Chem 103, Section F0F Lecture 10 - Chemical Bonding And .
Lecture 10 - Chemical Bonding and IonicCompoundsChem 103, Section F0FUnit III - Combining Atoms to MakeCompounds, Part I: Ionic CompoundsLecture 10 Reading in Silberberg- The atomic properties and chemical bonds Ionic bonding. Naming ionic compounds and representingthem with chemical formulasChapter 9, Section 1 Atomic Properties and Chemical BondsChapter 2, Section 7 Compounds: Introduction to BondingChapter 9, Section 2 The Ionic Bonding ModelChapter 2, Section 8 (pp. 64-70) Ionic Compounds: Formulas andNames2Lecture 10 - Atomic Properties and ChemicalBondsLecture 10 - IntroductionWe will look first at chemical bonding With a focus on ionic bonds and ionic compounds.Nearly all naturally occurring substances consist of atoms orions bonded to other atoms or ions. There are very few elements that occur uncombined inWe will then look at the source of energy needed to formionic compounds.nature Most exist combined with other elements to formcompounds.We will also look into how chemical formulas are used torepresent compounds And the systematic way of naming ionic compounds.34Lecture 10 - Atomic Properties and ChemicalBondsLecture 10 - Atomic Properties and ChemicalBondsChemical bonding allows atoms to lower their energy.Ionic bonding Occurs when metal atoms transfer valance electrons tononmetal atoms.- The resulting attraction of the opposingTypes of chemical bonding include: Ionic bonding (metals with nonmetals) Covalent bonding (nonmetals with nonmetals) Metallic bonding (metals with metals)5charges leads to the formation of ionicsolids.6
Lecture 10 - Atomic Properties and ChemicalBondsLecture 10 - QuestionIonic bonding For monatomic ions- The metals lose andWhat monatomic ions do barium (Z 56) and sulfur (Z 16)form?nonmetals gain that numberof electrons that will makethem isolectronic with thenearest noble gas.78Lecture 10 - Atomic Properties and ChemicalBondsLecture 10 - Atomic Properties and ChemicalBondsCovalent bonding Occurs most commonly between nonmetals.- In covalent molecules, the atoms shareCovalent bonding We will come back later to look a covalent molecules However, when considering ionic compounds we willencounter polyatomic ions- These are a group of atoms that are covalently bonded to onepairs of valence electrons.another, but have a net positive or negative charge.!They therefore also participate in ionic bonding.2-OCOOCarbonate Ion (CO32-910Lecture 10 - Atomic Properties and ChemicalBondsLecture 10 - QuestionMetallic bonding Occurs when many metal atoms pool their valenceelectrons.- This pool of electrons holds theAre molecules of MgBr2 present in a sample of MgBr2?Explainmetal atoms together.1112
Lecture 10 - QuestionLecture 10 - QuestionAre ions present in a sample of P4O6?ExplainPredict the type of bonding, ionic, covalent, or metallic, youwould predict for each of the following:A) CsF(s)B) H2S(g)C) N2O(g)D) CaO(s)E)F)13BrO2(g)Cr(s)14Lecture 10 - Atomic Properties and ChemicalBondsLecture 10 - Atomic Properties and ChemicalBondsLewis dot structures are used to represent the valenceelectrons for an atom They are usefull for illustrating the formation of both ionicand covalent compounds.Lewis dot structures are used to represent the valenceelectrons for an atom They are useful for illustrating the formation of both ionicand covalent bonded molecules.Forming lithium fluoride from lithium metal and fluorine gas1516Lecture 10 - QuestionLecture 10 - QuestionDraw a Lewis electron-dot symbol forA) BaB) KrC) SeD) PE) Rb17Give the group number an general elecron configuration ofan element with each electron-dot symbolA) XB) XC) XD) X18
Lecture 10 - QuestionLecture 10 - Ionic BondingIdentify the main group to which X belongs in each ioniccompound formula:A) XPO4B) MgX2C) Na3XD) Al2X3Ion formation by itself requires energy The negative Electron Affinities (EA’s) of the nonmetals arenot sufficient to compensate for the positive IonizationEnergies (IE’s) of the metals.IE’sEA’s20Lecture 10 - Ionic BondingLecture 10 - Ionic BondingIon formation by itself requires energy For the formation of lithium fluoride- IE1 (lithium) EA1 (fluoride) 520 - 328 192 kJ/molIon formation by itself requires energy The required energy for forming ionic compounds comesfrom the lattice energy.- The lattice energy is the energy absorbed when an ionic solidseparates into gaseous ions.!It is very large and is the major reason that ionic solids exist.- The lattice energy depends on ionic size and charge and can becalculated using Hess’s Law in the Born-Haber cycle. Hess’s Law - the enthalpy or energy change of an overallprocess is the sum of the enthalpy or energy changes of itsindividual steps.IE’sEA’s2122Lecture 10 - Ionic BondingLecture 10 - Ionic BondingIon formation by itself requires energy The required energy for forming ionic compounds comesfrom the lattice energy.- The ionic interactions can be described by Coulomb’s lawEelectrostatic 2324charge A ! charge Bdistance
Lecture 10 - Ionic BondingLecture 10 - Ionic BondingThe ionic bonding model pictures oppositely charged ionsheld together by strong electrostatic interactions. This model explains why ionic solids tend to fracture whenstruck.The smallerthe ions, thestronger theinteraction.As layer slip past onanother,charge repulsion leads toa fracture2526Lecture 10 - Ionic BondingLecture 10 - Ionic BondingThe ionic bonding model pictures oppositely charged ionsheld together by strong electrostatic interactions. This model explains whythey conduct electricityonly when melted ordissolved.2729The ionic bonding model pictures oppositely charged ionsheld together by strong electrostatic interactions. Gaseous ion pairsrequire very hightemperatures.28Lecture 10 - Chemical Formulas and Namesfor Ionic CompoundsLecture 10 - Chemical Formulas and Namesfor Ionic CompoundsChemical formulas describe the simplest atom ratio(empirical formula) the actual atom number (molecular formula) The atom arrangement (structural formula) of one unit of acompound.Ionic compounds are named by listing the cation first followedby the anion. For metal cations that can have more than one chargestate, Roman numerals are used to indicate the charge. Monatomic anions add the -ide suffix to the root name ofthe atom. Oxoanions (polyatomic) use suffixes and sometimeprefixes to indicate the relative number oxygen atoms. Some ionic compounds form crystal lattices which containwater molecules.- These crystals are called hydrates.- The number of waters is included in the chemical formula and in theType eMgCl2(formula ucturalFormulaH2O2H-O-O-Hname. Acid names are based on the anion names.30
Lecture 10 - Chemical Formulas and Namesfor Ionic CompoundsLecture 10 - Chemical Formulas and Namesfor Ionic CompoundsIonic compounds are named by listing the cation first followedby the anion. For metal cations fromedfrom Groups 1A, 2A and3A, the charge isunderstood.Ionic compounds are named by listing the cation first followedby the anion. For metal cations that can have more than one chargestate, Roman numerals are used to indicate the charge.3132Lecture 10 - Chemical Formulas and Namesfor Ionic CompoundsLecture 10 - Chemical Formulas and Namesfor Ionic CompoundsIonic compounds are named by listing the cation first followedby the anion. Monatomic anions add the-ide suffix to the root nameof the atom.Ionic compounds are named by listing the cation first followedby the anion. Oxoanions (polyatomic) use suffixes and sometimeprefixes to indicate the relative number oxygen atoms.3334Lecture 10 - Chemical Formulas and Namesfor Ionic CompoundsLecture 10 - QuestionIonic compounds are named by listing the cation first followedby the anion. Oxoanions (polyatomic) use suffixes and sometime prefixesto indicate the relative number oxygen atoms. The charge on a polyatomic ion is less straight forward topredict.- Oxoanions formed from the same non metal tend to have the sameGive the name and formula of the compound formed from thefollowing elementsA) 12L and 9MB) 17L and 38Mcharge!!!35nitrite (NO2-), nitrate (NO3-)sulfite (SO32-), sulfate (SO42-)hypochlorite (ClO-), chlorite (ClO2-), chlorate (ClO3-), perchlorate (ClO4-)36
Lecture 10 - QuestionUnit III - Up NextGive the systematic names for the following compoundsA) CuSO4 5H2OB) CoOC) Ba3(PO4)2D)E)Unit IV - Chemical Bookkeeping: Stoichiometry The concept of a mole Determining the chemical formulas for a compound Writing and balancing a chemical equation for a chemicalreactionPb(NO3)4Pb(NO3)23738The End
-Chapter 9, Section 1 Atomic Properties and Chemical Bonds-Chapter 2, Section 7 Compounds: Introduction to Bonding-Chapter 9, Section 2 The Ionic Bonding Model-Chapter 2, Section 8 (pp. 64-70) Ionic Compounds: Formulas and Names 2 Lecture 10 - Introduction We will look first at chemical bonding With a focus on ionic bonds and ionic compounds.
Chem 103, Section F0F Unit VI - Compounds Part II: Covalent Compounds Lecture 15 The formation of covalent bonds Naming binary covalent and organic compounds The covalent bonding model Lecture 15 - Covalent Bonding Reading in Silberberg Chapter 2, Section 7 (pp. 62-64)-The Formation of Covalent Compounds Chapter 2, Section 8 (pp. 70-72)-Compounds, Formulas and Names
Introduction of Chemical Reaction Engineering Introduction about Chemical Engineering 0:31:15 0:31:09. Lecture 14 Lecture 15 Lecture 16 Lecture 17 Lecture 18 Lecture 19 Lecture 20 Lecture 21 Lecture 22 Lecture 23 Lecture 24 Lecture 25 Lecture 26 Lecture 27 Lecture 28 Lecture
3. Most students are required to take Chem 103, General Chemistry Laboratory, concurrently with Chem 102. This 1 hour lab course provides active demonstration of principles covered in Chem 102B/C and introduces experimental skills. eference the R Chemistry 103 Experiments book for details concerning Chem 103.Chem 103 starts the week of .
UIUC Course Proficiency Credit Hours Earned UIUC Course Placement Chemistry 3 CHEM 102 (lecture only) 3 CHEM lab 103; CHEM 104-105; consult with advisor 4 or 5 CHEM 102 (lecture only) CHEM 104 (lecture only) 3
CHEM 103: General Chemistry- Fall 2010 University of Wisconsin-Eau Claire CHEM 103 course and its objective ‘Chemistry’ is the study of properties and transformations of matter. The main objective of CHEM 103 is to help you in developing a picture of matter and their properties at the atomic and molecular levels. Topics of the CHEM 103 .
CHEM 350B Topics in Chemistry 7.5 454.95 CHEM 351 Chemicals Big and Small: Nano- 15 909.90 CHEM 352 Advanced Concepts in Chemistry 15 909.90 CHEM 352A Advanced Concepts in Chemistry 7.5 454.95 CHEM 352B Advanced Concepts in Chemistry 7.5 454.95 CHEM 360 Contemporary Green Chemistry 15 909.90 CHEM 380 Materials Chemistry 15 909.90
CHEM 31X. Chemical Principles 4 CHEM 33. Structure and Reactivity 4 CHEM 35. Organic Monofunctional Compounds 4 CHEM 36. Organic Chemistry Laboratory I 3 MATH 41, 42, 51. Calculus, Linear Equations 5 5 5 SECOND YEAR CHEM 130. Organic Chemistry Laboratory II 4 CHEM 131. Organic Polyfunctional Compounds y3 CHEM 134.
MPhys Astrophysics with a Year Abroad (2021-22) This specification provides a concise summary of the main features of the programme and the learning outcomes that a typical student might reasonably be expected to achieve and demonstrate if s/he takes full advantage of the learning opportunities that are provided. Awarding Institution University of Southampton Teaching Institution University of .
