1 / 22

Bonding Basics

Bonding Basics. Bell Work 11/15. 6CF₄ How many Carbon atoms are in the above molecule. How many Flourine atoms are in the above molecule? C₆H₁₂O₆ How many Carbon atoms are in the above molecule. How many Hydrogen atoms are in the above molecule?.

sammy
Télécharger la présentation

Bonding Basics

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. Bonding Basics

  2. Bell Work 11/15 6CF₄ • How many Carbon atoms are in the above molecule. • How many Flourine atoms are in the above molecule? C₆H₁₂O₆ • How many Carbon atoms are in the above molecule. • How many Hydrogen atoms are in the above molecule?

  3. An atom that gains one or more electrons will have a negative charge. • An atom that loses one or more electrons will have a positivecharge.

  4. Ions • An atom that gains or loses one or more electrons is called an ion.

  5. 2 Types of Bonds • Ionic Bond • Covalent Bond

  6. Ionic Bond • A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion. In this example, will sodium have a positive or negative charge?

  7. 2 Types of Ions • A positive ion is called a cation • A negative ion is called an anion

  8. Polyatomic Ions • Polyatomic ions: ions that are made of more than one atom • Ex. An ammonium ion is made of nitrogen and hydrogen atoms.

  9. Covalent Bond • Atoms share one or more electrons with each other to form the bond. • Each atom is left with a complete outer shell.

  10. Covalent Bond

  11. Covalent Bond • Double bond: two atoms share two pairs of electrons

  12. Covalent Bond • Triple bond: atoms share three pairs of electrons

  13. Covalent Bond • Atoms of some elements pull more strongly on shared electrons than do atoms of other elements. As a result, the electrons are pulled more toward one atom, causing the bonded atoms to have slight electrical charges. • Polar bond: a covalent bond in which electrons are shared unequally • Nonpolar bond: a covalent bond in which electrons are shared equally

  14. Covalent Bond • Covalent bonds usually form between atoms of nonmetals. • In contrast, ionic bonds usually form when a metal combines with a nonmetal.

  15. Chemical Formulas • Subscript: tells you the ration of elements in the compound. • Ex. MgCl₂ • This means that for every magnesium ion there are two chloride ions. • Ex. CaCO₃ • This means one calcium, one carbon, and three oxygen ions.

  16. Chemical Formulas • If no subscript is written, the number 1 is understood. • Ex. NaCl • This means there is one chloride ion for every sodium ion (1 to 1 ratio).

  17. Chemical Formulas • Superscripts are the big number in front of an atom or molecule. They tell you how many atoms there are of that element. • Ex. 4H • This means four atoms of hydrogen.

  18. Chemical Formulas • When a superscript is in front of a molecule, it multiplies the whole molecule. • 3H₂O • Here there are 6 hydrogens and 3 oxygens • Basically like this: HHO HHO HHO

  19. Naming Covalent Bonds N2S4 dinitrogen tetrasulfide XeF6 xenon hexafluoride P2O5 diphosphoruspentoxide SO3 sulfur trioxide

More Related