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BONDING

BONDING. For Beginners or Advanced Students of Chemistry. chapters 15 and 16 in your text book (check it out). COVALENT BONDING. This involves the sharing of valence electrons by 2 atoms. EXAMPLES INCLUDE BONDS BETWEEN: H 2 F 2 O 2 Cl 2 HCl H 2 O. oxygen molecule.

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BONDING

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  1. BONDING For Beginners or Advanced Students of Chemistry chapters 15 and 16 in your text book (check it out)

  2. COVALENT BONDING This involves the sharing of valence electrons by 2 atoms. EXAMPLES INCLUDE BONDS BETWEEN: H2 F2O2Cl2 HCl H2O oxygen molecule

  3. these are NOT ionic bonds Ionic bonds ONLY happen with cations and anions (metals and non-metals)

  4. In a chlorine molecule, each of the atoms shares a pair of electrons circled in GREEN. They make a covalent bond. Since it’s just one pair being shared, this is a SINGLE COVALENT BOND. Each of the chlorine atoms also has three pairs each of UNSHARED ELECTRONS. THEY BOTH GET AN OCTET BY SHARING.

  5. unshared electrons When electrons are written into the Lewis diagrams, they are usually paired. The electrons prefer pairs. When they share themselves with other atoms, one electron from each atom connects together, making a SINGLE BOND. Electrons not involved in bonding are mostly paired away from the bond. They are the “unshared” electrons.

  6. Water has two hydrogen atomsbonded to one oxygen atom. It has 2 single polar covalent bonds. The oxygen has 2 pairs of unshared electronsas well.Oxygen gets the octet.

  7. ammonia NH3 has three single covalent bonds, and nitrogen has one unshared pair of electrons. Nitrogen gets the octet. Nitrogen’s electrons are RED and the Hydrogen electrons are inBLUE. Ammonia is a polar molecule because it does not exhibit RADIAL SYMMETRY. there are 2 unshared electrons of nitrogen down here

  8. methane Methane has FOUR single covalent bonds, and that leaves the carbon atom without any unshared pairs of electrons. THiS MOLECULE IS NON-POLAR because it has RADIAL SYMMETRY. Its shape is called TETRA-HEDRAL

  9. When 2 oxygen atoms combine to form a molecule, each shares a pair of electrons with the other so BOTH GET AN OCTET. This is a DOUBLE Non- Polar COVALENT BOND

  10. This is a dot diagram of nitrogen… Diatomic Nitrogen makes a TRIPLE COVALENT BOND and each atom keeps one pair of UNSHARED ELECTRONS.

  11. POLAR BONDS Polar bonds happen when ever atoms with large electro-negativity differences connect. The electrons are not shared evenly, they get taken more often by the one atom with the HIGHER EN value. COVALENT BONDS can be polar. IONIC BONDS ARE ALMOST ALWAYS POLAR.

  12. This is the SULFITE (–2) ion By gaining 2 electrons all together, sulfur as well as the three oxygen atoms end up with a complete octet. This poly atomic ion acts as a negative 2 ion. Sometimes in these Lewis dot diagrams, we use dots as well as X’s. The X’s just indicate electrons from the “other” atoms or ions. Although this is an anion that can bond ionically to a metal cation, the bonds in this anion are COVALENT.

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  14. bond polarity Bonds can be polar or non-polar. If a bond is non-polar, that means that there is a sharing of electrons, making for a positive side and a negative side of the bond. If a bond is polar, that means that the electrons are not shared equally, making one side of the bond more negative (where the electrons end up) and the other side more positive (where the electrons were).

  15. HCl is a polar covalent bond. It is NOT an Ionic bond, which are ONLY between metals and non-metals. Hydrogen and chlorine are both non-metals. Water also has polar covalent bonds between the H and the O. The oxygen is very attracted to the electrons of hydrogen, so they take them away, making an octet. The hydrogen side of the molecule ends up more positive while the oxygen side is more negative.

  16. MOLECULAR POLARITY a molecule can also be polar, if the molecule does not exhibit RADIAL SYMMETRY. this is water The oxygen side is negative since it takes the electrons, the hydrogen side is more positive because it lost the electrons.

  17. Sort of like, but not really like these love birds, molecules can also be attracted to each other. Different forces make them stick together. Love is not one of the forces. Neither is nesting instinct. But it really was a nice picture to use.

  18. Ionic Bonding requires a METAL and a Non-METALorrequires a CATION and an ANION this is NaCl

  19. IONIC BONDS DO NOT SHARE ELECTRONS!!! THE IONS STICK TOGETHER BECAUSE OF THE OPPOSITE CHARGES THAT ARE ATTRACTED TO EACH OTHER.

  20. aluminum oxide Aluminum oxide is an IONIC COMPOUND made up of 2 aluminum cations (each +3) and three oxygen anions (each –2). All of these five ions make up the LEWIS DOT DIAGRAM FOR THIS IONIC COMPOUND.

  21. Sodium chloride is made up of 2 ions, the sodium cation that GIVES UP one electron, and the chloride anion that ACCEPTS that electron from sodium. The Lewis Dot diagram shows the sodium with no valence electrons but with a bracket and a charge. The chlorine ion now has 8 electrons in the valence orbital, and the charge coincides with that fact. Lewis Dot diagrams of IONS and IONIC COMPOUNDS and require BRACKETS

  22. Enough with this IONIC BONDING, I’m SATURATED already!

  23. Metallic Bonding This of course only happens with METALS. It is REAL BONDING, but only between the atoms metals. note the multiple cations surrounded by that “sea” of loose valence electrons!

  24. Metal Properties are all because of METALLIC BONDING::: The bonding allows metals to be MALLEABLE, DUCTILE, and to conduct electricity well.

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