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Compounds and Chemical Bonding

Compounds and Chemical Bonding. Compounds. Compounds are formed when two or more atoms come together through a chemical bond. Usually, these come in two types: Ionic Compounds/Bonding: Between a metal and a non-metal. Molecular (Covalent) Compounds: Between two non-metals. Metals: Yellow

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Compounds and Chemical Bonding

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  1. Compounds and Chemical Bonding

  2. Compounds Compounds are formed when two or more atoms come together through a chemical bond. Usually, these come in two types: Ionic Compounds/Bonding: Between a metal and a non-metal. Molecular (Covalent) Compounds: Between two non-metals.

  3. Metals: Yellow Non-Metals: Blue

  4. Chemical Bonds Chemical bonding is simple to understand: Bonds are formed between two atoms either to share (covalent/molecular) or steal (ionic) each other’s electrons, becoming more stable in the process.

  5. Halogens: -1 Charges

  6. Chemical Bonds If we look closely at the halogens, we see that they are all one away from having their octets (one away from being fully stable like a noble gas). Being non-metals, they can steal electrons and have a (-) charge. Usually, we pair chemicals like this with those who would like to give up their electrons (metals, such as sodium, +1)

  7. Ionic Compounds Ionic compounds derive from a simple rule we’ve already seen once before: opposites attract. When a metal which wants to lose electrons (+) meets a non-metal who wants to steal them (-), they stick together. Compounds made from charged particles (ions), are therefore known as ionic.

  8. Naming • Naming these compounds is easy: • The first atom in the formula is always the metal and will have no change to its name with one exception. • We DO have to name the charge for D-block transition metals using parentheses and roman numerals by the stock system. • So, Fe3+ would be Iron (III) • The non-metal’s –ine suffix becomes –ide instead.

  9. Practice (Formulae  Names) NaBr Na3P CaO Fe2O3 FeO CuCl KCl MgBr2 Y2O4 U2O8

  10. Practice (Names  Formulae) Aluminum Fluoride Sodium Sulfide Magnesium Phosphide Manganese (IV) Iodide Cesium Oxide Mercury (II) Sulfide Cadmium (I) Phosphide Iridium (V) Sulfide Hydrogen Iodide Tin (IV) Chloride

  11. Covalent (Molecular) Compounds • Unlike metals, non-metals can form chemical bonds by sharing electrons rather than simply stealing or losing them. • Covalent compounds are formed when two non-metals form a bond by sharing their electrons. • Many chemicals, including the majority of those which build up your body, belong to this class of compound.

  12. Naming non-metals • Unlike metal/non-metal combinations, we have to treat covalent compounds differently when we name them. • When two different non-metals come together, we call them Binary Molecular Compounds. • Unlike before, we can use prefixes and suffixes to describe the number of atoms present rather than just their charges.

  13. Rules of Naming: • We usually don’t modify the first atom’s name, except to specify an amount of atoms greater than 1. • The second atom, on the other hand, must always have an amount specified and will end in –ide (as usual.) • The prefixes are as follows: • 1: Mono- 2: Di- • 3: Tri- 4: Tetra- • 5: Penta- 6: Hexa- • 7: Hepta- 8: Octa- • 9: Nona- 10: Deca-

  14. Examples: (Formulae  Names) • N2O • OF2 • Cl2O8 • SO3 • PCl3 • SF6 • CO • CO2 • PCl5 • BrF7

  15. Examples: (Names  Formulae) • Nitrogen trifluoride • Disulfur dichloride • Dinitrogen tetroxide • Tetraphosphorous decoxide • Pentacarbon monoxide • Heptasulfur decaphosphide • Nitrogen triiodide • Phosphorous monoxide • Boron trifluoride • Silicon dioxide

  16. Polyatomics • Polyatomics are charged covalent compounds which may form ionic bonds with metals. • Think of polyatomics as packs of non-metals which travel together and attack metals. • They have unique and specific names/charges that we rarely have to modify. • Polyatomics are typically found when you have a metal and more than one non-metal in combination.

  17. Common Polyatomics and Charges • NH4+ Ammonium ion • CN- Cyanide ion • OH- Hydroxide ion • C2H3O2- Acetate ion • ClO3- Chlorate ion • NO3- Nitrate ion • MnO4- Permanganate ion

  18. Polyatomics, cont’d • CO32- Carbonate ion • CrO42- Chromate ion • Cr2O72- Dichromate ion • SO42- Sulfate ion • PO43- Phosphate ion

  19. Polyatomics and Naming • Naming compounds with polyatomics is very similar to ionic nomenclature. • Ex. KNO3 would become “potassium nitrate.” • Note, however, that I did not have to add an –ide to the end. We will rarely be modifying the names of polyatomics under ionic conditions.

  20. Practice with Polyatomics • Formulas  Names • NH4C2H3O2 • Ca3(PO4)2 • Ba(OH)2 • Names  Formulas • Ammonium nitrate • Strontium cyanide • Sodium phosphate

  21. Oxyacids and Oxyanions • Many of the aforementioned polyatomics contain the element oxygen and are known as oxyanions for their characteristic negative charge.

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