electron structure and configuration of atoms and ions , Aufbau principle

What happens to the size of the orbital as the principal quantum number (n) increases?

What effect does an increase in shielding have on the energy of electrons in an orbital?

Which type of subshell has the most penetrating electrons?

What does the notation 4s2 represent?

How does an increase in the value of l within a shell affect electron penetration?

What is shielding as mentioned in the text?

What does the principal quantum shell number (n) indicate in an electron configuration?

How does an increase in energy due to n compare to an increase due to l for small orbitals?

What determines many of the chemical properties of an atom?

In the order of increasing energy, which atomic orbitals are arranged correctly?

Why does the energy of atomic orbitals increase within a shell in the order s < p < d < f?

Which orbital has electrons with the lowest energy according to Figure 6.24?

Why is it confusing for many students that the 5p orbitals fill immediately after the 4d and before the 6s orbitals?

Which quantum number has more influence on energy than the increasing azimuthal quantum number for small atoms?

What is the correct order for filling orbitals based on their increasing energy?

Why do electrons in orbitals that experience more shielding have higher energy levels?

What is the main reason behind the slight repulsion between electrons that are closer to the nucleus and those farther out?

In which order do the following types of atomic orbitals have electrons with increasing energy levels?

How does the energy increase due to the principal quantum number (n) compare to the increase due to the azimuthal quantum number (l) for larger orbitals?

Which factor contributes more significantly to determining the energy of electrons within small orbitals?

Why does the 3d orbital have higher energy than the 4s orbital in larger atoms?

How does the energy of orbitals change as we move up within a shell, from 1s to 3p?

Which statement best explains why the filling order of the orbitals can be confusing for students?

What characteristic of atomic orbitals determines their energies within a shell?

How do low-energy orbitals get filled as electrons move along the periodic table?

What causes the electron to shift from the 4s to the 3d orbital in Cr and Cu?

What is the electron configuration of niobium (Nb, atomic number 41) as observed experimentally?

Why are valence electrons more easily lost or shared compared to core electrons?

What determines the chemical properties of elements in the same group?

In which category do main group elements fall based on their outermost orbital characteristics?

Why do elements in the same group exhibit similar chemical properties?

What role do valence electrons play in chemical reactions?

Why is it challenging to predict exceptions for atoms with high electron repulsions?

'Main group' elements are characterized by adding electrons to which orbitals?

What is the main factor that leads to the electron shifting from the 4s to the 3d orbital in Cr and Cu?

Why does niobium (Nb) exhibit an electron configuration different from its predicted configuration?

What determines how elements react chemically?

Why do elements in the same group exhibit similar chemical properties?

What role do valence electrons play in chemical reactions?

What feature places main group elements into their respective category?

Which category includes all nonmetallic elements?

Why are valence electrons more easily lost or shared compared to core electrons?

How would you differentiate 'transition' elements from 'main group' elements based on their outermost electron addition?