1. Atoms, Ions and Molecules The Building Blocks of Matter Chapter 2

3. Chapter Outline 2.1The Rutherford Model of Atomic Structure 2.2Nuclides and Their Symbols 2.3Navigating the Periodic Table 2.4The Masses of Atoms, Ions, and Molecules 2.5Moles and Molar Mass 2.6Making Elements 2.7Artificial Nuclides

4. Experiments in Atomic Structure J. J. Thompson (1906 Nobel Prize in Physics) - cathode ray tube experiments; discovery of the electron; measurement of the charge-to-mass ratio. Robert Millikan (1923 Nobel Prize in Physics) - oil-drop experiments; measured the mass of the electron, therefore calculate the charge Ernest Rutherford (1908 Nobel Prize in Physics) - gold-foil experiments; the nuclear atom James Chadwick (1935 Nobel Prize in Physics) - discovery of the neutron

5. J.J. Thomson Cathode Ray Tube Experiments - Electrons

6. Results of “Cathode Ray” Experiments Travel in straight lines invisible independent of cathode composition bend in a magnetic field like a negatively-charged particle would charge/mass = -1.76 x 10 8 C/g

7. Thompson’s “Plum Pudding” Model of the Atom electrons distributed throughout a diffuse, positively charged sphere.

8. Robert Millikan’s oil drop Experiment - measured the mass of the electron

9. Millikan’s Results The air molecules in the chamber were ionized by a beam of X-rays, producing electrons and positively-charged fragments Fine mist of oil introduced into chamber; electrons adhere to the droplets Negatively-charged droplets settle to bottom of chamber under influence of gravity Charged repeller plates adjusted until droplets were suspended in mid-air From the physics and knowledge of the size of the gravitational and electrostatic forces, the charge on each droplet could be calculated Discovered that each droplet was a whole-number multiple of 1.60 X 10 -19 C, so the mass = 9.11 X 10 -28 g

10. Radioactivity and the Nuclear Atom Spontaneous emission of particles and/or radiation from a decaying, unstable nucleus  -particles =  -particles =  -rays =

12. Ernest Rutherford - the nuclear atom

13. Rutherford's Observations 1.the majority of particles penetrated undeflected 2.some particles were deflected at small angles 3.occasionally  -particles scattered back at large angles b) Expected results from “plum pudding” model. c) Actual results.

14. Rutherford’s Conclusions The atom is mainly empty space because most of the  -particles passed through undeflected The nucleus is very dense and positively charged because some of the  -particles were repulsed and deflected Electrons occupy the space around the nucleus The atom is electrically neutral

15. atomic radius ~ 100 pm = 1 x 10 -10 m nuclear radius ~ 5 x 10 -3 pm = 5 x 10 -15 m Rutherford’s Model of the Atom If the nucleus was the size of an orange, then the radius of the atom would be 2.5 miles

16. mass p  mass n = 1840 x mass e -

17. Chapter Outline 2.1The Rutherford Model of Atomic Structure 2.2Nuclides and Their Symbols 2.3Navigating the Periodic Table 2.4The Masses of Atoms, Ions, and Molecules 2.5Moles and Molar Mass 2.6Making Elements 2.7Artificial Nuclides

18. Atomic Mass Units Atomic Mass Units (amu) Comprise a relative scale to express the masses of atoms and subatomic particles. Scale is based on the mass of 1 atom of carbon: » 6 protons + 6 neutrons = 12 amu. 1 amu = 1 Dalton (Da)

19. Isotopes: Experimental Evidence

20. Atomic number (Z) = number of protons in nucleus Mass number (A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons Isotopes (nuclides) are atoms of the same element (X) with different numbers of neutrons in the nucleus X A Z H 1 1 H (D) 2 1 H (T) 3 1 U 235 92 U 238 92 Mass Number Atomic Number Element Symbol

21. Use the format A X to write the symbol for the nuclides having 28 protons and 31 neutrons. Practice: Isotopic Symbols Collect and Organize: Analyze: Solve: Think about It:

22. Complete the missing information in the table. Practice: Identifying Atoms and Ions Collect and Organize: Analyze: Solve: Think about It:

23. Chapter Outline 2.1The Rutherford Model of Atomic Structure 2.2Nuclides and Their Symbols 2.3Navigating the Periodic Table 2.4The Masses of Atoms, Ions, and Molecules 2.5Moles and Molar Mass 2.6Making Elements 2.7Artificial Nuclides

24. Mendeleev’s Periodic Table Dmitrii Mendeleev (1872): Ordered elements by atomic mass. Arranged elements in columns based on similar chemical and physical properties. Left open spaces in the table for elements not yet discovered. The Periodic Table of the Elements

25. The Modern Periodic Table Also based on a classification of elements in terms of their physical and chemical properties. Horizontal rows: called periods (1 → 7). Columns: contain elements of the same family or group (1 →18). Several groups have names as well as numbers.

26. Navigating the Modern Periodic Table – Groups and Families

28. Groups of Elements (cont.)

29. These 7 elements occur naturally as diatomics (memorize) - H 2 N 2 F 2 O 2 I 2 Cl 2 Br 2

30. Metals found to the left of the “diagonal line” lose electrons in chemical reactions solids (except for Hg, Cs, and Fr) conduct electricity ductile (draw into a wire) malleable (roll into sheets) form alloys ("solid-solution" of one metal in another)

31. Nonmetals found to the right of the “diagonal line” like to gain electrons from metals, or share electrons among themselves found as solids, liquids (Br), and gases (Inert gases, H, N, O, F, Cl) “diatomics” - H 2, N 2, F 2, O 2,I 2, Cl 2, Br 2 oxygen also exist as ozone, O 3 insulators (except for graphite or C) Helium-Neon lasers

32. Metalloids elements next to the “diagonal line” B, Si, Ge, As, Sb, and Te physical properties of a metal (can be “convinced” to conduct electricity) and chemical properties of a nonmetal Elemental Si is used in the semiconductor industry

33. Chapter Outline 2.1The Rutherford Model of Atomic Structure 2.2Nuclides and Their Symbols 2.3Navigating the Periodic Table 2.4The Masses of Atoms, Ions, and Molecules 2.5Moles and Molar Mass 2.6Making Elements 2.7Artificial Nuclides 33

34. AM = (mass 1)(abn) + (mass 2)(abn) + (mass 3)(abn) +……… Average Atomic Mass Weighted average mass of natural sample of an element, calculated by multiplying the natural abundance of each isotope by its exact mass in amu’s and then summing up these products.

35. One Mole of: CS CuFe Hg

36. Molecular Mass – the sum of the average atomic masses of the atoms in it. NOTE: the terms mass and weight are used interchangeably, e.g. molecular weight (MW) or atomic weight (AW) Molecular Mass e.g. H 2 SO 4

37. 37 Formula Units – for ionic compounds, the smallest electrically neutral unit in an ionic compound Formula Mass – the sum of the average atomic masses of the cations and anions that make up a neutral formula unit Formula Units and Formula Mass e.g. NaCl

38. Chapter Outline 2.1The Rutherford Model of Atomic Structure 2.2Nuclides and Their Symbols 2.3Navigating the Periodic Table 2.4The Masses of Atoms, Ions, and Molecules 2.5Moles and Molar Mass 2.6Making Elements 2.7Artificial Nuclides 38

39. The Mole - The mole is the Chemist’s counting unit Avogadro’s Number (N A ) = 6.022 X 10 23 = 1 mole of atoms, molecules, ions, etc. pair = 2 dozen = 12 gross = 144 ream = 500

40. Experiment – how many atoms must be added together so that the mass in grams = mass in amu’s? Analogy using coins: Mass ratio = 1 : 5 : 25

41. Significance of the Mole N A of carbon atoms weighs__________ N A of iron atoms weighs__________ Mass in amu’s Mass in grams/mole Equivalent to

42. To convert between number of particles and an equivalent number of moles. 42 Moles, Mass, and Particles

43. 43 Sample Exercise 2.5 The silicon used to make computer chips has to be extremely pure. Fpr example, it must contain less than 3 x 10-10 moles of phosphorus (a common impurity in Si) per mole of silicon. What is this level of impurity expressed in atoms of phosphorus per mole of Si?

44. e.g. carbon e.g. H 2 SO 4 sulfuric acid Using the Molar Mass as a Conversion Factor for Atoms & Molecules

45. 45 Moles, Mass, and Particles grams of atoms or molecules moles of atoms or molecules Numbers of atoms or molecules

46. How many moles of K atoms are present in 19.5 g of potassium? 46 Practice: Mole Calculations #1

47. How many moles are present in 58.4 g of chalk (CaCO 3 )? 47 Practice: Mole Calculations #2

48. The uranium used in nuclear fuel exists in nature in several minerals. Calculate how many moles of uranium are found in 100.0 grams of carnotite, K 2 (UO 2 ) 2 (VO 4 ) 2 3H 2 O. 48 Practice: Mole Calculations #3