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Atoms, Molecules and Ions

Atoms, Molecules and Ions

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Atoms, Molecules and Ions

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  1. Atoms, Molecules and Ions H.ImamRachmat,spd

  2. Objectives • To define the meaning of particles of matter (atom, ion and molecule) • To explain the difference of isotope, isotones and isobar • To explain the difference between the element molecule and the compound molecule • To mention some examples of simple molecules in daily life • To give examples of substances that consist of ions

  3. Particles of matter On grade VII you learned that all matters around us are made up of fundamental matter called ELEMENT. Element is a simple substance whch cannot be broken down into simpler subtances • Look at the figure ! A piece of iron is composed of a mass of iron atoms

  4. What is an atom??? • Atom is the smallest unit of an element, having the properties of that element. Democritus’s model ( the father of atomic theory) Fe Fe Fe Fe Fe Fe Fe This is atom Fe ( iron )

  5. How has the model of the atom changed over time ? • John Dalton, an English schoolteacher in the early nineteenth century, combined the idea of elements with the earlier theory of the atom. • He proposed the following ideas about matter: • Matter is made up of atoms, • Atoms cannot be divided into smaller pieces, • All the atoms of an element are exactly alike • Different elements are made of different kinds of atoms. • Dalton’s Concept Dalton’s model 1807

  6. Thomson’s model 1903 • Atom is continuous mass of positive charge containing negative electron Raisin pudding model

  7. Rutherford’s model 1903 • Atom has a nucleus surrounded by electron e- e- e- e- e- e- e- e- e-

  8. Niels Bohr’s model 1913 • Atom has a nucleus. Electrons move in fixed orbits around the nucleus e- nucleus e- e-

  9. Structure of atoms • THE STRUCTURE OF ATOMS • Atoms are made up of three subatomic • particles • Protons carry positive charge • Neutrons having no charge • Electrons carry negative charge • The protons and neutrons are tightly bound together to form the central portion of an atom called the nucleus. • The electrons are located outside of the nucleus and thought to move very rapidly throughout a relatively large volume of space surrounding the small but very heavy nucleus.

  10. The comparison of particles in atom

  11. Atomic Mass

  12. ISOTOPES Isotopes are atoms with the same atomic numbers but different mass numbers. EXAMPLES • Hydrogen • Chlorine • Carbon

  13. ISOBAR Atoms of different elements might have the samemass number. ISOTONES EXAMPLES Atoms of different elements might have the same number of neutron • EXAMPLES

  14. Electron Arrangement • According to Bohr, electrons move around the nucleus in fixed orbit or shells • The electron in each shell have different energy level. The shells closes to the nucleus have lower energy levels than those farther away • The biggest atoms can have up to 7 electron shells, • However, each shell can contain only a limited number of electrons. This number depends on their size: • 1st shell maximum filled with 2 electrons. • 2nd shell maximum filled with 8 electrons. • 3rd shell can hold up to 18electrons, but normally only holds up to 8 to make atom more stable. • 4th shell can hold up to 32electrons but, like the third shell, normally holds only up to 8 to make atom more stable

  15. Example of Electron arrangement • Sodium Electronic Configuration: 2, 8, 1 1st shell 2nd shell 3rd shell Electronic Structure Σp=11 Σe=11 Σn=12 The electron in the outermost shell of an atom are called the outer electron or valency electrons Sodium has 1 valency electron

  16. ions Ion is an atom having electric charge Loses electrons + Positive ion atom • When atoms lose or gain electrons, they become ions _ Negative ion Gains electrons An atom may gain or lose electrons

  17. cation– ion with a positive charge If a neutral atom loses one or more electrons it becomes a cation. 11 protons 11 electrons 11 protons 10 electrons Na+ Na 17 protons 18 electrons 17 protons 17 electrons Cl- Cl anion– ion with a negative charge If a neutral atom gains one or more electrons it becomes an anion.

  18. Predicting Ionic Charge • Metals tend to form cations (group 1 and 2) • Non-metals tend to form anions.(group 5, 6, 7 ) Be2+

  19. A monatomic ion contains only one atom Na+, Cl-, Ca2+, O2-, Al3+, N3- A polyatomic ion contains more than one atom OH-, CN-, NH4+, NO3- 2.5

  20. 1. Why do atoms bond together? Atoms bond to become more stable,like Noble Gases.

  21. 1. Ionic bonds • Ionic bonds are formed by one atom transferring electrons to another atom to form ions. • Ionic Compound – A compound that contains positively charged ions and negatively charged ions.  +

  22. Ionic Compounds • often a metal + nonmetal • anion (nonmetal), add “ide” to element name barium chloride BaCl2 potassium oxide K2O Mg(OH)2 magnesium hydroxide potassium nitrate KNO3 2.7

  23. +  + 2. Covalent Bonding • Covalent bonds are formed by atoms sharing electrons to form molecules. • This type of bond usually formed between two non-metallic elements.(between 2 gass) Example: • Two hydrogen atoms (1) form the molecule of the element hydrogen H2 • Two chlorine atoms (2.8.7) form the molecule of the element chlorine Cl2

  24. Another examples of covalent bond: • Oxygen (o2) • Water (H2O) • Ammonia (NH3) • Carbon Dioxide (CO2)

  25. Comparison properties of ionic and covalent compound

  26. C. Molecule A molecule is made up of two or more atoms chemically combined together. Molecules of Element • Molecules are made up of the same kinds of atoms Molecules of Compounds • Molecules are made up of two or more different kinds of atoms


  28. The using of ions and molecules in chemical product in daily life