ITB - Kuliah Online Kimia Dasar B-Latihan struktur atom dan tabel periodik-Dr. Grandprix T. M. Kadja

Summary

This educational video delves into various topics of chemistry, focusing on transition metals and their electron configurations, specifically zinc (Zn) and its ion Zn2+. The script explains concepts like orbital shapes, magnetic properties, and ionization energy, offering detailed examples of electron arrangement, including how different ions form. It covers the nature of paramagnetic and diamagnetic materials and discusses chemical reactions involving elements like copper (Cu) and sulfur (S). The content is rich in theoretical explanations, offering a comprehensive review of fundamental chemistry concepts relevant to basic inorganic chemistry.

Takeaways

• 😀 Transition metals, like zinc (Zn), have unique electron configurations due to the filling of d-orbitals.
• 😀 The electron configuration of zinc (Zn) is 1s2 2s2 2p6 3s2 3p6 4s2 3d10, with the outermost electrons in the 4s orbital.
• 😀 When zinc forms a Zn2+ ion, it loses two electrons from the 4s orbital, resulting in a configuration of 3d10.
• 😀 The shapes of orbitals vary: s orbitals are spherical, p orbitals have a dumbbell shape, and d orbitals have more complex shapes, such as cloverleaf and dz2 (with a ring).
• 😀 Magnetic properties of substances depend on electron pairing: paramagnetic substances have unpaired electrons, while diamagnetic substances have all electrons paired.
• 😀 Zinc (Zn) is classified as diamagnetic because all of its electrons are paired in its 3d10 and 4s2 orbitals.
• 😀 Atomic size increases as you move down a group in the periodic table due to additional electron shells, while it decreases across a period from left to right because of stronger nuclear attraction.
• 😀 Paramagnetism occurs when atoms or ions have unpaired electrons, while diamagnetism occurs when all electrons are paired, as seen in various examples of elements in the transcript.
• 😀 The first ionization energy increases as atomic size decreases, meaning that smaller atoms (like element B in the example) require more energy to remove an electron.
• 😀 Electron affinity is more negative (indicating more stable formation of anions) when the element is more likely to accept an electron, as seen with element B, which is more likely to form an anion due to its negative electron affinity.

Q & A

What is the electron configuration of zinc (Zn)?

The electron configuration of zinc (Zn) with atomic number 34 is: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰.

How does the electron configuration of the Zn²⁺ ion differ from that of Zn?

For the Zn²⁺ ion, two electrons are removed from the outermost 4s orbital, resulting in the electron configuration 3d¹⁰.

What is the shape of an s orbital?

An s orbital has a spherical shape.

What is the shape of a p orbital, and how many types of p orbitals are there?

A p orbital has a dumbbell or balloon shape, and there are three types of p orbitals: px, py, and pz, which are aligned along the x, y, and z axes respectively.

How do d orbitals differ from p orbitals in terms of shape?

D orbitals have five types, and their shapes are more complex than p orbitals, with some resembling double balloons oriented along different axes. For example, the dₓᵧ orbital lies between the x and y axes, while the dₓ²₋y² orbital lies along the x and y axes.

What are paramagnetic and diamagnetic substances?

Paramagnetic substances have unpaired electrons and are attracted to magnetic fields, while diamagnetic substances have all electrons paired and are not attracted to magnetic fields.

What is the magnetic property of zinc (Zn)?

Zinc (Zn) is diamagnetic because all its electrons are paired.

How do the number of electron shells affect the size of an atom?

The size of an atom increases as the number of electron shells increases, typically observed when moving down a group in the periodic table.

What does the term 'ionization energy' refer to, and how is it related to atomic size?

Ionization energy refers to the energy required to remove an electron from an atom. The ionization energy is higher for smaller atoms, as the electrons are closer to the nucleus and experience a stronger attractive force.

How is the energy of a photon absorbed by an atom calculated, and what is the result when a photon with a wavelength of 600 nm is absorbed?

The energy of a photon can be calculated using the formula E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of the light. For a photon with a wavelength of 600 nm, the energy absorbed is 3.35 × 10⁻¹⁹ Joules.