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Molecular Compounds

Molecular Compounds. Learning Goal:. Students will be able to name, draw and determine the formula of compounds. Agenda:. Ionic Compound Quiz Yesterday’s work – problems? Molecular Compounds Practice time…. Ionic Compounds metal + non-metal  compound

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Molecular Compounds

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  1. Molecular Compounds

  2. Learning Goal: • Students will be able to name, draw and determine the formula of compounds Agenda: • Ionic Compound Quiz • Yesterday’s work – problems? • Molecular Compounds • Practice time…

  3. Ionic Compounds • metal + non-metal  compound • metals lose electrons to non-metals • made of ions of opposite charges

  4. Polyatomic Compounds • Polyatomic Ion: An ion formed by a group of atoms with a shared charge • Found in lots of everyday • Substances • Copy the chart from p.182

  5. Polyatomic Compouds • Naming: • Name of positive ion first and polyatomic ion second • Formulas: • Use the crisscross method as before • Treat the polyatomic ion as one unit • Keep the polyatomic ion in brackets if there is a number behind it

  6. Covalent Bonds • a shared pair of electrons between two non-metal atoms • atoms share electrons to form a stable arrangement (like the noble gases)‏ • It’s like tug of war for the electrons that no atom wins thus they “Share” • Molecule: a particle in which atoms are joined by covalent bonds

  7. Example • Ammonia – NH3

  8. Ionic vs Covalent

  9. Diatomic Molecule • molecule made of two atoms • example: H2

  10. Name of Element Formula Hydrogen H2 Oxygen O2 Nitrogen N2 Fluorine F2 Chlorine Cl2 Bromine Br2 Iodide I2 Elements that Form Diatomic Molecules

  11. Where We Find Molecular Compounds? • molecular compounds are all around us • molecular compounds are found in water, sugar, and molecules that provide flavour and colour • example: can of pop

  12. Combining Capacity • Combining capacity is the number of electrons an atom can gain, lose, or share to form a stable molecule. • Example: Oxygen has a combining capacity of 2.

  13. Writing Formulas for Molecular Compounds • Write the symbols with combining capacities (element farthest left first)‏ • Crisscross the combining capacities • Reduce subscripts if possible • Example: carbon & sulfur • C4 S2 • C2S4 • CS2 – carbon disulfide

  14. Naming Molecular Compounds • 1) Some molecular compounds are named the same way as IONIC COMPOUNDS. • Ex. H2S is Hydrogen Sulfide

  15. Naming Molecular Compounds • 2) Many molecular compounds have COMMON NAMES. (Know these)‏ • Water (H2O)‏ • Ozone (O3)‏ • Ammonia (NH3)‏ • Hydrogen peroxide (H2O2)‏ • Methane (CH4)‏

  16. 3) PREFIXES are another method used to name molecular compounds. • Prefixes are used to count the number of atoms present in the compound. • If there is only one atom in the first element in the molecular compound, the prefix “mono” is not used. • Examples: • Carbon monoxide – CO • Carbon dioxide – CO2

  17. Prefixes in Molecular Compounds Prefix Number Example Mon(o)‏ 1 Carbon monoxide (CO)‏ Di 2 Carbon disulfide (CS2)‏ Tri 3 Sulfur trioxide (SO3)‏ Tetra 4 Carbon tetrafluoride (CF4)‏ Pent(a)‏ 5 d‏ Hexa 6

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