PARTIKEL PENYUSUN ATOM (isotop, isoton, isobar & isoelektron)

WIN'S CHEMISTRY CLASS

2 Aug 202008:41

Summary

TLDRThe video discusses the development of atomic theory, beginning with early philosophers like Democritus and Aristotle and advancing to modern quantum mechanics. It explains that atoms consist of subatomic particles: protons, neutrons, and electrons. The video highlights atomic structure, explaining atomic number, mass number, isotopes, ions, and concepts like cations and anions. It uses calcium as an example to demonstrate ion formation through electron gain or loss. Additionally, it explains isotopes, isobars, isotrons, and isolectrons, comparing different elements based on these characteristics.

Takeaways

🔬 The evolution of atomic theory has progressed from philosophers like Leucippus, Democritus, and Aristotle to modern quantum mechanics.
⚛️ Atoms are not the smallest particles; they consist of subatomic particles: protons, neutrons, and electrons.
➕ Protons are positively charged particles located in the atomic nucleus.
🟰 Neutrons are neutral particles also found in the nucleus.
➖ Electrons are negatively charged particles that orbit around the nucleus in electron shells.
🔢 The atomic number (Z) represents the number of protons and electrons (in a neutral atom), while the mass number (A) is the sum of protons and neutrons.
🧮 Electrons can move between energy levels and even between atoms, leading to the formation of ions (cations and anions).
🔀 Isotopes are atoms of the same element with the same atomic number but different mass numbers due to varying neutrons.
⚖️ Isobars are atoms with the same mass number but different atomic numbers.
⚙️ Isoelectrons are atoms or ions that have the same number of electrons.

Q & A

What are the three subatomic particles that make up an atom?
-The three subatomic particles are protons, neutrons, and electrons.
Where are protons and neutrons located within an atom?
-Protons and neutrons are located in the nucleus of the atom.
What is the charge of a proton and an electron?
-A proton has a positive charge, while an electron has a negative charge.
How can you determine the number of protons in an atom?
-The number of protons in an atom is equal to the atomic number, which is represented by the symbol Z.
How do you calculate the number of neutrons in an atom?
-The number of neutrons is calculated by subtracting the atomic number (Z) from the atomic mass (A).
What happens when an atom loses or gains electrons?
-When an atom loses electrons, it becomes a positively charged ion (cation). When it gains electrons, it becomes a negatively charged ion (anion).
What are isotopes, and how do they differ from one another?
-Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons, which gives them different atomic masses.
What are isobars, and how do they differ from isotopes?
-Isobars are atoms that have the same atomic mass but different atomic numbers, meaning they are different elements with the same total number of protons and neutrons.
What is an isoton, and how is it defined?
-Isotons are atoms that have the same number of neutrons but different numbers of protons, making them different elements with similar neutron counts.
What is the significance of isolectrons, and how do they relate to atoms and ions?
-Isoelectrons are atoms or ions that have the same number of electrons, even though they may differ in charge or atomic number.

Outlines

00:00

🔬 Evolution of Atomic Theory and Subatomic Particles

The video begins by revisiting the development of atomic theory, starting from ancient Greek philosophers Leucippus and Democritus, through to Aristotle, Dalton, Thomson, Rutherford, Bohr, and the quantum mechanical model of the atom. It explains that the atom, once thought to be the smallest unit of matter, is actually composed of smaller subatomic particles: protons, neutrons, and electrons. Protons carry a positive charge and are located in the nucleus, neutrons have no charge and are also in the nucleus, while negatively charged electrons orbit the nucleus in electron shells. Chemists have identified many different atoms, and symbols are used to represent them. These symbols typically feature the element symbol (X), the atomic number (Z) at the bottom left, and the mass number (A) at the top left. The atomic number equals the number of protons and, in a neutral atom, also equals the number of electrons.

05:04

⚛️ Calculating Atomic Properties: Example of Calcium

The example of a calcium atom (Ca) is used to demonstrate how atomic properties are calculated. The atomic number of calcium is 20, meaning it has 20 protons and, in a neutral state, 20 electrons. The mass number is 40, which is the sum of protons and neutrons. Therefore, the number of neutrons is calculated by subtracting the atomic number from the mass number: 40 - 20 = 20 neutrons. Bohr's atomic model suggests that electrons can move between shells or even between atoms, leading to ion formation. There are two types of ions: cations (positive ions formed by losing electrons) and anions (negative ions formed by gaining electrons).

🔋 Formation of Calcium Ions

The video continues with a deeper look at ion formation using calcium as an example. When a calcium atom loses two electrons, it becomes a cation with a +2 charge because the number of protons (20) exceeds the number of electrons (18). The charge is calculated by subtracting the number of electrons from the protons: 20 - 18 = +2. Conversely, if calcium gains two electrons, it forms an anion with a -2 charge, as the number of electrons (22) exceeds the number of protons (20), yielding a total charge of -2.

🧪 Isotopes, Isobars, Isotons, and Isoelectrons

The final segment introduces four important concepts: isotopes, isobars, isotons, and isoelectrons. Isotopes are atoms of the same element with the same atomic number but different mass numbers, such as Carbon-12 and Carbon-14. Isobars are atoms of different elements with the same mass number but different atomic numbers, like sodium and magnesium. Isotons refer to atoms with the same number of neutrons but different atomic and mass numbers, while isoelectrons are atoms or ions that have the same number of electrons, such as neon and sodium ions.

Mindmap

Keywords

💡Atom

An atom is the basic unit of a chemical element, composed of protons, neutrons, and electrons. The video discusses how early theories like those of Democritus and Aristotle considered atoms as the smallest particles, but modern theories reveal that atoms are made of subatomic particles such as protons, neutrons, and electrons. The atom serves as the foundation for understanding matter in the video's narrative.

💡Proton

A proton is a positively charged subatomic particle located in the nucleus of an atom. In the video, protons are essential in determining the atomic number of an element, which is equal to the number of protons in a neutral atom. For example, calcium has 20 protons, making its atomic number 20.

💡Neutron

A neutron is a neutral subatomic particle found in the nucleus of an atom, alongside protons. Neutrons contribute to the atomic mass but do not affect the charge of the atom. The video explains how neutrons, together with protons, help determine an element's atomic mass, as seen in calcium's mass number calculation (protons + neutrons).

💡Electron

Electrons are negatively charged particles that orbit the nucleus of an atom in different energy levels or shells. The video explains how electrons are involved in forming ions when they are either gained or lost, and also how they determine the overall charge of an atom. For instance, the loss of two electrons from calcium forms a positively charged ion (Ca²⁺).

💡Ion

An ion is an atom or molecule that has gained or lost one or more electrons, resulting in a net electric charge. The video distinguishes between cations, which are positively charged ions formed by losing electrons, and anions, which are negatively charged ions formed by gaining electrons. Calcium is used as an example where losing two electrons forms a Ca²⁺ ion.

💡Atomic number (Z)

The atomic number (Z) is the number of protons in the nucleus of an atom, which also equals the number of electrons in a neutral atom. This number defines the identity of an element. The video explains how the atomic number of calcium is 20, meaning it has 20 protons and 20 electrons in its neutral state.

💡Mass number (A)

The mass number (A) is the sum of protons and neutrons in the nucleus of an atom. This value is crucial for distinguishing between isotopes. The video shows that calcium has a mass number of 40, meaning its nucleus contains 20 protons and 20 neutrons.

💡Isotope

Isotopes are atoms of the same element that have the same number of protons (atomic number) but different numbers of neutrons, resulting in different mass numbers. The video illustrates this with carbon, which has isotopes like carbon-12 and carbon-14, both having six protons but differing in their number of neutrons.

💡Bohr model

The Bohr model of the atom describes electrons orbiting the nucleus in specific energy levels or shells. The video references this model to explain how electrons can move between energy levels and how these transitions play a role in ion formation, when electrons are either absorbed or released.

💡Cation

A cation is a positively charged ion formed when an atom loses one or more electrons. In the video, calcium is used as an example of a cation when it loses two electrons, forming a Ca²⁺ ion. This process is essential in understanding the formation of positive ions.

Highlights

The smallest part of matter is not the atom itself, but subatomic particles such as protons, neutrons, and electrons.

Protons carry a positive charge and are located within the atomic nucleus.

Neutrons are neutral particles found in the nucleus, contributing to the atom's mass.

Electrons carry a negative charge and orbit around the nucleus in atomic shells.

The atomic symbol notation includes the element symbol, atomic number (Z), and mass number (A).

The atomic number (Z) represents the number of protons and is equal to the number of electrons in a neutral atom.

The mass number (A) equals the sum of protons and neutrons within the atom's nucleus.

Bohr's theory suggests that electrons can move between atomic shells or even from one atom to another.

An ion is formed when electrons are lost or gained; losing electrons creates a positively charged ion (cation), and gaining electrons forms a negatively charged ion (anion).

For example, calcium (Ca) has 20 protons and electrons in its neutral state, and the loss of two electrons forms a Ca²⁺ ion.

Isotopes are atoms with the same number of protons (same atomic number) but different numbers of neutrons, leading to different mass numbers.

Isobars are atoms that have the same mass number but different atomic numbers, such as sodium (Na) and magnesium (Mg).

Isotones are atoms with the same number of neutrons but different numbers of protons, like calcium (Ca) and potassium (K).

Isoelectronic species are atoms or ions with the same number of electrons, such as neon (Ne) and Na⁺.

Atomic interactions such as electron transfer lead to the formation of ions, which are crucial for chemical bonding and reactions.