General Chemistry 1: Particles of Matter PDF
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This document explains the fundamental concepts of atoms and molecules, including their structure, properties, and common isotopes. It also describes the concept of isotopes and covers their different applications. This document serves as a general chemistry reference material.
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GENERAL CHEMISTRY 1 1.2. Two Regions of an Atom Chapter 2: Particles of Matter Objectives: 1. Recall the concept of atoms and its structure; 2. Calculate the percent abundance of an element; and 3. Recognize common isotopes and their uses....
GENERAL CHEMISTRY 1 1.2. Two Regions of an Atom Chapter 2: Particles of Matter Objectives: 1. Recall the concept of atoms and its structure; 2. Calculate the percent abundance of an element; and 3. Recognize common isotopes and their uses. Lesson 1: Atom and Its Structure 1.2.1. Atomic Nucleus 1.1. Particles of Matter Center of atom Generally made of neutrons and protons Atom Contains most of an atom's mass Basic building block of matter 1.2.2. Electron Cloud Single neutral particle Area surrounding nucleus that contains most of the Composed of sub-particles space in the atom o Electron Electron resides outside of the nucleus in this o Proton electron cloud o Neutron Molecule Neutral particles made of two or more atoms bonded together Two atoms of the same kind combined exist as diatomic molecule o H2 Lesson 2: Isotopes o N2 o F2 Atomic Number, Z o O2 Atomic number is the number of protons (p+) in the nucleus of o I2 the atom of an element. o Cl2 The number of protons (p+) is equal to the number of electrons (e- o Br2 𝒁 = 𝒑! = 𝒆" Atoms of different elements combined can form a molecule of compound – H2O. Mass Number, A The total number of protons (p+) and neutrons (n0) in the nucleus Ions of an atom. Particles that lose or gain electrons 𝑨 = 𝒑! + 𝒏𝟎 = 𝒁 + 𝑵 Charged particles 𝑵=𝑨−𝒁 o Cations – positively charged, LOSES electron Where:A = mass number o Anions – negatively charged, GAIN electron Z = atomic number or number of protons N = number of neutrons 2.1. Isotopic Notation 4. Phosphorous-32 – Added to fertilizer to study plant processes 5. Nitrogen-15 – Added to fertilizer to study plant processes 6. Cesium-137 – Use to kill bacteria 7. Fluorine-18 – Use for diagnosis and treatment of diseases 8. Gallium-67 – Use for diagnosis and treatment of diseases 9. Carbon-14 – Carbon dating process 2.2. Isotopes Atoms that have the same number of protons but different numbers of neutrons. Two Categories of Isotopes 1. Unstable – isotopes that continuously and spontaneously break down/decay in other lower atomic weight isotopes Radioisotopes – produce radiation during breaking down process 2. Stable – isotopes that do not naturally decay but can exist in natural materials in differing proportions Percent Abundance and Relative Atomic Mass Common Isotopes and their Uses 1. Sodium-24 – Injected into limb to detect blood clot 2. Cobalt-60 – Detect and treat cancer/ use to kill bacteria 3. Iodine-131 – Detect functions of thyroid gland
