...Zakita Jones February 25, 2014 –March 25, 2014 Labs # 3 and 4 Title: Chemical Bonding Lewis Structures and Shapes of Molecules and Ions References/Tools: 1. Chapter 9: Models of Chemical Bonding 2. Chapter 10: The Shapes of Molecules 3. The Modern Periodic Table 4. Electron Configuration (SPDF notation, Orbital diagram), Lewis Symbols, Lewis Structures, Molecular Formulas, and Molecular Diagrams 5. Ion and Molecules, Tetrahedral Geometry (109 degrees) , Planar Geometry (120 degrees), and Linear geometry (180 degrees) 6. Page 279 7. VESPR Theory (Chapter 10) (Valence Electrons Pair Repulsion Theory) Objective: To learn and study about chemical bonding, chemical formulas, Lewis structures, bond angles, geometry and shapes of molecules and molecular ions. Definitions/Concepts/Theories/Formulas Chapter 9 1. Ionic Bonding- the complete transfer of valence electrons between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the non-metal accepts those electrons to become a negatively charged anion. 2. Covalent Bonding- a chemical bond that involves the sharing of electron pairs between atoms. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding. 3. Metallic Bonding- the electrostatic attraction between the positively charged atomic nuclei of metal...
Words: 869 - Pages: 4
...the nature of each bonding present in these different types of substances and use this to explain the physical properties they exhibit and their structures. Ionic compounds are compounds that are composed of positive and negative ions. An ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. Usually, the positively charged portion consists of metal (cations) and the negatively charged portion is an (anion) or polyatomic ion. Ions in ionic compounds are held together by the electrostatic forces between oppositely charged bodies. The positive and negative ions in these compounds are thought to be arranged in an orderly three-dimensional lattice. For example, the structure of sodium chloride is shown. In the lattice, each positive sodium ion is surrounded by six negative chloride ions and each negative chloride ion is surrounded by six positive sodium ions. The position of the ions is fixed and apart from vibration about these fixed positions no other movement of the ions occurs in the solid compound. Each ion in an ionic solid is held in the crystal lattice by strong electrostatic attractions to the oppositely charged ions around it. These electrostatic forces between the positive and negative ions are called ionic bonds. Because ionic compounds have high melting points, in other words considerable energy is required to disrupt the attractive forces between the positive and negative ions; ionic bonding is regarded as an...
Words: 3332 - Pages: 14
...SPECIALIST ARTICLE Magnets and adhesives: A durable connection Ranjit Dhaliwal, Sales Manager, DELO Industrial Adhesives, Singapore Due to their special physical properties, magnets are used in many technical and electronic application areas. Especially in machine tool construction and the automotive sector – for example, in sensors and electric motors – the magnetic fluxes induced by magnets are utilized. Here, high-energy magnets, so-called permanent magnets of the rare-earth group, allow numerous new technical solutions due to their extremely high energy densities. For example, a high commercial relevance is attributed to, for example, cerium (Ce) in glass or steel production and lathanium (La) in Y-ray film production and production of catalysts for the reduction of harmful substances or exhaust gas treatment. Moreover, compared to conventional magnetic materials, like barium ferrite, modern permanent magnets on the basis of NdFeB alloys (neodymium iron boron) make it possible to considerably minimize magnetic systems or increase the magnetic energies at the same size to a great extent. The chart below makes it possible to compare the energy products of some magnetic materials: |Magnetic material |Energy product (WxH) max | |Plastic-bound barium ferrites, anisotropic |12 kJ/m³ | |Anisotropic strontium ferrites ...
Words: 869 - Pages: 4
...Alan Buczynski Iron Bonding I just don't get it.” We were up on the iron, about 120 feet, waiting for the gang below to swing up another beam. Sweat from under Ron's hard hat dripped on the 'beam we were sitting on and evaporated immediately, like water thrown on a saW1a stove. We were talking about the "men's movement" and "wildman weekends." "I mean," he continued, "if they want to get dirty and sweat and cuss and pOW1d on things, why don't they just get real jobs and get paid for it?" Below, the crane growled, the next piece lifting skyward. I replied: "Nah, Ron, that isn't the point. They don't want to sweat every day, just sometimes." He said: "Man, if you only sweat when you want to, I don't call that real sweatin." Although my degree is in English, I am an ironworker by trade; my girlfriend, Patti, is a graduate student in English literature. Like a tennis ball volleyed by two players with distinctly different styles, I am bounced between blue-collar maulers and precise academicians. My conversations range from fishing to Foucault, derricks to deconstruction. There is very little overlap, but when it does occur it is generally the academics who are curious about the working life. Patti and I were at a dinner party. The question of communication between men had arisen. Becky, the host, is a persistent interrogator: "What do you and Ron talk about?" I said, “Well, we talk about work, drinking, ah, women.” Becky asked, "Do you guys ever say...
Words: 1020 - Pages: 5
...Chapter 8 Covalent Bonding and Molecular Structure Chapter 8: Covalent Molecular Structure Bonding and Chapter In Context In this chapter and the next, we examine chemical bonding in detail. We examined ionic bonding briefly in Chapter 2 and will do so in more detail in Chapter 11. We will also examine intermolecular forces in detail in Chapter 11. Here we will apply what you have learned about atomic structure (Chapter 6), electron configurations, and periodic trends (Chapter 7) to the chemical bonds formed between atoms and ions and the shapes of molecules and ions that contain covalent bonds. • 8-1 Biology: Molecular shape of enzymes specifically allow only certain reactions to occur. Drugs are developed that specifically fit into active sites in the enzyme to affect or even stop its action. Chapter 8 8.1 Interactions Between Particles: Coulomb’s Law 8.2 Covalent Bonding Basics 8.3 Lewis Structures 8.4 Bond Properties 8.5 Electron Distribution in Molecules 8.6 Valence-Shell Electron-Pair Repulsion Theory and Molecular Shape 8.7 Molecular Polarity Chapter Goals • Apply Coulomb’s Law. • Understand forces involved in covalent bonding. • Write Lewis symbols and Lewis structures. • Predict bond properties. • Understand charge distribution in molecules. • Use VSEPR theory. • Identify polar and nopolar species. Chapter 8 Covalent Bonding and Molecular Structure 8-2 8.1 Interactions Between Particles: Coulomb’s Law OWL Opening Exploration 8.1 Coulomb’s Law Matter is...
Words: 8991 - Pages: 36
...polar bond | c. | structural formula | f. | hydrogen bond | ____ 1. a depiction of the arrangement of atoms in molecules and polyatomic ions ____ 2. a covalent bond in which only one pair of electrons is shared ____ 3. a covalent bond in which two pairs of electrons are shared ____ 4. a covalent bond in which the shared electron pair comes from only one of the atoms ____ 5. a covalent bond between two atoms of significantly different electronegativities ____ 6. a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA Match each item with the correct statement below. a. | network solid | e. | tetrahedral angle | b. | bonding orbital | f. | VSEPR theory | c. | dipole interaction | g. | sigma bond | d. | bond dissociation energy | ____ 7. energy needed to break a single bond between two covalently bonded atoms ____ 8. symmetrical bond along the axis between the two nuclei ____ 9. molecular orbital that can be occupied by two electrons of a covalent bond ____ 10. 109.5 ____ 11. shapes adjust so valence-electron pairs are as far apart as possible ____ 12. attraction between polar molecules ____ 13. crystal in which all the atoms are covalently bonded to each other Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 14. What information does a molecular formula provide...
Words: 5916 - Pages: 24
...Unit 7 Unit 8 Study Guide 1. Which of the following statements is incorrect? A) Ionic bonding results from the transfer of electrons from one atom to another. B) Dipole moments result from the unequal distribution of electrons in a molecule. C) The electrons in a polar bond are found nearer to the more electronegative element. D) A molecule with very polar bonds can be nonpolar. E) Linear molecules cannot have a net dipole moment. 2. Atoms having greatly differing electronegativities are expected to form: A) no bonds B) polar covalent bonds C) nonpolar covalent bonds D) ionic bonds E) covalent bonds 3. Choose the compound with the most ionic bond. A) LiCl B) KF C) NaCl D) LiF E) KCl 4. Atoms with very similar electronegativity values are expected to form A) no bonds. B) covalent bonds. C) triple bonds. D) ionic bonds. E) none of these 5. Which of the following bonds is least polar? A) C—O B) H—C C) S—Cl D) Br—Br E) They are all nonpolar. 6. For the elements Rb, F, and O, the order of increasing electronegativity is: A) Rb < F < O B) Rb < O < F C) O < F < Rb D) F < Rb < O E) None of these 7. For the elements Cs, F, and Cl, the order of increasing electronegativity is: A) F < Cl < Cs B) Cs < Cl < F C) Cl < Cs < F D) F < Cs...
Words: 3943 - Pages: 16
...between an ion and a neutral polar molecule which possess a dipole moment. Polar molecules are dipoles; they have a positive end and a negative end. The positive ions are attracted to the negative end of a dipole, while negative ions are attracted to the positive end. An example of ion-dipole interaction is K+ ---H2O d. Dispersion forces (London forces): London forces are weak intermolecular forces that arise from temporary multi-pole interactive forces between molecules without permanent multi-pole moment. A good example of London forces is CH4 (methane). e. Van der Waals forces: Van der Waals force is the attractive or repulsive force between molecules (or between parts of the same molecule) other than those due to covalent bonding or electrostatic interaction of...
Words: 2850 - Pages: 12
...the transfer of electrons. _____________________________________________________________________________________ Introduction The atoms in a compound are held together by a chemical bond. There are two types of chemical bond: ionic and covalent bond. An ionic or electrovalent bond results from the electrostatic attraction between metal and non-metal atoms by the transfer of electrons. One example is the formation of bond between a sodium metal atom and a chlorine non-metal atom [1]. In contrast, covalent bond involves the sharing of valence electrons between non-metal atoms. A covalent bond becomes polar when there is unequal sharing of bonding electrons. This happens when the elements involved in the bond has a significant difference in their electronegativity, such as in hydrochloric acid, HCl. Equal distribution of bonding electrons leads to the formation of a non-polar covalent bond. This happens when there is small or no difference in electronegativity between the atoms in a bond. Chlorine gas, Cl2, has a non-polar covalent bond. Electrical conductivity, the flow of electric current, can be used as a basis for determining the type of chemical bond present in a compound. An ionic compound, when dissolved in an aqueous solution, conducts electricity because it contains...
Words: 761 - Pages: 4
...reactions, the properties of synthetic material, or the intricate life-sustaining processes of living cells, molecular shape is a crucial factor. 10.1 Depicting Molecules and Ions with Lewis Structures Lewis structures, also called electron-dot structures or electron-dot diagrams, are diagrams that show the bonding between atoms of a molecule, and the lone pairs of electrons that may exist in the molecule. A Lewis structure can be drawn for any covalently-bonded molecule, as well as coordination compounds. Using the Octet Rule to Write Lewis Structures The octet rule tells us that all atoms want eight valence electrons (except for hydrogen, which wants only two), so they can be like the nearest noble gas. Use the octet rule to figure out how many electrons each atom in the molecule should have, and add them up. The only weird element is boron - it wants six electrons. Lewis Structures for Molecules with Single Bonds The atoms share a pair of electrons, and that pair is referred to as a bonding pair. The pairs of electrons which do not participate in the bond have traditionally been called "lone pairs". A single bond can be represented by the two dots of the bonding pair, or by a single line which represents that pair. The single line representation for a bond is commonly used in drawing Lewis structures for molecules. · Hydrogen atoms form one bond. · Carbon atoms four bonds. · Nitrogen atoms form three bonds. · Oxygen atoms form two bonds...
Words: 2714 - Pages: 11
...Centre for Foundation Studies, UTAR CHAPTER 2 Chemical Bonding Chapter Scopes Bond energies, bond lengths & bond polarities Drawing Lewis structure and calculate the formal charge Forms of Chemical Bonds 1) Intramolecular bond – forces hold the atoms _______ a molecule • Ionic / Electrovalent Bond • Covalent Bond • Metallic Bond 2) Intermolecular bond – forces ________ the molecules • Hydrogen bonding • Van der Waals 3) Co-ordinate / Dative Bond FHSC1114 Physical Chemistry Chapter Scopes • • • • Electrovalent / ionic bonding Covalent bonding Co-ordinate / dative covalent bonding Intermolecular bonding (including hydrogen bonding, Van der Waals) • Metallic bonding • Electronegativity Chemical Bond • Chemical bond − the force of attraction that binds atoms together in a chemical compound • When atoms react to form chemical bonds, only the electrons in the ______ ___________ are involved Electrons In An Atom 2 groups of electrons: a) Valence electrons • outermost shell electrons • chemical properties • = group number in periodic table b) Core electrons • inner shell electrons • not involved in chemical behaviour 1 Centre for Foundation Studies, UTAR Valence & Core Electrons B (1s22s22p1) Core e- = [He] Bond & Lone Pairs Electrons • Valence electrons are distributed as shared (bond pairs) & unshared (lone pairs) Valence e- = 2s22p1 Core e- = [Ar]3d10 Valence e- = 4s24p5 Lewis Symbol & Lewis...
Words: 2123 - Pages: 9
...This study confirms that stronger bonds with conventional institutions, including family, religion, marriage, civic participation, and education, reduce the likelihood of subsequent NPDU at 28-30 years of age. Trajectories marked by constantly high levels of social bonds are associated with lower likelihood of NPDU, compared to other shapes of trajectories. After controlling for baseline NPDU and other covariates, we further confirmed that the effects of social bonding trajectories are not caused by endogeneity—the argument that people using drugs are less likely to hold a stable social bond. These evidences reinforce social control theory (Gottfredson & Hirschi, 1990; Hirschi, 1969) that a stable and strong relationship with religious institutions,...
Words: 345 - Pages: 2
...Centre for Foundation Studies, UTAR Topic Scopes TOPIC 2 Chemical Bonding • • • • • Electrovalent Covalent bonding Co-ordinate/dative covalent bonding Metallic bonding Intermolecular bonding (including hydrogen bonding, Van der Waals) • Electronegativity 2 Chemical Bond Topic Scopes Bond energies, bond lengths & bond polarities Drawing Lewis structure and calculate the formal charge • Chemical bond the force of attraction that binds atoms together in a chemical compound • When atoms react to form chemical bonds, only the electrons in the outermost / valence shell are involved 3 Forms of Chemical Bonds 1) ________molecular bond – forces hold the atoms within a molecule • Ionic / Electrovalent Bond • Covalent Bond • Metallic Bond 2) ________molecular bond – forces between the molecules • Hydrogen bonding • Van der Waals 3) Co-ordinate / Dative Bond 5 FHSC1114 Physical Chemistry 4 Electrons In An Atom 2 groups of electrons: a) Valence electrons • ____________ shell electrons • similar chemical properties • similar group number in periodic table b) Core electrons • ________ shell electrons • not involved in chemical behaviour 6 1 Centre for Foundation Studies, UTAR Valence & Core Electrons Bond & Lone Pairs Electrons • Valence electrons are distributed as shared (bond pairs) & unshared (lone pairs) B (1s22s22p1) Core e- = [He] Valence e- = 2s22p1 Cl H ...
Words: 2144 - Pages: 9
...SCH4U – The Chemistry of Covalent Bonding Date_____________________ Orbital Hybridization One of the most influential chemistry books ever written was The Nature of the Chemical Bond by Linus Pauling (1901-1994). Published in 1939, Pauling was awarded the Nobel Prize in 1954. Pauling received a second Nobel Prize for peace in 1962. Pauling made tremendous contributions to the field of chemistry, and was an outspoken activist against war and nuclear weapons. If you consider the energy level diagram for carbon it presents a problem to the VB theory. If bonds are formed between orbitals that contain unpaired electrons, how many bonds does it appear carbon can form? | | 2 | | 1 | | Since Carbon only has 4 different 4 valence electrons, according to the Aufbau principle, the 2s orbital is filled first, and then the 2p sub shell has 2 orbitals with unpaired electrons. This suggests that Carbon can only form 2 bonds. However Carbon is clearly able to form 4 bonds, as evidenced by any carbon compound (e.g. methane, CH4). Linus Pauling suggested that carbon is able to create four unpaired orbitals by promoting one electron from the 2s orbital to the empty 2pz orbital. This hybridizes the one 2s and three 2p orbitals together. This configuration is called ‘sp3’. Like s and p orbitals, the ‘shape’ of sp3 orbitals can be defined by a probability density map of electron location around the nucleus. The shape of a sp3 orbital looks like this: Since carbon...
Words: 1840 - Pages: 8
...Jacinta Houng Comparing the Solubility of Chemicals in Water “Water is known as the “universal solvent” because so many different substances dissolve in it and we rely on this for many of our daily needs.” Introduction: Water is known as the ‘universal solvent’ as it is capable of dissolving a variety of different substances and dissolves more substances than any other liquid. However the ability to be soluble depends on a substances polarity and bonding. This then contributes to the various ways that different types of chemicals interact in water. Solubility is crucial to every living thing on earth as water can carry along valuable chemicals, minerals, and nutrients necessary for survival. In fact Water covers 70% of the Earths surface and composes 55-70% of the human body. Water is an excellent solvent due to its chemical composition and physical attributes. According to USGS (http://water.usgs.gov/edu/qa-solvent.html ) Water molecules have a polar arrangement of the oxygen and hydrogen atoms—one side (hydrogen) has a positive electrical charge and the other side (oxygen) has a negative charge. A polar bond is a covalent bond between two atoms where the electrons forming the bond are unequally distributed. This causes the molecule to have a slight electrical dipole moment where one end is slightly positive and the other is slightly negative. "Like dissolves like" is an expression used by chemists to help them remember how solvents work. The expression refers to...
Words: 3033 - Pages: 13
