Ch 6 Chemical Bonding
|
|
- Eunice Tamsyn Lindsey
- 5 years ago
- Views:
Transcription
1 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 is neither purely ionic or purely covalent Classify bonding type according to electronegativity differences. Introduction to Chemical Bonding There are very few atoms that exist as individual particles in nature. Most atoms are bonded to other atoms to form compounds. A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together. One reason atoms bond is to decrease their amount of potential energy. When atoms exist by themselves they have relatively high potential energy. Nature favors arrangements that have minimum potential energy. When atoms bond it decreases the amount of potential energy and creates a more stable arrangement of matter. It takes less energy to bond atoms together than to break the bonds between atoms. Bond energy is the amount of energy it takes to break a chemical bond. Types of Chemical Bonds Ionic bonding- chemical bonding that results from the electrical attraction between cations and anions. In purely ionic bonding atoms completely give up electrons to other atoms. Ionic bonding generally involves metals and nonmetals Covalent bonding- the sharing of electron pairs between two atoms. In a pure covalent bond the electrons are shared by the two bonded atoms. Covalent bonding generally involves two nonmetals. A nonpolar-covalent bond is when the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charges. When the distribution of charge is uneven we call this polar. Polar covalent bonds occur when the bonded atoms have an unequal attraction for the shared electrons.
2 Ionic or Covalent? Most chemical bonds are somewhere in between purely ionic and purely covalent. We use the difference in electronegativity values to determine the type of bond that is formed. Remember from Ch 5 that electronegativity is an atom s ability to attract electrons to its self. We use the following image to determine the bond type. Ionic- electronegativity difference is greater than 1.67 Polar covalent- electronegativity difference is less than 1.67 Use electronegativity differences to classify bonding between sulfur and the following elements: hydrogen, cesium, and chlorine. In each pair, which atom will be more negative? Problem A
3 Covalent Bonding and Molecular Compounds What you should learn in this section (objectives): Define molecule and molecular formula Explain the relationships among potential energy, distance between approaching atoms, bond length and bond energy. State the octet rule List the six basic steps used in writing Lewis structures Explain how to determine Lewis structures for molecules containing single bonds, multiple bonds, or both. Explain why scientists use resonance structures to represent some molecules. A molecule is a neutral group of atoms that are held together by covalent bonds. They can exist as two or more of the same elements bonded together or two or more different elements bonded together. A chemical compound whose simplest units are molecules is called a molecular compound. A chemical formula shows the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts. Remember sub means below. A molecular formula shows the types and numbers of atoms combined in a single molecule of a molecular compound. Formation of a Covalent Bond Nature favors chemical bonding because most atoms have lower potential energy when they are bonded to other atoms than they have as they are independent particles. When 2 hydrogen atoms approach each other 2 bad things happen: electron/electron repulsion and proton/proton repulsion. One good thing that happens: proton/electron attraction. When the attractive forces offset the repulsive forces, the energy of the tow atoms decreases and a bond is formed. Remember, nature is always striving for a lower energy state. too CLOSE too FAR just RIGHT
4 Bond length is the distance between the two nuclei where the energy is minimal between the two nuclei. In other words, it is the average distance between two bonded atoms. When bonds form individual atoms release energy as they change from isolated individual atoms to molecules. Bond energy is the amount of energy that is required to break the bond. The units for bond energy are usually kj/mol (kilojoule per mole).
5 Octet Rule Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level (outer most ring of the atom). When two atoms form a covalent bond, their shared electrons form overlapping orbitals. This achieves a noble-gas configuration. The bonding of two hydrogen atoms allows each atom to have the stable electron configuration of helium, 1s 2. Exceptions to the Octet Rule Fewer than 8: H at most only 2 electrons (one bond),beh 2, only 4 valence electrons around Be (only 2 bonds), Boron compounds only 6 valence electrons (three bonds) Expanded valence (more than 8): can only happen if the central element had d-orbitals which means it is from the 3 rd period or greater and can thus be surrounded by more than four valence pairs in certain compounds. The number of bonds depends on the balance between the ability of the nucleus to attract electrons and the repulsion between the pairs. Some of the more elements are fluorine, oxygen, chlorine and noble gases. Electron-Dot Notation To keep track of valence electrons, it is helpful to use electron-dot notation. Electron-dot notation is an electronconfiguration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element s symbol. The inner-shell electrons are not shown.
6 Lewis Structures H:H An unshared pair, also called a lone pair, is a pair of electrons that is not involved in bonding and that belongs exclusively to one atom. Lewis Structures are formulas in which atomic symbols represent nuclei and inner-shell electrons, dotpairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons. A structural formula indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule. Example F-F and H-Cl. Single bonds (sigma bonds) are a covalent bond in which one pair of electrons is shared between two atoms. They are represented by two dots (electrons) or one dash. These are the longest bonds, but also the weakest Double bonds (pi bonds) are covalent bonds in which two pairs of electrons are shared between two atoms. They are represented by four dots (electrons) or 2 dashes = Example C=C Triple bonds (pi bonds) are covalent bonds in which three pairs of electrons are shared between two atoms. They are represented by six dots (electrons) or 3 dashes. Example These are shortest, but also the strongest. Carbon, nitrogen, oxygen, phosphorous, and sulfur are the most common elements that form multiple bonds. Drawing Lewis Structures 1. H is always a terminal atom. ALWAYS connected to only one other atom. 2. Lowest electronegativity is the central atom in a molecule. 3. Find the total number of valence electrons by adding up group numbers of the elements. For ions add electrons for negative charges and subtract electrons for positive charges. 4. Place one pair of electrons (sigma bond) between each pair of bonded atoms.
7 5. Subtract from the total number of bonds you just used. 6. Place lone pairs about each terminal atom (except H) to satisfy the octet rule. Left over pairs are assigned to the central atom. 7. If the central atom is not yet surrounded by four electron pairs, convert on or more terminal atom lone pairs to a double or triple bond ( pi bonds). Only C, N, O, P, and S can form multiple bonds (pi bonds) Resonance Structures Resonance refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure. Ozone (O 3 ) exists as an average of these two images, so it must be shown both ways.
8 Ionic Bonding and Ionic Compounds What you should learn in this section (objectives): Compare and contrast a chemical formula for a molecular compound with one for an ionic compound. Discuss the arrangements of ions in crystals Define lattice energy and explain its significance List and compare the distinctive properties of ionic and molecular compounds Write the Lewis structure for a polyatomic ion given the identity of the atoms combined and other appropriate information. Formation of an Ionic Compound Ionic compounds are composed of positive (cation) and negative (anion) ions that are combined so that the numbers of positive and negative charges are equal Ionic Bond - Completely transfer electrons. Positive charge cation lost electrons to the anion. Negative charge anion gained electrons from the cation. Positive charge must equal and, therefore, cancel the negative charge. Example: Sodium Chloride sodium wants to lose one electron to become stable and chlorine wants to gain one electron to become stable. Formula unit a chemical formula of the smallest sample of an ionic compound. Ionic Character Ionic compounds have the greatest ionic character with full on charged ions. The further the ions are apart in electronegativity, the more the ionic character. Molecular compounds have very low electronegativity. The closer the ions are in electronegativity, the less the ionic character. Characteristics of Ionic Bonding Ionic compounds are crystalline solids at room temperature. They are arranged in repeating three-dimensional pattern called a crystal lattice. These structures are very orderly and stable. Example: In solid NaCl, each Na is surrounded by six Cl and each Cl is surrounded by six Na. These crystalline solids also have very high melting points. It is extremely hard to break the attraction between the cations and anions because of their stability. Example: NaCl melts at 800 Celsius. The energy released when one mole of an ionic crystalline compound is formed from gaseous ions is called lattice energy. Ionic compounds conduct electric currents when molten (liquid) or dissolved in water (aqueous). The cations and anions are then able to migrate freely.
9 Ionic compounds are electrically neutral salts (solids). Many of these compounds appear as minerals in the Earth s crust. Comparing Ionic and Molecular Compounds The force that holds ions together in an ionic compound is a very strong electrostatic attraction. In contrast, the forces of attraction between molecules of a covalent compound are much weaker. This difference in the strength of attraction between the basic units of molecular and ionic compounds gives rise to different properties between the two types of compounds. Molecular compounds have relatively weak forces between individual molecules. They melt at low temperatures. The strong attraction between ions in an ionic compound gives ionic compounds some characteristic properties, listed below. o very high melting points o hard but brittle o not electrical conductors in the solid state, because the ions cannot move Polyatomic Ions Polyatomic Ions a group of atoms that acts as a unit with a single charge Begin memorizing polyatomic ions get the list from the website and make flashcards. Know the formula, the charge, and the correct spelling of the name of the polyatomic ions listed on the website. We will have a quiz over these.
10 Metallic Bonding What you should learn in this section (objectives): Describe the electron-sea model of metallic bonding, and explain why metals are good electrical conductors Explain why metal surfaces are shiny Explain why metals are malleable and ductile but ionic crystalline compounds are not. The Metallic-Bond Model Metallic bonding is the chemical bonding that is a result from the attraction between metal atoms and the surrounding sea of electrons. A sea of electrons refers to the free moving valence electrons in an atom. These electrons are delocalized which means that they can freely move to any other atom Properties of Metals Good conductors of electricity electrons enter one end of the metal bar and leave the other. Ductile can be stretched into wires. Malleable can be pounded into shapes. Metals ions slide passed one another in a sea of drifting
11 Molecular Geometry What you should learn in this section (objectives): Explain VSEPR theory Predict the shapes of molecules or polyatomic ions using VSEPR theory Explain how the shapes of molecules are accounted for by hybridization theory Describe dipole-dipole forces, hydrogen bonding, induced dipoles, and London dispersion forces and their effects on properties such as boiling and melting points VSEPR Theory - Valence Shell Electron Pair Repulsion The VSEPR theory states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible. The electron dot structures are not flat 2D structures, but are 3D in real life. Molecules adjust their shapes so that the valence electron pairs are as far apart as possible. **See the chart on pg. 200 of your textbook Linear angles are 180 degrees definitely will be linear if only have two atoms in the molecule. No lone pairs and two covalent bonds or three lone pairs and one covalent bond around central atom. Example: CO 2 Bent again, unshared pair(s) strongly repels the covalent bonding pairs. Two lone pairs and two shared pairs around central atom. All angles are 105 degrees. Example: H 2 O Trigonal-Planar three shared pairs (covalent bonds ) separate as much as possible, but are unaffected by a lone pair (no lone pairs) of electrons like the pyramidal structure. Example: BF 3 Trigonal-Pyramidal one unshared pair strongly repels the three shared pairs (covalent bonding), pushing them closer together. All angles are 107 degrees. Example: NH 3 Tetrahedral four faced four shared pairs and no lone pairs, all angles are degrees. Example: CH 4 Trigonal Bipyramidal five shared pairs separate as much as possible, but are unaffected by a lone pair of electrons (no lone pairs). Example: PCl 5 Octahedral six shared pairs separate as much as possible, but are unaffected by a lone pair of electrons (no lone pairs). Example: SF 6 Hybridization Hybridization - two atoms combine, their atomic orbitals overlap to produce molecular orbitals. One electron from each atomic orbital combines to create a shared pair in a molecular orbital.
12 sp hybridization has electrons in 2 orbitals sp 2 hybridization has electrons in 3 orbitals sp 3 hybridization has electrons in 4 orbitals
13 Intermolecular Forces (IMF) The forces of attraction between molecules are known as intermolecular forces. These forces vary in strength and are generally weaker than bonds The strongest IMF exists between polar molecules. A dipole is created by equal but opposite charges that are separated by a short distance. The direction of a dipole is from the dipole s positive pole to its negative pole. The negative region in one polar molecule attracts the positive region in adjacent molecules. So the molecules all attract each other from opposite sides. Such forces of attraction between polar molecules are known as dipole-dipole forces. Dipole-dipole forces act at short range, only between nearby molecules. Dipole Interactions - when polar molecules are attracted to one another: opposite charged regions of polar molecules are attracted. Hydrogen Bonds a particularly strong dipole interaction specifically involving hydrogen at the partially positive pole. Hydrogen is covalently bonded to a very electronegative atom AND to an unshared pair of another atom.
14 Hydrogen is able to bond with the unshared pair of electrons from another molecule because its valence electrons are not shielded from the nucleus by another layer of electrons (hydrogen s valence electrons are directly up against the nucleus). Example: H 2 O The more electronegative the element that hydrogen is bonded to the stronger the intermolecular attractions. Dispersion Forces - weakest of all molecular interactions caused by the motion of electrons. Vibrating electrons may end up moving randomly closer to one atom or another creating a momentary dipole. The more electrons there are the greater the interaction between nonpolar molecules.
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 informationChapter 6. Preview. Objectives. Molecular Compounds
Section 2 Covalent Bonding and Molecular Compounds Preview Objectives Molecular Compounds Formation of a Covalent Bond Characteristics of the Covalent Bond The Octet Rule Electron-Dot Notation Lewis Structures
More informationChemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds
Chemical Bonding Table of Contents Section 1 Introduction to Chemical Bonding Section 2 Covalent Bonding and Molecular Compounds Section 3 Ionic Bonding and Ionic Compounds Section 4 Metallic Bonding Section
More informationIntroduction to Chemical Bonding
Chemical Bonding Introduction to Chemical Bonding Chemical bond! is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together Why are most
More informationUnit 3 - Chemical Bonding and Molecular Structure
Unit 3 - Chemical Bonding and Molecular Structure Chemical bond - A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together 6-1 Introduction
More informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
More informationChapter 6. 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 informationChapter 6. Preview. Lesson Starter Objectives Chemical Bond
Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in
More informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationIonic and Covalent Bonding
1. Define the following terms: a) valence electrons Ionic and Covalent Bonding the electrons in the highest occupied energy level always electrons in the s and p orbitals maximum of 8 valence electrons
More informationChapter 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 informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
More informationChemical Bonding. 5. _c Atoms with a strong attraction for electrons they share with another atom exhibit
CHAPTER 6 REVIEW Chemical Bonding SHORT ANSWER Answer the following questions in the space provided. 1. a A chemical bond between atoms results from the attraction between the valence electrons and of
More informationChapter 6 Chemical Bonding
Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between
More informationChapter 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 informationChapter 8 Covalent Boding
Chapter 8 Covalent Boding Molecules & Molecular Compounds In nature, matter takes many forms. The noble gases exist as atoms. They are monatomic; monatomic they consist of single atoms. Hydrogen chloride
More informationCHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS
CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence
More informationBonding. 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 informationUnit Six --- Ionic and Covalent Bonds
Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples
More informationCh. 12 Section 1: Introduction to Chemical Bonding
Name Period Date Chemical Bonding & Intermolecular Forces (Chapter 12, 13 &14) Fill-in the blanks during the PowerPoint presentation in class. Ch. 12 Section 1: Introduction to Chemical Bonding Chemical
More informationChapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
More informationBonding. 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***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 informationChapters 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 informationScientists learned that elements in same group on PT react in a similar way. Why?
Unit 5: Bonding Scientists learned that elements in same group on PT react in a similar way Why? They all have the same number of valence electrons.which are electrons in the highest occupied energy level
More informationCHEMICAL BONDING COVALENT BONDS IONIC BONDS METALLIC BONDS
CHEMICAL BONDING COVALENT BONDS IONIC BONDS METALLIC BONDS Metallic Bonds How atoms are held together in solid metals. Metals hold onto their valence electrons very weakly. Think of them as positive ions
More informationCovalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B
Covalent Bonding 1. Obtain the number of valence electrons for each of the following atoms from its group number and draw the correct Electron Dot Notation (a.k.a. Lewis Dot Structures). a. K b. N c. Cl
More informationChapter 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 informationCartoon 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 informationChapter 7 Chemical Bonding
Chapter 7 Chemical Bonding 7.1 Ionic Bonding Octet rule: In forming compounds atoms lose, gain or share electrons to attain a noble gas configuration with 8 electrons in their outer shell (s 2 p 6 ), except
More informationChemical 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 informationNa Cl Wants to lose ONE electron! Na Cl Ionic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding.
BONDING Chemical Bond Attraction that holds atoms together Types include IONIC, METALLIC, or COVALENT Differences in electronegativity determine the bond type Ionic Bond TRANSFER of electrons between atoms
More informationIonic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding. Ionic Bonding. Attraction that holds atoms together
BONDING Chemical Bond Attraction that holds atoms together Types include IONIC, METALLIC, or COVALENT Differences in electronegativity determine the bond type Ionic Bond TRANSFER of electrons between atoms
More informationChemistry Chapter 6 Test Review
Chemistry Chapter 6 Test Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A mutual electrical attraction between the nuclei and valence electrons
More informationIonic 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 informationNotes: 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 informationMolecular Compounds Compounds that are bonded covalently (like in water, or carbon dioxide) are called molecular compounds
Chapter 8: Covalent Bonding Section 1: Molecular Compounds Bonds are Forces that hold groups of atoms together and make them function as a unit. Two types: Ionic bonds transfer of electrons (gained or
More informationOften times we represent atoms and their electrons with Lewis Dot Structures.
They are trying to get their number of valence electrons to either 0 or 8. Group 1: 1 valence electron Group 2: 2 valence electrons Group 13: 3 valence electrons Group 14: 4 valence electrons Group 15:
More informationCHAPTER 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 informationCartoon 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 informationUnit 3 - Part 1: Bonding. Objective - to be able to understand and name the forces that create chemical bonds.
Unit 3 - Part 1: Bonding Objective - to be able to understand and name the forces that create chemical bonds. Bonding: Key Terms to Know 1. Chemical formula 2. Molecular formula 3. Bond Energy 4. Bond
More informationChapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
More informationUnit 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 informationbond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction
bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction ionic compound- a metal reacts with a nonmetal Ionic bonds form when an atom that
More informationUnit 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 informationCHAPTER 12 CHEMICAL BONDING
CHAPTER 12 CHEMICAL BONDING Core electrons are found close to the nucleus, whereas valence electrons are found in the most distant s and p energy subshells. The valence electrons are responsible for holding
More informationCh 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules
Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES
More informationCHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING
CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING 6.1 Introduction to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different
More informationHey, 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 informationChapter 8: Concepts of Chemical Bonding
Chapter 8: Concepts of Chemical Bonding Learning Outcomes: Write Lewis symbols for atoms and ions. Define lattice energy and be able to arrange compounds in order of increasing lattice energy based on
More informationUNIT 5.1. Types of bonds
UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence
More informationChemical Bonding AP Chemistry Ms. Grobsky
Chemical Bonding AP Chemistry Ms. Grobsky What Determines the Type of Bonding in Any Substance? Why do Atoms Bond? The key to answering the first question are found in the electronic structure of the atoms
More informationAtoms have the ability to do two things in order to become isoelectronic with a Noble Gas.
CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when
More informationCovalent Bonding bonding that results from the sharing of electron pairs.
Unit 5 Notes Covalent Bonding, Covalent Compounds, and Intermolecular Forces Chemical Bond a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms
More information6.1 Intro to Chemical Bonding Name:
6.1 Intro to Chemical Bonding Name: A. Chemical bond Favored by nature because: 3 main types of bonds 1. 2. 3. B. Ionic Bonds C. Covalent Bonds D. Metallic Bond E. Bond Determination RECALL: Electronegativity
More informationCHEMISTRY Matter and Change Section 8.1 The Covalent Bond
CHEMISTRY Matter and Change Section Chapter 8: Covalent Bonding CHAPTER 8 Table Of Contents Section 8.2 Section 8.3 Section 8.4 Section 8.5 Naming Molecules Molecular Structures Molecular Shapes Electronegativity
More informationChapter 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 informationHonors 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***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 informationWhat is Bonding? The Octet Rule. Getting an Octet. Chemical Bonding and Molecular Shapes. (Chapter Three, Part Two)
Chemical Bonding and Molecular Shapes (Chapter Three, Part Two) What is Bonding? Bonding describes how atoms interact with each other in an attractive sense. There are three types of bonding: Ionic bonding
More information4/4/2013. Covalent Bonds a bond that results in the sharing of electron pairs between two atoms.
A chemical bond is a mutual electrical attraction between the nucleus and valence electrons of different atoms that binds the atoms together. Why bond? As independent particles, atoms have a high potential
More informationPeriodic Trends. Homework: Lewis Theory. Elements of his theory:
Periodic Trends There are various trends on the periodic table that need to be understood to explain chemical bonding. These include: Atomic/Ionic Radius Ionization Energy Electronegativity Electron Affinity
More informationIB Chemistry. Chapter 4.1
IB Chemistry Chapter 4.1 Chemical Bonds Atoms or ions that are strongly attached to one another Chemical bonds will form if potential energy decreases (becomes more stable) 2 Valence Electrons Valence
More informationIts Bonding Time. Chemical Bonds CH 12
Its Bonding Time Chemical Bonds CH 12 What is a chemical bond? Octet Rule: Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its
More informationEdexcel Chemistry A-level
Edexcel Chemistry A-level Topic 2 - Bonding and Structure Flashcards What are ions? What are ions? Charged particles that is formed when an atom loses or gains electrons What is the charge of the ion when
More informationName Date Class MOLECULAR COMPOUNDS. Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides
8.1 MOLECULAR COMPOUNDS Section Review Objectives Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides Vocabulary covalent bond molecule diatomic molecule
More informationBonding 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 informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationChemical Bonding CHAPTER 6. ONLINE Chemistry. Why It Matters Video
CAPTER 6 Chemical Bonding ONLINE Chemistry MDSciencecom SECTION 1 Introduction to Chemical Bonding SECTION 2 Covalent Bonding and Molecular Compounds SECTION 3 lonic Bonding and lonic Compounds SECTION
More informationCHAPTER 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 informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and
More informationUnit 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 informationChemical Bonding I: Covalent Bonding. How are atoms held together in compounds?
I: Covalent Bonding How are atoms held together in compounds? IONIC or COVALENT bonds or forces For most atoms, a filled outer shell contains 8 electrons ----- an octet Atoms want to form octets when they
More informationRESONANCE STRUCTURE When a molecule has more than one possible structure. Draw all possible structures and place a double end arrow ( ) in between.
CHEMISTRY NOTES 6.1 COVALENT BONDS Objectives Explain the role and location of electrons in a covalent bond. Describe the change in energy and stability that takes place as a covalent bond forms. Distinguish
More informationMolecular 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 informationCartoon courtesy of NearingZero.net. Unit 3: Chemical Bonding and Molecular Structure
Cartoon courtesy of NearingZero.net Unit 3: Chemical Bonding and Molecular Structure Bonds Forces that hold groups of atoms together and make them function as a unit. Ionic bonds transfer of electrons
More informationChapter 8 The Concept of the Chemical Bond
Chapter 8 The Concept of the Chemical Bond Three basic types of bonds: Ionic - Electrostatic attraction between ions (NaCl) Metallic - Metal atoms bonded to each other Covalent - Sharing of electrons Ionic
More informationCh8 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 informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE The Ionic Bond Formation of Ions The
More informationCHEMICAL BONDS How can atoms form a molecule? Let s watch the video: Bond types CHEMICAL BONDING Ionic bonding
CHEMICAL BONDS How can atoms form a molecule? Let s watch the video: Bond types http://www.kentchemistry.com/links/bonding/bondingflashes/bond_types.swf CHEMICAL BONDING In 1916, the American chemist Gilbert
More informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds An attractive force that holds two atoms together in a more complex unit Three basic types of bonds Ionic Electrons are transferred from one
More informationNOTES: UNIT 6: Bonding
Name: Regents Chemistry: Mr. Palermo NOTES: UNIT 6: Bonding www.mrpalermo.com Name: Key Ideas Compounds can be differentiated by their chemical and physical properties. (3.1dd) Two major categories of
More informationSection 6.2 1/13/2014. Most Chemical Compounds. Molecular (or Covalent) Compound. Covalent Bonding and Molecular Compounds
Section 6.2 Covalent Bonding and Molecular Compounds Most Chemical Compounds Are molecules, a neutral group of atoms that are held together by covalent bonds. It is a single unit capable of existing on
More informationDEFINITION. 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 informationUnit 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 informationChapter 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 informationUnit 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 informationChapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective
Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry 11.1 Periodic Trends in Atomic Properties Discuss the atomic trends Metals are located on the left side of the periodic
More informationChapter 8 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 informationSTD-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 informationChapter 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 informationDownloaded from
Points to Remember Class: XI Chapter Name: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical
More informationCovalent 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 informationClass XI: Chemistry Chapter 4: Chemical Bonding and Molecular Structure Top Concepts
1 Class XI: Chemistry Chapter 4: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical species
More informationChapter 3.1 Structures and Properties of Substances. Chemical Bonding
Chapter 3.1 Structures and Properties of Substances Chemical Bonding The orbitals in the Periodic Table The elements of the periodic table can be classified according to the type of orbital that is being
More informationChemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together
Chemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together When atoms form chemical bonds their valence electrons move around. This makes atoms
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationHelpful Hints Lewis Structures Octet Rule For Lewis structures of covalent compounds least electronegative
Helpful Hints Lewis Structures Octet Rule Lewis structures are a basic representation of how atoms are arranged in compounds based on bond formation by the valence electrons. A Lewis dot symbol of an atom
More informationChapter 8 Notes. Covalent Bonding
Chapter 8 Notes Covalent Bonding Molecules and Molecular Compounds Helium and Neon are monoatomic, meaning they exist as single atoms Some compounds exist as crystalline solids, such as NaCl Others exist
More informationIntroduction to Chemical Bonding Chemical Bond
Introduction to Chemical Bonding Chemical Bond Mutual attraction between the and electrons of different atoms that binds the atoms together. Ionic Bond o that results from the attraction between large
More information