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CHEMICAL BONDING

Learn about the different types of chemical bonding - ionic and covalent - and how atoms gain, lose, or share electrons to form stable compounds. Discover the properties of ionic and covalent compounds, as well as the formation and naming of ions.

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CHEMICAL BONDING

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  1. CHEMICAL BONDING When atoms meet, they combine!

  2. Bonding • Atoms are most stable when they have 8 valence electrons (The Octet Rule) • Atoms can gain, lose, or shareelectrons to get 8 total valence electrons • When atoms gain, lose, or share electrons they are bonding • There are two types of bonding: ionic and covalent

  3. Ionic Bonding • Formed between metals and nonmetalsthrough a transfer of electrons • The metalslose valence electrons (+) • The nonmetalsgain valence electrons (-) • The positive and negative ions are then attracted to each other like magnets • Ionic compounds must have a balanced amount of + and - charge!

  4. Family Patterns for Ion Formation • Group 1: LOSE 1 valence electron (+1) • Group 2: LOSE 2 valence electrons (+2) • Group 13: LOSE 3 valence electrons (+3) • Group 14: SHARE 4 valence electrons, but could be +4 or – 4 • Group 15: GAIN 3valence electrons (-3) • Group 16: GAIN 2 valence electrons (-2) • Group 17: Gain 1 valence electrons (-1)

  5. Identify the following charges(find the group they are in first) • Lithium (Li) • Phosphorus (P) • Aluminum (Al) • Oxygen (O) • Bromine (Br) • Magnesium (Mg)

  6. Ions and Bonding - Practice • Sodium • Who would sodium bond with? • Ca (metal, + ion) • K (metal, +ion) • Li (metal, +ion) • Cl (nonmetal, - ion)

  7. Which Compound is Ionic? • CO2 • C6H12O6 • CH4 • MgCl2

  8. Polyatomic Ions • Ions that are made of a group of atoms, but they act like one atom (treat them like one ion with one charge) • Examples: • Hydroxide: (OH)-1 Carbonate: (CO3)-2 • Phosphate: (PO4)-3 Ammonium: (NH4)+1 • Nitrate: (NO3)-1

  9. Writing Ionic Formulas How do I write an ionic formula? 1. First find the charge on each Na+1 and S-2 2. Now, all you need to do is cross the charges over and write them as subscripts (but don’t worry about the signs). Na2S1 • The one (1) is “understood” so you don’t have to use it when you write it down. Na2S

  10. Writing Ionic Formulas • Try the following: • Sodium and oxygen • Lithium and Sulfur • Magnesium and Chlorine

  11. Naming Ionic Bonds • Start with the name of the positive ion. • Change the end of the negative ion to –ide • If the negative end is polyatomic, DO NOTchange its name • Example 1: Sodium + Chlorine = Sodium Chloride • Example 2: Lithium + Nitrate = Lithium Nitrate

  12. Properties of Ionic Compounds • Stronger bonds • High melting and boiling points • Crystalline structures (has tight, repetitive pattern) • High conductivity

  13. Covalent Bonding • Formed between two or more nonmetals • Also known as MOLECULAR BONDING • Two or more atoms share electrons so that each atom has eight valence electrons

  14. Which is the covalent bond? • NaCl • KF • CO2 • MgS

  15. Properties of Covalent Compounds • Weaker bonds • Lower melting and boiling points • Not good conductors

  16. Extra Info: Organic Compounds • Any compound that contains Carbon • Examples: CO2, C6H12O6, CH4 • Decide for the following: H2O O2 CO NaCl

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