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Atoms and Their Structure

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1 Atoms and Their Structure

2 History of the Atom Original idea (400 B.C.) came from Democritus, a Greek philosopher Democritus expressed the belief that all matter is composed of very small, indivisible particles, which he named atomos.

3 Who’s Next? John Dalton ( ), an English school teacher and chemist, studied the results of experiments by other scientists.

4 Dalton’s Atomic Theory
John Dalton proposed his atomic theory of matter in 1803. Although his theory has been modified slightly to accommodate new discoveries, Dalton’s theory was so insightful that it has remained essentially intact up to the present time.

5 Dalton’s Atomic Theory
All matter is made of tiny indivisible particles called atoms. Atoms of the same element are identical; those of different atoms are different.

6 Dalton’s Atomic Theory, cont.
Atoms of different elements combine in whole number ratios to form compounds Chemical reactions involve the rearrangement of atoms. No new atoms are created or destroyed.

7 Parts of the Atom Because of Dalton’s atomic theory, most scientists in the 1800s believed that the atom was like a tiny solid ball that could not be broken up into parts. In 1897, a British physicist, J.J. Thomson, discovered that this solid-ball model was not accurate.

8 Parts of the Atom Thomson’s experiments used a cathode ray tube.
It is a vacuum tube - all the air has been pumped out.

9 Thomson’s Experiment Voltage source - + Vacuum tube Metal Disks

10 - + Thomson’s Experiment Voltage source
At each end of the tube is a metal piece called an electrode, which is connected through the glass to a metal terminal outside the tube.

11 - + Thomson’s Experiment Voltage source
When the electrodes are charged, rays travel in the tube from the negative electrode, which is the cathode, to the positive electrode, the anode.

12 - + Thomson’s Experiment Voltage source
Because these rays originate at the cathode, they are called cathode rays.

13 Thomson’s Experiment Voltage source - +

14 Thomson’s Experiment Voltage source - +

15 Thomson’s Experiment Voltage source - +

16 Thomson’s Experiment Voltage source - +

17 Thomson’s Experiment Voltage source + - By adding an electric field,

18 Thomson’s Experiment Voltage source + -

19 Thomson’s Experiment Voltage source + -
Thomson found that the rays bent toward a positively charged plate and away from a negatively charged plate.

20 Thomson’s Experiment Voltage source + -
He knew that objects with like charges repel each other, and objects with unlike charges attract each other.

21 Thomson’s Experiment Voltage source + -
By adding an electric field he found that the moving rays were negative.

22 Thomson’s Experiment Voltage source + -
J.J. Thomson concluded that cathode rays are made up of invisible, negatively charged particles referred to as electrons.

23 Cathode Ray Tube

24 Thomson’s Model From Thomson’s experiments, scientists had to conclude that atoms were not just neutral spheres, but somehow were composed of electrically charged particles.

25 Thomson’s Model Sketch Thomson’s model of the atom in your notes.

26 Thomson’s Model Matter is not negatively charged, so atoms can’t be negatively charged either. If atoms contained extremely light, negatively charged particles, then they must also contain positively charged particles — probably with a much greater mass than electrons.

27 Thomson’s Model J.J. Thomson said the atom was like plum pudding, a popular English dessert.

28 Millikan’s Oil Drop Experiment
R.A. Millikan found the charge of an electron to be x Coulombs in his famous oil drop experiment.

29 The Proton In 1886, scientists discovered that a cathode-ray tube emitted rays not only from the cathode but also from the positively charged anode. Years later, scientists determined that the rays were composed of positively charged subatomic particles called protons.

30 The Proton At this point, it seemed that atoms were made up of equal numbers of electrons and protons.

31 Ernest Rutherford In 1909, a team of scientists led by Ernest Rutherford in England carried out the first of several important experiments that revealed an arrangement far different from the plum pudding model of the atom and discovered the nucleus.

32

33 Rutherford’s Experiment
The experimenters set up a lead-shielded box containing radioactive polonium, which emitted a beam of positively charged subatomic particles through a small hole.

34 Rutherford’s Experiment
The sheet of gold foil was surrounded by a screen coated with zinc sulfide, which glows when struck by the positively charged particles of the beam.

35 Florescent Screen Lead block Polonium Gold Foil

36 What Rutherford Expected
The alpha particles to pass through without changing direction very much.

37 Because he thought the mass was evenly distributed in the atom,

38 the alpha particles should go straight through.

39 What Rutherford Observed

40 How Rutherford Explained It
To explain the results of the experiment, Rutherford’s team proposed a new model of the atom. Because most of the particles passed through the foil, they concluded that the atom is nearly all empty space.

41 How Rutherford Explained It
Alpha particles are deflected by the nucleus if they get close enough it.

42 How Rutherford Explained It
Because so few particles were deflected, they proposed that the atom has a small, dense, positively charged central core, called a nucleus. Most of the atom’s mass is located in the nucleus. 42

43 The Nuclear Model of the Atom
Sketch Rutherford’s model of the atom in your notes.

44 Isotopes In 1910, J.J. Thomson discovered that neon consisted of atoms of two different masses.

45 C Isotopes Carbon-12 and carbon-14 are isotopes of one another.
6 C 14 Carbon-12 and carbon-14 are isotopes of one another. They are the same element with different masses.

46 Isotopes Atoms of an element that are chemically alike but differ in mass are called isotopes of the element. Because of the discovery of isotopes, scientists hypothesized that atoms contained still a third type of particle that explained these differences in mass.

47 The Neutron Isotopes of an element differ in the number of the subatomic particle called neutrons.

48 The Neutron Calculations showed that the neutron should have a mass equal to that of a proton but no electrical charge. The existence of this neutral particle, called a neutron, was confirmed in the early 1930s. James Chadwick is given credit for discovering the neutron.

49 Naming Isotopes C-12 C-14 Pb-210 Pb-212
Put the mass number after the symbol of the element. Carbon – amu C-12 Carbon – amu C-14 Pb-210 Lead – amu Pb-212 Lead – amu

50 Modern View of the Atom The atom has two regions and is 3-dimensional.
The nucleus is at the center and contains the protons and neutrons.

51 Modern View of the Atom The electron cloud is the region where you might find an electron and most of the volume of an atom.

52 Model of Atoms

53 Model of a Hydrogen Atom
Hydrogen has _____ proton, _____ electron and ______ neutrons. one one zero

54 Model of a Helium Atom Helium has _____ protons, _____ electrons and _____ neutrons. two two two

55 Model of a Boron Atom 5 p+ 6 no Boron has _____ protons, _____ electrons and _____ neutrons. five five six

56 Model of a Carbon Atom Carbon has _____ protons, _____ electrons and _____ neutrons. six six six

57 Subatomic Particles Name Electron e- -1 1/2000 Proton p+ +1 1 Neutron
Relative mass Relative mass Name Symbol Symbol Charge Charge Electron e- -1 1/2000 Proton p+ +1 1 Neutron n0 1

58 Atomic Number The atomic number (Z) of an element is the number of protons in the nucleus of an atom of that element. The number of protons determines identity of an element, as well as many of its chemical and physical properties.

59 Atomic Number Because atoms have no overall electrical charge, an atom must have as many electrons as there are protons in its nucleus. Therefore, the atomic number of an element also tells the number of electrons in a neutral atom of that element.

60 Masses The mass of a neutron is almost the same as the mass of a proton. The sum of the protons and neutrons in the nucleus is the mass number (Z) of that particular atom.

61 SYMBOLS 61

62 Isotopes Remember, isotopes of an element have different mass numbers because they have different numbers of neutrons, but they all have the same atomic number.

63 Isotopes Subtract the atomic number from the mass number to determine the number of neutrons. How many neutrons are in each lithium isotope below? 4 neutrons 3 neutrons 5 neutrons 63

64 Information in the Periodic Table
The average atomic mass is the weighted average mass of all the naturally occurring isotopes of that element.

65 Average Atomic Mass You are NOT responsible for knowing how to calculate average atomic mass, although a detailed example follows.

66 Calculating Atomic Mass

67 Calculating Atomic Mass
Copper exists as a mixture of two isotopes. The lighter isotope (Cu-63), with 29 protons and 34 neutrons, makes up 69.17% of copper atoms. The heavier isotope (Cu-65), with 29 protons and 36 neutrons, constitutes the remaining 30.83% of copper atoms.

68 Calculating Atomic Mass
To determine the average atomic mass, first calculate the contribution of each isotope to the average atomic mass, being sure to convert each percent to a fractional abundance.

69 Calculating Atomic Mass
Mass contribution = mass of isotope x abundance of isotope For Cu-63: Mass contribution = amu x = amu For Cu-65: Mass contribution = amu x = amu

70 Calculating Atomic Mass
The average atomic mass of the element is the sum of the mass contributions of each isotope. Atomic mass Cu = mass contribution Cu-63 + mass contribution Cu-65 Atomic mass Cu = = amu

71 SYMBOLS 71

72 Symbols Example F 19 9 Determine the complete symbol for a fluorine atom with a mass number of 19.

73 Symbols Example Determine the following for the fluorine atom depicted below. 19 F (9) number of protons 9 number of neutrons (10) number of electrons (9) atomic number (9) e) mass number (19) 73

74 Symbols Example Br 80 35 Determine the complete symbol for a bromine atom with a mass number of 80. 74

75 Symbols Problem Determine the following for the bromine atom depicted below. 80 Br (35) number of protons 35 number of neutrons (45) number of electrons (35) atomic number (35) e) mass number (80)

76 Symbols Problem If an element has an atomic number of 34 and a mass number of 78 what is the (34) number of protons number of neutrons (44) number of electrons (34) complete symbol 78 Se 34

77 Symbols Problem If an element has 91 protons and 140 neutrons what is the (91) atomic number mass number (231) number of electrons (91) complete symbol 231 Pa 91

78 Symbols Problem If an element has 78 electrons and 117 neutrons what is the (78) atomic number mass number (195) number of protons (78) complete symbol 195 Pt 78

79 Fill in the chart below. 19 20 19 39 19 18 22 18 40 18 Potas-sium
Element # of Protons # of Neutrons # of Electrons Mass # Atomic # Potas-sium Argon 19 20 19 39 19 18 22 18 40 18

80 Fill in the chart below. (When numbers are provided, the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table.) Element # of Protons # of Neutrons # of Electrons Mass # Atomic # Chlorine Oxygen 17 20 17 37 17 8 10 8 18 8

81 End of Day 1

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