1. Show the e- dot structure for CuCl2, I2 and H2O. State the bond type and name. Show charges where necessary.
We can't draw Lewis dot structures on this board. Look on google. Type in lewis dot structure H2O as one example. If you can't find them I'll try to find one or more for you.
To determine the electron dot structure of a molecule, you need to follow these steps:
1. Determine the total number of valence electrons in the molecule. You can find the valence electrons for each element from the periodic table. The valence electrons are the electrons in the outermost energy level.
2. Identify the central atom in the molecule. In CuCl2, copper (Cu) is the central atom. In I2, both iodine (I) atoms are central. And in H2O, oxygen (O) is the central atom.
3. Distribute the electrons around the central atom and the surrounding atoms such that each atom has an octet (except hydrogen, which only needs two electrons). Electrons are typically placed as lone pairs (dots) or shared pairs (lines) between atoms to form bonds.
Now, let's go through each molecule one by one:
1. CuCl2:
- Copper (Cu) is the central atom, and chlorine (Cl) atoms surround it.
- Copper has one valence electron, and chlorine has 7 valence electrons each. Since there are two chlorine atoms, we have a total of 2 * 7 = 14 valence electrons from chlorine and 1 from copper.
- Start by placing one electron dot between copper and each chlorine atom. This will account for 4 electrons (2 dots and a line). Then, place three lone pairs (dots) around each chlorine atom to complete their octets.
- The electron dot structure for CuCl2 would look like this:
Cl: . Cu . Cl (dots represent lone pairs, and the line represents a bond)
- The bond type in CuCl2 is ionic, as electrons are transferred from copper to chlorine. Copper has a +2 charge, and each chlorine atom has a -1 charge.
2. I2:
- Both iodine (I) atoms are central in this case.
- Iodine has 7 valence electrons each, so the total valence electrons for I2 is 2 * 7 = 14.
- Place three lone pairs (dots) around each iodine atom to complete their octets.
- The electron dot structure for I2 would look like this:
I . I (dots represent lone pairs)
- The bond type in I2 is covalent, as the electrons are shared between the two iodine atoms.
3. H2O:
- Oxygen (O) is the central atom, and hydrogen (H) atoms surround it.
- Oxygen has 6 valence electrons, and hydrogen has 1 valence electron each, so the total valence electrons for H2O is 6 + 2 = 8.
- Place four lone pairs (dots) around the oxygen atom to complete its octet. Then, place one hydrogen atom with a single bond (line) to the oxygen atom.
- The electron dot structure for H2O would look like this:
H: . O . H (dots represent lone pairs, and the line represents a bond)
- The bond type in H2O is covalent, as the electrons are shared between the oxygen and hydrogen atoms. Oxygen has a partial negative charge (δ-) due to its higher electronegativity, and each hydrogen atom has a partial positive charge (δ+).
Note: It's important to remember that the electron dot structures are simplified representations, and the actual bonding in molecules is more complex, involving molecular orbitals.