The Lewis dot model of a molecule is shown. A visual diagram of a PCl3 molecule is shown. Phosphorous is the central atom with a
horizontal line connecting to each of the three Chlorine atoms around it. Phosphorous has a pair of dots on it. Each of the three chlorine atoms have a pair of three dots on it. Based on the model, which of the following is true? ( a. The electronegativity difference between phosphorous and chlorine is greater than 1.7.
( b. Each chlorine has three non-bonded pairs and one bonded pair of electrons.
( c. Phosphorous has three non-bonded pairs and one bonded pair of electrons.
( d. Phosphorous has three valence electrons in the outermost energy level.
b. Each chlorine has three non-bonded pairs and one bonded pair of electrons.
Explanation:
Chlorine has three valance electrons. Each Cl atom forms a single covalent bond with the central P atom by sharing a pair of electrons. After forming a single covalent bond each Cl atom is left with six electrons that do not participate in any bond formation or there are three pairs of lone electrons.
Let's use Boyle's Law here. P1*V1 = P2*V2 Given: (assuming that there are decimals at the end for Sig Figs) P1 = 900.mmHg P2 = 1140.mmHg V1 = ??? V2 = 250.mL
