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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?.

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Bonding Basics

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  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

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