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Covalent Bonding Lewis dot structures

Covalent Bonding Lewis dot structures. Covalent Bonding - Bohr. Atoms overlap slightly, and one unpaired electron from each atom will pair together Both a toms are attracted to the same pair of electrons forming a covalent bond. 1 shell 2 shells 3 shells 4 shells. COVALENT COMPOUNDS.

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Covalent Bonding Lewis dot structures

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  1. Covalent Bonding Lewis dot structures

  2. Covalent Bonding - Bohr • Atoms overlap slightly, and one unpaired electron from each atom will pair together • Both atoms are attracted to the same pair of electrons forming a covalent bond

  3. 1 shell 2 shells 3 shells 4 shells

  4. COVALENT COMPOUNDS • Covalent bonds form when electrons are shared between two nonmetals. • Electrons stay with their atom but overlap with other shells. • Ex. H2O Shared electrons! Shared electrons!

  5. BOHR DIAGRAMS OF COVALENT COMPOUNDS Try it on your own! • HF • NH3 • CH4

  6. BOHR DIAGRAMS OF COVALENT COMPOUNDS Bonding electrons are shared. • Examples: HF; NH3; CH4

  7. WHAT IS A LEWIS DIAGRAM? • Lewis diagrams represent the atom of an element by showing only the outer valance electrons and the chemical symbol.

  8. Except for the transition elements (Groups 3–12), the last digit of the group number equals the number of e-s in the valence shell. Examples: • Group 1 = 1 valence electron • Group 2 = 2 valence electrons • Group 13 = 3 valence electrons • Group 14 = 4 valance electrons • Group 15 = 5 valence electrons • Group 16 = 6 valence electrons • Group 17 = 7 valence electrons

  9. WHAT IS A LEWIS DIAGRAM? • Dots representing electrons are placed around element symbols at the points of the compass (north, east, south and west). • Electron dots are placed singly first, until the 5th electron is reached and then they are paired.

  10. LONE PAIRS AND BONDING ELECTRONS • Pairs of electrons in Lewis Dot Diagrams are called LONE PAIRS. • Single electrons are called BONDING ELECTRONS – because they are looking for another electron to bond with!

  11. HOW MANY LONE PAIRS?

  12. Try it yourself! • Draw lewis dot structures for • HF • NH3 • CH4

  13. DIATOMICS – BECAUSE SOME ATOMS JUST CAN’T STAND TO BE ALONE There are 7 diatomics: • iodine (I2) • bromine (Br2) • chlorine (Cl2) • fluorine (F2) • oxygen (O2) • nitrogen (N2) • hydrogen (H2)

  14. IONIC COMPOUNDS • Ionic bonds are formed when electrons are transferred from a metal ion (cation) to a non-metal ion (anion). • Example: NaCl(s), FeCl2 (s) • Ionic Compounds are easy to recognize – they always contain a metal and a nonmetal.

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