Question

question 5 (1 point)
determine the number of lone pairs on a nitrogen molecule.
1
2
3
4
5
question 6 (1 point)
which group is least likely to form ions?
group 2 alkaline earth metals
group 17 - halogens
group 14 - carbon family
group 1 - alkali metals

Explanation:

Question 5

A nitrogen molecule (\(N_2\)) has a triple bond (\(N\equiv N\)). Each nitrogen atom has 5 valence electrons. In the \(N_2\) molecule, 3 pairs of electrons are used in the triple - bond. So, each nitrogen atom has \((5 - 3)=2\) non - bonding electrons, which form 1 lone pair per nitrogen atom. But the question asks for the number of lone pairs on the nitrogen molecule. Since there are 2 nitrogen atoms in \(N_2\) and 1 lone pair per nitrogen atom, there are 2 lone pairs in total.

• Group 1 Alkali metals: They have 1 valence electron and easily lose it to form \(+1\) ions (e.g., \(Na^+\)).
• Group 2 Alkaline Earth metals: They have 2 valence electrons and easily lose them to form \(+ 2\) ions (e.g., \(Mg^{2+}\)).
• Group 17 - Halogens: They have 7 valence electrons and easily gain 1 electron to form \(-1\) ions (e.g., \(Cl^-\)).
• Group 14 - Carbon family: Carbon (\(C\)) can form covalent bonds by sharing electrons. For example, in \(CH_4\) (methane), carbon shares electrons with hydrogen. It is less likely to form ions compared to alkali metals, alkaline earth metals, and halogens.

Answer:

2

Question 6