Metallic Character and Periodic Trends

The video explores trends in metallic character, defined by an element's ability to lose electrons. Metallic elements have low ionization energies, while nonmetals have higher ones. Down a group, metallic character increases due to a larger atomic radius and weaker nucleus-electron attraction. Across a period, it decreases as nuclear charge increases and atomic radius decreases, strengthening nucleus-electron attraction. Group 15 and period 3 elements illustrate these trends, with nitrogen and phosphorus as nonmetals, arsenic and antimony as metalloids, and bismuth as a metal in group 15, and sodium to chlorine in period 3 showing decreasing metallic character.

What is the definition of metallic character?

• The ability of an atom to form hydrogen bonds

• The ability of an atom to form covalent bonds

• How easily an atom can gain electrons

• How easily an atom can lose electrons

Which type of elements have low ionization energies?

• Noble gases

• Metals

• Metalloids

• Nonmetals

What is the trend in metallic character as you move down a group in the periodic table?

• It decreases

• It increases

• It fluctuates

• It remains the same

Which element in group 15 is a metal?

• Phosphorus

• Bismuth

• Nitrogen

• Arsenic

What type of ions does bismuth form?

• Three negative ions

• Two positive ions

• One negative ion

• Four positive ions

What is the trend in metallic character as you move across a period in the periodic table?

• It decreases

• It increases

• It remains the same

• It fluctuates

Which element in period 3 is a metalloid?

• Chlorine

• Silicon

• Magnesium

• Sodium

Which element in period 3 forms three negative ions?

• Sulfur

• Magnesium

• Phosphorus

• Chlorine

What causes the increase in metallic character down a group?

• Decreasing atomic radius

• Increasing atomic radius

• Decreasing nuclear charge

• Increasing nuclear charge

What causes the decrease in metallic character across a period?

• Decreasing nuclear charge

• Increasing atomic radius

• Decreasing atomic radius

• Increasing nuclear charge