Tougher Ionisation energies

First ionisation energy is:

• the minimum amount of energy required to remove the outermost electron from an atom in its solid state

• the maximum amount of energy required to remove the outermost electron from an atom in its gaseous state

• the minimum amount of energy required to remove the outermost electron from 1 mole of atoms in gaseous state

• none of the above

The equation for the first ionisation energy of a sodium atom is:

• Na (g) -> Na⁺ (g) + e^-

• Na⁺ (g) -> Na²⁺ (g) + e^-

• Na (s) -> Na⁺ (g) + e^-

• Na⁺ (g) + e^- -> Na (g)

Which of the following has a lowest first ionisation energy?

• Sodium (Na)

• Magnesium (Mg)

• Chlorine (Cl)

• Argon (Ar)

A shorter atomic radius of atoms in the same period will result in:

• A higher first ionisation energy

• A lower first ionisation energy

Which has the lower first ionisation energy between magnesium and aluminium elements and why

• Magnesium because it has a lower nuclear charge and higher atomic radius

• Aluminium because it has fewer protons

• Magnesium because its outermost electron is removed from an orbital further from the nucleus

• Aluminium because it is removed from an orbital which is higher in energy

which one is the most correct statement

ionisation energies increase across a period ( Na to Ne) because

• Sodium only has to lose a single 3s electron but Ne has to lose 8 electrons

• The size of the atomic radius increases from Na to Ne

• The nuclear charge decreases and shielding increases

• The nuclear charge increases but shielding remains similar

Which is the correct statement? (IE = ionisation energy)

• Magnesium has a higher FIRST IE than sodium because it wants to lose 2 electrons not one.

• Sulfur has a lower first IE than phosphorus because of repulsion between paired electrons in the 3p subshell.

• Sulfur has a lower first IE than phosphorus because of repulsion between paired electrons in the 2p subshell.

• First IE energy decreases across a period as the atoms get bigger

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which one is a correct statement? (IE = FIRST ionisation energy)

• ₁₃Al has a lower IE than ₁₄Mg because Al has fewer protons

• ₁₃Al has a lower IE than ₁₄Mg because Al has electron in 3p subshell which is higher energy and shielded.

• ₁₃Al has a lower IE than ₁₄Mg because Al has a pair of electrons repelling in 3p subshell.

• ₁₃Al has a lower IE than ₁₄Mg because Al has a larger atomic radius.