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IONS https:// youtube/watch?v=WWc3k2723IM UNIT 1B.10

IONS https:// www.youtube.com/watch?v=WWc3k2723IM UNIT 1B.10. Ionic Bonding https :// www.youtube.com/watch?v=hiyTfhjeF_U. The Bohr Model of the Atom. Electrons of hydrogen circle the nucleus in orbits 1. orbits have a fixed amount of ______ in the ground state

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IONS https:// youtube/watch?v=WWc3k2723IM UNIT 1B.10

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  1. IONShttps://www.youtube.com/watch?v=WWc3k2723IMUNIT 1B.10 Ionic Bonding https://www.youtube.com/watch?v=hiyTfhjeF_U

  2. The Bohr Model of the Atom • Electrons of hydrogen circle the nucleus in orbits 1. orbits have a fixed amount of ______ in the ground state 2. orbits are a fixed ________ from the nucleus 3.orbits furthest from the nucleus have the ________ energy

  3. Niels Bohr (1885 – 1962) Bohr Model of the Atom

  4. Bohr’s Model Nucleus Electron Orbit Energy Levels

  5. Bohr’s Model } • Further away from the nucleus means more ________. • There is no “in between” energy • Energy Levels Fifth Fourth Third Increasing energy Second First Nucleus

  6. IONS • An atom usually has a ______charge. That means it has the same number of _____ as ________ • Remember, a proton has a positive charge and an electron has a negative charge • ION – an atom that has lost or _____ one or more electrons and has become charged either ______ or ________

  7. Positive Ions • When an atom LOSES electrons, it becomes more _________ • Why? • If you are getting rid of ______ particles (electrons) but your number of positive particles (______) are staying the same. • In other words, you are subtracting negative numbers

  8. Examples • What would the charge be if: • The neutral form of Gold (Au) lost 4 of its 79 electrons. It now has 79 protons and _____electrons • The neutral form of Mg lost 2 of its 12 electrons. It now has __ protons and 10 electrons.

  9. Negative Ions • When an atom GAINS electrons it becomes more _________ • Why? • Electrons have a _______ charge, so the more you have, the more negative you become

  10. Representing Ions • Ions are represented by placing a “superscript” charge number next to the atomic symbol. • Ex. • O-2 = oxygen with a negative __charge • K+ = potassium with a ______ 1 charge • N-3 = nitrogen with a _______ 3 charge • And so on

  11. Keeping Track of Electrons 2. Atoms in the same column a. Have the same outer _______ configuration. b. Have the same ________ electrons. c. Easily found by looking up the group number on the ________ table. d. Group 2A - Be, Mg, Ca, etc.- 2 ________ electrons

  12. List the number of valence shell electrons are in each of the elements in groups • 1-2 13-18

  13. B. Electron Dot Diagrams: Lewis Structures 1. A way of keeping track of _______ electrons. 2. How to write them 3. Write the symbol. 4. Put one ___ for each valence electron 5. Don’t pair up until they have to X

  14. The Electron Dot diagram for Nitrogen • Nitrogen has __ valence electrons. • First we write the symbol. N • Then add __electron at a time to each side. • Until they are forced to pair up.

  15. Write the electron dot diagram for Na Mg C O F Ne He

  16. C. Ion Formation in Representative Elements Group Gain or Lose Charge of Ion 1 (1A) lose 1 +1 2 (2A) lose 2 +2 13 (3A) lose 3 +3 14 (4A) lose or gain 4* +4,-4* 15 (5A) gain 3 -3 16 (6A) gain 2 -2 17 (7A) gain 1 -1

  17. Electron Dots For Cations • Metals will have few valence electrons Ca

  18. Electron Dots For Cations • Metals will have few valence electrons • These will come ____ Ca

  19. Electron Dots For Cations • Metals will have few valence electrons • These will come off • Forming _______ions Ca+2

  20. D. Electron Configurations for Anions 1. Nonmetals gain _______ to attain noble gas configuration. 2. They make ______ ions.

  21. Electron Dots For Anions • Nonmetals will have many ______ .electrons. • They will gain electrons to fill _____ shell. P P-3

  22. E. Stable Electron Configuration 1.All atoms react to achieve noble gas configuration. 2. 8 valence electrons . 3. Also called the octet rule. Ar

  23. Write the electron configuration diagram label as anion or cation • Na • Mg • P • O • F • Cl • K

  24. quiz

  25. I. Properties of Ionic Compounds View Ionic video a. Crystalline structure. b. A regular ________ arrangement of ions in the solid. c. Structure is rigid.

  26. I. Chemical Bonds • A. The force that holds two atoms together. 1. Why do atoms form bonds? a. to acquire ___electrons in the valence shell (like noble gases 2. How do atoms form bonds? a. atoms may lose, ____ or share electrons to get 8 in the ______ shell

  27. A. Chemical Bond and valence electron 1.The electrons responsible for the chemical properties of atoms are those in the outer energy level: ____________________. a.Valence electrons - The electrons in the outer _______ level. b.Inner electrons -those in the energy _______ below.

  28. II. Ionic Bonding A. Anions and cations are held together by _________ charges. B. Ionic _________ are called salts. C. Simplest ratio is called the formula unit. D.The bond is formed through the transfer of __________. E. Electrons are transferred to achieve _____ gas configuration.

  29. Formation and Nature of Ionic Bonds F. 1. atom “M” loses electron(s)  ______ 2. atom “N” gains electron(s)  anion 3. cation and ______ attract each other a. electrostatic attraction 4. the electrostatic force that holds the oppositely charged ____ together is the ______ bond

  30. Sodium loses an electron forming a (+) ion. Chlorine gains an electron forming a ( - ) ion. ________ attraction between the (-) and (+) ion forms the ______bond between sodium and chlorine

  31. B. Ionic Compounds 1. compounds containing ______ bonds 2. types of ionic compounds a. oxides– metal + ________ Na2O, CaO, Al2O3, Fe2O3 b. salt – metal + _________ NaClCaFAgCl KI c. binary compounds – two elements 1)all of the compounds in a and b are binary compounds

  32. D. monoatomicion - ____atom 1) ex. K+ Fe3+ O2- N3- E. polyatomic ion – ion with more than one atom that acts as a _____ ion NO3- OH- SO42- NH4+

  33. III. Names and Formulas • Formulas for Ionic Compounds 1. vocabulary a. formula unit – simplest _____ of ions in a compound 1) ex. NaCl MgBr2 AlCl3 b.monoatomicion - ___ atom 1) ex. K+ Fe3+ O2- N3-

  34. B. Formulas For Ionic Compounds 1. write formula for the ______ first, then the ______ 2. use ________ to indicate number of ions (criss-cross the charges) a. sum of charges should equal 0 b. never change subscripts in __________

  35. Sodium Chloride Crystal

  36. Ionic Bonding Na Cl

  37. Ionic Bonding: Lewis Structure Na+ Cl -

  38. Ionic Bonding • All the electrons must be accounted for! Ca P

  39. Ionic Bonding Ca P

  40. Ionic Bonding Ca+2 P

  41. Ionic Bonding Ca+2 P Ca

  42. Ionic Bonding Ca+2 P-3 Ca

  43. Ionic Bonding Ca+2 P-3 Ca P

  44. Ionic Bonding Ca+2 P-3 Ca+2 P

  45. Ionic Bonding Ca Ca+2 P-3 Ca+2 P

  46. Ionic Bonding Ca Ca+2 P-3 Ca+2 P

  47. Ionic Bonding Ca+2 Ca+2 P-3 Ca+2 P-3

  48. Ionic Bonding Ca3P2 Formula Unit

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