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Electron Shells

Electron Shells. First Shell, maximum 2 electrons. Third shell, max # 8 electrons, (in this case, the last, so called the Valence Shell.). Second Shell, Maximum 8 electrons. Charges. The outer electrons on an atom are called: Valence electrons .

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Electron Shells

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  1. Electron Shells First Shell, maximum 2 electrons Third shell, max # 8 electrons, (in this case, the last, so called the Valence Shell.) Second Shell, Maximum 8 electrons

  2. Charges • The outer electrons on an atom are called: Valenceelectrons. • Atoms want an ASCVI Diagram that looks like a Noble Gas because… • Noble Gases have the most stable structure. • Usually, this means the atom ends up with a Charge.

  3. Ions • Ion= a Charged atom in which the number of ELECTRONS (-) is different from the number of PROTONS (+). • Ionic Charge= is the number of positive (+) or negative (-) Charges on an atom. Ex: Mg+2

  4. Groups Mg Be (Berylium)

  5. So… • Even though each element has a different # of PROTONS and ELECTRONS, each element in a group has a similar Bohr-Rutherford Diagram. • This means they want to gain or losethe same number of Electrons. • It also means elements in a Group will react similarly in Chemical Reactions.

  6. Group Name and Number Akali Metals Akaline Earth Metals Noble Gases Halogens Transition metals

  7. Cl & Na • Chlorine Gas is poisonous. • In terms of electrons, what does Chlorine want to do? • -Gain an electron. So what would the Charge be? • Would you eat Na? • In terms of electrons, what does Sodium want to do? • Lose an electron. So what would the Charge be?

  8. Cl & Na, cont’d • What would happen if we put Na and Cl together? • We get NaCl, a.k.a.: • SALT!

  9. Salt, what has Happened? • Sodium (Na) gave up its Valenceelectron to the Chlorine (Cl). Na + Cl Na+1 + electron + Cl Na+1 + Cl-1 NaCl • Why do you think they are now written together? Why are there no Charges?

  10. Ionic Bonding • Positives will be attracted to Negatives. The force of the attraction between a Positively Charged Ion and a Negatively Charged Ion is called an IONIC BOND. • When two Ions Bond, they form an Ionic Compound. Ex. NaCl • Check your new textbook…

  11. Ionic Compounds • PositiveIon is called a CATION. • Negative Ion is called an ANION. • Write down 2 other cations and anions that you think would fit together

  12. Ionic Compounds • Notice the cross over of Charges • The Cation is always written FIRST, Anion Second. • Ionic compounds are made up of metals and non-metals, the metal is written FIRST.

  13. Formation of Ionic CompoundsCrossing Rule Ca+2+ Cl-1 CaCl2

  14. Ionic Structure • Ionic Compounds:Compounds made up of positive and negativeions that have resulted from the transfer of electrons from a metal to a non-metal.

  15. Naming Ionic Compounds • Regular names: • Write the name of the metal first • Replace the ending of the non-metal with –ide • eg. Mg3P2 → Magnesium Phosphide

  16. Naming Ionic Compounds • Transition Metals: • When a metal can form more than one type of ion • State the charge using a Roman numeral • eg. CuBr → Copper I Bromide • Eg. CuO → Copper II Oxide

  17. Naming Ionic Compounds • Acids: • Recognized by the H+ ion out front (but not like in water, H2O, that’s covalent) • Name it using the non-metal, but with the ending -ic • eg. HCl → Hydrochloric acid • Eg. HF → Hydrofluoric acid • Try HI → Hydroiodic acid

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