1 / 17

Warm-up

Warm-up. Determine the number of valence electrons and the charge of an atom of these elements: Example: Chlorine: 7 valence electrons and -1 charge Beryllium Be: 2 valence and Be +2 Sulfur S: 6 valence and S -2 Fluorine F: 7 valence and F -1 Oxygen O: 6 valence and O -2. Bonding.

iain
Download Presentation

Warm-up

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. Warm-up • Determine the number of valence electrons and the charge of an atom of these elements: • Example: Chlorine: 7 valence electrons and -1 charge Beryllium Be: 2 valence and Be+2 Sulfur S: 6 valence and S-2 Fluorine F: 7 valence and F-1 Oxygen O: 6 valence and O-2

  2. Bonding Unit Four, Day One Kimrey 27 February 2013

  3. Chemical Bonding Its what happens when elements fall in love!

  4. 3 Types of Bonds • Covalent bonding • Ionic bonding • Metallic Bonding

  5. Bond Definitions • Covalent bonds – electrons are shared • Polar covalent bonds – electrons are shared unequally • Non-polar covalent bonds – electrons are shared equally • Ionic bonds – electrons are transferred • Metallic bonds – electrons float between the two atoms

  6. Electronegativity • You should know this definition!!! • Scale of 0-4 • Differences in electronegativity is used to determine the type of bond. 0 - 0.3 = Nonpolar covalent 0.3 - 1.7 = Polar Covalent 1.7 - 4.0 = Ionic • Example: Sodium bonded to bromine

  7. Practice • Identify the following bonds as polar or non-polar covalent: • Hbonded to H • H bonded to C • F bonded to F • C bonded to N

  8. Covalent Bonding-The perfect relationship • Bond is formed by the sharing of electrons between two nonmetals. • Two types of covalent bond polar and nonpolar. • Polar covalent bond- unequal sharing of electrons. • Occurs when the two non-metals are different • Nonpolar covalent bond- equal sharing of electrons. • Occurs when the two non-metals are the same

  9. Ionic bonding-The stage five clinger • One element steals all the electrons from another. -or more technically • A transfer of valence electrons between a cation (+) and an anion (-). • Between a metal and nonmetal or a metal and polyatomic ion. ex. NaCl, LiF, CaF2 • Polyatomic ion- a group of bonded atoms that have a charge. ex. OH-, SO42-, etc.

  10. Metallic Bonding-when two people merge into one. • Between two metals and forms a sea of mobile electrons. • Attraction between the positive nucleus and surrounding electrons. • Forms a sea of mobile electrons. • This is why metals are malleable and ductile. • Electrons don’t belong to either element – instead just float around the nuclei

  11. CATION ANION Answer these questions: An atom that gains one or more electrons will have a ____________________ charge. An atom that loses one or more electrons will have a ____________________ charge. An atom that gains or loses one or more electrons is called an ____________. A positive ion is called a ______________ and a negative ion is called an _______________. NEGATIVE POSITIVE ION

  12. What is an ionic bond? Atoms will transfer one or more ________________ to another to form the bond. Each atom is left with a ________________ outer shell. An ionic bond forms between a ___________ ion with a positive charge and a ________________ ion with a negative charge. Example B1: Sodium + Chlorine Example B2: Magnesium + Iodine ELECTRONS COMPLETE METAL NONMETAL

  13. What is a covalent bond? Atoms ___________ one or more electrons with each other to form the bond. Each atom is left with a ________________ outer shell. A covalent bond forms between two _________________. Example C1: Hydrogen + Hydrogen Example C2: 2 Hydrogen + Oxygen SHARE COMPLETE NONMETALS

More Related