Allright for <span><span>H2</span>O:</span>
- The central atom is? --> the oxygen atom
- How many atoms are bonded to the central atom? --> 2 hydrogen atoms
- How many lone pairs of electrons are on the central atom? --> O has 6 electrons and has 2 single bonds, so 2 pairs
- How many single bonds are there in this molecule? --> 2
- How many multiple bonds (double and/or triple) are there in this molecule? --> none
For each of your molecules, answer the following questions:
1. Determine the electronegativity between the atoms of each molecule.
Electronegativity O = 3.44
Electronegativity H = 2.20
3.44-2.20=1.24, so the electronegativity between O and H = 1.24
2. Identify the bond as either ionic or covalent.
Electronegativity of 0.0-1.7 = covalent
Electronegativity of 1.7-3.3 = ionic
So it's a covalent bond
3. State whether the molecule is polar or non polar.
Electronegativity of 0.5-1.7= polar covalent
4. Identify the structure as having hydrogen bonding, dipole-dipole moments or London dispersion forces (LDF).
<span><span>H2</span>O</span><span> = hydrogen bonding</span>
The student made a mistake because he did not convert a unit of volume from milliliters to liters. After all, molarity is defined as the number of moles of solute per liter of solution.
