Electronegativity and Ionization Energy Trends in the Periodic Table

The video tutorial discusses the concepts of electronegativity and ionization energy, key trends in the periodic table. Electronegativity is defined as an atom's tendency to attract electrons, while ionization energy is the energy required to remove a valence electron. Both properties increase across a period and decrease down a group. The video explains how these trends affect the reactivity of elements, with elements on the left of the periodic table being more willing to give up electrons, while those on the right are more eager to gain them.

What is the primary focus of electronegativity in an atom?

• The ability to attract its own electrons

• The ability to attract neighboring electrons

• The ability to repel other atoms

• The ability to lose electrons easily

Which element is likely to have high electronegativity?

• Calcium

• Sodium

• Fluorine

• Lithium

What does ionization energy measure?

• The energy required to remove a valence electron

• The energy required to add an electron

• The energy required to form a bond

• The energy required to split an atom

Which of the following elements would have a low ionization energy?

• Lithium

• Fluorine

• Chlorine

• Oxygen

How do electronegativity and ionization energy change as you move across a period?

• Both decrease

• Both increase

• Electronegativity increases, ionization energy decreases

• Electronegativity decreases, ionization energy increases

What happens to electronegativity and ionization energy as you move down a group?

• Electronegativity increases, ionization energy decreases

• Electronegativity decreases, ionization energy increases

• Both decrease

• Both increase

Why do elements at the bottom left of the periodic table tend to be more reactive?

• They have low electronegativity

• They have high electronegativity

• They have low ionization energy

• They have high ionization energy

Which area of the periodic table is highly reactive due to a strong desire for electrons?

• Bottom right

• Top left

• Bottom left

• Top right

What is the shielding effect in relation to ionization energy?

• It has no effect on ionization energy

• It decreases the attraction between nucleus and electrons

• It increases the ionization energy

• It increases the attraction between nucleus and electrons

Which of the following statements is true about elements with high ionization energy?

• They easily lose electrons

• They have a strong hold on their electrons

• They are found at the bottom of the periodic table

• They are highly reactive metals