2. Chapter 5 “Atomic Structure”

3.  Draw and label the model of an atom.  What are the characteristics that make the atom found in one substance different for that of others?

4. The structure of the atom

5. PIONEERS OF THE ATOM ARISTOTLE ARISTOTLE DEMOCRITUS DEMOCRITUS JOHN DALTON JOHN DALTON J.J. THOMPSON J.J. THOMPSON ERNEST RUTHERFORD ERNEST RUTHERFORD NIEHL BOHR NIEHL BOHR ARISTOTLE ARISTOTLE DEMOCRITUS DEMOCRITUS JOHN DALTON JOHN DALTON J.J. THOMPSON J.J. THOMPSON ERNEST RUTHERFORD ERNEST RUTHERFORD NIEHL BOHR NIEHL BOHR

6. Section 4.1 Defining the Atom OBJECTIVES: OBJECTIVES: Identify three types of subatomic particles. Identify three types of subatomic particles. Describe Democritus’s ideas about atoms. Describe Democritus’s ideas about atoms. Explain Dalton’s atomic theory. Explain Dalton’s atomic theory. Describe and Explain the history of the atomic model (Dalton, Thompson, Rutherford & Bohr) Describe and Explain the history of the atomic model (Dalton, Thompson, Rutherford & Bohr) Identify what instrument is used to observe individual atoms. Identify what instrument is used to observe individual atoms.

7. Who studied the atom? Studied by many scientists for centuries Studied by many scientists for centuries Democritus (400 BC); – phrase “atomos” Democritus (400 BC); – phrase “atomos” John Dalton (1766-1844) John Dalton (1766-1844) J. J. Thompson (1856-1940); – “Plum Pudding Model” J. J. Thompson (1856-1940); – “Plum Pudding Model” Ernest Rutherford (1871-1937); - 1911 – nucleus (gold foil expt) Ernest Rutherford (1871-1937); - 1911 – nucleus (gold foil expt) *Bohr - (1885- 1962); 1913 – planetary model of the atom *Bohr - (1885- 1962); 1913 – planetary model of the atom

8. THE EARLY ATOM DEMOCRITUS IS THE MAN!!! DEMOCRITUS IS THE MAN!!! YOU KNOW IT! YOU KNOW IT! DEMOCRITUS IS THE MAN!!! DEMOCRITUS IS THE MAN!!! YOU KNOW IT! YOU KNOW IT! IT’S ALL GREEK TO ME...

9. Section 4.1 Defining the Atom The Greek philosopher Democritus (460 B.C. – 370 B.C.) was among the first to suggest the existence of atoms (from the Greek word “atomos”) The Greek philosopher Democritus (460 B.C. – 370 B.C.) was among the first to suggest the existence of atoms (from the Greek word “atomos”) He believed that atoms were indivisible and indestructible He believed that atoms were indivisible and indestructible His ideas did agree with later scientific theory, but did not explain chemical behavior, and was not based on the scientific method – but just philosophy His ideas did agree with later scientific theory, but did not explain chemical behavior, and was not based on the scientific method – but just philosophy

10. Aristotle Early Greek Theories 400 B.C. - Democritus thought matter could not be divided indefinitely. 400 B.C. - Democritus thought matter could not be divided indefinitely. 350 B.C - Aristotle modified an earlier theory that matter was made of four “elements”: earth, fire, water, air. Democritus Aristotle was wrong. However, his theory persisted for 2000 years. fire air water earth This led to the idea of atoms in a void.

11. ARISTOTLE = SKEPTIC ARISTOTLE = SKEPTIC DEMOCRITUS IS ANIGNORAMUS! ARISTOTLE WAS MUCH MORE POPULAR AND HE OPPOSED THE IDEA OF ATOMS!

12. DEMOCRITUS’ ATOMS

13. SO...CHEMISTRY DIED FOR ABOUT 1400 YEARS UNTIL...

14. SO...CHEMISTRY DIED FOR ABOUT 1400 YEARS IN THE 1700’S IN THE 1700’S

15. Sizing up the Atom  Elements are able to be subdivided into smaller and smaller particles – these are the atoms, and they still have properties of that element  If you could line up 100,000,000 copper atoms in a single file, they would be approximately 1 cm long  Despite their small size, individual atoms are observable with instruments such as scanning tunneling (electron) microscopes

16. John Dalton - John Dalton - 1766 – 1844 1800 -Dalton proposed a modern atomic model 1800 -Dalton proposed a modern atomic model based on experimentation not on pure reason. All matter is made of atoms. Atoms of an element are identical. Each element has different atoms. Atoms of different elements combine in constant ratios to form compounds. Atoms are rearranged in reactions. His ideas account for the law of conservation of mass (atoms are neither created nor destroyed) and the law of constant composition (elements combine in fixed ratios).

17. Section 4.2 Structure of the Nuclear Atom One change to Dalton’s atomic theory is that atoms are divisible into subatomic particles: One change to Dalton’s atomic theory is that atoms are divisible into subatomic particles: Electrons, protons, and neutrons are examples of these fundamental particles Electrons, protons, and neutrons are examples of these fundamental particles There are many other types of particles, but we will study these three There are many other types of particles, but we will study these three

18. Thomson’s Atomic Model Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model. J. J. Thomson

19. Discovery of the Electron In 1897, J.J. Thomson used a cathode ray (- Charge) tube to deduce the presence of a negatively charged particle: the electron

20. Modern Cathode Ray Tubes  Cathode ray tubes pass electricity through a gas that is contained at a very low pressure. TelevisionComputer Monitor

21. Conclusions from the Study of the Electron: a)Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged electrons. b)Atoms are neutral, so there must be positive particles in the atom to balance the negative charge of the electrons c)Electrons have so little mass that atoms must contain other particles that account for most of the mass

22. Section 4.2 Structure of the Nuclear Atom OBJECTIVES: OBJECTIVES: Describe the structure of atoms, according to the Rutherford atomic model (Nuclear model). Describe the structure of atoms, according to the Rutherford atomic model (Nuclear model).

23. Ernest Rutherford (movie: 10 MIN) Most particles passed through. So, atoms are mostly empty. Some positive  -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass. Radioactive substance path of invisible  -particles Rutherford shot alpha (  ) particles at gold foil. Rutherford shot alpha (  ) particles at gold foil. Lead block Zinc sulfide screenThin gold foil

24. Ernest Rutherford’s Gold Foil Experiment - 1911  Alpha particles are helium nuclei - The alpha particles were fired at a thin sheet of gold foil  Particles that hit on the detecting screen (film) are recorded

26. IN THE EXPERIMENT, RUTHERFORD DIRECTED A NARROW BEAM OF ALPHA PARTICLES AT A VERY THIN SHEET OF GOLD FOIL

28. Rutherford’s Findings a) The nucleus is small b) The nucleus is dense c) The nucleus is positively charged  Most of the particles passed right through  A few particles were deflected  VERY FEW were greatly deflected “Like howitzer shells bouncing off of tissue paper!” Conclusions:

29. Thomson’s Atomic Model Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model. J. J. Thomson

30. Section 4.3 Distinguishing Among Atoms OBJECTIVES: OBJECTIVES: Explain what makes elements and isotopes different from each other. Explain what makes elements and isotopes different from each other.

31. Bohr’s model There are 2 types of spectra: continuous spectra & line spectra. It’s when electrons fall back down that they release a photon. These jumps down from “shell” to “shell” account for the line spectra seen in gas discharge tubes (through spectroscopes). Electrons orbit the nucleus in “shells” Electrons can be bumped up to a higher shell if hit by an electron or a photon of light.

32. Adding Electrons to the Model 1) Dalton’s “Billiard ball” model (1800-1900) Atoms are solid and indivisible. 2)Thompson “Plum pudding” model (1900) Negative electrons in a positive framework. 3)The Rutherford model (around 1910) Atoms are mostly empty space. Negative electrons orbit a positive nucleus. Materials, when rubbed, can develop a charge difference. This electricity is called “cathode rays” when passed through an evacuated tube (demos). These rays have a small mass and are negative. Thompson noted that these negative subatomic particles were a fundamental part of all atoms.

33. Section 4.3 Distinguishing Among Atoms OBJECTIVES: OBJECTIVES: Calculate the number of neutrons in an atom. Calculate the number of neutrons in an atom.

34. Section 4.3 Distinguishing Among Atoms OBJECTIVES: OBJECTIVES: Calculate the atomic mass of an element. Calculate the atomic mass of an element.

35. Section 4.3 Distinguishing Among Atoms OBJECTIVES: OBJECTIVES: Explain why chemists use the periodic table. Explain why chemists use the periodic table.

36. Atomic Number Atoms are composed of identical protons, neutrons, and electrons Atoms are composed of identical protons, neutrons, and electrons How then are atoms of one element different from another element? How then are atoms of one element different from another element? Elements are different because they contain different numbers of PROTONS Elements are different because they contain different numbers of PROTONS The “atomic number” of an element is the number of protons in the nucleus The “atomic number” of an element is the number of protons in the nucleus # protons in an atom = # electrons # protons in an atom = # electrons

37. Atomic Number Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element. Element # of protons Atomic # (Z) Carbon66 Phosphorus1515 Gold7979

38. Mass Number Mass number is the number of protons and neutrons in the nucleus of an isotope: Mass # = p + + n 0 Nuclide p+p+p+p+ n0n0n0n0 e-e-e-e- Mass # Oxygen - 10 -3342 - 31 - 3115 8 8 18 Arsenic 7533 75 Phosphorus 15 31 16

39. Complete Symbols Contain the symbol of the element, the mass number and the atomic number. Contain the symbol of the element, the mass number and the atomic number. X Mass number Atomic number Subscript → Superscript →

40. Symbols n Find each of these: a) number of protons b) number of neutrons c) number of electrons d) Atomic number e) Mass Number Br 80 35

41. Symbols n If an element has 91 protons and 140 neutrons what is the a) Atomic number b) Mass number c) number of electrons d) complete symbol

42. Symbols n If an element has 78 electrons and 117 neutrons what is the a) Atomic number b) Mass number c) number of protons d) complete symbol

43. Isotopes Dalton was wrong about all elements of the same type being identical Dalton was wrong about all elements of the same type being identical Atoms of the same element can have different numbers of neutrons. Atoms of the same element can have different numbers of neutrons. Thus, different mass numbers. Thus, different mass numbers. These are called isotopes. These are called isotopes.

44. Isotopes Frederick Soddy (1877-1956) proposed the idea of isotopes in 1912 Frederick Soddy (1877-1956) proposed the idea of isotopes in 1912 Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons. Soddy won the Nobel Prize in Chemistry in 1921 for his work with isotopes and radioactive materials. Soddy won the Nobel Prize in Chemistry in 1921 for his work with isotopes and radioactive materials.

45. Naming Isotopes We can also put the mass number after the name of the element: We can also put the mass number after the name of the element: carbon-12 carbon-12 carbon-14 carbon-14 uranium-235 uranium-235

46. Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons. IsotopeProtonsElectronsNeutronsNucleus Hydrogen–1 (protium) (protium)110 Hydrogen-2(deuterium)111 Hydrogen-3(tritium)112

47. Isotopes Elements occur in nature as mixtures of isotopes. Isotopes are atoms of the same element that differ in the number of neutrons.

48. Atomic Mass  How heavy is an atom of oxygen?  It depends, because there are different kinds of oxygen atoms.  We are more concerned with the average atomic mass.  This is based on the abundance (percentage) of each variety of that element in nature.  We don’t use grams for this mass because the numbers would be too small.

49. Measuring Atomic Mass Instead of grams, the unit we use is the Atomic Mass Unit (amu) Instead of grams, the unit we use is the Atomic Mass Unit (amu) It is defined as one-twelfth the mass of a carbon-12 atom. It is defined as one-twelfth the mass of a carbon-12 atom. Carbon-12 chosen because of its isotope purity. Carbon-12 chosen because of its isotope purity. Each isotope has its own atomic mass, thus we determine the average from percent abundance. Each isotope has its own atomic mass, thus we determine the average from percent abundance.

50. To calculate the average: Multiply the atomic mass of each isotope by it’s abundance (expressed as a decimal), then add the results. Multiply the atomic mass of each isotope by it’s abundance (expressed as a decimal), then add the results. If not told otherwise, the mass of the isotope is expressed in atomic mass units (amu) If not told otherwise, the mass of the isotope is expressed in atomic mass units (amu)

51. Atomic Masses IsotopeSymbol Composition of the nucleus % in nature Carbon-12 12 C 6 protons 6 neutrons 98.89% Carbon-13 13 C 6 protons 7 neutrons 1.11% Carbon-14 14 C 6 protons 8 neutrons <0.01% Atomic mass is the average of all the naturally occurring isotopes of that element. Carbon = 12.011

52. - Page 117 Question Solution Answer Knowns and Unknown

53. The Periodic Table: A Preview  A “periodic table” is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties  The periodic table allows you to easily compare the properties of one element to another

54. The Periodic Table: A Preview  Each horizontal row (there are 7 of them) is called a period  Each vertical column is called a group, or family  Elements in a group have similar chemical and physical properties  Identified with a number and either an “A” or “B”  More presented in Chapter 6

55. Subatomic Particles ParticleCharge Mass (g) Location Electron (e - ) (e - ) 9.11 x 10 -28 9.11 x 10 -28 Electron cloud Proton (p + ) +1 1.67 x 10 -24 1.67 x 10 -24Nucleus Neutron (n o ) (n o )0 1.67 x 10 -24 1.67 x 10 -24Nucleus