STRUKTUR ATOM : PARTIKEL SUB ATOM

Trivia Educhem

24 Jul 202014:21

Summary

TLDRThis video explains atomic structure, covering subatomic particles like protons, electrons, and neutrons. It delves into their properties, with protons having a positive charge, electrons a negative charge, and neutrons being neutral. The video also discusses atomic and ion notation, mass and atomic numbers, and how to calculate protons, electrons, and neutrons for different elements and ions. Additionally, concepts like isotopes, isobars, isotones, and isoelectrons are introduced, with examples to clarify their distinctions. The video concludes with a complex isotopic problem involving neutron calculations and periodic elements.

Takeaways

📘 The atom consists of subatomic particles: protons, electrons, and neutrons, with protons having a positive charge, electrons a negative charge, and neutrons being neutral.
🔬 Protons and neutrons have almost the same mass, which is around 1000 times greater than the mass of electrons.
⚖️ Proton, electron, and neutron masses are in a ratio of 1:0:1, with protons and neutrons located in the atom's nucleus, and electrons in the atomic shell.
🔭 Protons were discovered by Goldstein in 1886, electrons by Thomson in 1897, and neutrons by Chadwick in 1932.
🧲 Protons are deflected toward the negative pole in a magnetic field, electrons toward the positive pole, and neutrons are unaffected.
🧮 The deflection of particles in a magnetic field is inversely proportional to their mass and directly proportional to their charge.
🧑‍🔬 Atomic notation consists of the mass number (A), the atomic symbol (X), and the atomic number (Z). The mass number is the total of protons and neutrons in the nucleus.
⚛️ For neutral atoms, the number of protons equals the number of electrons. For ions, positive charges indicate electron loss, and negative charges indicate electron gain.
🔢 Isotopes are atoms with the same number of protons but different numbers of neutrons. Isobars have the same mass number but different atomic numbers, and isotones have the same number of neutrons.
🧮 Isoelectronic species have the same number of electrons, even though they may differ in other atomic or ionic properties.

Q & A

What are the three subatomic particles that make up an atom?
-The three subatomic particles that make up an atom are protons, neutrons, and electrons.
What are the charges of protons, electrons, and neutrons?
-Protons have a positive charge (+), electrons have a negative charge (-), and neutrons have no charge (neutral).
Why do protons and neutrons have more mass compared to electrons?
-Protons and neutrons have a mass that is approximately 1000 times greater than the mass of electrons, making them more massive and less affected by electrical fields.
How are particles like protons, electrons, and neutrons affected by a magnetic field?
-In a magnetic field, protons are deflected toward the negative pole, electrons are deflected toward the positive pole, and neutrons are not affected because they are neutral.
Who discovered the proton, electron, and neutron, and when?
-The proton was discovered by Goldstein in 1886, the electron was discovered by Thomson in 1897 through the cathode ray experiment, and the neutron was discovered by Chadwick in 1932.
How is the atomic mass of an atom calculated?
-The atomic mass is the total sum of protons and neutrons in the nucleus, as electrons have negligible mass.
What is the significance of atomic number and mass number in an atom's notation?
-The atomic number (Z) represents the number of protons in an atom, which is equal to the number of electrons in a neutral atom. The mass number (A) is the sum of protons and neutrons in the atom's nucleus.
How do you determine the number of neutrons in an atom?
-The number of neutrons is determined by subtracting the atomic number (number of protons) from the mass number: Neutrons = Mass number - Atomic number.
What happens to the number of electrons in an ion compared to its neutral atom?
-In a positive ion, the atom loses electrons, so the number of electrons decreases. In a negative ion, the atom gains electrons, so the number of electrons increases.
What are isotopes, isobars, and isoelectrons?
-Isotopes are atoms with the same number of protons but different numbers of neutrons. Isobars are atoms with the same mass number but different atomic numbers. Isoelectrons are atoms or ions with the same number of electrons.

Outlines

00:00

🔬 Introduction to Atomic Structure

This paragraph introduces the concept of atomic structure and its subatomic particles: protons, electrons, and neutrons. Protons have a positive charge, electrons have a negative charge, and neutrons are neutral. It also discusses the relative masses of these particles, with protons and neutrons having nearly the same mass, which is 1000 times greater than that of electrons. The positions of these particles within the atom are explained: protons and neutrons reside in the nucleus, while electrons are found in the atomic shell. The discoveries of these particles by scientists such as Goldstein (proton), Thomson (electron), and Chadwick (neutron) are mentioned, along with how magnetic and electric fields affect each particle. The paragraph concludes by linking these properties to the periodic table, introducing atomic notation and symbols used to represent elements and ions.

05:00

📊 Understanding Atomic Notation and Ions

This paragraph delves deeper into atomic notation, explaining the symbols for mass number (A), atomic number (Z), and their significance. Mass number (A) is the sum of protons and neutrons, while the atomic number (Z) indicates the number of protons, which is equal to the number of electrons in a neutral atom. The paragraph then transitions to ion notation, discussing how an atom becomes an ion when it gains or loses electrons, resulting in a positive or negative charge. Various examples using sodium (Na) and other elements are provided to calculate the number of protons, neutrons, and electrons, depending on the given atomic and mass numbers. Key formulas and steps are outlined for identifying the properties of elements and their ionic states.

10:02

🧮 Calculating Properties of Elements and Ions

This paragraph presents examples of different atoms and ions, including sodium, nitrogen, sulfur, and chromium. For each, the atomic number, mass number, and number of protons, electrons, and neutrons are calculated. It covers cases where elements are neutral and where they exist as ions with positive or negative charges, explaining how these charges alter the electron count. The concepts of isotopes, isobars, and isotones are introduced and explained through specific examples, such as variations of carbon and nitrogen atoms. This section emphasizes the importance of understanding atomic and mass numbers for predicting the structure and properties of atoms and ions.

🔍 Isotopes, Isobars, Isotones, and Isoelectrons

This paragraph introduces and explains four related concepts in atomic structure: isotopes, isobars, isotones, and isoelectrons. Isotopes are defined as atoms with the same number of protons but different numbers of neutrons (e.g., Carbon-12 and Carbon-13). Isobars are atoms with the same mass number but different atomic numbers (e.g., Carbon-13 and Nitrogen-13). Isotones have the same number of neutrons but different atomic numbers (e.g., Sodium-23 and Magnesium-24). Isoelectronic species have the same number of electrons, even if they differ in protons or charge. Examples include various ions such as fluoride (F-) and sodium (Na+), demonstrating how these classifications help categorize atomic similarities and differences.

📐 Example Problem: Isotonic Elements

The final paragraph provides a detailed solution to an example problem involving isotonic elements. It describes two elements (Nb and Sr) with the same number of neutrons and works through a series of equations to find their respective atomic and mass numbers. By using known relationships and substituting values step-by-step, the paragraph demonstrates how to solve for unknowns in atomic equations. It concludes by summarizing the properties of the two elements based on the calculated values and encourages viewers to ask questions for further clarification.

Mindmap

Keywords

💡Atom

An atom is the smallest unit of matter that retains the identity of an element. In the video, it is explained that atoms are composed of subatomic particles, including protons, neutrons, and electrons. The concept is central to the video's discussion of atomic structure, where different particles within the atom are highlighted, along with their properties such as mass and charge.

💡Proton

A proton is a positively charged subatomic particle found in the nucleus of an atom. The video explains that protons, along with neutrons, determine the mass of an atom. Proton numbers also define the atomic number of an element, which is critical in determining the element’s identity and properties.

💡Electron

An electron is a negatively charged subatomic particle that orbits the nucleus of an atom in various energy levels, also referred to as atomic shells. The video describes how electrons play a role in chemical reactions and bonding, and also how their behavior is affected by magnetic and electric fields.

💡Neutron

A neutron is a subatomic particle found in the nucleus of an atom, with no electrical charge. Neutrons contribute to the mass of an atom and, along with protons, are involved in determining isotopes. In the video, neutrons are discussed in relation to atomic mass and their role in differentiating isotopes of elements.

💡Atomic Number (Z)

The atomic number, denoted by Z, represents the number of protons in the nucleus of an atom. The video explains that the atomic number defines the element and its position in the periodic table. For example, sodium (Na) has an atomic number of 11, meaning it has 11 protons.

💡Mass Number (A)

The mass number (A) is the total number of protons and neutrons in an atom’s nucleus. The video illustrates how to calculate the mass number of elements, such as sodium, where the mass number helps determine the isotope and the overall mass of the atom.

💡Ion

An ion is an atom or molecule that has gained or lost one or more electrons, giving it a positive or negative charge. The video discusses ions like sodium (Na+) and sulfur (S2-), explaining how ions form through electron transfer and how their electron configuration changes.

💡Isotope

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. In the video, examples like carbon-12 and carbon-13 are used to explain isotopes. These isotopes have identical atomic numbers but different mass numbers due to the difference in neutron count.

💡Periodic Table

The periodic table is a tabular arrangement of elements, ordered by increasing atomic number. The video briefly refers to the periodic table when explaining how the atomic number and mass number are represented for each element. It also uses examples from the table, such as sodium (Na) and nitrogen (N).

💡Subatomic Particle

Subatomic particles are the smaller components that make up an atom, including protons, neutrons, and electrons. The video explores how these particles interact within the atom and how they are affected by external factors such as magnetic fields, as demonstrated in the behavior of protons and electrons under electric fields.

Highlights

Atoms are not the smallest particles; they contain subatomic particles like protons, neutrons, and electrons.

Proton has a positive charge, electron has a negative charge, and neutron is neutral.

Protons and neutrons are about 1000 times heavier than electrons, and this affects their deflection by electric fields.

Proton was discovered by Goldstein in 1886, electron by Thomson in 1897, and neutron by Chadwick in 1932.

The mass of an atom is determined by the total number of protons and neutrons in the nucleus.

An atom's charge is neutral when the number of protons equals the number of electrons.

In ion notation, positive ions indicate electron loss, while negative ions indicate electron gain.

Protons, neutrons, and electrons behave differently in a magnetic field, with protons deflecting towards the negative pole and electrons towards the positive.

The concept of isotopes refers to atoms with the same atomic number but different numbers of neutrons.

Isobars are atoms with the same mass number but different atomic numbers.

Isotones are atoms that have the same number of neutrons but different numbers of protons.

Isoelectronic species are atoms or ions that have the same number of electrons.

Atomic mass is the sum of protons and neutrons; in the example of sodium, its mass number is 23.

In sodium's positive ion (Na+), it loses one electron, so the number of electrons is one less than the number of protons.

The periodic table symbol for each element includes its atomic number (proton count) and mass number (proton + neutron count).