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Bellringer

Bellringer. Draw a model for the following elements: A. Sodium B. Chlorine 2. How many valence electrons does sodium have? 3. If sodium lost its valence electrons, what would its charge be? 4. How many valence electrons does chlorine have?

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Bellringer

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  1. Bellringer • Draw a model for the following elements: • A. Sodium • B. Chlorine • 2. How many valence electrons does sodium have? • 3. If sodium lost its valence electrons, what would its charge be? • 4. How many valence electrons does chlorine have? • 5. If chlorine gained an electron, what would its charge be?

  2. Chlorine Sodium X X 1 A. 1 B. X X X X X X X X X X X P: 11 N: 12 P: 17 N: 18 X X X X X X X X X X X X X X X One +1 Seven -1

  3. I. Bonding Atoms Atoms bond because their valence electrons interact Bonding occurs so that atoms will have stable outer energy levels What is a stable outer energy level? How many electrons? 1st Energy level: 2e- ii. 2nd, 3rd, 4th, etc…Energy level: 8e-

  4. Example: Hydrogen Valence electrons: 1 Energy levels: 1 X X The valence electron in each hydrogen is shared, giving each atom a stable outer energy level.

  5. II. Ionic Bonds Ionic Bonds – Formed between oppositely charged ions Metals form positive ions 2. Nonmetals form negative ions B. When one atom loses an electron, another atom gains that same electron Salt is formed from positively charged sodium ions and negatively charged chlorine ions

  6. Example: Sodium Ion (positive) Na - [Na]+ Cl + [ Cl ]- Chloride Ion (negative)

  7. C. The chemical formula, NaCl, tells the ratio of sodium to chloride ions D. Characteristics of ionic compounds: Conduct electricity when dissolved Metallic bonds – the attraction between a nucleus of one atom and the electrons from another atom Causes atoms to pack close to each other

  8. III. Covalent Bonds Molecules, made when electrons are shared between atoms Covalent Bond –

  9. Example: Chlorine Seven Valence Electrons X X X X X X X X X X X X X X X X X X X X X X X X X X X X X X X X X X The line indicates shared electrons ClCl

  10. Elements can form double or triple bonds O O N N The compounds above share electrons equally, so they form nonpolar covalent bonds 2. Not all covalent bonds are nonpolar Water is a polar covalent molecule

  11. IV. Polyatomic Ions Polyatomic Ions – Groups of covalently bonded atoms that have either gained or lost electrons Polyatomic Ion Examples:

  12. B. A polyatomic ion that is bonded with another atom is often indicated with parentheses (NH4)2SO4 Ammonium sulfate But not always NH4NO3 Ammonium nitrate C. Polyatomic ions usually end in -ate or -ite -ate indicates one additional oxygen atom than the polyatomic ion with -ite

  13. Quiz: Match the polyatomic ion with its name • ____ 1. SO42- • A. sulfite B • ____ 2. SO32- • B. sulfate A • _____ 3. AsO43- • C. arsenate C • ____ 4. AsO33- • D. arsenite D

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