Chapter 7 chem

• CO2 is a covalent bond because they are both non metals meaning they are covalent bonding
• LiF is ionic as it has one metal and one non-metal
• Ionic bonds are only good at conducting electricity in solutions
• Nomenclature- systematic way of writing and naming compounds

  purpose: So we don’t have to memorize all the common names . example: sodium by carbonate (nomenclature) baking Soda ( common name). By using the nomenclature you can figure out the formula by looking for sodium (Na) on th periodic table and knowing the polynomial, carbonate (CO3^2-)

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• Zn (Zinc) is always 2+, Ag (silver) is always 1+
• Bonding-

  • chemical bond: mutual attraction between the nuclei and the valance electrons of different atoms that binds them together

  Types of bonds

  • ionic bonds: force of attraction between oppositely charged atoms ( non metal and metal)
  • Covalent bond: force of attraction for electrons, that result in a pair of electrons being shared by two atoms ( 2 non metals) - metallic bond: force of attraction between diloclization atoms (metal and metal)
• Ionic bonding-

  • Ionic compounds: composted of positive and negative ions of equal but opposite charge ( Na- 1+ Cl- 1-)
  • formula unit: simplest collection of ion in which the ionic compound can be formed. ex NaCl the ratio is 1:1 if a ration was 4:2 it would be simplified to 1:2
• Ionic bonding can have many atoms bonded but covalent bonding only has two atoms bonded because they’re sharing.
• Crystal Lattice-

  3 dimensional geometric arrangement of particles

  • positive and negitive ions surround one another due to the size and number of the particles affects the home of the lattice (cube)

  Lattice Energy

  • Energy needed to break or separate 1 mole (bond) of ions in an ionic compounds. Every bond must be broken so it needs a lot of energy. these bonds are strong so they’re usually in solid state.
• Ionic bonds are stronger than any type of bond including covalent because of the array of forces holding the solid together. Basically because they’re bonds are really strong.
• Ionic compounds

  • higher melting point
  • more brittle (if you throw it, it will shatter)
  • does not vaporize easily
  • conductors if electricity when dissolved in H2O. Can only be conductors if in a solution.
  • Great repulsion when layers shift
• Random things to remember:

  • always put paranthesis around polyions and Roman numerals. However, if there is only 1 amount of a polyion there is no need for paranthasis.
  • zinc will always be 2+ and silver will always be 1+
  • The d block, f block, and group four ion charges are unknown so they should be given to you when your writing a formula a ionic compound. However, if your naming an ionic compound, you need to find the charge by Using the box method
• Formula unit: simplest ratio between two ions that combine in an ionic compound
• Oxidation numbers:

  representation of an atom of it were to have a charge
• Lewis dot- it uses electron dot notation to sketch the exchange of valance electron in atoms as they form ionic bonds
• Oxidation rules: (Ignore peroixide)

  
• Oxidation example:

  
• Ionic compounds - composed of positive and negitive ions of equal but opposite charge (can be many ions)
• Metallic bonding: bonding resulting form the attraction for positive ions and mobile electrons (metal and metal)

  • electrons are de localized (electrons do not belong to any one ion)
• Lewis dot diagram example: