular Compounds

Chapter 8 : Covalent Bonding. Section 8.1: Molecular Compounds Chapter 8 : Covalent Bonding Section 8.1: Molecular Compounds What is a molecule? A molecular compound? A molecule is a neutral group of atoms joined together by covalent bonds A molecular compound is

More information

Chemical Bonds. Chapter 6

Chemical Bonds. Chapter 6 Chemical Bonds Chapter 6 1 Ch. 6 Chemical Bonding I. How and Why Atoms Bond A. Vocabulary B. Chemical Bonds - Basics C. Chemical Bonds Types D. Chemical Bonds Covalent E. Drawing Lewis Diagrams F. Bond

More information

Chapter 6. Preview. Objectives. Molecular Compounds

Chapter 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 information

Chapter 7. Ionic & Covalent Bonds

Chapter 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 information

Chemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds

Chemical 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 information

Chapter 8 H H H H. Molecular Compounds & Covalent Bonding. Why do covalent bonds form? 8.1 Molecular Compounds. Properties of Molecular Compounds

Chapter 8 H H H H. Molecular Compounds & Covalent Bonding. Why do covalent bonds form? 8.1 Molecular Compounds. Properties of Molecular Compounds Chapter 8 Molecular Compounds & Covalent Bonding Why do covalent bonds form? If only group 5A, 6A, 7A atoms existed, ionic bonds can t form. NNMETALS Each atom needs electrons so they are not willing to

More information

Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas.

Atoms 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 information

Chapter 6. Preview. Lesson Starter Objectives Chemical Bond

Chapter 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 information

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules

Ch 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 information

Chapter 6. Preview. Lesson Starter Objectives Chemical Bond

Chapter 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 information

of its physical and chemical properties.

of its physical and chemical properties. 8.4 Molecular Shapes VSEPR Model The shape of a molecule determines many of its physical and chemical properties. Molecular l geometry (shape) can be determined with the Valence Shell Electron Pair Repulsion

More information

CHEMISTRY Matter and Change Section 8.1 The Covalent Bond

CHEMISTRY 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 information

Chemical bonding is the combining of elements to form new substances.

Chemical bonding is the combining of elements to form new substances. Name Covalent Bonding and Nomenclature: Unit Objective Study Guide Class Period Date Due 1. Define chemical bonding. What is chemical bonding? Chemical bonding is the combining of elements to form new

More information

Chapters and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity

Chapters and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity Chapters 7.1-2 and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity Chemical Bonds and energy bond formation is always exothermic As bonds form, chemical potential energy is released as other

More information

CHAPTER 12 CHEMICAL BONDING

CHAPTER 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 information

CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING

CHAPTER 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 information

Bonding Practice Exam

Bonding Practice Exam Bonding Practice Exam Matching Match each item with the correct statement below. a. halide ion e. valence electron b. octet rule f. coordination number c. ionic bond g. metallic bond d. electron dot structure

More information

Chapter 4. Molecular Structure and Orbitals

Chapter 4. Molecular Structure and Orbitals Chapter 4 Molecular Structure and Orbitals Chapter 4 Table of Contents (4.1) (4.2) (4.3) (4.4) (4.5) (4.6) (4.7) Molecular structure: The VSEPR model Bond polarity and dipole moments Hybridization and

More information

LET S FIRST REVIEW IONIC BONDING

LET S FIRST REVIEW IONIC BONDING COVALENT BONDING LET S FIRST REVIEW IONIC BONDING In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds. K F K F K F K F K F K F K + F _ The compound potassium

More information

Chapter 7. Chemical Bonding I: Basic Concepts

Chapter 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 information

Unit 9: CHEMICAL BONDING

Unit 9: CHEMICAL BONDING Unit 9: CHEMICAL BONDING 1 Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to

More information

Unit 9: CHEMICAL BONDING

Unit 9: CHEMICAL BONDING Unit 9: CHEMICAL BONDING 1 Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to

More information

Ch. 12 Section 1: Introduction to Chemical Bonding

Ch. 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 information

Chapter 6. Chemical Bonding

Chapter 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 information

Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure

Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure Cartoon courtesy of NearingZero.net Chemical Bonding and Molecular Structure Chemical Bonds Forces that hold groups of atoms together and make them function as a unit. 3 Major Types: Ionic bonds transfer

More information

SL Score. HL Score ! /30 ! /48. Practice Exam: Paper 1 Topic 4: Bonding. Name

SL Score. HL Score ! /30 ! /48. Practice Exam: Paper 1 Topic 4: Bonding. Name Name Practice Exam: Paper 1 Topic 4: Bonding SL SL Score! /30 HL Score! /48 1. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen? A. B. C. D.

More information

Subtopic 4.2 MOLECULAR SHAPE AND POLARITY

Subtopic 4.2 MOLECULAR SHAPE AND POLARITY Subtopic 4.2 MOLECULAR SHAPE AND POLARITY 1 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to

More information

Chapter 7 Chemical Bonding

Chapter 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 information

Name Date Class MOLECULAR COMPOUNDS. Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides

Name 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 information

Covalent bonding does not involve electrostatic attraction between oppositely charged particles.

Covalent bonding does not involve electrostatic attraction between oppositely charged particles. SCH3U7 - Topic 4: Bonding Review SL Which of these bonding types would not be classified as strong? Metallic Covalent Ionic Dipole dipole The bond dissociation energy of NaCl is 411 kj mol -1, while that

More information

NOTES: Unit 4: Bonding

NOTES: Unit 4: Bonding Name: Regents Chemistry: Mr. Palermo Student Version NOTES: Unit 4: Bonding Name: 1. Ion 2. Positive/Negative ion 3. Stable Octet 4. Diatomic Molecules 5. Electronegativity 6. Ionic Bond 7. Covalent Bond

More information

Chemical Bonding. Burlingame High School

Chemical Bonding. Burlingame High School Chemical Bonding Electronegativity Is a measure of the ability of an atom in a molecule to attract electrons to itself. Concept proposed by Linus Pauling 1901-1994 Electronegativity Trends Forms of Chemical

More information

What is Bonding? The Octet Rule. Getting an Octet. Chemical Bonding and Molecular Shapes. (Chapter Three, Part Two)

What 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 information

Unit 3 - Chemical Bonding and Molecular Structure

Unit 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 information

Chapter 7 Chemical Bonding and Molecular Structure

Chapter 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 information

Bonding. Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms

Bonding. Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms Chemical Bonding Bonding Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms Type of bond depends on electron configuration and electronegativity Why do

More information

UNIT 5.1. Types of bonds

UNIT 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 information

Honors Chemistry - Unit 9 Chapter 6: Bonding & Molecular Structures. Unit 9 Packet Page 1 of 14

Honors Chemistry - Unit 9 Chapter 6: Bonding & Molecular Structures. Unit 9 Packet Page 1 of 14 Honors Chemistry - Unit 9 Chapter 6: Bonding & Molecular Structures Unit 9 Packet Page 1 of 14 Vocab Quiz: UT Due: Test Date: Quiz Date(s): FORMULAS/CONSTANTS Memorize VSEPR Chart First 6 Shapes!! OBJECTIVES:

More information

NOTES: 8.4 Polar Bonds and Molecules

NOTES: 8.4 Polar Bonds and Molecules NOTES: 8.4 Polar Bonds and Molecules ELECTRONEGATIVITY: We ve learned how valence electrons are shared to form covalent bonds between elements. So far, we have considered the electrons to be shared equally.

More information

Chemical Bonding Chapter 8

Chemical 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 information

VSEPR. Valence Shell Electron Pair Repulsion Theory

VSEPR. Valence Shell Electron Pair Repulsion Theory VSEPR Valence Shell Electron Pair Repulsion Theory Vocabulary: domain = any electron pair or bond (single, double or triple) is considered one domain. bonding pair = shared pair = any electron pair that

More information

***Occurs when atoms of elements combine together to form compounds.*****

***Occurs when atoms of elements combine together to form compounds.***** CHEMICAL BONDING ***Occurs when atoms of elements combine together to form compounds.***** Formation of compounds involve adjustments in the position of one or more valence electrons. PE is lower in bonded

More information

CHAPTER 12: CHEMICAL BONDING

CHAPTER 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 information

CHEMICAL 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) 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 information

Chapter 6 Chemistry Review

Chapter 6 Chemistry Review Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in

More information

Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules

Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules 1. Ionic bonds 2. Covalent bonds (also co-ordinate covalent bonds) 3. Metallic bonds 4. Van der Waals forces

More information

Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit

Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit Covalent Bonding Section 8.1 The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes Section 8.5 Electronegativity and Polarity Click a hyperlink or

More information

Notes: Covalent Bonding

Notes: Covalent Bonding Name Chemistry Pre-AP Notes: Covalent Bonding Period The main focus of this unit is on the covalent bond; however, we will briefly treat the ionic and metallic bond as well. I. Chemical Bonding Overview

More information

Chapter 12. Chemical Bonding

Chapter 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 information

Molecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2

Molecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2 1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact

More information

Chapter 8: Covalent Bonding. Chapter 8

Chapter 8: Covalent Bonding. Chapter 8 : Covalent Bonding Bonding Ionic Bonding - attracted to each other, but not fully committed Covalent Bonding - fully committed, and shares everything Two methods to gain or lose valence electrons: Transfer

More information

AS91164 Bonding, structure, properties and energychanges Level 2 Credits 5

AS91164 Bonding, structure, properties and energychanges Level 2 Credits 5 AS91164 Bonding, structure, properties and energychanges Level 2 Credits 5 LEWIS DIAGRAMS, SHAPES OF MOLECULES, POLAR AND NON POLAR MOLECULES Lewis diagrams: use dots (or x) to represent electrons, show

More information

Molecular Geometry & Polarity

Molecular Geometry & Polarity Molecular Geometry & Polarity Learn Shapes you will Because the physical and chemical properties of compounds are tied to their structures, the importance of molecular geometry can not be overstated. Localized

More information

Chapter 6 PRETEST: Chemical Bonding

Chapter 6 PRETEST: Chemical Bonding Chapter 6 PRETEST: Chemical In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.The charge on an ion is a. always positive.

More information

Chapter 8 Notes. Covalent Bonding

Chapter 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 information

Covalent Bonding. Chapter 8. Diatomic elements. Covalent bonding. Molecular compounds. 1 and 7

Covalent Bonding. Chapter 8. Diatomic elements. Covalent bonding. Molecular compounds. 1 and 7 hapter 8 ovalent bonding ovalent Bonding A metal and a nonmetal transfer An ionic bond Two metals just mix and don t react An alloy What do two nonmetals do? Neither one will give away an electron So they

More information

Chemical Bonding AP Chemistry Ms. Grobsky

Chemical 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 information

Ex. 1) F F bond in F = 0 < % covalent, no transfer of electrons

Ex. 1) F F bond in F = 0 < % covalent, no transfer of electrons #60 Notes Unit 8: Bonding Ch. Bonding I. Bond Character Bonds are usually combinations of ionic and covalent character. The electronegativity difference is used to determine a bond s character. Electronegativity

More information

Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry

Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents

More information

Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry

Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents

More information

Covalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B

Covalent 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 information

Chem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept

Chem 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 information

Chapter 6. The Chemical Bond

Chapter 6. The Chemical Bond Chapter 6 The Chemical Bond Some questions Why do noble gases rarely bond to other elements? How does this relate to why the atoms of other elements do form bonds? Why do certain elements combine to form

More information

c. Ionic bonding d. Covalent bonding i. nonpolar covalent bonding

c. Ionic bonding d. Covalent bonding i. nonpolar covalent bonding Chapter 11: Chemical Bonding I. Introduction to Chemical Bonding a. Types of chemical bonding i. A chemical bond is a mutual attraction between nuclei and the valence electrons of different atoms that

More information

Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit

Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit Covalent Bonding Section 8.1 The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes Section 8.5 Electronegativity and Polarity Click a hyperlink or

More information

Unit 9: CHEMICAL BONDING

Unit 9: CHEMICAL BONDING Unit 9: CEMICAL BNDING Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to the

More information

* one of these choices is not used

* one of these choices is not used IONIC BONDING REVIEW WORKSHEET Part 1 - Complete each of the following sentences by filling in the appropriate word or phrase from the list below. negative noble gas octet anion positive electrons ions

More information

Chemistry Chapter 6 Test Review

Chemistry 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 information

Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons

Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent bonds there is a of electrons to get an

More information

AP Chemistry. Unit #7. Chemical Bonding & Molecular Shape. Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING. Discrete molecules formed

AP Chemistry. Unit #7. Chemical Bonding & Molecular Shape. Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING. Discrete molecules formed AP Chemistry Unit #7 Chemical Bonding & Molecular Shape Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING INTRA (Within (inside) compounds) STRONG INTER (Interactions between the molecules of a compound)

More information

Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts

Name 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 information

CHEMICAL BONDING. Valence Electrons. Chapter Ten

CHEMICAL BONDING. Valence Electrons. Chapter Ten CHEMICAL BONDING Chapter Ten Valence Electrons! The electrons occupying the outermost energy level of an atom are called the valence electrons; all other electrons are called the core electrons.! The valence

More information

STD-XI-Science-Chemistry Chemical Bonding & Molecular structure

STD-XI-Science-Chemistry Chemical Bonding & Molecular structure STD-XI-Science-Chemistry Chemical Bonding & Molecular structure Chemical Bonding Question 1 What is meant by the term chemical bond? How does Kessel-Lewis approach of bonding differ from the modern views?

More information

Chapter 10. Valence Electrons. Lewis dot symbols. Chemical Bonding

Chapter 10. Valence Electrons. Lewis dot symbols. Chemical Bonding Chapter 10 Chemical Bonding Valence Electrons Recall: the outer electrons in an atom are valence electrons. Valence electrons are related to stability Valence electrons can be represented with dots in

More information

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. CHAPTER 4 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. A substance is a brittle crystal that conducts electricity in molten liquid state

More information

Unit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence.

Unit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Unit 5: Bonding Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Intramolecular Forces: forces of attraction within the same molecule. Examples:

More information

Chemistry I Chemical Bonding / Molecular Geometry / Intermolecular Forces Lecture Notes

Chemistry I Chemical Bonding / Molecular Geometry / Intermolecular Forces Lecture Notes Chemistry I Chemical Bonding / Molecular Geometry / Intermolecular Forces Lecture Notes Since most elements do not have a filled outer shell, they attempt to achieve an octet arrangement by combining with

More information

Chapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories

Chapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories Chapter 9 Chemical Bonding II: Molecular Geometry and Bonding Theories Topics Molecular Geometry Molecular Geometry and Polarity Valence Bond Theory Hybridization of Atomic Orbitals Hybridization in Molecules

More information

CHAPTER 6 CHEMICAL BONDING SHORT QUESTION WITH ANSWERS Q.1 Dipole moments of chlorobenzene is 1.70 D and of chlorobenzene is 2.5 D while that of paradichlorbenzene is zero; why? Benzene has zero dipole

More information

Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction

Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent

More information

Ch8 Test. Multiple Choice Identify the choice that best completes the statement or answers the question.

Ch8 Test. Multiple Choice Identify the choice that best completes the statement or answers the question. h8 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. n ionic bond is. a. attraction of an atom for its electrons. b. attraction of atoms for electrons

More information

IB Chemistry. Chapter 4.1

IB 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 information