Math

QuestionWhich of the following are reasons why the chemical properties of phosphorus are quite different from those of nitrogen, even though they are located very closely on the periodic table?
1. the greater electronegativity of nitrogen II. the larger size of the phosphorus atom III. nitrogen's ability to form stronger pi bonds IV. the empty valence dd orbitals on phosphorus

Studdy Solution

STEP 1

1. Phosphorus and nitrogen are elements located in the same group on the periodic table.
2. We need to evaluate each given reason to determine if it explains the difference in chemical properties between phosphorus and nitrogen.

STEP 2

1. Analyze the electronegativity difference.
2. Consider the atomic size difference.
3. Evaluate the ability to form pi bonds.
4. Assess the presence of empty valence d d orbitals.

STEP 3

Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Nitrogen has a higher electronegativity than phosphorus, which affects their chemical reactivity and bonding characteristics.

STEP 4

The size of an atom influences its chemical properties. Phosphorus has a larger atomic radius than nitrogen, which affects its ability to form bonds and its reactivity.

STEP 5

Pi bonds are formed by the overlap of p orbitals. Nitrogen can form stronger pi bonds due to its smaller size and higher electronegativity, which allows for better orbital overlap compared to phosphorus.

STEP 6

Phosphorus has empty valence d d orbitals, which nitrogen lacks. This allows phosphorus to expand its valence shell and form more bonds, influencing its chemical properties.
The reasons that explain the difference in chemical properties between phosphorus and nitrogen are:
I, II, III, IV \boxed{\text{I, II, III, IV}}

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