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H 2 O

H 2 O.

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H 2 O

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  1. H2O

  2. Valence Electrons: the electron(s) in the outer shell of an atom’s electron cloud, which can combine with other atoms to form molecules*The number of valence electrons in an atom of an element determines many properties of that element, including the ways in which the atom can bond with other atoms.

  3. Chemical bonds hold molecules together . A chemical bond is a union between atoms formed when they give up, gain, or share electrons .

  4. 3 types of bonds • Ionic • Covalent –Non-polar –Polar • Hydrogen

  5. Ions and Ionic Bonds You and a friend walk past a market that sells apples for 40 cents each and pears for 50 cents each. You have 45 cents and want an apple. Your friend also has 45 cents but wants a pear.

  6. Ions and Ionic Bonds When an atom loses an electron, it loses a negative charge and become a positive ion. When an atom gains an electron, it gains a negative charge and becomes a negative ion.

  7. Ions and Ionic Bonds •An atoms gives up 1 or more of its electrons to another. •The resulting oppositely charged ions attract one another, forming an ionic bond.

  8. Ions and Ionic Bonds For example, in table salt (sodium chloride) the negative chlorine ion attracts the positive sodium ion, forming an ionic bond.

  9. Covalent Bonds • A covalent bond holds together two atoms that share one or more pair of electrons • Electrons in a covalent bond may be equally or unequally shared between the atoms. • Non-polar covalent bond: atoms share electrons evenly • Polar covalent bond: atoms share electrons unequally

  10. Covalent Bonds Those atoms with greater positive nuclear charge pull more strongly on electrons in a covalent bond.

  11. . A carbon dioxide molecule is a nonpolar molecule because of its straight-line shape. In contrast, a water molecule is a polar molecule because of its bent shape.

  12. Covalent Bonds H2O is a polar molecule –The (slightly) positively charged pole is around each hydrogen –The (slightly) negatively charged pole is around the oxygen

  13. Graphic Organizer Polar Covalent Bond Nonpolar Covalent Bond Metallic Bond Feature Ionic Bond Attraction between positive ions and surrounding electrons. Attraction between oppositely charged ions How Bond Forms Equal sharing of electrons Unequal sharing of electrons Charge on Bonded Atoms? Yes, slightly positive or slightly negative Yes; positive or negative No Yes; positive H2O molecule (or other polar covalent molecule) NaCl crystal (or other ionic compound) Example Calcium (or other metal) O2 molecule

  14. Hydrogen Bonds Polar molecules have partially charged atoms at their ends. Hydrogen bonds form when partial opposite charges in different polar molecules attract each other. Individual hydrogen bonds are rather weak, but collectively they are quite strong

  15. Self Quiz Do atoms always have an equal number of protons, neutrons and electrons? 1.Yes. 2.No. A chemical bond is formed through: 1.The gaining, losing, or sharing of protons. 2.The gaining, losing, or sharing of neutrons. 3.The gaining, losing, or sharing of electrons. 4.The gaining, losing, or sharing of isotopes. 5.The gaining, losing, or sharing of ions.

  16. Self Quiz After sodium loses an electron, it is: 1.A positive ion. 2.A negative ion. 3.A neutral ion. 4.An isotope. 5.A compound. After chlorine gains an electron, it is: 1.A positive ion. 2.A negative ion. 3.A neutral ion. 4.An isotope. 5.A compound.

  17. Self Quiz What is the difference between a nonpolar covalent bond and a polar covalent bond? 1.A polar covalent bond results when there is unequal sharing of electrons in a molecule, whereas electrons are shared equally in a nonpolar covalent bond. 2.A polar covalent bond has two equal sides and a nonpolar covalent bond has two different sides. 3.A nonpolar covalent bond is positively charged and a polar covalent bond is negatively charged. 4.A polar covalent bond is positively charged and a nonpolar covalent bond is negatively charged.

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