Consider group 5a elements: nitrogen, phosphorus, and arsenic. these elements show an increase in their atomic numbers. which element has the highest ionization energy?

It will be nitrogen.

The energy associated with the formation of 1 mol of gaseous cations is The ionization energy. 1 mole of electrons will form 1 mole of gaseous atoms under standard conditions. The ionization energy decreases as you go down a group on the periodic table.

Explanation:

Ionization energy is defined as the energy required to remove the most loosely bound electron from a neutral gaseous atom.

With increase in atomic number there will also occur an increase in atomic size of the atom. As a result, there will be less force of attraction between the nucleus and the valence electrons of the atom.

Hence, it is easy to remove the most loosely bound electron. Therefore, with increase in size there will occur a decrease in the size of atom.

Since, out of the given group 5A elements, arsenic is larger in size and nitrogen is the smallest. Therefore, ionization energy for nitrogen will be the highest.

Thus, we can conclude that nitrogen is the element which has the highest ionization energy.

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.