1 / 25

Chemical Bonds

Chemical Bonds. Chapter 20. Sec. 1 - Combined Elements. Elements make  ________________ Properties of compounds are different from ______________ Ex: Sodium Chloride, __________ (table salt) Na: silver, metal, reacts violently w/ _____ Cl: _______________ greenish-yellow gas.

lorand
Download Presentation

Chemical Bonds

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. Chemical Bonds Chapter 20

  2. Sec. 1 - Combined Elements • Elements make ________________ • Properties of compounds are different from ______________ • Ex: Sodium Chloride, __________ (table salt) • Na: silver, metal, reacts violently w/ _____ • Cl: _______________ greenish-yellow gas

  3. Chemical Formulas • H2O  ___ atoms H and 1 atom O

  4. Atomic Stability • Why do atoms form compounds? • To be ______________ • Why don’t noble gases form compounds? • Stable!  __________ energy levels!! • All atoms form compounds to get FULL ________________ LEVELS  stable

  5. Atomic Stability

  6. Atomic Stability • 1st energy level full with ______ e- • Other levels full with ______ e-

  7. Stability is Reached • NaCl is made from atoms ___________ or gaining electrons • H2O is different  elements _________ electrons • Both ways make a… • Chemical ______________: force that holds atoms together in a compound

  8. Types of Bonds Section 2

  9. Ionic Bonds • Atoms can lose or ____________ e- to make an ion • ____________: a charged particle because it now has either more or fewer e- than p+ • ______ charge: if fewer e- than p+ • ______ charge: if more e- than p+

  10. Calcium Oxide - CaO • Calcium has __ valence e- • ___________ 2 e- and becomes an ion • Ca+2 • Oxygen has __ valence e- • ____________ 2 e- and becomes an ion • O-2 • Calcium ___________ e- to Oxygen • Opposite charges ATTRACT!!

  11. Ionic Bond – Metal and Nonmetal • Def: the force of attraction between ________________ charges of the ions • Ex: MgCl2 – ___________ net charge • Smallest Particle = formula _________

  12. Covalent Bond – 2 Nonmetals • Def: attraction between atoms when they _____________ electrons • Smallest particle = ______________ • H2O • CO2 • N2

  13. Covalent Bonds • Single Covalent Bond: ______ shared electrons • Multiple Bonds: • Double (____ shared e-) • Triple (_____ shared e-)

  14. Naming Compounds Section 3

  15. Naming Ionic Compounds • Binary compound: has ____ elements • Ionic compounds – name of _______ makes name of compound • ____________ Ions: name of element • Na+ = Sodium ion • Negative ions end in – _________ • Cl- = Chloride ion

  16. Special Ions

  17. Polyatomic Ions

  18. Sec. 3 – Writing Formulas • Remember… compounds are __________________!! • Write the (_____) ion • Write the (_____) ion • _____________ charges: criss-cross method • ______________ to smallest whole #s

  19. Write the Formula • Lithium Nitride • Lead(IV) Phosphide • Calcium Fluoride • Ammonium Phosphate • Magnesium Hydroxide

  20. Naming Ionic Compounds • Put the two ion names together! • NaCl • Na+ = _____________ ion • Cl- = ______________ ion • Sodium Chloride

  21. Practice Naming • RbCl • Mg3N2 • AlF3 • CrCl3 • Ca(OH)2 • Na2CO3 • NH4Cl

  22. Naming Covalent Compounds • _______ ions involved • Same ______________ can make different compounds: CO, CO2 • Naming: Use ______________ to tell how many atoms of each element • Second element ends in -_________ • Prefix ___________ is left out with the first element

  23. Prefixes

  24. Practice Naming • N4O6 • C2O5 • PH3 • Sulfur Hexafluoride • Dihydrogen Monoxide

  25. Hydrates • Def: has water chemically attached to its ions • CoCl2• 6H2O • ___________________________ • CaSO4 • 2H2O • ___________________________

More Related