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ATOMIC STRUCTURE. ATOMIC STRUCTURE. Rutherford’s Experiment Basic Particles of Atom Atomic Number and Mass Number Isotope, Isobar, Isotone, and Isoelectron Electron Configuration and Valence Electron Development of Atom ic Theory. CONCLUSION:
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ATOMIC STRUCTURE • Rutherford’s Experiment • Basic Particles of Atom • Atomic Number and Mass Number • Isotope, Isobar, Isotone, and Isoelectron • Electron Configuration and Valence Electron • Development of Atomic Theory
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 1. RUTHERFORD’S EXPERIMENT
1. RUTHERFORD’S EXPERIMENT 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 ray radium gold Plumbum plate Detector (ZnS)
2. Basic Particles of Atom ATOM NUCLEUS ELECTRON NEUTRON PROTON
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
EXERCISEComplete the table below! 10 18 10 10 8 47 108 47 61 47 50 69 50 50 119 83 83 83 209 126 56 81 137 56 56 56 26 26 26 30 16 31 16 15 16 28 31 28 59 28
IONIC REACTION EQUATION POSITIVE ION (KATION) + e + 2e e = 10 p = 11 n = 12 e = 4 p = 4 n = 5 e = 2 p = 4 n = 5 e = 11 p = 11 n = 12 NEGATIVE ION (ANION) + 3e + e e = 18 p = 17 n = 18 e = 18 p = 15 n = 16 e = 17 p = 17 n = 18 e = 15 p = 15 n = 16
EXERCISEComplete the table below! 39 19 20 19 18 80 36 35 45 35 13 13 10 14 27 8 10 8 8 16
ISOTOPE DEFINITION OF ISOTOPE: The atoms which have similar atomic number but the mass number is different. EXAMPLE: and , and
ISOBAR DEFINITION OF ISOBAR: The atoms which have different atomic number (the element is different) but the mass number is same. EXAMPLE: and and
ISOTONE DEFINITION OF ISOTONE: The atoms which come from different element, but the amount of neutron is same EXAMPLE: and and
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
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, eventhough the third shell (M) has not full yet. 2 8 18
EXERCISECOMPLETE THE TABLE BELOW! 2 1 2 8 2 8 3 2 18 2 8 18 18 4 8 18 2 5 18 6 8 18 2 8 18 7 2 8 18 32 18 8 2
VALENCE ELECTRON 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 Quantity of valence electron: 8
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
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
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) Cloud of proton electron - - - - - Atom model of J.J. Thomson
ATOM THEORY OF RUTHERFORD • 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. • Some light electrons that can’t restrained the high speed of alpha particles go around the nucleus like planets that orbit to the sun. • 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. electron Skin of atom - nucleus + Atom model of Rutherford Atom radius
ATOM THEORY OF NIELS BOHR 1.An atom consist of a nucleus (positive) that is surrounded by electrons (negative)
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.
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.
