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Presentation On Ions And Ionic Bonds

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Published in: Chemistry
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This PPT is suitable for the IGCSE and O Level Chemistry students. It only provides theoretical background of the topic. The practice questions, worksheets and topical questions will be discussed during the tutoring sessions

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  1. Ions and Ionic Bonds Chemistry (IGCSE / O-Level)
  2. What will you learn in this lesson? • Formation of cations and anions • Ionic bonding between metals and non-metals • Dot-and-cross representation of ionic compounds • Physical properties of ionic compounds
  3. Formation of Ions • Ion is an electrically charged particle which are formed when atom lose or gain electrons • Atoms transfer electrons to achieve stable state that is similar to the nearest noble gas electronic configuration an atom of sodium an ion of sodium, Na• Hen ihe sodium atom loses an electron, It forms a sodium ion. • Sodium ion is positively charged (+1) because of greater number of protons in its nucleus than electrons
  4. Formation of Ions (contd.) • The chloride ion is negatively charged (-1) because it has more electrons (18) as compared to protons in the nucleus (17) • The ease with which Group I (alkali metals) and Group Vll (halogens) elements loose and gain electrons make them very reactive [2871 ion of:eblot'ioe
  5. Ionic Bonding • Compounds between metals and non-metals involve a type of bonding known as ionic bonding • Electrons are transferred from one atom to another forming ions. These ionic compounds are held together by electrostatic force of attraction between opposite charges sodium Chloride (NCI) In this case, Nat and Cl- ions are formed and held together by electrostatic force of attraction
  6. Ionic Bonding (contd.) Important Features: The electrons involve in the formation of ions are those in the outer shell of the atoms • Metal atoms lose their electrons to become positive ions (cations). In doing so they achieve the more stable electronic configuration similar to the nearest noble gas to them in periodic table. • Non-metal atoms (except hydrogen) gain electrons to become negative ions (anions). In doing so they achieve the more stable electronic configuration similar to the nearest noble gas to them in periodic table An ionic lattice where each ion is surrounded by oppositely charged ions
  7. Dot-and-Cross Representation [Mgr . magnesium oxide (MgO) 2- O Now represent the formation of ionic compound using any Group I alkali metal and Group Vll halogen non- metal using dot-and-cross Also represent the formation of CaC12 ionic compound using dot-and-cross
  8. Physical Properties of Ionic Compounds Of typical ionic They have high melting points and boiling points. They are crystalline solids at room temperature. They are Often soluble in water (not usually soluble in organic solvents, e.g. ethanol, methylbenzene). They conduct electricity when molten or dissolved in water (not when solid). for these prope Ions are attracted to each other by strong electrostatic forces. Large amounts of energy are needed to separate them. There is a regular arrangement of the ions in a lattice. Ions with opposite charge are next to each Other. water is attracted to charged ions and therefore many ionic solids dissolve. In the liquid or solution, the ions are free to move about. They can move towards the electrodes when a voltage is applied.

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