Chap 6.1 Covalent Bonds and Structures
|
|
- Harold Bruce Jefferson
- 5 years ago
- Views:
Transcription
1 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 you will be looking at the structure of molecules and molecular shape is linked to the structures. Dec 4 8:43 PM Chap 6.1 Covalent Bonds and Structures Molecular compounds come in a great variety of shapes These shapes are determined by the covalent bonds which form the molecules Lewis structures can be used to predict the structures and properties of molecules Oct 16 7:42 PM 1
2 METHOD 1 1.Find the valence number for each element.put the element with the lowest number in the middle. Place the other elements around it. 2.Fill in the electrons for the center element.add outside element's electrons so that all valence electrons are used. Check for the octet rule.you may have to move pairs to make double or triple bonds. Apr 7 7:44 AM Example: Draw the Lewis structure for CH 2 O. Step 1: Total # of valence electrons: C H O Total = Step 2: Skeleton Structure: Step 3: Put lone pairs around the outer electrons: Step 4: Put lone pairs around the central atoms make double or triple bonds if necessary. May 16 3:29 PM 2
3 Example 1: H2O Example 2: CO 2 Dec 4 9:40 PM Example 3: NH 3 Dec 4 9:41 PM 3
4 VSEPR Valence Shell Electron Pair Repulsion Theory The VSEPR theory states that the bonding pairs and lone pairs of electrons in the valence level of an atom repel each other due to their negative charges. This helps us to predict the shapes of molecules. To determine the shape of a molecule, first look at the number of electron groups that the molecule has. Electron groups can be either bonded electrons or lone pairs of electrons. Oct 16 8:16 PM VSEPR has 2 basic rules. 1.Bonding electron pairs repel each other, therefore adjust to be as far apart as possible. Example: Methane Apr 7 7:56 AM 4
5 2. Unshared pairs of electrons are held closer to the atom than the bonding pairs.the unshared pairs of electrons strngly repel the bonding electron pairs,pushing them closer together. EXAMPLE AMMONIA WATER CARBON DIOXIDE Apr 7 7:58 AM Electron pair repulsions are not always equal.the repulsions can be ranked as : STRONGEST: 2 unshared pairs MEDIUM: One unshared and one shared pair (bond) WEAKEST:2 shared pairs(bonds) Apr 7 8:02 AM 5
6 Number of Electron Groups Name of Molecular Shape Shape Angle Example 2 Linear CO 2 3 Trigonal Planar CH 2O 4 Tetrahedral CH 4 4 Pyramidal NH 3 4 Bent H 2O May 17 3:43 PM How to predict molecular shape using VSEPR: 1. Draw a Lewis structure for the molecule 2. Determine the total number of electron groups around the central atom. (**double and triple bonds count as 1 group). 3. Look at where the bonds and lone pairs are, and determine which of the 5 shapes best accommodates the combination of electron groups. May 17 3:46 PM 6
7 Example: Draw a Lewis structure for CH 2 Cl 2 and use VSEPR to determine its shape and bond angle. May 17 3:50 PM Example: Use VSEPR to determine the shape and bond angle of PH 3. May 17 5:04 PM 7
8 BUILD ASSIGNMENT skeleton shape bond angle SH GeSe SiH PH Apr 7 8:21 AM Question: Draw Lewis structures for each of the following. a CBr 4 b NCl 3 c NCl 4 + d PS 2 + e NS 2 Oct 16 8:02 PM 8
9 Drawing Lewis Dot Diagrams (with a central atom): method 2 Step 1 Determine the total number of valence electrons of all the atoms in the molecule. Step 2 Draw a skeleton structure. Put the atom with the lowest group number in the middle Join the atoms with a pair of bonding electrons (subtract 2 electrons from the total for each bond you make) Step 3 Put lone pairs around all atoms except the central atom (follow the octet rule). Note: The most electronegative atoms get the electrons first! Step 4 Put the remaining electrons around the central atom (octet rule!) If all the valence electrons are used up but the central atom does not have an octet of electrons, move one or more lone pairs from the outer atoms to form double or triple bonds. Oct 16 7:44 PM Apr 7 9:50 AM 9
10 Resonance Structures > Occur when there is more than one possible Lewis structure Example: O 3 (ozone) Dec 4 9:47 PM Example: SO 2 Dec 4 10:12 PM 10
11 More Challenging Lewis Structures How do we determine the central atom? The atom with the most unpaired valence electrons will be the central atom of a molecule. Example: CH 3 NH 2 Example: CH 3 OH Dec 4 10:13 PM Drawing Lewis Structures for Polyatomic Ions (charges) Example : PO 4 3 Dec 5 1:07 PM 11
12 Coordinate Covalent Bonds: Bonds formed when one atom contributes both electrons to make a shared pair to satisfy an octet. Example : The ammonium ion, NH 4+, is formed when ammonia joins with H+. Example : CO May 16 3:32 PM Example : Show the coordinate covalent bond formed when water joins with H+. May 16 7:11 PM 12
13 Polarity of Molecules A non polar molecule has no net dipole. This is when molecules have: only non polar bonds polar bonds arranged symmetrically so that dipoles cancel out A polar molecule has a net dipole. This can be found in molecules made up of polar bonds arranged so that the dipoles do not cancel out. Dec 11 3:10 PM Polarity of Bond Types: Linear polar or non polar Trigonal Planar polar or non polar Tetrahedral polar or non polar Pyramidal always polar Bent Always polar Oct 16 8:38 PM 13
14 Oct 24 1:27 PM How to tell if a molecule is polar or non polar? Are there electrons on the central atom? Are there different atoms bonded to the central atom? YES YES NO POLAR Check change in EN: Is there a diff. greater than 0.5? If yes then, POLAR. 1) Draw arrows in the direction of the most electronegative atom. 2) If the arrows cancel our, then the molecule is nonpolar. If they do not cancel out, the molecule is polar and has dipoles. NON POLAR Dec 11 3:13 PM 14
15 Determine the polarity of the following molecules: 1) SO 3 2) SCl 2 3) CS 2 4) CH 2 O 5) CH 2 Cl 2 Oct 16 8:49 PM Use VSPER to predict the shape of the following molecules, then determine it's polarity. 1) COCl 2 2) BeF 2 3) [NO 2 ] + 4) NOF Oct 16 8:51 PM 15
16 sa Chap 6.2 : Intermolecular Forces Ever Wonder?... -How Salt Dissolves? -Why Water only freezes on the Top of the lake? -What holds our DNA together? ANSWER = Intermolecular Forces! Oct 16 8:55 PM When a substance melts or boils, intermolecular forces are broken (NOT intramolecular bonds) * a high boiling point indicates strong attractive forces Dec 12 6:33 PM 16
17 -Intramolecular Forces = Forces that bond the ATOMS to each other within a molecule. Example = Covalent Bonds, ionic bonds, metallic bonds. -Intermoleccular Forces = Forces that bond the MOLECULES to each other. Weak relative to covalent and ionic bonds. Oct 16 8:58 PM Types of Intermolecular Forces 1 : Dipole-Dipole Forces 2 : Dispersion (London) Forces 3 : Hydrogen Bonding Oct 16 9:01 PM 17
18 1.Dipole Interactions(Dipole dipole) occurs when the slightly positive end of one dipole attracts to the slighty negative end of another dipole. They help explain why polar molecules have higher boiling points than non polar molecules. Apr 7 1:14 PM 2: Dispersion (London) Forces h Also called Londen Forces. In a non polar molecule,the motion of the electrons causes a momentary uneven dstribution of charge. A non polar moleule becomes slightly polar for an instant.the result is an attraction similar to a dipole interaction. These are the main forcec between non polar molecules. The larger the molecule,the stonger the Londen forces F and CL are gases at room temp. Br is a liquid I is a solid Oct 16 9:21 PM 18
19 3: Hydrogen Bonding Electrostatic Attraction between the nucleus of a hydrogen atom (bonded to a highly electronegative atom such as O, F, N) and the negative end of a nearby dipole. ~ only 5% as strong as a covalent bond. Oct 16 9:31 PM WATER hydrogen bonding accounts for the many unique properties of water in liquid water hydrogen is bonded to at least four other water molecules is the only pure substance that exists in nature in all three states of matter at the same time. Oct 16 9:53 PM 19
20 Hydrogen bonds explain why: 1. Ice floats in water INSULATES OCEAN LIFE Water is not like most liquids. ~Normally a liquid contracts when cooled so it becomes more dense and sinks in its own liquid, but water expands when frozen. ~Water expands when frozen because as the temperature of the water is getting lower the H bonds pull the water into an orderly pattern called a HONEYCOMB FRAMEWORK. ~At low temperatures the KE of the water molecules is too low to break out of this shape. This honeycomb framework gives the ice a bigger volume for its mass which in turn decreases the density allowing ice to float in water. Oct 16 9:55 PM 2. Water has a high Boiling Point Water has an unusually high boiling point. As a general rule, the lower the molar mass the lower the boiling point, but the H bonds in water disrupt this rule. This allows the earth to be cooled. Water acts as a heat sink! Moderates th seasons. 3. Water has a high surface tension INSECTS FLOAT ON WATER SURFACE TENSION an inward force or pull that tends to minimize the surface area of a liquid. H bonds cause the inward pull to create water s high surface tension (Activities to accompany) SURFACTANT a substance that decreases the surface tension of water. Eg detergent. 4.ADHESION Water molecules attach to objects.water sticks to the xylem. 5.COHESION_Water molecules attach to other molecules. This is how water goes up a tree after being started by transpiration. Oct 16 9:57 PM 20
21 Intermolecular Forces YouTube Oct 17 10:17 AM Chap 6.3 Structure Determines Properties TEMPERATURE is defined as a measure of the average kinetic energy of the particles. To increase the KE of particles you increase the temperature. ~A substance will change states from a solid to a liquid or a liquid to a gas when the average kinetic energy of the particles is great enough to overcome the force of attraction holding the particles together. When no attractive forces exist with other particles the substance will exist as a gas. Oct 16 10:00 PM 21
22 Melting Point and Boiling Point Depends on the attractive forces holding the particles together. In order for metals and ionic compounds to melt or boil, they must break the ionic bonds or metallic bonds. BUT when molecular compounds melt or boil, the intermolecular attractions between the molecules must break (NOT the covalent bonds within) Ionic and metallic bonds are very strong while intermolecular attractions are weak. So metals and ionic compounds melt or boil at much higher temperatures than molecular compounds. Polar molecules boil at higher temperatures than nonpolar substances because of the extra intermolecular attractions (and the bond energy of these attractions) Metals > ionic > polar > non polar Oct 16 10:03 PM Ionic Compounds Metallic Compounds Molecular Compounds Eg. NaCl Eg. Mg Eg. C 6 H 12 O 6 must break ionic bonds must break metallic bonds intermolecular bonds between molecules break, not the covalent bonds May 23 3:14 PM 22
23 Strength of Intramolecular and Intermolecular Forces STRONGEST 1. Metallic Ex: Cu, Fe, CoI 2. Ionic Ex: LiCl (NOT aqueous) 3. Covalent Ex: O H bond in water INTRA 4. hydrogen bonding 5. dipole dipole 6. London dispersion WEAKEST INTER Dec 16 12:31 PM How would you determine the higher boiling point between two ionic compounds? Check charges! Higher set of charges wins! Examples: 1. NaCl and BaO 2. Na 3 N and K 2 O Dec 16 12:36 PM 23
24 How would you determine the higher boiling point between two London dispersion? Size! Example: 1. Only type I will ever give! a) C 2 H 6 and C 3 H 8 b) C 4 H 10 and C 5 H 12 Dec 16 12:45 PM Circle the one that has the highest boiling point: 1. Cu or H 2 O 2. CF 4 or LiBr 3. Sr 3 N 2 or NaCl 4. NH 3 or PH 3 5. LiCl (aq) or C 2 H 6 6. HF or NaCl (aq) 7. C 2 H 6 or C 3 H 8 Dec 16 12:50 PM 24
25 Electrical Conductivity To conduct an electrical current, electrons or ions must be able to move independently of oppositely charged ions. ~Metals are good conductors of electricity as solids. ~Ionic compounds are good conductors of electricity when melted or dissolved in water. ~Molecular compounds are poor conductors of electricity. Oct 16 10:10 PM 25
26 Attachments imgres.webloc
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 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 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 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 informationChapter 6. Chemical Bonding
Chapter 6 Chemical Bonding Section 6.1 Intro to Chemical Bonding 6.1 Objectives Define chemical bond. Explain why most atoms form chemical bonds. Describe ionic and covalent bonding. Explain why most chemical
More 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 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 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 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 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 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 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 informationUnit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence.
Unit 5: Bonding Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Intramolecular Forces: forces of attraction within the same molecule. Examples:
More informationAS91164 Bonding, structure, properties and energychanges Level 2 Credits 5
AS91164 Bonding, structure, properties and energychanges Level 2 Credits 5 LEWIS DIAGRAMS, SHAPES OF MOLECULES, POLAR AND NON POLAR MOLECULES Lewis diagrams: use dots (or x) to represent electrons, show
More informationUnit Six --- Ionic and Covalent Bonds
Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples
More informationChapter 7 Chemical Bonding
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 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 informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More 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 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 informationCovalent 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 informationof 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 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 informationNOTES: 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 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 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 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 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 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 informationBonding. Computer Lab: Ionic Bonds. Important Notes 3/22/18
Bonding What are ionic bonds, and how are they formed? Computer Lab: Ionic Bonds Go to http://www.pbslearningmedia.org/asset/ lsps07_int_ionicbonding/ Read each screen and follow the directions where appropriate.
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. 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 information4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups.
Chapter 10 Lecture Chapter 10 Bonding and Properties of Solids and Liquids 10.3 Shapes of Molecules and Ions (VSEPR Theory) Learning Goal Predict the three-dimensional structure of a molecule or a polyatomic
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 informationBonding Test pg 1 of 4 Name: Pd. Date:
Bonding Test pg 1 of 4 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many electrons are shared in a single covalent bond? 1. A) 2 B) 3 C)
More informationChemical Bonding Basic Concepts
Chemical Bonding Basic Concepts Valence electrons are the outer shell electrons of an atom. The valence electrons are the electrons that particpate in chemical bonding. Group e - configuration # of valence
More 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 informationChem 11 Unit 4 POLARITY, MOLECULE SHAPE, and BEHAVIOUR
Chem 11 Unit 4 POLARITY, MOLECULE SHAPE, and BEHAVIOUR Polarity is unequal distribution of a charge on a molecule caused by: 1) some degree of ionic character in the bonding (i.e. unequal electron sharing)
More informationWhat 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 informationChemical 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 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 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 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 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 informationName: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
Name: Class: Date: SCH4U Chapter 4 Formative Test Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following statements about
More informationLewis 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 informationUnit 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 informationUnit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence.
Unit 5: Bonding Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Intramolecular Forces: 1. I can define intramolecular forces and intermolecular
More informationTest Bank for Introductory Chemistry Essentials 5th Edition by Tro
Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Sample Introductory Chemistry, 5e (Tro) Chapter 10 Chemical Bonding 10.1 True/False Questions 1) Bonding theories are used to predict
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 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 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 informationBONDING 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 informationChemical Bonding Chapter 8
Chemical Bonding Chapter 8 Get your Clicker, 2 magnets, goggles and your handouts Nov 15 6:15 PM Recall that: Ionic-Involves the transfer of electrons - forms between a metal and a nonmetal Covalent-Involves
More informationCP 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 informationChemical Bonding. Burlingame High School
Chemical Bonding Electronegativity Is a measure of the ability of an atom in a molecule to attract electrons to itself. Concept proposed by Linus Pauling 1901-1994 Electronegativity Trends Forms of Chemical
More 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 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 informationVSEPR & Molecular Geometry
Bonding Packet Page 1 of 10 Chemistry Bonding Revisited and molecular structures PLEASE BRING YOUR OLD BONDING PACKET, too! VOCABULARY: 1. ionic bonds 2. covalent bonds 3. molecule 4. metallic bond 5.
More informationThe 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 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 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 informationDate: Monday, February 6, Obj: Write electron dot structures. Complete: How many valence electrons in the following? H Be B C.
Do Now Date: Monday, February 6, 2017 Obj: Write electron dot structures. Complete: How many valence electrons in the following? H Be B C N O F Ne Valence Electrons Remember: in chemical bonds we re talking
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 informationCh. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic
More information1. What is a chemical bond? 2. What is the octet rule? Why do atoms in bonding follow it?
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations 1. What is a chemical bond? 2. What is the octet rule? Why do atoms in bonding follow it? 3. What are oxidation numbers? How do we find them? 4.
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 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 informationChemical 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 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 informationBonding. 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 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 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 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 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 informationIntermolecular 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 informationChapter 16 Covalent Bonding
Chemistry/ PEP Name: Date: Chapter 16 Covalent Bonding Chapter 16: 1 26; 28, 30, 31, 35-37, 40, 43-46, Extra Credit: 50-53, 55, 56, 58, 59, 62-67 Section 16.1 The Nature of Covalent Bonding Practice Problems
More informationVSEPR. Valence Shell Electron Pair Repulsion Theory
VSEPR Valence Shell Electron Pair Repulsion Theory Vocabulary: domain = any electron pair or bond (single, double or triple) is considered one domain. bonding pair = shared pair = any electron pair that
More informationMolecular shapes. Balls and sticks
Molecular shapes Balls and sticks Learning objectives Apply VSEPR to predict electronic geometry and shapes of simple molecules Determine molecule shape from electronic geometry Distinguish between polar
More informationBonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
More informationLewis Dot Formulas and Molecular Shapes
Lewis Dot Formulas and Molecular Shapes Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent chemical bonds are formed by valence electrons
More informationExperiment Seven - Molecular Geometry
Experiment Seven - Geometry Introduction Although it has recently become possible to image molecules and even atoms using a highresolution microscope, our understanding of the molecular world allows us
More informationBonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
More 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 informationElectrons 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 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 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 information2.2.2 Bonding and Structure
2.2.2 Bonding and Structure Ionic Bonding Definition: Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form
More informationCovalent Bonds. Unit 4b.1: Covalent bonds. Unit 4b ( se ven c la s s peri od s) Name:
Name: Covalent Bonds Unit 4b ( se ven c la s s peri od s) Unit 4b.1: Covalent bonds 1) A different type of intramolecular force (bond) a) Ionic compounds form between ions i) Electrons are transferred
More informationChapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and
More informationChapter 8: 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 informationName: Practice Packet. Regents Chemistry: Dr. Shanzer. Chapter 9: Chemical Bonding.
Name: Regents Chemistry: Dr. Shanzer Practice Packet Chapter 9: Chemical Bonding http://drshanzerchemistry.weebly.com 1 Chemical Bonding Objectives Describe the 2 major types of chemical bonds in terms
More informationCHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM)
CHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM) Associate Degree in Engineering Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore Community College
More informationAdapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent
More informationUnit 5: Bonding Covalent & Intermolecular
Name Unit 5: Bonding Covalent & Intermolecular Date Part 2 Questions 1. Ozone, O3 (g), is produced from oxygen, O2 (g) by electrical discharge during thunderstorms. The unbalanced equation below represents
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 informationCovalent Bonding. Chapter 8. Diatomic elements. Covalent bonding. Molecular compounds. 1 and 7
hapter 8 ovalent bonding ovalent Bonding A metal and a nonmetal transfer An ionic bond Two metals just mix and don t react An alloy What do two nonmetals do? Neither one will give away an electron So they
More informationCHAPTER 12 CHEMICAL BONDING
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 12 CHEMICAL BONDING Day Plans for the day Assignment(s) for the day 1 Begin Chapter
More informationChapter 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