VSEPR Theory. Chemistry Warm-up: 1. Pick up a set of the skeleton notes from the first lab table.
|
|
|
- Dale Davidson
- 5 years ago
- Views:
Transcription
1 Chemistry Warm-up: 1. Pick up a set of the skeleton notes from the first lab table. 2. Complete the words of the week assignment. You need to have answers for Tuesday, Thursday and today. Today s : Draw Lewis Dot Structures for boron triiodide and oxygen difluoride.
2 Valence
3 Valence Shell
4 Valence Shell Electron
5 Valence Shell Electron Pair
6 Valence Shell Electron Pair Repulsion
7 Valence Shell Electron Pair Repulsion Theory
8 Valence Shell
9 Valence Shell Remember that the outermost energy level of an atom is referred to as the valence shell.
10 Valence Shell Remember that the outermost energy level of an atom is referred to as the valence shell. The electrons within this energy level, valence shell, are the only ones that are used in forming chemical bonds.
11 Electron Pair A lone pair of electrons is described as two electrons, on a central atom, that are not used within a chemical bond.
12 Electron Pair A lone pair of electrons is described as two electrons, on a central atom, that are not used within a chemical bond. N H H H Nitrogen has one LONE PAIR of electrons on the central atom.
13 Repulsion As you learned long ago, the two north ends of two different magnets will repel each other.
14 Repulsion As you learned long ago, the two north ends of two different magnets will repel each other. The same holds true for like charges within the atom. Lone pairs of electrons, on a central atom, will repel each other as well as the electrons within a bond to make the most stable arrangement for that molecule.
15 Repulsion As you learned long ago, the two north ends of two different magnets will repel each other. The same holds true for like charges within the atom. Lone pairs of electrons, on a central atom, will repel each other as well as the electrons within a bond to make the most stable arrangement for that molecule. N H H H That lone pair of electrons within the NH3 molecule occupy space and repel the electrons within the bonds causing the molecule to be shaped sort of like a tripod.
16 VSEPR Theory is based on the idea that the geometry of a molecule is determined primarily by repulsions among the pairs of electrons associated with a central atom. Only valence electrons of the central atom influence the molecular shape in a meaningful way.
17 There are some basic assumptions that must be considered: 1. Pairs of electrons in the valence shell of a central atom repel each other. 2. These pairs of electrons tend to occupy positions in space that minimize repulsion and maximize the distance of separation between them. 3. The valence shell is taken as a sphere with electron pairs localizing on the spherical surface at maximum distance from one another. 4. A multiple bond is treated as if it is a single electron pair and the two or three electron pairs of a multiple bond are treated as a single super pair.
18 There are five basic shapes of molecules that can be predicted using the above assumptions. They are: 1. Linear 2. Angular / V-shaped / Bent 3. Tetrahedral 4. Trigonal Planar and 5. Trigonal Pyramidal. For each of these we will follow the same format of shape, number of atoms bonded to the central atom, number of lone pairs of electrons on the central atom, and an example with a Lewis Dot Structure.
19 Example Lewis Dot Structure HBr (hydrogen monobromide) H Br Linear None (there is no central atom) # of atoms bonded to the central atom None (there is no central atom) # of lone pairs of electrons on the central atom
20 Example BeH2 (beryllium hydride) Lewis Dot Structure H Be H Linear Two None # of atoms bonded to the central atom # of lone pairs of electrons on the central atom
21 Example H2O (dihydrogen monoxide) Two Angular (V-shaped, Bent) Lewis Dot Structure H O H Two # of atoms bonded to the central atom # of lone pairs of electrons on the central atom
22 Example CH4 (methane or carbon tetrahydride) Four Tetrahedral Lewis Dot Structure H H C H H None # of atoms bonded to the central atom # of lone pairs of electrons on the central atom
23 Example BF3 (boron trifluoride) Three Trigonal planar Lewis Dot Structure F B F F None # of atoms bonded to the central atom # of lone pairs of electrons on the central atom
24 Example Lewis Dot Structure NH3 (ammonia or nitrogen trihydride) Trigonal H N H H pyramidal Three One # of atoms bonded to the central atom # of lone pairs of electrons on the central atom
25 Name the shape for each of the following molecules. A: B: C: D:
Fill in the chart below to determine the valence electrons of elements 3-10
Chemistry 11 Atomic Theory IV Name: Date: Block: 1. Lewis Diagrams 2. VSEPR Lewis Diagrams Lewis diagrams show the bonding between atoms of a molecule. Only the outermost electrons of an atom (called electrons)
Name: Period: Date: What Is VSEPR? Now explore the Compare Two Structures link. Try changing the display to explore different combinations.
Name: Period: Date: What Is VSEPR? Exploring The Valence Shell Electron Pair Repulsion (VSEPR) model. Go to the Purdue University website to explore VSEPR theory. http://www.chem.purdue.edu/gchelp/vsepr/structur2.html
4.2.7 & Shapes, and bond angles for molecules with two, three and four negative charge centers
4.2.7 & 4.2.8 Shapes, and bond angles for molecules with two, three and four negative charge centers The shape of a molecule has an important part to play in determining its chemical (e.g. reactivity and
VSEPR Theory. Shapes of Molecules. Molecular Structure or Molecular Geometry
VSEPR Theory VSEPR Theory Shapes of Molecules Molecular Structure or Molecular Geometry The 3-dimensional arrangement of the atoms that make-up a molecule. Determines several properties of a substance,
MOLECULAR MODELS OBJECTIVES
MOLECULAR MODELS OBJECTIVES 1. To learn to draw Lewis structures for common compounds 2. To identify electron pairs as bonding pairs or lone pairs 3. To use electron pair repulsion theory to predict electronic
At the end of this lesson, students should be able to :
At the end of this lesson, students should be able to : (a) Explain Valence Shell Electron Pair Repulsion theory (VSEPR) (b) Draw the basic molecular shapes: linear, planar, tetrahedral, and octahedral.
Check Your Solution A comparison with the figures in Figure 4.31 on page 234 of the student textbook confirms the results.
Predicting the Shape of a Molecule (Student textbook page 236) 11. What molecular shape is represented by each of the following VSEPR notations? a. AX 3 b. AX 5 E You need to assign a molecular shape that
Chemical Bonding I: Basic Concepts
Chemical Bonding I: Basic Concepts Chapter 9 Chang & Goldsby Modified by Dr. Hahn Copyright McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent
Chemical Bonds, Molecular Models, and Molecular Shapes
Chemical Bonds, Molecular Models, and Molecular Shapes PRELAB ASSINGMENT Read the entire laboratory write up and answer the following questions before coming to lab. Read the entire laboratory write up
Chem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept
Chem 1075 Chapter 12 Chemical Bonding Lecture Outline Slide 2 Chemical Bond Concept Recall that an atom has and electrons. Core electrons are found to the nucleus. Valence electrons are found in the s
Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion.
VSEPR & Geometry Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion. Lewis structures are not intended to show the 3-dimensional structure (i.e. shape or geometry)
Molecular 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
CHAPTER 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
SECTION II: BUILDING MODELS
SECTION II: BUILDING MODELS Lesson 9 New Smells, New Ideas Lesson 10 Two s Company Lesson 11 Let s Build It Lesson 12 What Shape Is That Smell? Lesson 13 Sorting It Out Lesson 14 How Does the Nose Know?
Chemistry and the material world Lecture 3
Chemistry and the material world 123.102 Lecture 3 Electronic bookkeeping we need a way of finding out in which proportions two or more atoms make up a molecule is it CH 3 or CH 4 or CH 5? counting valence
Chapter 9 Molecular Geometries. and Bonding Theories
Chapter 9 Molecular Geometries and Bonding Theories Coverage of Chapter 9 9.1 All 9.2 All 9.3 All 9.4 All 9.5 Omit Hybridization Involving d Orbitals 9.6 All 9.7 and 9.8 Omit ALL MOLECULAR SHAPES The shape
Shapes of Molecules. Lewis structures are useful but don t allow prediction of the shape of a molecule.
Shapes of Molecules Lewis structures are useful but don t allow prediction of the shape of a molecule. H O H H O H Can use a simple theory based on electron repulsion to predict structure (for non-transition
Chemistry 212 MOLECULAR STRUCTURES AND GEOMETRIES
Chemistry 212 MOLECULAR STRUCTURES AND GEOMETRIES LEARNING OBJECTIVES To build models of selected molecules using VSEPR theory. To illustrate patterns of molecular shapes. BACKGROUND The shapes exhibited
1. Which of the following is an example of a structural formula?
1. Which of the following is an example of a structural formula? A. B. C. D. 2. According to the VSEPR Theory, which of the following molecules will have a linear geometry? A. B. C. D. 3. Which type of
Shapes The shape of a molecule can play a large role in how it reacts and how we as chemists can use it. POS Checklist:
hem 20 Unit A Bonding Molecular Shapes and VSEPR Theory You will... PS hecklist: apply VSEPR theory to predict molecular shapes for, angular (V shaped, bent) tetrahedral, trigonal pyramidal and trigonal
Lewis Dot Structures for Methane, CH 4 The central C atom is bonded by single bonds (-) to 4 individual H atoms
Chapter 10 (Hill/Petrucci/McCreary/Perry Bonding Theory and Molecular Structure This chapter deals with two additional approaches chemists use to describe chemical bonding: valence-shell electron pair
Molecular Geometry. Valence Shell Electron Pair. What Determines the Shape of a Molecule? Repulsion Theory (VSEPR) Localized Electron Model
Molecular Geometry 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 Electron
4/25/2017. 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
Covalent Compounds: Bonding Theories and Molecular Structure
CHM 123 Chapter 8 Covalent Compounds: Bonding Theories and Molecular Structure 8.1 Molecular shapes and VSEPR theory VSEPR theory proposes that the geometric arrangement of terminal atoms, or groups of
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
Introduction to VSEPR Theory 1
1 Class 8: Introduction to VSEPR Theory Sec 10.2 VSEPR Theory: The Five Basic Shapes Two Electron Groups: Linear Geometry Three Electron Groups: Trigonal Planar Geometry Four Electron Groups: Tetrahedral
Chapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent
CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols
CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen
Do now: Brainstorm how you would draw the Lewis diagram for: H 2 O CO 2
Do now: Brainstorm how you would draw the Lewis diagram for: 2 O CO 2 Shapes of molecules C 4 N 3 2 O C 2 O CO 2 Shapes of molecules Shapes of molecules are determined by the number of bonding and non-bonding
Lewis Dot Structures and Molecular Geometry
Experiment 11 Lewis Dot Structures and Molecular Geometry Pre-Lab Assignment Before coming to lab: Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise. Purpose
Chemical Bonding and Molecular Models
25 Chemical Bonding and Molecular Models A chemical bond is a force that holds groups of two or more atoms together and makes them function as a unit. Bonding involves only the valence (outer shell) electrons
Name. Molecular Models
Name Molecular Models Lab Day Introduction: The atom and molecule are truly small; 6 10 23 carbon atoms occupy about 4 cm 3, or each atom has a volume of about 6 10 24 cm 3. Molecules, though larger than
Lewis Structure and Electron Dot Models
Lewis Structure and Electron Dot Models The Lewis Structure is a method of displaying the electrons present in any given atom or compound. Steps: 1. Make a skeleton structure 2. Count all e- available
Chapter 9. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Problems with Lewis Theory Lewis theory generally predicts trends in properties, but does not give good numerical predictions.
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,
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
Molecular Geometry and Bonding Theories. Molecular Shapes. Molecular Shapes. Chapter 9 Part 2 November 16 th, 2004
Molecular Geometry and Bonding Theories Chapter 9 Part 2 November 16 th, 2004 8 Molecular Shapes When considering the geometry about the central atom, we consider all electrons (lone pairs and bonding
EXPERIMENT #13 Lewis Structures and Molecular Geometry
OBJECTIVES: EXPERIMENT #13 s and Draw Lewis structures of atoms, ions, and molecules Build models of linear, trigonal planar tetrahedral, trigonal bipyramidal, and octahedral arrangements of electron pairs
End of chapter exercises
End of chapter exercises Problem 1: Give one word/term for each of the following descriptions. 1. The distance between two adjacent atoms in a molecule. 2. A type of chemical bond that involves the sharing
Valence-Shell Electron-Pair Repulsion Theory (VSEPR)
; Set 09- Molecular Geometry All course materials, including lectures, class notes, quizzes, exams, handouts, presentations, and other materials provided to students for this course are protected intellectual
Experiment #2. Lewis Structures
Experiment #2. Lewis Structures A Lewis structure shows how the valence electrons are arranged and indicates the bonding between atoms in a molecule. We represent the elements by their symbols. The shared
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
Section 12: Lewis Structures
Section 12: Lewis Structures The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 12.01 Electronegativity Chemistry (5)(C) 12.02 Electron
Chemical Bonds, Molecular Models, and Molecular Shapes
Chemical Bonds, Molecular Models, and Molecular Shapes PRELAB ASSINGMENT Write an objective, and answer the following questions in your laboratory notebook before coming to lab. Read the entire laboratory
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. How to get the book of
Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
Covalent bonds and shapes of molecules
Covalent bonds and shapes of molecules Determining number of bonds We use Lewis dot structures The number of unpaired electrons will be the number of bonds How many bonds would each typically form? H Be
Lewis 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
PREDICTING THE SHAPE OF A MOLECULE FROM ITS STRUCTURAL FROMULAE
CH 11 TOPIC 24 PREDICTING MOLECULAR SHAPES 1 You have mastered this topic when you can: 1) determine the shape of a molecule based on its Lewis Structure.. PREDICTING THE SHAPE OF A MOLECULE FROM ITS STRUCTURAL
Molecular Geometry and Chemical Bonding Theory
Molecular Geometry and Chemical Bonding Theory The Valence -Shell Electron -Pair Repulsion (VSEPR) Model predicts the shapes of the molecules and ions by assuming that the valence shell electron pairs
CHEMICAL BONDING. Valence Electrons. Chapter Ten
CHEMICAL BONDING Chapter Ten Valence Electrons! The electrons occupying the outermost energy level of an atom are called the valence electrons; all other electrons are called the core electrons.! The valence
Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond
Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H
Localized Electron Model
Localized Electron Model Models for Chemical Bonding Localized electron model (Valence bond model) Molecular orbital model Localized Electron Model Useful for explaining the structure of molecules especially
If we write the condensed electron configuration, then we can easily see the valence electrons.
Lewis structures Lewis notation uses dots and crosses to represent the valence electrons on different atoms. The chemical symbol of the element is used to represent the nucleus and the inner electrons
Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules
Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES
The VSEPR Model applied to Steric Numbers 2 through 4. (VSEPR Part 3)
This work is licensed by Shawn Shields under a Creativ e Commons Attribution-NonCommercial-ShareAlike 4.0 International License. The VSPR Model applied to Steric Numbers 2 through 4. (VSPR Part 3) By Shawn
Announcements. 10pm Room assignments for Exam III and TA Exam Review Sessions are posted on website. Look under Exam Info link
Announcements 1. Exam #3: Thursday, Dec. 6 th, 7:00-8:15pm (Conflict: 5:15-6:30pm) No calculators allowed 2. Activity 3: Making Models of Molecules lab write-up due tomorrow in discussion 3. Lon-capa HW
Ch 13: Covalent Bonding
Ch 13: Covalent Bonding Section 13: Valence-Shell Electron-Pair Repulsion 1. Recall the rules for drawing Lewis dot structures 2. Remember the special situations: - Resonance structures - ormal charges
Lewis Structures and Molecular Shapes
Lewis Structures and Molecular Shapes Drawing Lewis Structures Determine from formula if ionic or covalent Count the electrons If ionic : add valence # to charge if (-), subtract if (+) - = 7+1 electrons;
Covalent Bonding and Molecular Structure (key)
ovalent Bonding and Molecular Structure (key) AX 2 : 2 1. What is the bond angle? 180 2. Which element is more electronegative, carbon, or oxygen? xygen 3. Would you expect 2 to be a polar or a nonpolar
Lesson Plan. Lesson: Shape of Molecules. Aim: To investigate the shapes of molecules and ions. Learning Outcomes :
Lesson Plan Lesson: Shape of Molecules Aim: To investigate the shapes of molecules and ions Learning Outcomes : At the end of the lesson, students will be able to : 1. explain the Valence Shell Electron
Lab Lecture on VSEPR and SPARTAN Chem 141 Lab Dr Abrash 10/3/2011
Q: What is the purpose of this lab? Lab Lecture on VSEPR and SPARTAN Chem 141 Lab Dr Abrash 10/3/2011 To learn two methods to study and predict the shapes of molecules. One is a rule based paper method
8.3 Bonding Theories > Chapter 8 Covalent Bonding. 8.3 Bonding Theories. 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding
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
Chapter Molecules are 3D. Shapes and Bonds. Chapter 9 1. Chemical Bonding and Molecular Structure
Chapter 9 Chemical Bonding and Molecular Structure 1 Shape 9.1 Molecules are 3D Angle Linear 180 Planar triangular (trigonal planar) 120 Tetrahedral 109.5 2 Shapes and Bonds Imagine a molecule where the
Chapter 12 Structures and Characteristics of Bonds Objectives
Objectives 1. To learn about ionic and covalent bonds and explain how they are formed - what holds compounds together? 2. To learn about the polar covalent bond are all covalent bonds equal? 3. To understand
4 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
CHEMISTRY & YOU 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.
Honors Chemistry Unit 6 ( )
Honors Chemistry Unit 6 (2017-2018) Lewis Dot Structures VSEPR Structures 1 We are learning to: 1. Represent compounds with Lewis structures. 2. Apply the VSEPR theory to determine the molecular geometry
Chemical Bonding II. Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds Hybridization MO theory
Chemical Bonding II Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds ybridization MO theory 1 Molecular Geometry 3-D arrangement of atoms 2 VSEPR Valence-shell
Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie
Intramolecular Bonding Chapters 4, 12 Chemistry Mr. McKenzie What determines the type of intramolecular bond? An intramolecular bond is any force that holds two atoms together to form a compound; 3 types
Valence Bond Model and Hybridization
Valence Bond Model and ybridization APPENDIX 4 1 Concepts The key ideas required to understand this section are: Concept Book page reference VSEPR theory 65 More advanced ideas about electronic structure
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Valence shell electron
CHM151LL: VSEPR and Molecular Geometry Tables
CHM151LL: VSEPR and Molecular Geometry Tables VSEPR Model VALENCE-SHELL ELECTRON-PAIR REPULSION (VSEPR) MODEL Lewis structures show the two-dimensional distribution of atoms and electrons. The molecular
Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit
Covalent Bonding Section 8.1 The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes Section 8.5 Electronegativity and Polarity Click a hyperlink or
Chem 121 Exam 4 Practice Exam
Chem 121 Exam 4 Practice Exam 1. What is the correct electron configuration for bromine? b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 9 4s 2 4p 6 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5 d. 1s 2 2s 2 2p 6 3s 2 3p
Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit
Covalent Bonding Section 8.1 The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes Section 8.5 Electronegativity and Polarity Click a hyperlink or
VSEPR Theory, Valence Bond Theory, Characteristic of Covalent Compounds 1. Which of the following is not correct? 1. A sigma bond is weaker than pi bond. 2. A sigma bond is stronger than pi bond.. A double
(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) Question 1 An atom loses an electron to another atom. Is this an example of a physical or chemical change? Question 2 Physical
Chapters 8 and 9. Octet Rule Breakers Shapes
Chapters 8 and 9 Octet Rule Breakers Shapes Bond Energies Bond Energy (review): The energy needed to break one mole of covalent bonds in the gas phase Breaking bonds consumes energy; forming bonds releases
CHEM 130 Exp. 8: Molecular Models
CHEM 130 Exp. 8: Molecular Models In this lab, we will learn and practice predicting molecular structures from molecular formulas. The Periodic Table of the Elements IA 1 H IIA IIIA IVA VA VIA VIIA 3 5
Chapter 9. Molecular Geometries and Bonding Theories. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 9 Theories John D. Bookstaver St. Charles Community College Cottleville, MO Shapes The shape of a molecule plays an important role in its reactivity. By noting the number of
Test 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
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Chang & Goldsby Modified by Dr. Juliet Hahn Copyright McGraw-Hill Education. All rights reserved. No reproduction
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: and Hybridization of Atomic Orbitals Chapter 10 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Valence shell electron pair repulsion (VSEPR)
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
Chapter 9: Molecular Geometries and Bonding Theories Learning Outcomes: Predict the three-dimensional shapes of molecules using the VSEPR model.
Chapter 9: Molecular Geometries and Bonding Theories Learning Outcomes: Predict the three-dimensional shapes of molecules using the VSEPR model. Determine whether a molecule is polar or nonpolar based
Chapter , Exam 2
Chapter 4 4.5-4.7, 4.9-4.10 Exam 2 Covalent Bonding Covalent bonds are formed when two nonmetals combine The atoms share electrons. If the atoms share 2 electrons a single covalent bond is formed. If the
Chapter 9. Covalent Bonding: Orbitals. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 9 Covalent Bonding: Orbitals Chapter 9 Table of Contents (9.1) (9.2) (9.3) (9.4) (9.5) (9.6) Hybridization and the localized electron model The molecular orbital model Bonding in homonuclear diatomic
Covalent Bonding. Click a hyperlink or folder tab to view the corresponding slides. Exit
Covalent Bonding Section 8.1 The Covalent Bond Section 8.2 Naming Molecules Section 8.3 Molecular Structures Section 8.4 Molecular Shapes Section 8.5 Electronegativity and Polarity Click a hyperlink or
Molecular Geometry. Objectives N H H. The objectives of this laboratory are to:
Objectives The objectives of this laboratory are to: Molecular Geometry Write Lewis structure representations of the bonding and valence electrons in molecules. Use the VSEPR model to predict the molecular
Chemical bonding & structure
Chemical bonding & structure Ionic bonding and structure Covalent bonding Covalent structures Intermolecular forces Metallic bonding Ms. Thompson - SL Chemistry Wooster High School Topic 4.3 Covalent structures
Chapter 12. Chemical Bonding
Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and
8.3 Bonding Theories > Chapter 8 Covalent Bonding. 8.3 Bonding Theories. 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding
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 Molecular Shape What information does a structural formula give
Chemistry Day 30. Tuesday, November 13 th Wednesday, November 14 th, 2018
Chemistry Day 30 Tuesday, November 13 th Wednesday, November 14 th, 2018 Do-Now: Covalent Bonding CN B 1. Write down today s FLT 2. How can you tell if atoms will form an ionic or a covalent bond? 3. What
Chapter 9 Molecular Geometry and Bonding Theories
Lecture Presentation Chapter 9 Geometry James F. Kirby Quinnipiac University Hamden, CT Shapes Lewis Structures show bonding and lone pairs, but do not denote shape. However, we use Lewis Structures to
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
OFB Chapter 3 Chemical Periodicity and the Formation of Simple Compounds
OFB hapter 3 hemical Periodicity and the Formation of Simple ompounds 3-1 Groups of Elements 3-2 The Periodic Table 3-3 Ions and Ionic ompounds 3-4 ovalent Bonding and Lewis Structures 3-5 3-6 Naming ompounds
B. (i), (iii), and (v) C. (iv) D. (i), (ii), (iii), and (v) E. (i), (iii), (iv), and (v) Answer: B. SO 3, and NO 3 - both have 24 VE and have Lewis
SCCH 161 Homework 3 1. Give the number of lone pairs around the central atom and the molecular geometry of CBr 4. Answer: Carbon has 4 valence electrons and bonds to four bromine atoms (each has 7 VE s).
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
Name Date Class. covalent bond molecule sigma bond exothermic pi bond
Date Class 8 Covalent Bonding Section 8.1 The Covalent Bond In your textbook, read about the nature of covalent bonds. Use each of the terms below just once to complete the passage. covalent bond molecule