Search Results

b9509307-f4ef-457a-b044-a8b782f7d938 Know that an α particle is the nucleus of a helium atom Summary An α particle, often denoted as ^4He, is a fundamental subatomic particle that serves as the nucleus of a helium atom. It is composed of two protons and two neutrons, giving it a mass number of 4 and an atomic number of 2. The α particle is named after the Greek letter α (alpha) due to its historical significance in early studies of radioactivity and nuclear physics. Being the nucleus of a helium atom means that the α particle carries the essential components responsible for the atom's identity. It contains the positively charged protons, which determine the atomic number and chemical properties of the helium atom. The presence of two protons in the α particle gives it a net positive charge of +2, balancing the negatively charged electrons surrounding the nucleus in a helium atom. The α particle is highly stable due to its tightly bound configuration of protons and neutrons within the nucleus. This stability contributes to its occurrence in various nuclear reactions and natural processes. In certain radioactive decays, such as alpha decay, a parent nucleus emits an α particle, reducing its atomic number by 2 and its mass number by 4. This emission results in the formation of a daughter nucleus with a different atomic identity. The α particle possesses unique properties that distinguish it from other subatomic particles. It has a relatively large mass compared to other particles and can penetrate matter to a limited extent due to its charge and mass. In practical applications, α particles are commonly used in radiation detectors and nuclear research. Their distinctive properties make them useful for studying particle interactions, measuring radiation levels, and investigating the properties of atomic nuclei. Understanding that an α particle is the nucleus of a helium atom is fundamental to comprehending the structure of matter and the behavior of subatomic particles. It allows us to appreciate the role of α particles in nuclear processes and their significance in the overall composition of atoms. In summary, an α particle serves as the nucleus of a helium atom, consisting of two protons and two neutrons. It carries a net positive charge of +2 and possesses unique properties that distinguish it from other subatomic particles. Recognizing the α particle as the nucleus of a helium atom contributes to our understanding of atomic structure, nuclear reactions, and radiation phenomena.

Expert SABIS Grade 12 Chemistry tuition in UAE and online . Weekly live sessions. Boost grades with a top private tutor. Register today at K-Chemistry.com

fbd10ecb-3a32-403a-9a11-d4bc3d88fd79 Physical properties of Gp I - they are all: solid metals, stored under kerosene, soft enough to be cut with a knife, quickly lose their luster when exposed to air, have low density. Summary

d377aebc-40c6-4007-aa48-8c2f6c5c5cc4 The burning of a magnesium ribbon in air Summary Exothermic

< Back Previous Next Chapter 1: Equilibrium

dc07a4f4-6e82-4ceb-a538-6e70005c9038 Condensation Summary The process of a substance changing from a gaseous to a liquid state at a specific temperature.

f33ec294-ddf7-4081-99b2-d8f3e36a355e Generally, reactions with high activation energy tend to be slow. Summary

e596d313-9489-42d3-ab3d-59f48e3e57cf Iodine is shiny yet is a non-metal Summary

9d851dde-33ff-409b-97a8-7a3f534c0feb Any reaction or process that consumes heat energy Summary Endothermic

8e91fe7d-48d9-478d-8486-2505ec7ebf28 Dissolving salt into water to make a solution Summary Physical

9c31eef2-81e0-4428-b3e5-8b1df166529a easy examples for Given the average atomic mass of an element, find the % abundance of its isotopes Summary Example 1: Average atomic mass: 15.8 Isotope A mass: 14 Isotope B mass: 16 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 14) + (y * 16) = 15.8 Equation 2: x + y = 100 Solving the equations, we find that x = 40 and y = 60. Answer: Isotope A: 40% abundance Isotope B: 60% abundance Example 2: Average atomic mass: 18.9 Isotope A mass: 17 Isotope B mass: 20 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 17) + (y * 20) = 18.9 Equation 2: x + y = 100 Solving the equations, we find that x = 30 and y = 70. Answer: Isotope A: 30% abundance Isotope B: 70% abundance Example 3: Average atomic mass: 27.5 Isotope A mass: 26 Isotope B mass: 28 To find the percentage abundance: Let's assume the abundance of Isotope A is x, and the abundance of Isotope B is y. Equation 1: (x * 26) + (y * 28) = 27.5 Equation 2: x + y = 100 Solving the equations, we find that x = 60 and y = 40. Answer: Isotope A: 60% abundance Isotope B: 40% abundance

39ffe242-f6e2-44ab-a7af-5802dcfdfa7c Filtrate Summary The liquid that passes through the filter paper during the filtration process.