1. ATOMIC STRUCTURE

2. 1.Rutherford’s Experiment 2.Basic Particles of Atom 3.Atomic Number and Mass Number 4.Isotope, Isobar, Isotone, and Isoelectron 5.Electron Configuration and Valence Electron 6.Development of Atomic Theory

3. 1. RUTHERFORD’S EXPERIMENT CONCLUSION: TThe atom consist of nucleus which has positive charge and the mass of atom is centered in the nucleus TThere are many electrons which move around nucleus outside the nucleus and the amount of electrons equal to the charge of nucleus, so the atom has neutral characteristic

4. CONCLUSION:  The atom consist of nucleus which has positive charge and the mass of atom is centered in the nucleus  There are many electrons which move around nucleus outside the nucleus and the amount of electrons equal to the charge of nucleus, so the atom has neutral characteristic radium Plumbum plate  ray gold Detector (ZnS) 1. RUTHERFORD’S EXPERIMENT

5. 2. Basic Particles of Atom ATOM ELECTRON NEUTRON NUCLEUS PROTON

6. 3. Atomic Number and Mass Number Explanation: X : symbol of atom A : mass number, shows the amount of proton + neutron Z : atomic number, shows the amount of proton/electron

7. EXERCISE Complete the table below! Atomic Number Mass Number ProtonNeutronElectronSymbol 10 8 18 47 6147108 28 16 26 56 83 50 59 31 56 137 209 119 28 16 26 56 83 50 31 15 30 81 126 69 28 16 26 56 83 50

8. IONIC REACTION EQUATION + e e = 11 p = 11 n = 12 +e e = 17 p = 17 n = 18 e = 10 p = 11 n = 12 e = 18 p = 17 n = 18 POSITIVE ION (KATION) + 2e e = 2 p = 4 n = 5 e = 4 p = 4 n = 5 +3e e = 15 p = 15 n = 16 e = 18 p = 15 n = 16 NEGATIVE ION (ANION)

9. EXERCISE Complete the table below! Atom Number Mass Number ProtonNeutronElectronSymbol 1918 201939 8 13 35 16 27 80 35 13 8 8 14 45 10 10 36

10. 4. ISOTOPE ISOBAR ISOTONE ISOELECTRON

11. ISOTOPE DEFINITION OF ISOTOPE: The atoms which have similar atomic number but the mass number is different. EXAMPLE: and,

12. ISOBAR DEFINITION OF ISOBAR: The atoms which have different atomic number (the element is different) but the mass number is same. EXAMPLE: and

13. ISOTONE DEFINITION OF ISOTONE: The atoms which come from different element, but the amount of neutron is same EXAMPLE: and

14. ISOELECTRON DEFINITION OF ISOELECTRON: The atoms which come from different element, but the amount of electron is same EXAMPLE: and, p = 13 n = 14 e = 10 p = 8 n = 8 e = 10 p = 10 n = 10 e = 10

15. 5. Electron Configuration and Valence Electron

16. ELECTRON CONFIGURATION An electron configuration is the spreading of the electron in shells of an atom. The configuration must follow the regulations below: The maximum quantity of electron in the shell is 2n2 n Value of K shell = 1, so, the max. quantity of electron = n Value of L shell = 2, so, the max. quantity of electron = n Value of M shell = 3, so, the max. quantity of electron = etc. The maximum quantity of electrons in the external shell is 8 Normally, the filling of electrons starts at the inner shell (K). Elements with atom number 1 to 18, is filled with electrons in their external shell only if the inner shell is full. The elements with atomic number more than 18, the external shell, which is the fourth shell (N) and other shell levels, can be filled with electrons, even though the third shell (M) has not full yet. 2 8 18

17. EXERCISE COMPLETE THE TABLE BELOW! Atom Electron Skin KLMNOPQ 3 Li 12 Mg 31 Ga 50 Sn 33 As 52 Te 35 Br 86 Rn 2 2 2 2 2 2 2 2 1 8 8 8 8 8 8 8 2 3 18 4 5 6 7 32188

18. VALENCE ELECTRON Valence electron is the quantity of electron on the external shell of which the maximum quantity is 8. Valence electron is the quantity of electron on the external shell of which the maximum quantity is 8.Example: 1. 11 Na Electron configuration: 2 8 1 Quantity of valence electron: 1 2. 20 Ca Electron configuration: 2 8 8 2 Quantity of valence electron: 2 3. 54 Xe Electron configuration: 2 8 18 18 8 Electron configuration: 2 8 18 18 8 Quantity of valence electron: 8

19. 6. Development of Atomic Theory  Atomic theory of Dalton  Atomic theory of J.J. Thomson  Atomic theory of Rutherford  Atomic theory of Niels Bohr  Modern atom theory

20. ATOMIC THEORY OF DALTON A substance consist of minute particles that can’t be divided, and this is called an atom with a small massive ball shape Atoms of an element are identical but they are different from atoms of the other elements Chemically, atoms are interwoven to each other to perform a molecule with a simple comparison A compound is the product of the reaction of atom An atom of an element is permanent, can’t de divided or created or destroyed Atom model of Dalton

21. ATOM THEORY OF J.J. THOMSON Negative charged electrons spread inside the positive charged ball (looks like the currants that spread over a piece of cake, so, its called COOKIE THEORY) Atom model of J.J. Thomson electron Cloud of proton - - - - -

22. ATOM THEORY OF RUTHERFORD AAll of positive charge and most of atom mass are concentrated at a particle at the center of the atom. This particle is the nucleus of an atom. SSome light electrons that can’t restrained the high speed of alpha particles go around the nucleus like planets that orbit to the sun. AAn atom is neutral, meaning that in an atom, the charge of the electrons (negative) is equal with the charge of the nucleus (positive) Unfortunately Rutherford can’t explain, why an electron can’t attach to the nucleus. Each of them have different charges, an electrons will attach to the nucleus in a spiral orbit track and then hits the nucleus. Atom model of Rutherford + - Skin of atom electron Atom radius nucleusnucleus

23. ATOM THEORY OF NIELS BOHR 1.An atom consist of a nucleus (positive) that is surrounded by electrons (negative)

24. 2. An electron goes around the nucleus in a given orbit known as stationary energy. This is called the major energy level or the major quantum number.

25. 3. If an electron stays on its stationary energy level, there will be no ray sparks. 4. An electron can move to the upper level if it absorbs an energy, and an electron can move to the lower level if it releases some of its energy.

26. THAT’S ALL

27. Periodic table of elements-2