electron structure and configuration of atoms and ions , Aufbau principle

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

The size decreases

The size increases (correct)

The size remains constant

The shape changes

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

Stabilizes them more

Stabilizes them less (correct)

Reduces the speed of electrons

Doesn't affect their energy

Which type of subshell has the most penetrating electrons?

p

s (correct)

d

f

What does the notation 4s2 represent?

2 electrons in an s subshell Signup and view all the answers

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

Decreases penetration Signup and view all the answers

What is shielding as mentioned in the text?

Electrons closer to the nucleus repel those farther out Signup and view all the answers

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

Energy level of the orbital Signup and view all the answers

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

Increase due to n is more significant Signup and view all the answers

What determines many of the chemical properties of an atom?

The arrangement of electrons in orbitals Signup and view all the answers

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

$1s < 2s < 2p < 3s$ Signup and view all the answers

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

Due to the increasing value of the azimuthal quantum number (l) Signup and view all the answers

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

$1s$ Signup and view all the answers

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

Because of the overlapping energies of atomic orbitals Signup and view all the answers

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

$n$ Signup and view all the answers

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

$1s < 2s < 2p < 3s < 3p < 4s$ Signup and view all the answers

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

As a result of less stabilization caused by shielding Signup and view all the answers

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

Opposite charges of electrons and nuclei Signup and view all the answers

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

$f < s < d < p$ Signup and view all the answers

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?

Both increases are comparable and cannot be simply predicted Signup and view all the answers

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

Principal quantum number, n Signup and view all the answers

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

The 3d orbital has more electron-electron repulsion than the 4s orbital. Signup and view all the answers

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

The energy increases due to increasing n value. Signup and view all the answers

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

The energy difference between orbitals with different values of l is not consistent. Signup and view all the answers

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

Principal quantum number (n) Signup and view all the answers

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

Electrons preferentially fill low-energy orbitals first before moving to higher-energy ones. Signup and view all the answers

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

The stability of a half-filled 3d subshell (in Cr) or a filled 3d subshell (in Cu) Signup and view all the answers

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

[Kr]5s14d4 Signup and view all the answers

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

Valence electrons have higher energy levels Signup and view all the answers

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

Valence electron configuration Signup and view all the answers

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

Representative elements Signup and view all the answers

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

They possess the same number of valence electrons Signup and view all the answers

What role do valence electrons play in chemical reactions?

Influencing reactivity and bonding behavior Signup and view all the answers

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

Repulsions are greater than energy differences between subshells Signup and view all the answers

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

(n-1)s or (n-1)p orbitals Signup and view all the answers

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

Half-filled 3d subshell Signup and view all the answers

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

Electron–electron repulsions in the 5s orbital Signup and view all the answers

What determines how elements react chemically?

Number of valence electrons Signup and view all the answers

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

They have the same number of valence electrons Signup and view all the answers

What role do valence electrons play in chemical reactions?

Defining how elements react Signup and view all the answers

What feature places main group elements into their respective category?

Last electron added entering an s or p orbital Signup and view all the answers

Which category includes all nonmetallic elements?

'Main group' elements Signup and view all the answers

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

Higher energy level Signup and view all the answers

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

'Transition' elements add to d orbitals, 'main group' add to s or p orbitals Signup and view all the answers

electron structure and configuration of atoms and ions , Aufbau principle

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Questions and Answers

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?

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