Ionic Compounds and Lattice Energy
|
|
- Lindsay Long
- 5 years ago
- Views:
Transcription
1 Ionic Compounds and Lattice Energy Directions for Class Activities: 1. A reader will be assigned for each group. This person will read each question aloud. 2. The group should discuss what the answer should be. If no consensus is reached, raise your hand for the instructor s guidance. 3. When a consensus is reached, everyone should write down the answer. Make sure everyone is writing very similar words. 4. This packet will be given to the person on your right. You will receive a packet from your left. This rotation occurs after every question (Q) to ensure your group is on the same problem. This is why it is important to follow Step 3, since you don t know which packet you will end up with at the end of today s lesson. You don t want to be left with a partially blank packet because someone in your group didn t do their job! As its name suggests, an ionic compound (or salt) is composed of oppositely charged ions. Q1. In the following list of chemical formulas, circle those that are ionic compounds: ClBr 3 NCl 3 CaSO 4 OF 2 NaI Al 2 S 3 PO 4 3- C 7 H 16 XeF 4 Pb(NO 3 ) 2 Fe 2 O 3 NH 4 + Q2. You should have circled five compounds in Q1. What are the features that allow you to identify an ionic compound based on its chemical formula? Imagine two charged particles (called ions). One is positive (called the cation, pronounced cat-eye-on ) and the other is negative (called the anion, pronounced ann-eye-on ). They will feel an attraction to each other because they are oppositely charged. For the next two questions give an answer that is based on intuition and common sense. If you are stuck, then take the best guess you can for Q3 and Q4 and then move on to Q5. Q3. As the ions move apart, do you think the attractive force between them increases or decreases? Q4. If the positive ion has a +2 charge and the negative ion has a -2 charge, do you think the attraction between them is bigger or smaller than if their charges were +1 and -1? (Assume the only difference between the ions is the charge). Page 1 of 6
2 Model 1. The attraction between oppositely charged ions increases with charge and decreases with the distance between the ions, and is given by Coulomb s Law: F = k where F is the attractive (Coulombic) force between the ions (in units of Newtons), q 1 and q 2 are the charges of the two ions (each given by units of Coulombs), d is the distance between the ions (in meters), and k is a constant. q q d Q5. Use the relationships in Coulomb s Law to check your answers to Q3 and Q4. Did your intuition lead you to the correct answers in both cases? Q6. In Q4 you were asked to compare the attractive force between a pair of +2/-2 charged ions and +1/-1 charge ions. Using Coulomb s Law, did the attractive force of the +2/-2 pair double that of the other pair? Explain. Information. The size of atoms and ions is related to the number of electrons and occupied shells. The more electrons there are, the larger the atom or ion becomes due to the filling of more shells. In addition, the repulsions between the electrons cause the electron clouds to swell. The less electrons there are, the greater effect the nucleus has on pulling in the electrons and making the atom or ion smaller. Q7. Based on the text above, which is larger, a Li atom or a Li + ion? A Na atom or a Na + ion? Q8. Based on the text above, which is larger, a F atom or a F - ion? A Cl atom or a Cl - ion? Q9. Which pair of ions would you expect to have a stronger attraction: Li + /F -, or Na + /Cl -? (Hint: Consider Coulomb s Law. What factor would be different in these two pairs?). Page 2 of 6
3 Q10. To check your answer to Q9, consider the following two ions, Li + and F -. The ionic radius of Li + is 76 pm (picometer, m). The ionic radius of F - is 133 pm. Sketch these values on the drawing below. What is the distance between the centers of these ions? The ionic radius of Na + is 102 pm and Cl - is 181 pm. What is the distance between the centers of these ions? Based on Coulomb s Law, which pair of ions has the greater attraction? Q11. Due to the attractive forces between oppositely-charged ions, do you believe the decomposition (breaking apart) of an ionic compound would be exothermic (release energy) or endothermic (absorb energy)? Would the change in enthalpy for the decomposition be positive or negative? Then write an equation for the decomposition of an ionic compound into its ions. Q12. Based on your response above, do you believe the formation of an ionic compound would be exothermic or endothermic? Would the change in enthalpy for the formation be positive or negative? Then write an equation for the formation of an ionic compound from its ions. Page 3 of 6
4 Calculating Lattice Energies by using the Born-Haber Cycle Q13. The energy that is released from the formation of an ionic compound from a gaseous cation and gaseous anion is called the Lattice Energy. For example: A) Li + (g) + F - (g) LiF (s) H lattice =? You are probably familiar instead with the enthalpy of formation, H f º. As a review, complete the thermochemical equation for the formation of one mole of solid lithium fluoride from its elements in their standard states. Don t forget to label physical states! It s very important in this exercise!!! The enthalpy of formation value for this process is provided below. B) H f º = -612 kj/mol Equation B is much different from equation A. To find the lattice energy, let s start with equation B and step through all the processes to transform equation B into equation A. To do so, write out the following thermochemical equations: C) The conversion of solid lithium into gaseous lithium is a sublimation process that requires 161 kj/mol of energy. H subl = D) The diatomic gaseous fluorine molecules must be dissociated into gaseous atoms. Find this enthalpy value in Appendix J of your textbook. H dissociation = E) The gaseous lithium atoms from equation C are ionized by losing an electron. Find the ionization energies from Figure 7.20 in your textbook. IE lithium = F) The gaseous fluorine atoms from equation D are ionized by adding an electron. The energy associated with an atom GAINING an electron is called the electron affinity (EA). Find the EA from Table 7.10 in your textbook. EA fluorine = After you are finished writing Equations B through F, notify your instructor who will check them or send you to another group to check answers. Make sure the energy signs are correct and the balanced equation is correct. After verifying they are correct, use Hess Law and equations B through F to find the lattice energy in equation A. This method for solving multistep sequences is called the Born-Haber cycle. The cycle is visualized in the following diagram: Page 4 of 6
5 The Born-Haber Cycle The energy associated with each change is shown next to the arrow for that process. You should understand each process and know the name for the energy involved in that process. H f º M (s) + ½ X 2 (g) MX (s) H sublimation H dissociation M (g) X (g) Lattice energy Ionization energy, IE Electron Affinity, EA M + (g) + X - (g) Exercises (you do not need to rotate papers) This material is covered in Section 3.5 on ionic compounds, Section 7.12 and It is a good idea to read these sections. You should also review Sections This website is recommended for further reading: These Questions for Review and Thought are recommended (Chapter 7): p #96, 106,108, 110, 118, 119, 142. Your first quiz will be on anything from this activity, exercises, and recommended problems from the text. You will not be asked to submit any of this work. 1. List three examples of ionic compounds that you can think of without referring to any compounds mentioned in this exercise. 2. For practice, provide names of all the compounds in Q1 (page 1 of this activity). You are still expected to recall polyatomic ion names and formulas from memory! 3. Predict which compound will have the greater Coulombic attraction between its ions: NaCl or KCl. 4. The formation of NaCl from its gaseous ions has a lattice energy of -788 kj/mol: Na + (g) + Cl - (g) NaCl (s) H lattice = -788 kj/mol The formation of KCl from its gaseous ions has a lattice energy of -718 kj/mol: K + (g) + Cl - (g) KCl (s) H lattice = -718 kj/mol a) Which is requires more energy to decompose, NaCl or KCl? b) Which is held together by a stronger attraction, NaCl or KCl? c) Were you correct in exercise #3? Continued on page 6 Page 5 of 6
6 5. As the lattice energy increases (gets more positive), the Coulombic attraction between the ions (increases or decreases) 6. What do you think is the relationship between the lattice energy of an ionic compound and its melting point? Try to think it through without looking in the textbook. The more positive the lattice energy, the (higher or lower) the melting point. 7. Is the sign of most lattice energies positive or negative? Explain why. 8. Is the lattice energy proportional to the Coulombic force? To find out, do parts a and b below. a) Without calculating the Coulombic force (you do not have k ), use the following data to predict the lattice energy for BaO: Ionic radii of Na + =102 pm, Cl - =181 pm, Ba 2+ =135pm, O 2- =275pm; The lattice energy for NaCl is -786 kj/mol. (Hint: Use proportions). b) The actual lattice energy for BaO is kj/mol. How was your prediction? Does the lattice energy seem to be proportional to the Coulombic force experience by two ions? 9. a) Write an equation for the sublimation of sodium metal. What is the energy of this process called? b) Write an equation for the ionization of sodium metal. What is the energy of this process called? c) Write an equation for the formation of sodium chloride from its elements. What is the energy of this process called? d) The lattice energy of NaCl is -786 kj/mol. Write a thermochemical equation. 10. Show how the Born-Haber cycle can be used to calculate the lattice energy of KBr (s). Use the following values (in kj/mol): sublimation of K H=90; dissociation of Br2 H=112; IE of K=419; EA of Br = -325; H f º of KBr(s)=-392. To check your answer, go to the recommended website listed at the top of the page (under Exercises ) and click on Lattice Energy U under the diagram for the Born-Haber cycle. Look up the value for KBr. An answer key with worked out solutions for these exercises will be posted online. To prepare for the quiz that will be given at the beginning of the next class period, go through this entire activity and make sure you understand the point of every question. If you do not, please go to office hours. If you cannot, then send an or call your instructor. In addition, you should do the reading and the recommended problems from the text. Page 6 of 6
15.2 Born-Haber Cycles
15.2 Born-Haber Cycles 15.2.1 - Define and apply the terms lattice enthalpy and electron affinity Lattice Enthalpy The energy required to completely separate one mole of a solid ionic compound into its
More information5.2.1 Answers Lattice Enthalpy 2012
5.2.1 Answers Lattice Enthalpy 2012 Introduction In this topic we will construct a Born-Haber cycle (or lattice enthalpy cycle) which allows us to calculate numerical values for processes which occur in
More informationThe Octet Rule Most atoms seek the same electron configuration as the closest noble gas, which is very stable.
Ionic Bonding Isn t it Ionic? Don t you Think? Chemical Bonds Chemical bonds result from changes in the locations of the valence electrons of atoms. Because electronic structures are described by their
More informationEnergetics of Bond Formation
BONDING, Part 4 Energetics of Bond Formation 167 Energetics of Covalent Bond Formation 168 1 169 Trends in Bond Energies the more electrons two atoms share, the stronger the covalent bond C C (837 kj)
More informationWS 1: Ionic Bonds 1. Charge on particle 1= q1 Charge on particle 2 = q2
Part I: The Ionic Bonding Model: i WS 1: Ionic Bonds 1 Trends in ionization energies and electron affinities indicate that some elements for ions more readily than others. We know that ions with opposite
More informationLattice Energy: The Born-Haber cycle. Introduction. Lattice Energy. Born-Haber Cycle
Lattice Energy: The Born-Haber cycle Ionic solids tend to be very stable compounds. The enthalpies of formation of the ionic molecules cannot alone account for this stability. These compounds have an additional
More informationThermodynamics. Standard enthalpy change, H
Standard enthalpy change, H Thermodynamics Enthalpy change, H, is defined as the heat energy change measured under conditions of constant pressure. The value of the enthalpy change for a particular reaction
More information13 Energetics II. Eg. Na (g) Na + (g) + e - ΔH = +550 kj mol -1
13 Energetics II First ionisation energy I(1) or IE (1): the energy required to remove one mole of electrons from one mole of the gaseous atoms of an element to 1 mole of gaseous monopositive ions. Eg.
More information1 P a g e h t t p s : / / w w w. c i e n o t e s. c o m / Chemistry (A-level)
1 P a g e h t t p s : / / w w w. c i e n o t e s. c o m / Lattice energy (Chapter 19 TB) Chemistry (A-level) Lattice energy is the enthalpy change when 1 mole of an ionic compound is formed from its gaseous
More informationElectron Configuration and Periodic Trends - Chapter 5 section 3 Guided Notes
Electron Configuration and Periodic Trends - Chapter 5 section 3 Guided Notes There are several important atomic characteristics that show predictable that you should know. Atomic Radius The first and
More informationlattice formation from gaseous ions
BORN HABER CYCLES The Born Haber cycles is an adaption of Hess s law to calculate lattice enthalpy from other data The lattice enthalpy cannot be determined directly. We calculate it indirectly by making
More informationCHEMISTRY - CLUTCH CH.9 - BONDING & MOLECULAR STRUCTURE.
!! www.clutchprep.com CONCEPT: ATOMIC PROPERTIES AND CHEMICAL BONDS Before we examine the types of chemical bonding, we should ask why atoms bond at all. Generally, the reason is that ionic bonding the
More information15.2 Born-Haber Cycle
15.2 Born-Haber Cycle Our calculations of enthalpies so far have involved covalent substances. Now we need to look at the enthalpy changes involved in the formation of giant ionic lattices. Lattice enthalpy
More informationChapter 11 Intermolecular Forces, Liquids, and Solids
Chapter 11 Intermolecular Forces, Liquids, and Solids Dissolution of an ionic compound States of Matter The fundamental difference between states of matter is the distance between particles. States of
More informationTypes of Bonding : Ionic Compounds. Types of Bonding : Ionic Compounds
Types of Bonding : Ionic Compounds Ionic bonding involves the complete TRANSFER of electrons from one atom to another. Usually observed when a metal bonds to a nonmetal. - - - - - - + + + + + + + + + +
More information6.3 Periodic Trends > Chapter 6 The Periodic Table. 6.3 Periodic Trends. 6.1 Organizing the Elements. 6.2 Classifying the Elements
1 63 Periodic Trends > Chapter 6 The Periodic Table 61 Organizing the Elements 62 Classifying the Elements 63 Periodic Trends 2 63 Periodic Trends > CHEMISTRY & YOU How are trends in the weather similar
More informationTrends in Atomic Size. What are the trends among the elements for atomic size? The distances between atoms in a molecule are extremely small.
63 Periodic Trends > 63 Periodic Trends > CHEMISTRY & YOU Chapter 6 The Periodic Table 61 Organizing the Elements 62 Classifying the Elements 63 Periodic Trends How are trends in the weather similar to
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Questions to Consider What is meant by the term chemical bond? Why do atoms bond with each other to form compounds? How do atoms bond with each other to form
More informationCHEMICAL BONDS. Electrical forces. Reflect a balance in the attractive and repulsive forces between electrically charged particles
CHEMICAL BONDS Chemical Bonds: Electrical forces. Reflect a balance in the attractive and repulsive forces between electrically charged particles Lewis Theory of Bonding: Electrons play a fundamental role
More informationChapter 9 Ionic and Covalent Bonding
Chem 1045 Prof George W.J. Kenney, Jr General Chemistry by Ebbing and Gammon, 8th Edition Last Update: 06-April-2009 Chapter 9 Ionic and Covalent Bonding These Notes are to SUPPLIMENT the Text, They do
More informationChemistry: The Central Science
Chemistry: The Central Science Fourteenth Edition Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds Three basic types of bonds Ionic Electrostatic attraction between ions Covalent Sharing of
More information1.8 Thermodynamics. N Goalby chemrevise.org. Definitions of enthalpy changes
1.8 Thermodynamics Definitions of enthalpy changes Enthalpy change of formation The standard enthalpy change of formation of a compound is the energy transferred when 1 mole of the compound is formed from
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 informationCH1810 Lecture #1 Solutions of Ionic Compounds
CH1810 Lecture #1 Solutions of Ionic Compounds Solutions Homogeneous mixtures are called solutions. The component of the solution that changes state is called the solute. The component that keeps its state
More informationCHEMISTRY - TRO 4E CH.9 - CHEMICAL BONDING I: THE LEWIS MODEL
!! www.clutchprep.com CONCEPT: ATOMIC PROPERTIES AND CHEMICAL BONDS Before we examine the types of chemical bonding, we should ask why atoms bond at all. Generally, the reason is that ionic bonding the
More informationModels Of Chemical Bonding. Chapter Nine. AP Chemistry
Models Of Chemical Bonding Chapter Nine AP Chemistry Q. Why do atoms bond? A. To lower the potential energy between positive and negative particles. Atoms like humans seek to become more stable. Metals
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 informationName: Hr: 8 Basic Concepts of Chemical Bonding
8.1-8.2 8.3-8.5 8.5-8.7 8.8 Name: Hr: 8 Basic Concepts of Chemical Bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule State the type of bond (ionic, covalent, or metallic) formed between any
More informationChapter 9. Chemical Bonding I: The Lewis Model. HIV-Protease. Lecture Presentation
Lecture Presentation Chapter 9 Chemical Bonding I: The Lewis Model HIV-Protease HIV-protease is a protein synthesized by the human immunodeficiency virus (HIV). This particular protein is crucial to the
More informationChapter 8 Concepts of Chemical. Bonding
Chapter 8 Concepts of 8.1 Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms. Electrons are free
More informationChemistry 101 Chapter 9 CHEMICAL BONDING. Chemical bonds are strong attractive force that exists between the atoms of a substance
CHEMICAL BONDING Chemical bonds are strong attractive force that exists between the atoms of a substance Chemical Bonds are commonly classified into 3 types: 1. IONIC BONDING Ionic bonds usually form between
More information5.2 Energy. N Goalby chemrevise.org Lattice Enthalpy. Definitions of enthalpy changes
5.2 Energy 5.2.1 Lattice Enthalpy Definitions of enthalpy changes Enthalpy change of formation The standard enthalpy change of formation of a compound is the energy transferred when 1 mole of the compound
More informationCopyright 2018 Dan Dill 1
TP Do we get the same amount of energy back from making bonds between an ion and water molecules, as it took to break the ionic bonds holding an ion in the solid? + 1. The energy is the same 2. More energy
More informationCHEM 110: CHAPTER 8 Basic Concepts of Chem Bonding. Lewis Structures of Atoms: The Lewis Dot Diagram
1 CHEM 110: CHAPTER 8 Basic Concepts of Chem Bonding Lewis Structures of Atoms: The Lewis Dot Diagram Lewis Dot Diagrams (developed by chemist Gilbert Lewis) are used to indicate the number of valence
More informationIonic Bonding and Ionic Compounds
Main Ideas Ionic bonds form from attractions between positive and negative ions Differences in attraction strength give ionic and molecular compounds different properties Multiple atoms can bond covalently
More informationWork hard. Be nice. Name: Period: Date: UNIT 3: Electrons Lesson 5: Atomic Radius and Ionic Radius
UNIT 3: Electrons Lesson 5: Atomic Radius and Ionic Radius Do Now: By the end of today, you will have an answer to: How the does the radius change when an atom becomes an ion? 1. How many protons, neutrons,
More informationChapter Nine. Chemical Bonding I
Chapter Nine Chemical Bonding I 1 The Ionic Bond and Lattice Energies 2 Lewis Dot Symbols Consists of atomic symbol surrounded by 1 dot for each valence electron in the atom Only used for main group elements
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.2 Electronegativity 8.3 Bond Polarity and Dipole Moments 8.4 Ions: Electron Configurations and Sizes 8.5 Energy
More informationChemical Bonding I: Basic Concepts
Chemical Bonding I: Basic Concepts Chapter 9 Valence electrons are the outer shell electrons of an atom. The valence electrons are the electrons that participate in chemical bonding. Group e - configuration
More information12A Entropy. Entropy change ( S) N Goalby chemrevise.org 1. System and Surroundings
12A Entropy Entropy change ( S) A SPONTANEOUS PROCESS (e.g. diffusion) will proceed on its own without any external influence. A problem with H A reaction that is exothermic will result in products that
More informationChapter 6 INORGANIC THERMODYNAMICS. Exercises
Chapter 6 INORGANIC THERMODYNAMICS Exercises 6. (a) A reaction that occurs without external help, or a reaction for which G is negative. (b) A measure of disorder. (c) The enthalpy change when a mole of
More informationThermodynamics Born- Haber cycles
Thermodynamics Born- Haber cycles Born Haber cycles Is when Hess s Law is extended towards ionic compounds. We usually calculate Enthalpy of formation for substances using bond energy data. But, we cannot
More informationGHW#3. Chapter 3. Louisiana Tech University, Chemistry 481. POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3.
GHW#3. Chapter 3. Louisiana Tech University, Chemistry 481. POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Energetics of Ionic Bonding. Why? What are the properties of ionic compounds?
More informationChemistry 101 Chapter 9 CHEMICAL BONDING
CHEMICAL BONDING Chemical bonds are strong attractive force that exist between the atoms of a substance. Chemical bonds are commonly classified into 3 types: Ionic Bonding Ionic bonds form between metals
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 informationPeriodicity SL (answers) IB CHEMISTRY SL
(answers) IB CHEMISTRY SL Syllabus objectives 3.1 Periodic table Understandings: The periodic table is arranged into four blocks associated with the four sublevels s, p, d, and f. The periodic table consists
More informationUnit 4: Presentation A Covalent Bonding. Covalent Bonding. Slide 2 / 36. Slide 1 / 36. Slide 4 / 36. Slide 3 / 36. Slide 6 / 36.
Slide 1 / 36 New Jersey Center for Teaching and Learning Progressive Science Initiative This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and
More informationChapter 8. Chemical Bonding I: Basic Concepts
Chapter 8 Chemical Bonding I: Basic Concepts Topics Lewis Dot Symbols Ionic Bonding Covalent Bonding Electronegativity and Polarity Drawing Lewis Structures Lewis Structures and Formal Charge Resonance
More informationWhat is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds?
Chapter 8 What is a Bond? A force that holds atoms together. Why? We will look at it in terms of energy. Bond energy- the energy required to break a bond. Why are compounds formed? Because it gives the
More informationName AP CHEM / / Chapter 8 Outline Bonding: General Concepts
Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Types of Chemical Bonds Information about the strength of a bonding interaction is obtained by measuring the bond energy, which is the energy
More informationChapter 7: Chemical Bonding and Molecular Structure
Chapter 7: Chemical Bonding and Molecular Structure Ionic Bond Covalent Bond Electronegativity and Bond Polarity Lewis Structures Orbital Overlap Hybrid Orbitals The Shapes of Molecules (VSEPR Model) Molecular
More informationSodium, Na. Gallium, Ga CHEMISTRY Topic #2: The Chemical Alphabet Fall 2017 Dr. Susan Findlay See Exercises 6.1 to 6.5 and 7.1.
Sodium, Na Gallium, Ga CHEMISTRY 1000 Topic #2: The Chemical Alphabet Fall 2017 Dr. Susan Findlay See Exercises 6.1 to 6.5 and 7.1 Forms of Carbon What is an alkali metal? Any element in Group 1 except
More informationChapter 9. Chemical Bonding I: Basic Concepts
Chapter 9 Chemical Bonding I: Basic Concepts to: This is the first of two chapters on bonding. Upon completion of Chapter 9, the student should be able 1. Identify the valence electrons for all representative
More informationMore Chemical Bonding
More Chemical Bonding Reading: Ch 10: section 1-8 Ch 9: section 4, 6, 10 Homework: Chapter 10:.31, 33, 35*, 39*, 43, 47, 49* Chapter 9: 43, 45, 55*, 57, 75*, 77, 79 * = important homework question Molecular
More informationBond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons shared
ch9blank Page 1 Chapter 9: Chemical Bonding I: Lewis Theory Three types of chemical bonding: Bond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons
More informationThree types of chemical bonding: Recall that we can use dots to show valence electrons - these are called Lewis electron-dot structures:
Chapter 9: Chemical Bonding I: Lewis Theory Three types of chemical bonding: Bond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons shared Metallic
More informationThe energy associated with electrostatic interactions is governed by Coulomb s law:
Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other
More informationWorksheet 5 - Chemical Bonding
Worksheet 5 - Chemical Bonding The concept of electron configurations allowed chemists to explain why chemical molecules are formed from the elements. In 1916 the American chemist Gilbert Lewis proposed
More informationBONDING. Covalent bonding Two non- metal atoms can form a stable octet structure by sharing electrons.
BODIG In the process of bonding electrons move to a lower energy level to form a more stable structure. This can be done by transferring electron(s) to another atom or by pairing with an electron from
More informationBonding in Chemistry. Chemical Bonds All chemical reactions involve breaking of some bonds and formation of new ones where new products are formed.
CHEMICAL BONDS Atoms or ions are held together in molecules or compounds by chemical bonds. The type and number of electrons in the outer electronic shells of atoms or ions are instrumental in how atoms
More informationPeriodic Table trends
2017/2018 Periodic Table trends Mohamed Ahmed Abdelbari Atomic Radius The size of an atom is defined by the edge of its orbital. However, orbital boundaries are fuzzy and in fact are variable under different
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 informationTypes of bonding: OVERVIEW
1 of 43 Boardworks Ltd 2009 Types of bonding: OVERVIEW 2 of 43 Boardworks Ltd 2009 There are three types of bond that can occur between atoms: an ionic bond occurs between a metal and non-metal atom (e.g.
More informationTrends in the Periodic Table
Trends in the Periodic Table Effective nuclear charge: < effective nuclear charge is the attraction felt by the valence electrons from the nucleus < increases across a period : increases across because
More informationCh. 8 Chemical Bonding: General Concepts. Brady & Senese, 5th Ed
Ch. 8 Chemical Bonding: General Concepts Brady & Senese, 5th Ed Index 8.1. Electron transfer leads to the formation of ionic compounds 8.2. Lewis symbols help keep track of valence electrons 8.3. Covalent
More informationCh. 8 Chemical Bonding: General Concepts. Brady & Senese, 5th Ed
Ch. 8 Chemical Bonding: General Concepts Brady & Senese, 5th Ed Index 8.1. Electron transfer leads to the formation of ionic compounds 8.2. Lewis symbols help keep track of valence electrons 8.3. Covalent
More informationChapter 8 Concepts of Chemical. Bonding. Ionic vs Covalent Simulation 3/13/2013. Why do TiCl 4 & TiCl 3 have different colors?
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 8 Concepts of John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice
More informationChapter 3 (part 3) The Structures of Simple Solids
CHM 511 chapter 3 page 1 of 9 Chapter 3 (part 3) The Structures of Simple Solids Rationalizing Structures Ionic radii As noted earlier, a reference value is needed. Usually oxygen is assumed to be 140
More informationGeneral Chemistry Notes Name
Bio Honors General Chemistry Notes Name Directions: Carefully read the following information. Look for the ** directions in italics** for prompts where you can do some work. Use the information you have
More information8.6,8.7 Periodic Properties of the Elements
Pre -AP Chemistry 8.6,8.7 Periodic Properties of the Elements READ p. 305 315, 294-296 Practice Problems Pg 315 -Exercise 8.9 Pg 318-321 #36, 55, 64, 66, 67, 69, 72, 80 Periodic Trends are predictable
More informationChemical Bonds. How atoms connect to form... everything.
Ch09 Chemical Bonds How atoms connect to form... everything. When carbon, oxygen and hydrogen atoms bond in a certain way to form sugar, the resulting compound has a sweet taste. The sweetness resides
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 informationCHEMISTRY XL-14A CHEMICAL BONDS
CHEMISTRY XL-14A CHEMICAL BONDS July 16, 2011 Robert Iafe Office Hours 2 July 18-July 22 Monday: 2:00pm in Room MS-B 3114 Tuesday-Thursday: 3:00pm in Room MS-B 3114 Chapter 2 Overview 3 Ionic Bonds Covalent
More informationConcepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds. David A. Katz Pima Community College Tucson, AZ
Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds David A. Katz Pima Community College Tucson, AZ Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction
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 informationForming Chemical Bonds
Forming Chemical Bonds Chemical Bonds Three basic types of bonds 2012 Pearson Education, Inc. Ionic Electrostatic attraction between ions. Covalent Sharing of electrons. Metallic Metal atoms bonded to
More information1.8 Thermodynamics. Lattice formation enthalpy Enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions
1.8 Thermodynamics Review: In 1.3 we looked at ionic bonding and learned that: Giant ionic lattice structure Ionic bonding: Strong electrostatic force of attraction between oppositely charged ions that
More informationFifth Exam CHEM 1A Summer 2017
ifth Exam EM 1A Summer 2017 Name: Last KEY irst Instructions: Read every problem carefully. Gauge your time. Use the proper number of significant figures on your results. Don t just believe the calculator,
More informationChapter Nine. Chapter Nine. Chemical Bonds: A Preview. Chemical Bonds. Electrostatic Attractions and Repulsions. Energy of Interaction
1 Chemical Bonds: A Preview 2 Chemical Bonds Forces called chemical bonds hold atoms together in molecules and keep ions in place in solid ionic compounds. Chemical bonds are electrostatic forces; they
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 informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8. Basic Concepts of Chemical Bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule 8.2 Ionic Bonding Consider the reaction between sodium and chlorine: Na(s) + ½ Cl 2 (g) NaCl(s) H o f
More informationPeriodic Table and Trends Structure and Properties of Matter. Background
Background Periodic trends are the patterns observed in elemental properties across a row or down a column on the Periodic Table. Some of these trends were observed when the Periodic Table was first being
More informationCHEMISTRY. CHM202 Class #3 CHEMISTRY. Chapter 11. Chapter Outline for Class #3. Solutions: Properties and Behavior
CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies CHM202 Class #3 1 Chemistry, 5 th Edition Copyright 2017, W. W. Norton & Company CHEMISTRY Fifth Edition Gilbert Kirss Foster Bretz Davies Chapter
More informationChapter 8. forces of attraction which hold atoms or ions together. 3 fundamental types of bonding. Ionic - metals & nonmetals
Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds forces of attraction which hold atoms or ions together 3 fundamental types of bonding Ionic - metals & nonmetals Covalent - nonmetals (semimetals)
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 informationAP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
More informationChapter 9: Chemical Bonding I: Lewis Theory
C h e m i s t r y 1 A : C h a p t e r 9 P a g e 1 Chapter 9: Chemical Bonding I: Lewis Theory Homework: Read Chapter 9: Work out sample/practice exercises. Check for the MasteringChemistry.com assignment
More informationØ Draw the Bohr Diagrams for the following atoms: Sodium Potassium Rubidium
Chemistry 11 Atomic Theory V Name: Date: Block: 1. Atomic Radius 2. Ionization Energy 3. Electronegativity 4. Chemical Bonding Atomic Radius Periodic Trends Ø As we move across a period or down a chemical
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.3 Bond Polarity and Dipole Moments 8.5 Energy Effects in Binary Ionic Compounds 8.6 Partial Ionic Character
More informationMetallic & Ionic Solids. Crystal Lattices. Properties of Solids. Network Solids. Types of Solids. Chapter 13 Solids. Chapter 13
1 Metallic & Ionic Solids Chapter 13 The Chemistry of Solids Jeffrey Mack California State University, Sacramento Crystal Lattices Properties of Solids Regular 3-D arrangements of equivalent LATTICE POINTS
More informationChapter 8. Basic Concepts of Chemical Bonding. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 8 of Chemical John D. Bookstaver St. Charles Community College Cottleville, MO Chemical Bonds Chemical bonds are the forces that hold the atoms together in substances. Three
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 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 informationOctet rule Naming and writing formulas
Octet rule Naming and writing formulas Definitions The octet rule states that atoms are most stable when they have a full shell of 8 electrons in the OUTERMOST shell Ionic bonding forms between a metal
More informationTopic 10 Thermodynamics Revision Notes
1) Enthalpy Changes Topic 10 Thermodynamics Revision Notes An enthalpy change is a change in heat energy measured at constant pressure. Enthalpy changes refer to the chemicals not the surroundings. The
More informationSOLID STATE CHEMISTRY
SOLID STATE CHEMISTRY Crystal Structure Solids are divided into 2 categories: I. Crystalline possesses rigid and long-range order; its atoms, molecules or ions occupy specific positions, e.g. ice II. Amorphous
More informationCK-12 Chemistry - Basic Answer Key
CK-12 Chemistry - Basic Answer Key Chapter 8: Ionic and Metallic Bonding 8.1 Ions Practice 8.1 Write the ground state configuration for the metal calcium, and predict the ion form it must become to be
More informationYou have mastered this topic when you can:
CH 11 T17 IONIC COMPOUNDS IONIC BONDS 1 You have mastered this topic when you can: 1) define or describe these terms: IONIC BOND, CATION, ANION and FORMULA UNIT. 2) predict the formation of an IONIC BOND
More information