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Atomic structure.KM
The document provides an overview of atomic structure, detailing the components of an atom, including protons, neutrons, and electrons. It explains concepts like atomic number, atomic mass, and the calculation of charges in ions, along with examples of isotopes and relative atomic mass. Additionally, it offers learning objectives and resources for further exploration of the material.
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Atomic structure.KM
- 1. Atomic structure D.M K.MS.H Z.M I.S
- 2. Contents Introduction: Learning Objectives Whatis an Atom? 2 What is an element? Calculations of protons, neutrons and electrons Charge of ions Examples and questions.
- 3. Introduction: Learning Objectives 2.Define atomic number and atomic mass 3. Calculate the number of protons, neutrons and electrons 4. Deduce the charge of ions 1. Describe structure of an atom
- 4. What is anAtom? Atom is made of 2 parts: 1. Electrons that appear around the nucleus in particular energy levels 2. Nucleus that is made up of protons and neutrons 2.1. Protons 2.2. Neutrons Helium atom - - + + Atom the smallest chemically indivisible particle of a substance
- 5. What is anAtom? Particles Symbol Charge Atomic mass (g) Proton Neutron Electron p or Z n e– 1 0 – 1 1/1840 + 1,673∙10-24 1,675∙10-24 0,911∙10-27 1 carbon atom weights 20,088 ∙10-24 g Charge – physical quantity that shows the ability of particles to be a source of electromagnetic fields. There are positive (+) and negative (–) charges.
- 6. Tips for remembering pProtons + Positive n Neutrons 0 Neutral = 0 e Electrons - Negative Relative Mass 1 amu 1 amu negligible 1 amu = 1.67377 x 10 -24 gram Charge
- 7. Atomic Number (Z)= Proton Number = Electron Number (in neutral atom) Atomic Mass (A) = Protons + Neutrons A = Z + n https://phet.colorado.edu/sims/html/build-an-atom/latest/build-an-atom_en.html Atomic number and Atomic mass Charge of particle (C) = difference between protons and electrons C = Z – e–
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- 9. Calculations of protons,neutrons and electrons Electron number = ? Neutron number = ? Proton number = ? Atomic number = ? Atomic mass = ? Charge = ?
- 10. Charge of ions. 12protons = +12 10 electrons = -10 Total charge= ? +2 Magnesium ion: Mg 12 protons = +12 12 electrons = -12 Total charge= ? 0 Mg Magnesium atom:
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- 12. What is Isotope? Porsche X Porsche Y Porsche Z Radio Leather Seats Red Chrome Wheels CD Player Blue Massaging Seats Platinum Wheels Yellow All Porsche
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- 14. Examples of Isotopes + 0 + + + ++ 0 0 0 0 0 - - - - - - ı ıı + Proton Neutron 0 Electron (s) - Electron (p) -
- 15. Examples of Isotopes + 0 + + + ++ 0 0 0 0 0 - - - - - - ı ıı + Proton Neutron 0 Electron (s) - Electron (p) - 0
- 16. Examples of Isotopes + 0 + + + ++ 0 0 0 0 0 - - - - - - ı ıı + Proton Neutron 0 Electron (s) - Electron (p) - 0 0
- 17. Summary Element: Carbon Protons: 6 Neutrons:6 Element: Carbon Protons: 6 Neutrons: 7 Element: Carbon Protons: 6 Neutrons: 8 Protons are same Isotopes Quick Tip: “Iso” means Same (Same number of Protons)
- 18. Examples of Isotopes–> Group Work Click For Correct Answers Isotope or Not ? Group B Group A Group D Group C
- 19. Relative Atomic Mass:What is happening ? Why ? Isotopes Relative Atomic Mass Average Mass of Atoms in Element (A r) Standard: mass of 1 C-12 = 12
- 20. Relative atomic mass Theaverage mass of a large number of atoms of an element is called its relative atomic mass (Ar) Calculated according to percentage abundance of all the isotopes of an element which exist. Standard: Carbon-12 = 12 amu
- 21. Average Mass Weight: 100gram Count: 4 Weight: 50 gram Count: 3 Abundance (%) 75 25
- 22. Examples of RelativeAtomic Mass Silicon (Si) Mass Number Natural Abundance 28 92.22% 29 4.69% 30 3.09% Phosphorus (P) Mass Number Natural Abundance 32 94.99% 33 0.75% 34 4.25% 36 0.01% Potassium (K) Mass Number Natural Abundance 39 93.26% 40 0.01% 41 6.73% Thallium (Tl) Mass Number Natural Abundance 203 29.52% 205 70.48%
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