Ionization Energy and Atomic Radius

The video tutorial explains ionization energy, a key chemical property, and its periodic trends. Ionization energy is the minimum energy required to remove an electron from a gaseous atom. The video details how this energy is measured and discusses its periodic trends, showing that it increases with atomic number and decreases with atomic radius. An example using lithium illustrates how ionization energy changes as electrons are removed. The tutorial also highlights exceptions to these trends and concludes with a call to action for viewers to engage with the content.

What is ionization energy?

• The energy required to break a chemical bond.

• The energy required to add an electron to an atom.

• The energy required to remove an electron from an atom in its gaseous state.

• The energy released when an atom gains an electron.

Why must the atom be in a gaseous state when measuring ionization energy?

• To ensure there are no neighboring atoms or intermolecular forces affecting the measurement.

• To ensure the atom is in its most stable state.

• To increase the energy required to remove an electron.

• To decrease the energy required to remove an electron.

In what units is ionization energy measured?

• Joules per mole

• Electron volts per mole

• Kilojoules per mole

• Calories per mole

Why do elements have multiple ionization energies?

• Because they have multiple protons.

• Because they have more than one electron.

• Because they can form multiple bonds.

• Because they exist in different states.

What is the first ionization energy of lithium?

• 500 kJ/mol

• 11815 kJ/mol

• 7300 kJ/mol

• 520 kJ/mol

Why does the second ionization energy of lithium require more energy than the first?

• Because the atom is in a different state.

• Because the remaining electrons are closer to the nucleus and more strongly attracted.

• Because there are more electrons to remove.

• Because the protons repel the electrons.

How does ionization energy change across a period in the periodic table?

• It fluctuates randomly.

• It remains constant.

• It increases from left to right.

• It decreases from left to right.

How does ionization energy change down a group in the periodic table?

• It increases from top to bottom.

• It fluctuates randomly.

• It remains constant.

• It decreases from top to bottom.

What is the relationship between atomic radius and ionization energy?

• Larger atomic radius leads to higher ionization energy.

• Atomic radius and ionization energy are inversely proportional.

• Smaller atomic radius leads to higher ionization energy.

• Atomic radius does not affect ionization energy.

Why do elements with a larger atomic radius have lower ionization energy?

• Because they have more protons.

• Because they have fewer electrons.

• Because the electrons are closer to the nucleus.

• Because the electrons are farther from the nucleus and less strongly attracted.