ATOMIC STRUCTURE. Atoms are really small. Gold and Palladium Atoms

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2 ATOMIC STRUCTURE Atoms are really small. Gold and Palladium Atoms

3 Theory vs Model Models are diagrams or apparatuses used to simplify the description of a complicated idea

4 John Dalton English scientist that developed a theory on the composition of matter based on his observations and experiments. He stated that each element is composed of a particle called an atom. He also said that elements that were the same had equal size and mass atoms. His model theory on matter is sometimes called the billiard ball model because he thought atoms were solid spheres.

5 Law of Definite Composition Elements combine in characteristic mass ratios By weight, water is always 11% hydrogen and 89% oxygen. ratio of 1:8 of hydrogen to oxygen in water

6 Law of Multiple Proportions when two elements combine to form more than one compound, the mass of one element, which combines with a fixed mass of the other element, will always be ratios of whole numbers.

7 Example Carbon monoxide and carbon dioxide 100 g of C may react with 133 grams of oxygen to produce 233 g of carbon monoxide 100 g of C may react with 266 grams of oxygen to produce carbon dioxide

8 The ratio of the masses of oxygen that can react with 100 grams of carbon is 266:133 = 2:1

9 Conservation of Mass The total mass involved in a chemical reaction remains constant

10 J.J. Thomson First person to discover a subatomic particle the electron. He determined that electrons are negatively charged subatomic particles. He determined this by showing that a beam of electricity had less mass compared to hydrogen particles. He thought the electrons were mixed into the atom. His model of the atom is sometimes called the raisin bun model or plum pudding model

11 J. J. Thomson and the Electron

12 J. J. Thomson Plum Pudding Model Positive sphere with negative electrons scattered throughout.

13 Ernest Rutherford Experimented with particles by shooting them at each other and different substances. Through his experiments, he determined a positively charged centre of an atom the nucleus. Discovered the proton, predicted the existence of the neutron He also calculated the size of the nucleus is about 1/ th the size of the whole atom. Imagine a green pea in a football field.

14 results showed most of the particles went straight through but a small number scattered at very large angles (not possible according to Thomson)

15 The Discovery of the Atomic Nucleus

16 Hantaro Nagaoka Hantaro Nagaoka refined J. J. Thomson s model by suggesting that the atom resembled a miniature solar system (Planetary model). The centre of the atom was positively charged and the electrons orbited around the centre. Most scientists of his day did not believe in his ideas.

17 James Chadwick In 1932 James Chadwick discovered the neutron, which was critical in developing the atomic bomb. He is credited with discovering the nucleus of an atom to be made up of protons (positively charged subatomic particles) and neutrons (neutrally charged subatomic particles).

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19 Awarded the Nobel Prize in 1922 in Physics. Suggested that electrons do not orbit randomly, they move in a specific circular orbits called electron shells. He suggested that when electrons move from different electron shells, they either gain or lose energy. Niels Bohr

20 Electrons would fill energy levels according to rules 1 st level: only 2 electrons max 2 nd level: 8 electrons max 3 rd level: 8 electrons max

21 Bohr Model of Nitrogen

22 You try one! Try Chlorine: 17p + 18n 0 Chlorine

23 ELECTRON LEVEL DIAGRAMS Based on Bohr s theory of energy levels (shells). 19p + 20n 0 Potassium This atom is neutral. It has the same number of protons(+) and electrons(-). Valence electrons are the ones involved in chemical reactions

24 Simplified Bohr diagram 8 e - 2 e - 10 p + 10 n 0 Neon

25 When energy was added to an atom, the electrons would be lifted to higher energy levels and then fall down Light would be emitted

26 each element has a unique bright line spectrum Mercury Neon

27 Quantum Mechanical (Electron Cloud) Electrons do not exist in well-defined regions around the nucleus Theory predicts the probability of finding electrons in various regions

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29 What are atoms made up of? Sub-Atomic Particles Particle Symbol Charge Proton p + 1+ Neutron n o 0 Electron e - 1- Mass (kg) 1.7 x x x Location Nucleus Nucleus Surrounding the nucleus

30 Reading: A Short History of Nearly Everything p.106 Demitri Ivanovich Mendeleyev Published the first Periodic Table of Elements in 1871.

31

32 THE MODERN PERIODIC TABLE

33 THE MODERN PERIODIC TABLE

34 Metals To the left of the staircase Gray, shiny Conduct heat and electricity Ductile and malleable Solids at room temperature

35 Metalloids properties of both metals and non-metals e.g. silicon, boron, arsenic

36 Non-Metals Solid, liquid or gas at room temp. Some are highly reactive; others almost never react

37 PERIODS AND FAMILIES Periods are rows They have the same number of energy levels (shells) PERIOD 2 PERIOD 4 PERIOD 6 PERIOD 6

38 Columns Groups Elements in the same group tend to have very similar chemical properties

39 Alkali Metals (Group 1) react violently in water to form basic solutions compounds containing them are usually white Reactivity increases down the group

40 Alkali Metals Hydrogen is usually included because it shares some properties with the metals Very soft metals 1 valence electron

41 Alkaline-Earth Metals (Group 2) compounds containing them are usually white powders that tend to be less soluble. 2 valence electrons

42 Halogens (Group 17) React readily with alkali metals to form salts (KCl (s) ) Not full valence level

43

44

45 Noble Gases (Group 18) Non-reactive (inert) gases. Full valence level

46 Transition metals The transition metals are placed in the centre of the periodic table (groups 3 to 11). usually hard and dense, and less reactive than the alkali metals. Iron, copper, silver and gold are important transition metals.

47 Rare Earth Metals Elements 58 to 71

48 The Definition of an Element Atoms of the same element have the same number of protons The number of protons is called the atomic number

49 Atoms An atom is neutral, same number of protons as electrons

50 ATOMIC Mass Number The total number of protons and neutrons in an atom is the mass number (what is lithium s mass number?)

51 ISOTOPES Varieties of a particular element that vary by atomic mass. What makes the mass different is the neutrons. 1 H 2 H 3 H The atomic molar mass on the periodic table is just the average of the mass of all the different isotopes.

52 Another example: 12 6C 13 6C 14 6C

53 Atomic Mass Atomic mass unit amu" is 1 12 mass of a carbon-12 atom of the

54 Calculating Atomic Mass Chlorine has 2 isotopes: 35 Cl amu 75.77% 37 Cl amu 24.23% Calculate the atomic mass of naturally occurring chlorine

55 Calculating Atomic Mass 35 Cl amu 75.77% 37 Cl amu 24.23% 35 Cl amu x = amu 37 Cl amu x = amu Add amu amu = amu

56 IONS Most atoms are very unhappy when they are neutral (p + = e - ). The desperately want to complete their valence (outer-most) shell. They will either gain or loss electrons to do this through a process called ionization. If they loss electrons, they become positive and are called cations If they gain electrons, they become negative and are called anions.

57 THE OCTET RULE Every atom wants to have a complete valence shell In almost every case this means eight valence electrons. What are the exceptions?

58 An example of ionization: + 19p + +18e - 1 net positive charge 19p + 20n 0 Potassium ion

59 Another example: Draw sulphur, and then ionize it! 2-16p + +18e - 2e - 16p + 18n 0 Sulphur ion

60 Notice that the common ion charges (the most common ion that forms for each element) are shown on your periodic table for the metals.

61 Common Ion Charges Some metals can form more than 1 ion charge depending on the chemical conditions. The most common charge is always listed first

62 Nonmetallic ion charges Nonmetals form negative ions Noble gases DO NOT usually form ions B, C, Si rarely form ions

63 Remember the octet rule: how many electrons must be gained to fill the valence level?

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