1 / 26

Unit 5 Notes

Unit 5 Notes. Chemistry Mr. Nelson 2009. Chemical Bonds. Today we will learn about ionic bonds Ionic Electrostatic attraction between ions. Why do atoms bond?. Why DON’T some atoms bond? The noble gases – why? Why do other atoms bond, then? They are more chemically stable when bonded.

monte
Download Presentation

Unit 5 Notes

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Unit 5 Notes ChemistryMr. Nelson 2009

  2. Chemical Bonds • Today we will learn about ionic bonds • Ionic • Electrostatic attraction between ions

  3. Why do atoms bond? • Why DON’T some atoms bond? • The noble gases – why? • Why do other atoms bond, then? • They are more chemically stable when bonded

  4. How do atoms bond? • The octet rule • The octet rule, or rule of eight, says that an atom will strive for a full s and p subshell • Atoms will either lose or gainelectrons to get 8 in the outer shell • NOTE: when an atom loses or gains electrons, it’s nucleus remains the same – only the outer electron shell has changed!!!

  5. Bonding and energy changes • Energy is the ability to do work • Stability is a measure of inability to do work • So, the lower the energy, the more stable something is! • When atoms bond, the process favors stability (lower energy). Things will never go from a stable to an unstable state on their own!

  6. Electrons, bonding, and IONS • When they do this, they get a CHARGE, because protons (+) and electrons (-) are no longer equal. They are now IONS • Positive and negative IONS come together and balance each other out in IONIC BONDS.

  7. + + + Cations and Anions • Remember: An “antion” A “plussy cat”

  8. Ionic Bonding • Sodium wants to GIVE an electron, Chlorine wants to GET an electron.

  9. Ionic Bonding • The low ionization energy of sodium and the high electronegativity of chlorine is one reason this works so well.

  10. Naming ions • Monatomic ions = • One atom ions • Naming monatomic ions • To name positive ions, just add the word “ion” • Example: Magnesium’s ion is Magnesium ion • To name negative ions, drop the last part of the word, and add “-ide ion” • Oxygen’s ion is called oxide

  11. Naming monatomic ions

  12. Compounds made of two monatomic ions • These are called BINARY COMPOUNDS • You always put the positive part first and the negative part last: Na+ + Cl- NaCl • Names = name of the positive ion + name of the negative ion: Sodium Chloride

  13. Examples: Name the following

  14. Back to ions: Writing Ionic Formulas • The nomenclature (naming system): • Write the symbols for the ions side by side. Write the cation first. Al3+ O2- • Find the lowest common multiple that will make the charges on each ion cancel out Al3+ O2- • Check the subscripts for the lowest whole number ratio of ions. Then write the formula. Al2O3

  15. Write the formulas of the following:

  16. d-block • The d-block (yo) has its own rules • Metals in the d-block have variable charges • All d-block metals must get a ROMAN NUMERAL to indicate the charge • EXAMPLE: copper (I) chloride is made of Cu1+ and Cl- • EXAMPLE: copper (II) chloride is made of Cu2+ and Cl- • Don’t use roman numerals if you don’t have to

  17. Examples • Write the formulas for • Tin(II) iodide • Cobalt(III) chloride

  18. Working backward • If you are given the formula you need to calculate the charge of the d-block metal. • Assume the anion did not change its charge (they are very consistent) • Example: FeO, to write the name we need the charge of iron.

  19. A few more examples • PbS2 • MnBr3 • Cu3P2

  20. Polyatomic ions • When two or more ions are clumped together it is a polyatomic ions. • They usually end with –ates or -ites

  21. Nomenclature of Oxyanions • They are not standard! • Example Sulfate vs Phosphate • Nomenclature examples • Perchlorate • Chlorate Nitrate • Chlorite Nitrite • hypochlorite

  22. Writing formulas for compounds with polyatomic ions • Polyatomic ions should ALWAYS be treated like a LUMP. Don’t ever break it up! • If you need more than one polyatomic ion to balance a charge, use PARENTHESES ( )

  23. Polyatomic ions • Naming compounds that contain polyatomic ions: • The steps are the same: • the name of the first ion + the name of the second: • NH4+ = ammonium ion (polyatomic) • Cl- = chloride ion (monatomic) • NH4Cl = ammonium chloride

  24. Example • Write the formulas for: • potassium perchlorate • tin(IV) sulfate • Iron(II) chromate • ammonium sulfate

  25. Ionic vs. Metallic bonds • In an IONIC BOND, the electrons of one atom (that wants to lose electrons) are donated to the electrons of another atom (that wants to gain electrons). The charges on each ion balance each other out and equal ZERO. • In a METALLIC BOND, all the atoms are the same (all copper, for example) and the electrons don’t belong to any one atom. They move around a lot – that’s why electricity is conducted.

  26. Metallic Bonds • A “sea” of mobile outer electrons. • Low ionization energies means the atoms don’t hold electrons well.

More Related