Exploring Periodic Trends and Coulomb's Law

The video explores periodic trends in the periodic table, focusing on ionization energy, atomic and ionic radii, electron affinity, and electronegativity. It begins with Coulomb's law, explaining how the effective nuclear charge affects these trends. The video discusses how atomic radius decreases across a period and increases down a group, while ionization energy and electron affinity generally increase across a period. The concepts of electron affinity and electronegativity are also covered, highlighting their importance in chemical reactivity.

What fundamental law is used to explain the trends in the periodic table?

• Boyle's Law

• Coulomb's Law

• Newton's Law

• Avogadro's Law

What does the effective nuclear charge (Z effective) represent?

• The total number of electrons in an atom

• The difference between the number of protons and core electrons

• The number of valence electrons

• The atomic mass of an element

Which group of elements has an effective charge of approximately 1?

• Group 1 elements

• Halogens

• Noble gases

• Group 2 elements

How does the atomic radius change as you move from left to right across a period?

• It decreases

• It remains the same

• It increases

• It fluctuates

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

• It first increases then decreases

• It remains constant

• It increases

• It decreases

Which element is considered to have the smallest atomic radius?

• Neon

• Francium

• Helium

• Hydrogen

What is ionization energy?

• The energy released when an electron is added to a neutral atom

• The energy released when an electron is removed from a neutral atom

• The energy required to remove an electron from a neutral atom

• The energy required to add an electron to a neutral atom

Where on the periodic table would you expect to find elements with the highest ionization energy?

• Top left

• Bottom left

• Top right

• Bottom right

What is electron affinity?

• The energy released when an electron is removed from a neutral atom

• The energy required to remove an electron from a neutral atom

• The energy released when an electron is added to a neutral atom

• The energy required to add an electron to a neutral atom

Which elements are known to have high electron affinity?

• Transition metals

• Halogens

• Alkali metals

• Noble gases