Exploring Atomic and Ionic Radius Trends

The video tutorial covers periodic trends in atomic and ionic radii, explaining both vertical and horizontal trends. It discusses how atomic size changes with electron shells and effective nuclear charge. The video provides examples of ranking elements and ions based on these trends, considering factors like charge and position on the periodic table. Key concepts such as shielding, penetration, and effective nuclear charge are highlighted.

What happens to the atomic radius as you move down a group in the periodic table?

• It decreases

• It fluctuates

• It increases

• It remains the same

Why do atoms get smaller as you move to the right across a period?

• Because the number of electron shells decreases

• Because the effective nuclear charge increases

• Because the number of protons decreases

• Because the shielding effect increases

Which element is smaller: Carbon (C) or Fluorine (F)?

• Cannot be determined

• They are the same size

• Fluorine

• Carbon

What is the trend in atomic radius as you move down a group?

• Atoms get smaller

• Atoms get larger

• Atoms first get smaller then larger

• Atoms remain the same size

How does the size of a cation compare to its neutral atom?

• Cation is larger

• Cation is smaller

• Cation size varies randomly

• Cation is the same size

Which ion is larger: O- or O2-?

• Cannot be determined

• They are the same size

• O2-

• O-

What does the term 'isoelectronic' mean?

• Same number of neutrons

• Same number of protons

• Same number of electrons

• Same atomic radius

Which of the following ions is the smallest: Ca2+, S2-, or Cl-?

• Ca2+

• S2-

• Cl-

• They are all the same size

In the same period, which ion is generally larger: an anion or a cation?

• Cannot be determined

• They are the same size

• Cation

• Anion

Which of the following has the largest atomic radius: Na+, Mg2+, Cl-, or O2-?

• O2-

• Cl-

• Mg2+

• Na+