1. Chapter 4

2. Greek philosopher (460 B.C.-370 B.C.) 1 st to suggest the existence of atoms Said that atoms were indivisible and indestructible Democritus’s Atomic Philosophy Early Models of the Atom

3. English chemist and school teacher (1766-1844). 1. 1.All elements are composed of indivisible ‘solid sphere’ atoms. 2. All atoms of a given element are identical. 3. Atoms are different elements differ in their masses. 4. Different atoms combine in simple whole number ratios to form compounds. Dalton’s Atomic Theory Early Models of the Atom

4. All elements are composed of atoms All atoms of the same element are identical Atoms of different elements combine to form compounds Atoms of one element can never be changed into another element Defining the Atom

5. Structure of the Nuclear Atom Atoms are divisible Three kinds of subatomic particles are: 1. Electrons 2. Protons 3. Neutrons

6. 1.Electrons Orbit the nucleus of the atom Have a negative (-1) charge Mass ~0 atomic mass unit (amu) Shorthand symbol (e - ) J.J. Thomson discovered the electron using the cathode-ray tube

7. CATHODE RAY A cathode ray produced in a discharge tube travels from left to right. The ray itself is invisible, but the fluorescence of a zinc sulfide coating on the glass causes it to appear green

8. CATHODE RAY When the polarity of the magnet is reversed, the ray bends in the opposite direction

9. CATHODE RAY The cathode ray is bent downwar d when the south pole of the bar magnet is brought toward it

10. THE PLUM PUDDING MODEL JJ Thomson’s Atom

11. 2. Protons Charge of +1 (positive) Mass of 1 amu (atomic mass unit) Located inside the nucleus Shorthand symbol (p + )

12. 3.Neutrons Consists of charge of 0 (neutral) Mass of 1 amu Located inside the nucleus Shorthand symbol (n 0 )

13. Discovering the Atomic Nucleus When the particles were discovered, scientists wondered how these particles were put together. Ernest Rutherford made it possible to understand how the subatomic particles were assembled

17. Rutherford’s Gold-Foil Experiment Proposed that the atom is made up of empty space The mass and positive charge of the atom is located in the nucleus (a dense region)

18. The Nuclear Atom 1. Nucleus Contains positive electrical charge Makes up the most of the mass of the atom There are two subatomic particles: protons and neutrons The electrons are distributed around the nucleus and occupy almost all the volume of the atom

21. Atomic Number Elements are different because they contain different number of protons Atomic number is the number of protons in the nucleus of an atom of that element Atomic Number = protons or electrons Is usually written as a subscript Ex: 12 Mg or Mg 12

22. What element has 11 protons? How many protons does potassium have? Sodium 19

23. Element Atomic Number ProtonsElectrons K19 5 S16 V23 Complete the Table

24. Mass Number Mass Number = Protons + Neutrons Mass number is also known as atomic mass The number of neutrons in an atom is the difference between the mass number and the atomic number # of neutrons = mass number – atomic number Usually located at the top of the element symbol Ex: 12 C C 12 C-12

25. Sample Problems How many protons, electrons, and neutrons are in each atom? Beryllium (Be) - Neon (Ne) - Sodium(Na) - 4, 4, 5 10, 10, 10 11, 11, 12

26. How many neutrons are in each atom? 8 O 16 47 Ag 108 82 Pb 207 16 – 8 = 8 108 – 47 = 61 207 – 82 = 125

27. Express the composition of each atom in shorthand form. Nitrogen -14 Sodium - 23 Phosphorus -31 p + = 7, n 0 = 7, e - = 7 p + = 11, n 0 = 12, e - = 11 p + = 15, n 0 = 16, e - = 15

28. Atomic# Mass # # of proton # of Neutron # of e - Symbol 910 1415 4722 5525

29. Isotopes

30. Determine the number of protons, neutrons and electrons in the following: 1H11H1 1H21H2 1H31H3 p + = 1, n 0 = 0, e - = 1 p + = 1, n 0 = 1, e - = 1 p + = 1, n 0 = 2, e - = 1 Sample Exercise

31. Natural Abundance of Stable Isotopes of Some Elements NameSymbolNatural Percent Abundance Mass (amu) Average Atomic Mass Nitrogen 7 N 14 7 N 15 99.63 0.37 14.003 15.000 14.007 Chlorine 17 Cl 35 17 Cl 37 75.77 24.23 34.969 36.966 35.453 Helium 2 He 3 2 He 4 0.0001 99.9999 3.0160 4.0026 Sulfur 16 S 32 16 S 33 16 S 34 16 S 36 95.002 0.76 4.22 0.014 31.972 32.971 33.967 35.967 32.06

32. Uncovering Atomic Mass Atomic mass # is an average of atom’s naturally occurring isotopes Copper has 2 isotopes Cu -63 and Cu -65. Which isotope is most abundant? There are 3 isotopes of Silicon with mass numbers of 28, 29, and 30. Which is more abundant? 63 Si -28

33. Practice Exercise Boron has two isotopes: boron – 10 and boron – 11. Which is more abundant, given that the atomic mass of boron is 10.81? Answer : B-11

34. Calculating Atomic Mass Multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products.

35. Sample Exercise An element consists of two isotopes. Isotope A has an abundance of 75%, and its mass is 14.000 a.m.u. Isotope B has an abundance of 25% and its mass is 15.000 a.m.u. What is the atomic mass of the element? Ans: 14.25

36. Sample Exercise Boron in nature has two isotopes. Boron -10 has a mass of 10.0130 a.m.u. and abundance is 19.9%. B – 11 has a mass of 11.0093 a.m.u., and abundance is 80.1%. Calculate the atomic mass of boron. Ans: 10.8109 a.m.u

37. Sample Exercise There are four isotopes of Lead: Pb – 204, Pb – 206, Pb – 207, Pb – 208. Their weights are 1.37%, 26.26%, 20.82%, and 51.55% respectively. Using this data calculate the atomic mass of lead. 207.2118

38. Calculate the atomic mass of bromine. The two isotopes of bromine have atomic masses and relative abundance of 78.92 amu (50.69%) and 80.92 amu (49.31%).

39. Ions An atom with an electrical charge Occurs 2 ways: Oxidation – loss of an e - results in a (+) charge Reduction – gain of an e - results in a (-) charge Mnemonic: ‘LEO says GER’ Loss of electrons = oxidation Gain of electrons = reduction

40. Examples of Ions H + Cl - As 3- Mg 2+ Oxidation State – Number found on the periodic table Shows the number of e - gained or lost Many elements have more than one number Ions & Subatomic Particles Lost 1e - Gained 1e - Gained 3e - Lost 2e -

41. Review and Assessment Would you expect two electrons to attract or repel each other? What charge does the atom become when it loses/gains an electron? What were the results of Rutherford’s experiment? What is the charge – positive or negative – of the nucleus of every atom?

42. Review and Assessment Which subatomic particles are located in the nucleus? Name two ways that isotopes of an element can differ? What is the atomic mass of an element? How are the elements arranged in the modern periodic table?