THE BIG IDEA: BONDING AND INTERACTIONS.

Size: px
Start display at page:

Download "THE BIG IDEA: BONDING AND INTERACTIONS."

Transcription

1 HONORS CHEMISTRY - CHAPTER 8 COVALENT BONDS OBJECTIVES AND NOTES - PART 2 - V12 NAME: DATE: PAGE: THE BIG IDEA: BONDING AND INTERACTIONS. Essential Questions 1. How is the bonding in molecular compounds different from the bonding in ionic compounds? 2. How do electrons affect the shape of a molecule? 3. What factors affect molecular properties? Chapter Objectives 1. Differentiate between ionic and molecular compounds, and between formula units and molecules. (8.1, 9.1, & pp ) 2. Compare and contrast a chemical formula and a molecular formula. (8.1) 3. Identify and list the names and formulas of the common monatomic and diatomic molecules. (8.1 & 9.1) 4. Describe a covalent bond. (8.1 & 8.2) 5. Interpret and write/draw molecular formulas, structural formulas, and Lewis structures/lewis diagrams/lewis dot diagrams/dot diagrams, for simple covalent molecules containing single, double, or triple bonds. (8.1 & 8.2) 6. Interpret ball and stick molecular models and space filling molecular models for simple covalent molecules containing single, double, or triple bonds. (8.1 & 8.2) 7. Describe the formation and characteristics of a covalent bond and the types of elements involved in this type of bonding. (8.1 & 8.2) 8. Predict, identify, write, and describe single, double, and triple covalent bonds. (8.2) 9. Predict, identify, write, and describe shared and unshared pairs of electrons. (8.2) 10. Predict, identify, write, and describe incomplete octets. (8.2) 11. Describe bond dissociation energy and how it relates to bond type. (8.2) 12. Identify, write and describe resonance structures. (8.2) 13. Describe the VSEPR theory. (8.3) 14. Predict and describe common electron pair geometries found in simple molecules with a maximum of four pairs of electrons around the central atom. (8.3) 15. State the corresponding bond angles for common electron pair (electronic) geometries found in simple molecules with a maximum of four pairs of electrons around the central atom. (8.3) 1

2 16. Predict and describe the molecular shapes for electron pair geometries found in simple molecules. (8.3) 17. Define and identify central atoms and related terminology. (8.3) 18. Use electronegativity values to determine whether a bond is nonpolar covalent, polar covalent, or ionic. (8.4) 19. Describe and show the relationship between polar covalent bonds & polar molecules. (8.4) 20. Name, identify and describe the weak attractive forces that hold molecules together and the physical manifestations that occur because of those forces. (8.4) 21. Demonstrate and be able to describe all aspects of laboratory safety rules and procedures. (Applicable every chapter) 8.3 Polar Bonds and Molecules A. Bond Polarity 1. Bond polarity is caused by the unequal sharing of electrons that exists in many covalent bonds. The sharing of electrons is based on the electronegativities of the two atoms involved in the bond. An atom with a higher electronegativity has more pull on the electrons than an atom with lower electronegativity. Therefore, an atom with a higher electronegativity has more electrons than protons much of the time, producing an area of partial negative charge. At the other end of the bond will be an atom with lower electronegativity, thus it will have more protons than electrons much of the time, producing an area of partial positive charge. If the two atoms in the bond have the same electronegativity the electrons are shared equally and there is no area of charge created. The polarity of a bond and the resulting molecule can be represented in the following ways: a. The use of the lowercase Greek letter delta, δ, which indicates partial. Area of Partial Positive Charge Area of Partial Negative Charge b. A color grid. VIB G YOR (ROY G BIV backwards). Unless, of course, I had made the color grid go from partial negative to partial positive. Or else you were looking from the other side of the paper! Area of Partial Positive Charge Neutral (Switzerland) Area of Partial Negative Charge 2 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

3 c. An arrow pointing toward the atom(s) with greater electronegativity; i.e., the area with an excess of electrons and thus, the partial negative charge. Area of Partial Positive Charge Area of Partial Negative Charge 2. nonpolar covalent bond: A covalent bond in which the shared electrons are shared equally between the two atoms involved in the bond. Homonuclear diatomic molecules always form nonpolar covalent bonds. The electronegativity difference between the atoms involved is equal to zero. a. Example: Electron clouds in N 2 can be seen below. 3. polar covalent bond: A covalent bond in which the shared electrons are shared unequally between the two atoms involved in the bond; the electrons spend more time revolving around the more electronegative atom. As a result of this unequal sharing, the bonded atoms form partial positive and partial negative areas. The partial negative area forms around the more electronegative atom and the partial positive area forms around the less electronegative (more electropositive) atom. The electronegativity difference between the atoms involved is greater than zero and approximately less than 1.7. Bonds between different nonmetals form polar covalent bonds. a. Example: The bond in HF can be seen below. 3 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

4 4. polar molecule/dipole/permanent dipole: A polar molecule; a molecule held together by unsymmetrical polar bonds, the centers of positive and negative charge do not correspond or symmetrically cancel each other out. The molecule has areas of partial positive and partial negative charge. a. The shape of a molecule and the polarity of its bonds determine the charge distribution in the molecule. b. Examples: See HF above and H 2 O below. 5. nonpolar molecule Molecules held together with nonpolar bonds or polar bonds arranged symmetrically so that they cancel each other out. a. CO 2 is an example of a molecule that contains polar bonds, but is a nonpolar molecule; see below. B. Attractions Between Molecules 1. intra: A prefix meaning "inside". 2. inter: A prefix meaning "between or among". 3. intramolecular forces: Forces inside individual particles, such as covalent bonds. 4. van der Waals forces/weak forces/intermolecular forces/interparticle force: Forces between or among individual particles. The individual particles are usually molecules, but sometimes are independent atoms or ions. The strength of these forces greatly affects the physical state of a substance. These forces are only about 15% of the strength of covalent or ionic bonds. a. The different types of weak forces are seen in the table on the van der Waals Forces Flowchart Addendum on the Chapter 8 webpage. 1. They are listed on the table from strongest on the left to weakest on the right. 4 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

5 5. ion-dipole forces: The attraction between an ion and a dipole, it depends on the charge on the ion and the magnitude of the dipole moment of the dipole. a. These forces are important when ionic solutes are dissolved in polar solvents such as H 2 O. b. It is the strongest of all of the interparticle weak forces. c. Examples: When sodium chloride is dissolved, the forces between the sodium ions and water molecules (see below) or the forces between the chloride ions and water molecules. 6. dipole-dipole forces: The attractive force between the oppositely charged ends of two permanent dipoles. It is the strongest major type of intermolecular force. a. Example: The forces between two HCl molecules (see below) b. hydrogen bond: One of the world's stupidest names; it is not a true bond, but rather, a special type of dipole-dipole force. It occurs when one at least one molecule is composed of hydrogen and elements with a very high electronegativity (N, O, or F) and the adjacent molecule is polar and contains N, O, or F. The resulting molecules are extremely polar, resulting in a strong dipole-dipole force between the very partially positive hydrogen of one dipole and the partially negative element of another dipole. The high melting and boiling points of substances with hydrogen bonds is a reflection of the strength of these intermolecular forces. Hydrogen bonds are the strongest type of dipole-dipole forces. 1. Examples: The forces found among NH 3 molecules and/or H 2 O molecules; the forces between a H 2 O molecule and an HF molecule (see below). 5 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

6 7. ion-induced dipole forces: The attractive force between an ion and the oppositely charged end of an induced dipoles. a. induced dipole: A nonpolar atom or molecule in which a nearby charged area, such as an ion or a dipole, distorts the electron cloud. Induced dipoles can be created when the electron cloud of a nonpolar molecule is repelled by a negative ion or when a positive ion attracts the electron cloud (see below). When the nearby ion is removed, the induced dipole reverts back to its nonpolar state. 1. Example of an ion-induced dipole force: The Fe 2+ in hemoglobin attracting O 2. Ion Nonpolar Molecule Ion O - O Induced Dipole 8. dipole-induced dipole forces: The attractive force between the oppositely charged ends of permanent dipoles and induced dipoles. a. Example of dipole-induced dipole forces: O 2 dissolved in water. Polar Molecule Nonpolar Molecule Dipole O - O Induced Dipole 6 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

7 9. London dispersion forces/london forces/dispersion forces: The attractive forces between the oppositely charged ends of two temporary dipoles or the forces between a temporary dipole and an induced dipole created by that temporary dipole. a. temporary dipole/instantaneous dipole: An atom or molecule in which the electrons become unsymmetrically arranged, creating a dipole for a fraction of a second. A temporary dipole is created the instant an atom or nonpolar molecule has an unequal number of electrons on one side of the particle; when this occurs the side with the extra electrons becomes negatively charged and the other side of the atom or molecule becomes positively charged. Within a fraction of a second after a temporary dipole is formed the electrons rearrange themselves symmetrically due to electron-electron repulsion; this reverts the atom or molecule back to its nonpolar state. 1. See creation of temporary dipole and resultant London forces in I2 below. I I Nonpolar Molecule Temporary Dipole I I Nonpolar Molecule Induced Dipole 2. polarizability: The ease in which an atom or molecule forms a temporary or induced dipole. The larger the radius of the atom or molecule, the easier it is for a dipole to form; thus, polarizability and radius size are directly related. These factors are clearly reflected in the melting and boiling points of monatomic and diatomic molecules. a. Examples: In the VIIA column, the first two elements, F2 and Cl2, are both gases at room temperature, the third element, Br2, is a liquid, and the last two elements, I2 and At2, are both solids. The intermolecular forces increase as the degree of polarizability increases. 7 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

8 1. The increase is molecular mass going down the column also plays a role in the increase in melting and boiling points. At any temperature, all substances have the same kinetic energy: thus, the greater the molecular mass the lower the velocity. (Who pulled the sled?) b. Polarizability usually increases as molecular mass increases. Note: This is because in most cases, the larger the molecular mass the more electrons an atom has and thus, the larger the radius of the atom, making it easier to form an induced or temporary dipole. 8 - HC - Chapter 8 - Objectives and Notes - Part 2 - V12

THE BIG IDEA: BONDING AND INTERACTIONS.

THE BIG IDEA: BONDING AND INTERACTIONS. ADVANCED HONORS CHEMISTRY - CHAPTER 8 COVALENT BONDS OBJECTIVES AND NOTES - PART 2 - V12 NAME: DATE: PAGE: THE BIG IDEA: BONDING AND INTERACTIONS. Essential Questions 1. How is the bonding in molecular

More information

What are covalent bonds?

What are covalent bonds? Covalent Bonds What are covalent bonds? Covalent Bonds A covalent bond is formed when neutral atoms share one or more pairs of electrons. Covalent Bonds Covalent bonds form between two or more non-metal

More information

Intermolecular Forces I

Intermolecular Forces I I How does the arrangement of atoms differ in the 3 phases of matter (solid, liquid, gas)? Why doesn t ice just evaporate into a gas? Why does liquid water exist at all? There must be some force between

More information

Intermolecular Forces

Intermolecular Forces Intermolecular Forces Molecular Compounds The simplest molecule is H 2 : Increased electron density draws nuclei together The pair of shared electrons constitutes a covalent bond. Intermolecular Forces

More information

Covalent Bonding bonding that results from the sharing of electron pairs.

Covalent 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 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

Unit 6: Molecular Geometry

Unit 6: Molecular Geometry Unit 6: Molecular Geometry Molecular Geometry [6-5] the polarity of each bond, along with the geometry of the molecule determines Molecular Polarity. To predict the geometries of more complicated molecules,

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

Solutions and Intermolecular Forces

Solutions and Intermolecular Forces Solutions and Intermolecular Forces REVIEW Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other

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

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

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

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

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

For the following intermolecular forces:

For the following intermolecular forces: Lecturenotes 1 unit6_review_exercise_2017.odt Lecturenotes 2 unit6_review_exercise_2017.odt Lecturenotes 3 unit6_review_exercise_2017.odt Lecturenotes 4 unit6_review_exercise_2017.odt Answers: 1. Ionic

More information

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules?

Chapter 10. Dipole Moments. Intermolecular Forces (IMF) Polar Bonds and Polar Molecules. Polar or Nonpolar Molecules? Polar Bonds and Polar Molecules Chapter 10 Liquids, Solids, and Phase Changes Draw Lewis Structures for CCl 4 and CH 3 Cl. What s the same? What s different? 1 Polar Covalent Bonds and Dipole Moments Bonds

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

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

Intermolecular Forces OR WHY IS WATER SPECIAL?

Intermolecular Forces OR WHY IS WATER SPECIAL? Intermolecular Forces OR WHY IS WATER SPECIAL? Define the prefixes Inter Between, as internet, interstate Intra Inside, as intramural Intermolecular Forces (2) Forces between covalent molecules These are

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

One Q partial negative, the other partial negative Ø H- bonding particularly strong. Abby Carroll 2

One Q partial negative, the other partial negative Ø H- bonding particularly strong. Abby Carroll 2 Chemistry Notes v Polarity Experiment Ø Things involved Polarity Solubility Dispersion Ø Polarity Shaving cream has soap steric acid Water is polar Food coloring is polar/ionic because dissolved Like dissolves

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

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

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

Name: Date: Blk: Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed:

Name: Date: Blk: Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed: Name: Date: Blk: NOTES: BONDING Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed: I. IONIC BONDING Ionic bond: formed by the

More information

CP Covalent Bonds Ch. 8 &

CP Covalent Bonds Ch. 8 & CP Covalent Bonds Ch. 8 & 9 2015-2016 Why do atoms bond? Atoms want stability- to achieve a noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent

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. 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

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

When intermolecular forces are strong, the atoms, molecules, or ions are strongly attracted to each other, and draw closer together.

When intermolecular forces are strong, the atoms, molecules, or ions are strongly attracted to each other, and draw closer together. INTERMOLECULAR FORCES: THE FORCE BEHIND VARIOUS PROPERTIES WHY? Intermolecular forces are largely responsible for the properties of affinity, solubility, volatility, melting/ boiling point, and viscosity.

More information

Q. What happens when you boil (melt) a compound?

Q. What happens when you boil (melt) a compound? Intermolecular Forces (MHR Text p. 202 206) Molecular compounds are: 1) made up of molecules 2) are made up of two or more nonmetallic atoms 3) held together by covalent bonds (sharing e ) Q. But what

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

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

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

Intermolecular Forces of Attraction

Intermolecular Forces of Attraction Name Unit Title: Covalent Bonding and Nomenclature Text Reference: Pages 189-193 Date Intermolecular Forces of Attraction Intramolecular vs. Intermolecular So far in our discussion of covalent bonding,

More information

Bonding. Honors Chemistry Unit 6

Bonding. Honors Chemistry Unit 6 Bonding Honors Chemistry Unit 6 Bond Types Ionic: transfer of electrons Covalent: sharing electron pair(s) Metallic: delocalized electrons Predicting Bonds Based on electronegativity difference (look at

More information

States of Matter. Intermolecular Forces. The States of Matter. Intermolecular Forces. Intermolecular Forces

States of Matter. Intermolecular Forces. The States of Matter. Intermolecular Forces. Intermolecular Forces Intermolecular Forces Have studied INTRAmolecular forces the forces holding atoms together to form compounds. Now turn to forces between molecules INTERmolecular forces. Forces between molecules, between

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

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

There are two types of bonding that exist between particles interparticle and intraparticle bonding.

There are two types of bonding that exist between particles interparticle and intraparticle bonding. There are two types of bonding that exist between particles interparticle and intraparticle bonding. Intraparticle bonding describes the forces that exist within a particle such as a molecule or ionic

More information

Chapter 6 Bonding Diary

Chapter 6 Bonding Diary Chapter 6 Bonding Diary Bonding deals primarily with how ionic compounds and molecular compounds form. As you might remember from early on, it s all about the ELECTRONS. Are they present, or have they

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

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

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

DEFINITION. The electrostatic force of attraction between oppositely charged ions

DEFINITION. The electrostatic force of attraction between oppositely charged ions DEFINITION The electrostatic force of attraction between oppositely charged ions Usually occurs when a metal bonds with a non-metal Ions are formed by complete electron transfer from the metal atoms to

More information

Chemistry II Unit 5b Practice Test

Chemistry II Unit 5b Practice Test Practice for Unit 5b Exam 2013 1 Unit5Practicetest2013.odt Chemistry II Unit 5b Practice Test Reading: This material is covered in chapter 5 and chapter 12 in your book. Your notes and your molecular drawings

More information

The attractions that hold together the atoms in water and carbon dioxide can not be explained by ionic bonding. Ionic bonding =

The attractions that hold together the atoms in water and carbon dioxide can not be explained by ionic bonding. Ionic bonding = In unit six, we discussed ionic compounds, which are generally crystalline solids with high melting points. Other compounds, however, have very different properties. Water is a liquid at room temperature.

More information

Step 1: Solute particles must separate from each other. Since energy must be absorbed to overcome the forces of attraction between solute particles,

Step 1: Solute particles must separate from each other. Since energy must be absorbed to overcome the forces of attraction between solute particles, Step 1: Solute particles must separate from each other. Since energy must be absorbed to overcome the forces of attraction between solute particles, this process is endothermic. Step 2: Solvent particles

More information

Electonegativity, Polar Bonds, and Polar Molecules

Electonegativity, Polar Bonds, and Polar Molecules Electonegativity, Polar Bonds, and Polar Molecules Some Definitions Electronegativity: the ability of an atom to attract bonding electrons to itself. Intramolecular forces: the attractive force between

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

***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

How do electronegativity values determine the charge distribution in a polar bond?

How do electronegativity values determine the charge distribution in a polar bond? Chapter 8 Covalent Bonding 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding 8.3 Bonding Theories 8.4 Polar Bonds and Molecules 1 Copyright Pearson Education, Inc., or its affiliates. All Rights

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

Polar Bonds and Molecules

Polar Bonds and Molecules Chemistry 1 of 33 Snow covers approximately 23 percent of Earth s surface. Each individual snowflake is formed from as many as 100 snow crystals. The polar bonds in water molecules influence the distinctive

More information

Chapter 5 Compounds and Their Bonds

Chapter 5 Compounds and Their Bonds General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds A closer look at bonding type the concept of electronegativity General Rules for Bond Type

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

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 11 Liquids and Intermolecular Forces John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Gases, Liquids, and Solids State Volume Shape of State Density

More information

DIFFERENT TYPES OF INTEMOLECULAR FORCES INTERMOLECULAR FORCES

DIFFERENT TYPES OF INTEMOLECULAR FORCES INTERMOLECULAR FORCES DIFFERENT TYPES OF INTEMOLECULAR FORCES Do all the exercises in your studyguide COMPARISON OF THE THREE PHASES OF MATTER. Matter is anything that occupy space and has mass. There are three states of matter:

More information

1). Ionic bond electron from Na is transferred to Cl. Na is a metal and Cl is a nonmetal

1). Ionic bond electron from Na is transferred to Cl. Na is a metal and Cl is a nonmetal Chemical Bonds 1). Ionic bond electron from Na is transferred to Cl. Na is a metal and Cl is a nonmetal Salt versus Molecules A metal cation and nonmetal anion are joined together by an ionic bond called

More information

Chemical Bonding. Chemical Bonding 20/03/2015. The atomic radius increases from right to left. The atomic radius increases from top to bottom

Chemical Bonding. Chemical Bonding 20/03/2015. The atomic radius increases from right to left. The atomic radius increases from top to bottom Chemical Bonding Atomic Radius: This distance from the nucleus to the outermost electron. Chemical Bonding Chemistry 11 Two factors must be taken into consideration in explaining this periodic trend: Increasing

More information

Unit Six --- Ionic and Covalent Bonds

Unit 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 information

Dipole-Dipole Interactions https://www.youtube.com/watch?v=cerb1d6j4-m London Dispersion Forces https://www.youtube.com/watch?

Dipole-Dipole Interactions https://www.youtube.com/watch?v=cerb1d6j4-m London Dispersion Forces https://www.youtube.com/watch? CATALYST Lesson Plan GLE Physical Science 22. Predict the kind of bond that will form between two elements based on electronic structure and electronegativity of the elements (e.g., ionic, polar, nonpolar)

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

Polarity. Q

Polarity.  Q Unit 6 Polarity Polarity Reflect: Hydrogen has a very low affinity for electrons, while oxygen has a very high affinity. What do you think the bond between the two is like? Polarity http://www.youtube.com/watch?v=kj3o0xvhvq

More information

Lewis Theory of Shapes and Polarities of Molecules

Lewis Theory of Shapes and Polarities of Molecules Lewis Theory of Shapes and Polarities of Molecules Sulfanilamide Lewis Structures and the Real 3D-Shape of Molecules Molecular Shape or Geometry The way in which atoms of a molecule are arranged in space

More information

liquids_solids_15dec2017_1st.notebook Liquids and solids Chapters 11 and 12

liquids_solids_15dec2017_1st.notebook Liquids and solids Chapters 11 and 12 liquids_solids_15dec2017_1st.notebook December 15, 2017 Liquids and solids Chapters 11 and 12 Intermolecular forces Intermolecular: forces between molecules Intramolecular: within molecules (i.e. covalent)

More information

Hey, Baby. You and I Have a Bond...Ch. 8

Hey, Baby. You and I Have a Bond...Ch. 8 I. IONIC BONDING FUNDAMENTALS A. They form between... 1. A and a a. A to become b. A to become B. How it happens (Let s first focus on two atoms): 1. When a metal and a nonmetal meet, electrons get transferred

More information

Salt vs. Sugar. 1. Ionic Compounds. 2. Molecular Compounds (Cont.) 12/18/2014. What is this Compound You Speak Of? Sodium Chloride Dissolving in Water

Salt vs. Sugar. 1. Ionic Compounds. 2. Molecular Compounds (Cont.) 12/18/2014. What is this Compound You Speak Of? Sodium Chloride Dissolving in Water Salt vs. Sugar Unit 7: Chemical Compounds & Formulas Lesson#7.1: Types of Compounds What is this Compound You Speak Of? Compound: Any substance that is formed by the chemical bonding of atoms. We classify

More information

Chap 6.1 Covalent Bonds and Structures

Chap 6.1 Covalent Bonds and Structures Chapter 6 Structure and Properties of Substances In chapter 5 you learned about the different types of bonds and their individual properties: 1. Ionic 2. Covalent/Molecular 3. Metallic In this chapter

More information

BONDING REVIEW. You need a Periodic Table, Electronegativity table & Polarity chart!

BONDING REVIEW. You need a Periodic Table, Electronegativity table & Polarity chart! BONDING REVIEW You need a Periodic Table, Electronegativity table & Polarity chart! What is the correct bond angle for Bent with 2 lone pairs on the central atom? 105 What is the predicted bond angle for

More information

Dipole Moment, Resonance. Dr. Sapna Gupta

Dipole Moment, Resonance. Dr. Sapna Gupta Dipole Moment, Resonance Dr. Sapna Gupta Dipole Moment This indicates whether a molecule is polar or not. Dipole moment ( ) is when a molecule can move in presence of an electric current. The higher the

More information

Lecture Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten

Lecture Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Lecture 1101 John D. Bookstaver St. Charles Community College Cottleville, MO Molecular Comparison

More information

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces Pearson Education, Inc.

Lecture Presentation. Chapter 11. Liquids and Intermolecular Forces Pearson Education, Inc. Lecture Presentation Chapter 11 Liquids and States of Matter The fundamental difference between states of matter is the strength of the intermolecular forces of attraction. Stronger forces bring molecules

More information

Outline Introduction: Multiple bonds, Bond. strength. Naming molecules Drawing Lewis Structures Molecular shapes and VSEPR theory Bond Polarity

Outline Introduction: Multiple bonds, Bond. strength. Naming molecules Drawing Lewis Structures Molecular shapes and VSEPR theory Bond Polarity Covalent Bonding Outline Introduction: Multiple bonds, Bond strength Naming molecules Drawing Lewis Structures Molecular shapes and VSEPR theory Bond Polarity Why do atoms bond? Recall that noble gases

More information

Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a

Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a Chemistry Final Exam Review and Practice Chapters Covered ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 13, 14, 15, 16, 19, 20 Topics to Expect: Periodic Table: s, p, d, f blocks Metal,

More information

Ionic Bonds. H He: ... Li Be B C :N :O :F: :Ne:

Ionic Bonds. H He: ... Li Be B C :N :O :F: :Ne: Ionic Bonds Valence electrons - the electrons in the highest occupied energy level - always electrons in the s and p orbitals - maximum of 8 valence electrons - elements in the same group have the same

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 Big Ideas in Unit 6 How do atoms form chemical bonds? How does the type of a chemical bond influence a compounds physical and

More information

Ch 6.1 Chemical Bonding

Ch 6.1 Chemical Bonding Ch 6.1 Chemical Bonding Chemical Bonds the attractive forces that hold different atoms or ions together (Intramolecular or electrostatic Forces Why Bond? Atoms bond to achieve a full outer energy level

More information

INTERMOLECULAR FORCES: Polarity of Molecules. Seventh Course (General Chemistry) by Dr. Istadi

INTERMOLECULAR FORCES: Polarity of Molecules. Seventh Course (General Chemistry) by Dr. Istadi INTERMOLECULAR FORCES: Polarity of Molecules Seventh Course (General Chemistry) by Dr. Istadi 1 Types of Intermolecular Forces The nature of the phases and their changes are due primarily to forces among

More information

Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES

Name: Date: Period: #: BONDING & INTERMOLECULAR FORCES BONDING & INTERMOLECULAR FORCES Page 1 INTERMOLECULAR FORCES Intermolecular forces (van der Waals forces) relative weak interactions that occur between molecules. Most of the physical properties of gases,

More information

Chemical Bonding I: Covalent Bonding. How are atoms held together in compounds?

Chemical 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 information

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces

Chapter 11 Intermolecular Forces, Liquids, and Solids. Intermolecular Forces Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in the solid and liquid states particles

More information

Unit 4:Chemical Bonding Practice Packet

Unit 4:Chemical Bonding Practice Packet Name: KEY Unit 4:Chemical Bonding Practice Packet 1. I can state the three types of chemical bonds. 2. I can state the number of valence electrons that an atom attains to be most stable. 3. I can state

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 Involves valence electrons. PE is lower in bonded atoms. Attractive force that develops

More information

Scientists learned that elements in same group on PT react in a similar way. Why?

Scientists 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 information

Electrons and Molecular Forces

Electrons and Molecular Forces Electrons and Molecular Forces Chemistry 30 Ms. Hayduk Electron Configuration Atomic Structure Atomic Number Number of protons in the nucleus Defines the element Used to organize the periodic table 1 Bohr

More information

Intermolecular Forces and Physical Properties

Intermolecular Forces and Physical Properties Intermolecular Forces and Physical Properties Attractive Forces Particles are attracted to each other by electrostatic forces. The strength of the attractive forces depends on the kind(s) of particles.

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

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

NOTES: UNIT 6: Bonding

NOTES: 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 information

Phase Change DIagram

Phase Change DIagram States of Matter Phase Change DIagram Phase Change Temperature remains during a phase change. Water phase changes Phase Diagram What is a phase diagram? (phase diagram for water) Normal melting point:

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

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

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11, Liquids, and Solids States of Matter The fundamental difference between states of

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

Chapter 11 Intermolecular Forces, Liquids, and Solids

Chapter 11 Intermolecular Forces, Liquids, and Solids Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 11, Liquids, and Solids John D. Bookstaver St. Charles Community College Cottleville,

More information

Chemical Bonding: Chemical Formulas HL

Chemical Bonding: Chemical Formulas HL Name: Chemical Bonding 5. Chemical Bonding: Chemical Formulas Ionic Bonding Covalent Bonding Electronegativity Shapes of Molecules and Intermolecular Forces Objectives -understand that compounds can be

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

Comparing Ionic and Covalent Compounds

Comparing Ionic and Covalent Compounds Comparing Ionic and Covalent Compounds It takes energy to overcome the forces holding particles together. Thus, it takes energy to cause a substance to go from the liquid to the gaseous state. The boiling

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