1. It include three branches

2. 1808 John Dalton suggested that all matter was made up of tiny spheres called them ATOMS 3. 1898 Joseph John Thomsonfound that atomscould sometimes ejecta far smaller negativeparticle which hecalled an ELECTRON 4. J.J. Thomson, measured mass/charge of e-(1906 Nobel Prize in Physics) 5. Eugene Goldstein (1850-1930) observed in 1886 thatin a cathode-ray tube therewere rays going in theopposite direction. Heconcluded they werepositively chargedparticles. Proton are positivelycharged subatomicparticles. Each proton has a massabout 1840 times that of anelectron. 6. In 1932 Englishphysicist JamesChadwick (1891-1974)confirmed theexistence of anothersubatomic particle. Neutrons aresubatomic particleswith no charge but amass nearly equal tothe proton. 7. 1910 Ernest Rutherford They fired Helium nuclei at a piece of gold foil which was only a few atoms thick.They found that while most of thehelium nuclei passed through thefoil, a small number were deflectedand, to their surprise, some heliumnuclei bounced straight back. 8. (1908 Nobel Prize in Chemistry)particle velocity ~ 1.4 x 107 m/s(~5% speed of light)1. atoms positive charge is concentrated in the nucleus2. proton (p) has opposite (+) charge of electron3. mass of p is 1840 x mass of e- (1.67 x 10-24 g) 9. Rutherfords Model ofthe Atomatomic radius ~ 100 pm = 1 x 10-10 mnuclear radius ~ 5 x 10-3 pm = 5 x 10-15 m 10. 1913 Niels Bohrstudied under Rutherford atthe Victoria University inManchester.Bohr refined Rutherfords ideaby adding that the electronswere in orbits. Rather likeplanets orbiting the sun. Witheach orbit only able to containa set number of electrons. 11. Subatomic Particles MassCharge ChargeParticle(g)(Coulombs) (units)Electron (e-) 9.1 x 10-28 -1.6 x 10-19 -1Proton (p) 1.67 x 10-24 +1.6 x 10-19 +1Neutron (n) 1.67 x 10-240 0 mass p = mass n = 1840 x mass e- 12. Nucleus - the central portion of the atom. Contains the protons and neutrons.Electron Cloud - area around the nucleus where electrons are found. Electrons are arranged within the electron cloud in energy levels (Energy levels are sometimes called shells or orbits). 13. Proton - positive charged particle found in the nucleus. Mass = 1 amu. (a.m.u - Atomic Mass Unit) p+1Neutron - particle with no charge. Found in the nucleus. Mass = 1 amu. nElectron - negative charged particle found within the electron cloud . Mass = 1/1836 amu.e-1 14. p+ 15. HELIUM ATOM Shellproton+N-+ -NelectronneutronWhat do these particles consist of? 16. Proton NeutronElectron Electron shell / Electron cloudNucleusThe Atom 17. Particle ChargeMassproton + ve charge1neutronNo charge1electron -ve charge nil 18. ProtonMade ofd3 Quarks1 up2 downud 19. NeutronMade of3 Quarks u2 up1 down d u 20. ATOMIC STRUCTURE4HeAtomic number the number of protons in an atom2Atomic massthe number of protons andneutrons in an atomnumber of electrons = number of protons 21. ATOMIC STRUCTUREElectrons are arranged in Energy Levels orShells around the nucleus of an atom. first shell a maximum of 2 electrons second shella maximum of 8 electrons third shell a maximum of 8 electrons 22. Proton Neutron ElectronS orbitalP orbital 23. ATOMIC STRUCTUREThere are two ways to represent the atomicstructure of an element or compound; 1. Electronic Configuration 2.Dot & Cross Diagrams 24. ELECTRONIC CONFIGURATIONWith electronic configuration elements are representednumerically by the number of electrons in their shellsand number of shells. For example; Nitrogenconfiguration = 2,514 N2 in 1st shell 2 + 5 = 75 in 2nd shell 7 25. ELECTRONIC CONFIGURATIONWrite the electronic configuration for the followingelements;40 2316a) Ca b) Na c) O 118202,8,8,22,8,1 2,63528 11d) Cl e) Si f) B 51714 2,8,7 2,8,4 2,3 26. DOT & CROSS DIAGRAMSWith Dot & Cross diagrams elements and compoundsare represented by Dots or Crosses to show electrons,and circles to show the shells. For example;X NNitrogen X XN X X14 7XX 27. DOT & CROSS DIAGRAMSDraw the Dot & Cross diagrams for the followingelements; 16 35 Xa) Ob)Cl 17 XX8XXX XXX X X Cl X X XX O X X XXX XX XXX 28. SUMMARY1. The Atomic Number of an atom = number of protons in the nucleus.2. The Atomic Mass of an atom = number of Protons + Neutrons in the nucleus.3. The number of Protons = Number of Electrons.4. Electrons orbit the nucleus in shells.5. Each shell can only carry a set number of electrons. 29. Introduction to thePeriodic Table Atomic Number Symbol Atomic Weight Element Compound Mixture 30. I am Dmitri Mendeleev! I made the PERIODIC TABLE ! 31. Noble Gas HalogenGroupPeriodAlkali Earth Metal Alkali Metal 32. that make up everything in the universe 33. METALSNONMETALS METALLOIDSA substance or mixtureAn element that doesAn element having boththat has a characteristic not exhibit the metallic andluster or shine, is characteristics of anonmetallic properties.generally a goodmetal; they are They are usually goodconductor of heat & generally solids or gases semiconductorselectricity, & is and are usually hard,malleable & ductile.brittle substances.Except for mercury, the Bromine is the onlymetallic elements are liquid nonmetal.solids at roomtemperature (~20 C) 34. Which pair of elements isMOST similar?Ca and FNa and ClNe and ArLi and H 35. What is the smallest particle ofthe element gold (Au) that canstill be classified as gold?atommoleculeneutronproton 36. All plant and animal life on Earthcontains what element?sulfurcarbonsiliconaluminum 37. What is the PERIODIC TABLE?o Shows all known elements in the universe.o Organizes the elements by chemical properties. 38. How do you read thePERIODIC TABLE? 39. What is the ATOMIC NUMBER? o The number of protons found in the nucleus of an atomOr o The number of electrons surrounding the nucleus of an atom. 40. Atomic NumberThe number of Protonsin an atom.H +111.008Hydrogen 41. What is the SYMBOL?o An abbreviation of the element name. 42. What is the ATOMIC WEIGHT?o The number of protons and neutrons in the nucleus of an atom. 43. How do I find the number of protons,electrons, and neutrons in an elementusing the periodic table?o # of PROTONS = ATOMIC NUMBERo # of ELECTRONS = ATOMIC NUMBERo # of NEUTRONS = ATOMIC _ ATOMIC WEIGHT NUMBER 44. What is an ELEMENT?o A substance composed of a single kind of atom.o Cannot be broken down into another substance by chemical or physical means. 45. What is a COMPOUND?o A substance in which two or more different elements are CHEMICALLY bonded together. 46. What is a MIXTURE?o Two or more substances that are mixed together but are NOT chemically bonded. 47. Element, Compound or Mixture? 48. Element, Compound or Mixture? 49. Element, Compound or Mixture? 50. Element, Compound or Mixture? 51. Element, Compound or Mixture? 52. Element, Compound or Mixture? 53. Atomic number (Z) = number of protons in nucleusMass number (A)=number of protons + number of neutron =atomic number (Z) + number of neutronsIsotopes are atoms of the same element (X) withdifferent numbers of neutrons in the nucleusMass NumberA ZXElement Symbol Atomic Number1231H 1H (D) 1H (T) 23523892 U 92 U 54. Atomic Symbols Show the mass number and atomic number Give the symbol of the elementsymbol maas numberAtomicnumber 55. Isotopes are: atoms of the sameelement which have different massnumbers and same atomic no. due todifferent numbers of neutrons in eachnucleus.Most elements exist as a mixture ofisotopes, e.g. chlorine has 2 isotopes 35 37Cl Cl 17 17 56. Do You Understand Isotopes?How many protons, neutrons, and electrons are in 146 C?6 protons, 8 (14 - 6) neutrons, 6 electronsHow many protons, neutrons, and electrons are in 11 ?6 C 6 protons, 5 (11 - 6) neutrons, 6 electrons 57. Isotopes1H 2H 3H 58. Isotopes12C13C6 protons6 protons6 Neutrons 7 Neutrons 59. A molecule is an aggregate of two or moreatoms in a definite arrangement held togetherby chemical bonds H2 H2O NH3 CH4A diatomic molecule contains only two atomsA polyatomic molecule contains more than two atoms 60. When an atom lose or gain electron ion areformed. An ion is an atom, or group of atoms,that has a net positive or negative charge.cation ion with a positive chargeIf a neutral atom loses one or more electronsit becomes a cation.Na11 protons11 protonsNa+11 electrons10 electronsanion ion with a negative chargeIf a neutral atom gains one or more electronsit becomes an anion. 17 protonsCl17 protonsCl- 18 electrons17 electrons 61. +Cationan ion with a positive charge.Anion - Aan ion with a Negative charge.ION 62. A monatomic ion containsonly one atomA polyatomic ion contains more thanone atom 63. Do You Understand Ions?How many protons and electrons are in 27 3+ 13 Al ?13 protons, 10 (13 3) electronsHow many protons and electrons are in782-34 Se ?34 protons, 36 (34 + 2) electrons 64. Hydrogen 65. Hydrogen ionH -1 66. Lithium 67. Li Li +12211 68. Beryllium 69. Chart of Cat ions- H+ Hydrogen ion Li+, Na+, k+, Rb+, Cs+ Alkali metal ion( Li + -Lithium, Na+ -Sodium, k + -Potassium, Rb+ -Rubidium, Cs+ -Cesium) NH4+ Ammonium ion Ag+ Silver ion 70. Be+2,Mg+2,Ca+2,Sr+2,Ba+2 Alkalineearth metal ion(Be+2-Beryllium,Mg+2-Magnesium,Ca+2 -Calcium, Sr+2 -StrontiumBa +2 -Barium)Cu+2 Cupric ionFe +2 Ferous ionZn+2 Zinc ion 71. Fe+3 Ferric ionAl+3 Aluminium ionCr +3 Chromium ionBi+3 Bismuth ionAu +3 Auric ionPb+4 Plumbic ionSi +4 Silicon ion 72. Chart of Anions F-1 Fluoride ion Cl-1 Chloride ion Br-1 Bromide ion I -1 Iodide ionHalide ion 73. H - Hydrideion,OH - HydroxideONO- Nitrite ion,NO2- Nitro ionNO3 - Nitrate ion,CN- Cyanide ionHCO3- Bicarbonate ionCH3COO- Acetate ionMnO4- Permagnate ionHSO4- Bisulphate ionNC - Isocyanide ionO2- Superoxide ion 74. O -2 -Oxide ion, O2-2-Peroxide ionSO3-2-Sulphite ion,S-2-Sulphide ionCO3 -2 Carbonate ionSO4-2 Sulphate ionSiO3-2 Silicate ionMnO4 -2 Magnate ionC2O4-2 Oxalate ionCr2O7 -2 Dichromate ion 75. [Fe(CN)6-3]Ferricyanide ionN-3 Nitrite ionPO4-3 Phosphate ionP -3 Poshpide ionBO4 -3 Borate ion[Fe(CN)6-4]Ferrocyanide ionC -4 Carbide ion 76. An Acid can be defined as a substance thatyields hydrogen ions (H+) when dissolved inwater. They are Sour in taste.For exampleH2SO4 Sulphuric acidH2CO3 Carbonic acidHNO3 Nitric acidH2PO3 Phosphoric acidHCl Hydrochloric acid (H +Cl -)C6H8O7 Citric acidCH COOH Acetic acid 77. Acid 78. A Base can be defined as a substance thatyields hydroxide ions (OH-) when dissolvedin water . They are Bitter in taste. + - 2.7 79. Base 80. Acid-Base Neutralization Reactions When an acid reacts with a base to yieldwater and a salt. Acid= compounds that produce H+ ionswhen dissolved in water Base= compounds that produce OH- ionswhen dissolved in water. Neutralization involves H+ and OH- ionsand always yields water (H O) and a salt. 81. pH paperRed Litmus paperBlue Litmus paper 82. A Salt can be defined as a substance that notyields hydroxide ions (OH-) and hydrogenions (H+) when dissolved in water . They areNeutral or salty in taste.+ - 83. SALT - a Cation and an Anion heldtogether by an ionic bond. 84. Learning CheckState the number of protons for atoms of each of thefollowing:A. Nitrogen1) 5 protons 2) 7 protons 3) 14 protonsB. Sulphur1) 32 protons 2) 16 protons 3) 6 protonsC. zirconium1) 40 protons2) 40.1 protons 3) 39 protons 85. SolutionState the number of protons for atoms of each of thefollowing:A. Nitrogen 2) 7 protonsB. Sulfur 2) 16 protonsC. zirconium 1) 40 protons 86. Subatomic Particles in Some AtomsO 16 P 31 Zn 658 15 308 p+15 p+ 30 p+8n16 n35 n8 e-15 e- 30 e-LecturePLUS Timberlake102 87. Learning Check Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms.6C126C13 6 C14#p _______ ______________#n _______ ______________#e _______ _______ _______ 88. Solution 6 C12 6 C136 C14#p6 66#n6 78#e6 66 89. Learning CheckAn atom of zinc has a mass number of 65.A. Number of protons in the zinc atom1) 302) 35 3) 65B. Number of neutrons in the zinc atom1) 302) 35 3) 65C. What is the mass number of a zinc isotope with 37 neutrons? 1) 372) 653) 67 90. SolutionAn atom of zinc has a mass number of 65.A. Number of protons in the zinc atom1) 30B. Number of neutrons in the zinc atom2) 35C. What is the mass number of a zinc isotope with 37 neutrons?3) 67LecturePLUS Timberlake 106 91. Learning CheckWrite the atomic symbols for atoms with thefollowing:A. 8 p+, 8 n, 8 e-___________B. 17p+, 20n, 17e- ___________C. 47p+, 60 n, 47 e-___________ LecturePLUS Timberlake107 92. SolutionA. 8 p+, 8 n, 8 e-8O16B. 17p+, 20n, 17e-17Cl37 107C. 47p+, 60 n, 47 e-47Ag LecturePLUS Timberlake 108 93. Biologists follow universally acceptedprinciples to provide scientific names toknown organisms. Each name has twocomponents the Generic name and thespecific epithet. This system of providing aname with two components is called Binomialnomenclature. This naming system given byCarolus Linnaeus is being practised bybiologists all over the world. 94. The scientific name of mango is written as Mangiferaindica. Let us see how it is a binomial name. In thisname Mangifera represents the genus while indica, isa particular species, or a specific epithet. Otheruniversal rules of nomenclature are as follows:1. Biological names are generally in Latin and written initalics.They are Latinised or derived fromLatinirrespective of their origin.2. The first word in a biological name represents thegenus while the second component denotes the specificepithet.3. Both the words in a biological name, when handwritten,are separately underlined, or printed in italics to indicatetheir Latin origin.4. The first word denoting the genus starts with a capitalletter while the specific epithet starts with a small letter.It can be illustrated with the example of Mangifera indica. 95. MatterSince the atom istoo small to be seeneven with the mostpowerfulmicroscopes,scientists rely upon Believe it or not this is a microscope. Even with themodels to help us to worlds best microscopes we cannot clearly see theunderstand the structure or behavior of the atom.atom. 96. MatterMatter = any materialsubstance with Mass& Volume 97. Matter comes in 3 phases 98. SolidDefinite Shape Definite Volume 99. Solid 100. LiquidIndefinite Shape takes the shape ofthe container Definite Volume 101. Liquid 102. GasIndefinite Shape takes the shape ofthe containerIndefinite Volume can expand and becompressed 103. Gas 104. Boiling CondensationFreezingMelting 105. PlasmaSuperheated GasWhen atoms are so hot,they lose ALLof theirelectrons. 106. Solid Liquid Gas PlasmaMade ofAtomsHoldsits shapeAtoms moveeach other 107. Cell Structure& Functionhttp://koning.ecsu.ctstateu.edu/cell/cell.html 108. Cell Theory All living things are made up of cells. Cells are the smallest working units of allliving things. All cells come from preexisting cellsthrough cell division. 109. Definition of CellThe fundamental and structural unit of life.A cell is the smallest unit that iscapable of performing life functions. 110. Examples of Cells Amoeba ProteusPlant StemBacteria Red Blood Cell Nerve Cell 111. Two Types of CellsProkaryoticEukaryotic 112. Prokaryotic Do not have structures surrounded by membranes Few internal structures One-celled organisms, Bacteriahttp://library.thinkquest.org/C004535/prokaryotic_cells.html 113. Eukaryotic Contain organelles surrounded by membranes Most living organisms PlantAnimalhttp://library.thinkquest.org/C004535/eukaryotic_cells.html 114. Typical Animal Cellhttp://web.jjay.cuny.edu/~acarpi/NSC/images/cell.gif 115. Typical Plant Cellhttp://waynesword.palomar.edu/images/plant3.gif 116. A Sense of Scale and Abundance Bacteria on the Head of a Pin 117. An Idealized Animal Cell 118. Conversion Factors and Unit Cancellation 119. A physical quantity must include:Number + Unit 120. Calculation Corner: Unit Conversion 1 foot = 12 inches 121. Calculation Corner: Unit Conversion 1 foot = 12 inches 1 foot= 1 12 inches 122. Calculation Corner: Unit Conversion 1 foot = 12 inches 1 foot= 1 12 inches 12 inches= 1 1 foot 123. Calculation Corner: Unit Conversion 1 foot12 inches 12 inches 1 footConversion factors 124. Calculation Corner: Unit Conversion1 foot12 inches12 inches 1 foot Conversion factors12 inches( 3 feet )(1 foot ) = 36 inches 125. How many cm are in 1.32 meters?equality: 1 m = 100 cm (or 0.01 m = 1 cm)applicable conversion factors: ______ 1m or100 cm______ 100 cm 1m X cm = 1.32 m( 100 cm______1m ) = 132 cmWe use the idea of unit cancellationto decide upon which one of the twoconversion factors we choose. 126. How many meters is 8.72 cm?equality: 1 m = 100 cmapplicable conversion factors: ______ 1m or100 cm______ 100 cm 1m X m = 8.72 cm( 1m______100 cm ) = 0.0872 mAgain, the units must cancel. 127. How many feet is 39.37 inches? equality: 1 ft = 12 in applicable conversion factors:______1 ftor______ 12 in 12 in1 ft X ft = 39.37 in( )____ 1 ft12 in=3.28 ftAgain, the units must cancel. 128. How many kilometers is15,000 decimeters?X km = 15,000 dm ( )(1m ____ 10 dm1 km ______ 1,000 m ) = 1.5 km 129. How many seconds is 4.38 days? X s = 4.38 d( )( 24 h ____1d 60 min _____ 1h )( )60 s ____ 1 min = 378,432 sIf we are accounting for significantfigures, we would change this to3.78 x 105 s 130. Simple MathwithConversion Factors 131. Example ProblemMeasured dimensions of a rectangle: length (L) = 9.70 cm width (W) = 4.25 cmFind area of rectangle.A=L.WL= (9.70 cm)(4.25 cm) 2.= 41.2 cm cmW 132. Convert 41.2 cm2 to m2.X m2 = 41.2 cm2( 1m )______ = 0.412 m2100 cmWRONG! = 0.412 cm.mRecall that 41.2 cm2 = 41.2 cm.cmX m2 = 41.2 cm.cm( 1m______100 cm)( 1m ______ 100 cm )= 0.00412 m2X m2 = 41.2 cm2( 1m______100 cm ) 2 =0.00412 m2 133. Convert 41.2 cm2 to mm2.Recall that 41.2 cm2 = 41.2 cm.cmX mm2 = 41.2 cm.cm (10 mm_____ 1 cm)(10 mm_____ 1 cm)= 4,120 mm22X mm2 = 41.2 cm2 ( 10 mm _____ 1 cm) =4,120 mm2 134. Measured dimensions of a rectangular solid:Length = 15.2 cm Width = 3.7 cm Height = 8.6 cm HFind volume of solid.W LV=L.W.H = (15.2 cm)(3.7 cm)(8.6 cm)3 = 480 cm 135. Convert to m3. cm.cm.cm 21m( X m3 = 480 cm 3 _____ 100 cm)( 1m_____100 cm )(1m_____ 100 cm) =or3X m3 = 480 cm3 ( 1m_____ 100 cm) = 0.000480 m3orX m3 = 480 cm3 ( _________1m1000000 cm3)3= 4.80 x 10-4 m3 136. Convert to m3...Measured dimensions of a rectangular solid:Length = 15.2 cm0.152 m Width = 3.7 cm 0.037 m Height = 8.6 cm0.086 m HFind volume of solid. WLV=L.W.H = (0.152 m)(0.037 m)(0.086 m) = 0.000480 m 3 137. Convert to mm3. 138. By what factor do mm and cm differ?101 cm = 10 mmBy what factor do mm2 and cm2 differ? 100(1 cm)2= 100 mm2 2 1 cm2 = (10 mm)By what factor do mm3 and cm3 differ? 1,000 1 cm3 = (10 mm3(1 cm)3= 1000mm)3 139. 1 2 3 4nucleus 140. ELECTRONIC CONFIGURATIONnl Electrons are arranged in Energy Levels or Shellsthe arrangement of the electron in the atom. around the nucleus of an atom. x SubMain energyno.ofelectronslevel energy levelff = 7 x 2 = 14 1 2 p3 d 4 dp pd = 5 x 2 = 10ss snucleus sp=3 x2=6 s=1 x2=22e- 8e-32e-Atomic orbital 18e- 1 Atomic orbital = 2 e- 141. Given the27 Complete the Element13 missing data.Location in theNumber of atomp+1)4)e-2)5)n03)6) 142. Multiple choice7. The maximum number of electrons that can becontained in an atomic orbital is a. 2 b. 8 c. 68. The particles in an atomic nucleus are collectivelyknown as _______a. Nucleusb. Nucleons c. Nucleolus 143. 9. There are __ orbitals in the 3rd energy level. a. 10b. 16 c. 310. The total number of electrons in the 4th energy level a. 36b. 28 c. 32 144. Given the 27Complete theElement 13missing data. Location in theNumber ofatomp+1) 4) Inside the 13nucleuse-2) 135)Electron cloud n0 3) 146) Inside the nucleus 145. Multiple choice7. The maximum number of electrons that can becontained in an atomic orbital is a. 2 b. 8 c. 68. The particles in an atomic nucleus are collectivelyknown as _______a. Nucleusb. Nucleons c. Nucleolus 146. 9. There are a total of __ orbitals in the 3rd energy level. a. 10b. 16 c. 310. The total number of electrons in the 4th energy level a. 36b. 28c. 32