Ionization Energy Trends

What is Electronegativity?

• A measure of the tendency of an atom to attract electrons to get a full outer energy level and become stable.

• The ability of an atom to lose electrons easily.

• The measure of the size of an atom in a molecule.

• The energy required to remove an electron from an atom.

How does the shielding effect influence periodic trends?

• It increases the attraction between the nucleus and valence electrons, making it harder to remove electrons.

• It reduces the attraction between the nucleus and valence electrons, making it easier to remove electrons and causing trends like increased atomic radius and decreased ionization energy down a group.

• It has no effect on the atomic radius or ionization energy.

• It increases ionization energy and decreases atomic radius down a group.

Do Valence electrons increase or decrease across a period from left to right?

• Valence electrons increase and are the same as the group number (1A = 1 valence electron)

• Valence electrons decrease across a period from left to right

• Valence electrons remain constant across a period

• Valence electrons first increase and then decrease across a period

Why are noble gases generally unreactive?

• They have a full outer energy level, making them stable and unlikely to gain or lose electrons.

• They have a high electronegativity, which makes them less likely to react.

• They are found in solid form at room temperature, which limits their reactivity.

• They have a low atomic mass, making them less reactive.

Why does Ionization energy decreases down a group.

• Valence electrons are further away from the nucleus as energy levels are added thus taking less energy to remove the electron.

• The nucleus becomes more positively charged, attracting electrons more strongly.

• Electrons are added to the same energy level, increasing electron-electron repulsion.

• The overall size of the atom decreases, making it harder to remove an electron.

Why does Ionization energy increases across a period from left to right?

• Protons added to the nucleus which hold the electrons closer and increasing the amount of energy needed to remove an electron.

• Electrons are added to the outer shell, making them easier to remove.

• The atomic radius decreases, making it easier for electrons to be removed.

• The number of neutrons increases, affecting the stability of the nucleus.

Element with the highest electronegativity

• Oxygen

• Chlorine

• Fluorine

• Nitrogen

What is Ionization Energy?

• The energy required to remove an electron from an atom's outermost energy level.

• The energy released when an electron is added to an atom.

• The energy needed to split an atom into smaller parts.

• The energy required to change an atom from a solid to a liquid state.

Why does Electronegativity increase across a period from left to right?

• As elements gain electrons, they get closer to a full outer energy level to become stable.

• Elements with fewer electrons tend to gain more electrons easily.

• Electronegativity is unrelated to the number of electrons in the outer shell.

• All elements become more electronegative as they lose electrons.

What is the trend for electronegativity as you move down a group?

• Electronegativity increases as you move down a group.

• Electronegativity decreases as you move down a group because the outer electrons are farther from the nucleus and experience less attraction.

• Electronegativity remains constant as you move down a group.

• Electronegativity fluctuates randomly as you move down a group.