Name: reading element symbols and isotope notation
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 2 min 31 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.1.1

Elements: Chemical Symbols and Isotopes

원소는 한 종류의 원자만 포함하는 순수한 물질입니다. 현재 118개의 원소가 발견되었으며 일부는 자연에서 발견하고 일부는 실험실에서 합성되었습니다. 원소들은 매우 다양한 양으로 존재합니다.

지각에서 가장 풍부한 원소는 산소, 실리콘, 알루미늄, 철, 그리고 칼슘입니다. 이에 비해 지구의 대기는 대부분 질소와 산소로 이루어져 있습니다. 주기율표의 각 사각형에는 최소한 원자 번호와 화학 기호가 포함되어 있습니다.

화학 기호는 원소에 할당된 한 개 또는 두 개의 문자 약어입니다. 첫 번째 문자는 대문자이고 두 번째 문자는 필요한 경우 소문자로 써서 두 개의 원소가 포함된 화합물과의 혼동을 피합니다. 보통 이 기호는 원소의 영어 이름의 첫 번째 문자 또는 일부 문자들입니다.

하지만 일부 기호들은 그리스어, 라틴어 또는 독일어에서 유래합니다. 화학 기호에 추가적인 세부사항을 추가할 수 있습니다. 양성자의 개수인 원자 번호는 왼쪽 아래첨자 위치에 기록됩니다.

이 번호는 한 원소에 대해 항상 동일하며 변경되지 않으므로 생략되기도 합니다. 양성자 수와 중성자 수의 합인 질량수는 왼쪽 위첨자 위치에 표시됩니다. 이 숫자는 탄소-12 또는 탄소-13과 같이 원소의 특정 동위원소를 정의합니다.

동위원소는 핵에 있는 중성자의 수는 서로 다르지만 양성자의 수, 즉 원자 번호가 같은 원소의 변종입니다. 동위원소들은 원자 질량이 서로 다르지만 원자의 전하는 동일합니다. 예를 들어 수소 원소는 세 개의 자연 발생 동위원소를 가지고 있습니다.

가장 많은 형태는 중성자가 없는 수소이고, 두 번째는 중성자 1개를 포함하는 중수소이며, 세 번째는 중성자 2개를 포함하는 삼중수소입니다. 표준 수소 원자와 중수소는 자연 조건에서 안정적이지만, 삼중수소와 같은 다른 동위원소는 에너지를 방출하면서 다른 물질로 됩니다. 이런 원소들을 방사성 동위원소라고 합니다.

<ol>
	<li>Pothoof, Justin, Grace Nguyen, Dawn Archey, E. Prasad Venugopal 및 Mark A. Benvenuto. "요소 118 : 새로운 학생에게 새로운 요소 교육." 오래된 요소와 새로운 요소 : 발견, 개발, 도전 및 환경 영향, pp. 195-201. 미국화학회, 2017.</li>
	<li>Krebs, Robert E. 지구의 화학 원소의 역사와 사용: 참조 가이드. 그린우드 출판 그룹, 2006.</li>
	<li>클레이튼, 도널드. 우주의 동위원소 핸드북: 수소에서 갈륨으로. 1권. 케임브리지 대학 출판부, 2003.</li>
</ol>

요소: 화학 기호 및 동위원소

화학 기호는 원소나 원소의 원자를 나타내는 데 사용되는 약어입니다. 예를 들어, 수은의 기호는 Hg입니다. 동일한 기호는 수은 원자 하나(미시적 영역)를 나타내거나 수은 원소의 여러 원자가 담긴 용기(거시적 영역)를 표시하는 데 사용됩니다.

일부 기호는 요소의 일반적인 영어 이름에서 파생됩니다. 다른 것들은 라틴어, 그리스어, 독일어 등 다른 언어로 된 이름의 약어입니다. 예를 들어, 알루미늄(일반명)의 기호는 Al이고, 철의 기호는 Fe이며 이는 라틴어 이름 "Ferrum"에서 유래되었습니다. 대부분의 기호는 한두 글자로 구성되지만, 원자 번호가 112보다 큰 일부 원소를 설명하는 데 세 글자 기호가 사용되었습니다. 다른 표기법과의 혼동을 피하기 위해 기호의 첫 글자만 대문자로 표시합니다. 예를 들어, Co는 코발트 원소의 기호이지만 CO는 탄소(C)와 산소(O) 원소의 원자를 포함하는 일산화탄소 화합물의 표기법입니다.

전통적으로 새 요소의 발견자(또는 발견자들)가 요소의 이름을 지정합니다. 그러나 IUPAC(국제순수응용화학연맹)에서 이름을 인정할 때까지 새 원소의 권장 이름은 원자 번호에 해당하는 라틴어 단어를 기반으로 합니다. 예를 들어, 106번 원소는 운닐헥슘(Unh), 107번 원소는 운닐셉튬(Uns), 108번 원소는 우닐록튬(Uno)으로 불렸습니다. 이러한 요소는 이제 과학자(또는 가끔 위치)의 이름을 따서 명명됩니다. 예를 들어, 106번 원소는 현재 여러 중원소 발견에 적극적으로 참여한 노벨상 수상자 글렌 시보그(Glenn Seaborg)를 기리기 위해 시보그늄(Sg)으로 알려져 있습니다.

주기율표의 각 사각형에는 최소한 원자 번호(양성자 수이기도 함)와 화학 기호가 포함되어 있습니다.

동위원소의 경우에는 질량수 또는 양성자와 중성자의 합을 기호와 원자번호와 함께 표시한다. 질량수는 원소의 특정 동위원소를 정의합니다. 예를 들어, 다음은 질소의 두 동위원소입니다.



<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/805/805_Equation_1.png" style="height: 25px;" />



모든 원소의 특정 동위원소에 대한 기호는 원소 기호 왼쪽에 위 첨자로 질량수를 배치하여 작성됩니다. 원자번호는 원소의 기호와 마찬가지로 원소의 정체성을 정의하기 때문에 생략되는 경우가 많습니다. 예를 들어, 마그네슘은 각각 원자 번호가 12이고 질량수가 각각 24, 25, 26인 세 가지 동위원소의 혼합물로 존재합니다. 이 동위원소는 ^24Mg, ^25Mg, ^26Mg로 식별될 수 있습니다. 이러한 동위원소 기호는 “원소, 질량수”로 읽으며 이 읽는 것과 일관되게 기호화할 수 있습니다. 예를 들어, ^24Mg는 "마그네슘 24"로 읽히고 "마그네슘-24" 또는 "Mg-24"로 쓸 수 있습니다. ^25Mg는 "마그네슘 25"로 읽으며 "마그네슘-25" 또는 "Mg-25"로 쓸 수 있습니다. 모든 마그네슘 원자는 핵에 12개의 양성자를 가지고 있습니다. ^24Mg 원자에는 핵에 12개의 중성자가 있고, ^25Mg 원자에는 13개의 중성자가 있고, ^26Mg에는 14개의 중성자가 있다는 점만 다릅니다.

표준 이름과 기호 외에도 수소 동위원소는 흔히 일반 이름과 그에 수반되는 기호를 사용하여 언급됩니다. 2^H로 표시되는 수소-2는 중수소라고도 하며 때로는 D로 표시되기도 합니다. 3^H로 표시되는 수소-3은 삼중수소라고도 하며 때로는 T로 표시됩니다.

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/2-3-atomic-structure-and-symbolism">Openstax Chemistry 2e, Section 2.3: Atomic Structure and Symbolism.</a>

화학 기호는 원소 또는 원소의 원자를 나타내는 데 사용되는 약어입니다. 예를 들어, 수은의 기호는 Hg입니다. 같은 기호는 ...

Education

교육

JoVE Core

화학

하나

Atoms and Elements

원자와 원소

KEY TERMS AND CONCEPTS

주요 용어 및 개념

reading element symbols and isotope notation

Chemical symbols and isotope notation help identify elements and their atoms. A chemical symbol is an abbreviation for an element or a single atom of that element. Mercury, for example, is written as Hg. The same symbol can point to one atom in the microscopic domain or to many atoms of the element in a container or sample.

Many symbols come from the element’s common English name. Others come from Latin, Greek, or German names. Aluminum uses Al, while iron uses Fe from the Latin word Ferrum. Most symbols have one or two letters. Some elements with atomic numbers greater than 112 have used three-letter symbols.

Capital letters matter in chemical symbols. Only the first letter is capitalized to avoid confusion with other notation. Co means cobalt, but CO means carbon monoxide. Carbon monoxide contains carbon, C, and oxygen, O. New element names are usually chosen by the discoverer, but they must be recognized by the International Union of Pure and Applied Chemistry, or IUPAC.

Before IUPAC approves a new name, temporary names based on Latin number words may be used. Element 106 was called unnilhexium, with the symbol Unh. Element 107 was unnilseptium, Uns. Element 108 was unniloctium, Uno. These elements are now named after scientists or sometimes places. Element 106 is now seaborgium, Sg, named for Glenn Seaborg, who helped discover several heavy elements.

The periodic table gives key information in each square. It includes the atomic number and a chemical symbol. The atomic number is also the number of protons. For isotopes, the mass number is shown too. The mass number is the total number of protons and neutrons, and it identifies the specific isotope.

Isotope symbols place the mass number as a superscript to the left of the element symbol. The atomic number is often left out because the symbol already identifies the element. Magnesium has three isotopes: magnesium-24, magnesium-25, and magnesium-26. They can also be written as 24 Mg, 25 Mg, and 26 Mg. Each magnesium atom has 12 protons, but they differ in neutrons. Magnesium-24 has 12 neutrons, magnesium-25 has 13, and magnesium-26 has 14.

Hydrogen isotopes also have special names. Hydrogen-2, written as 2 H, is called deuterium and may also be shown as D. Hydrogen-3, written as 3 H, is called tritium and may also be shown as T. These names and symbols are commonly used alongside the standard isotope notation.

Reading Element Symbols and Isotope Notation

reading-element-symbols-and-isotope-notation

the atomic theory of matter

Dalton’s Laws and Early Atomic Ideas

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab. The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and...

subatomic particles

Atomic Structure: Protons, Neutrons, and Electrons

Atomic structure is built from three subatomic particles: protons, neutrons, and electrons. Atoms make up all matter, and these particles explain an atom’s mass and charge. The electron was first identified at the end of the 19th century by J.J. Thomson. He used a cathode ray tube, a sealed glass tube with almost all the air removed and two metal electrodes. When high voltage was applied, a visible beam called a cathode ray formed. The beam bent toward positive charge and away from negative...

elements: chemical symbols and isotopes

Chemical symbols and isotope notation help identify elements and their atoms. A chemical symbol is an abbreviation for an element or a single atom of that element. Mercury, for example, is written as Hg. The same symbol can point to one atom in the microscopic domain or to many atoms of the element in a container or sample. Many symbols come from the element’s common English name. Others come from Latin, Greek, or German names. Aluminum uses Al, while iron uses Fe from the Latin word Ferrum.

ions and ionic charges

Predicting Ion Charges on the Periodic Table

Ion charges can often be predicted from an element’s position on the periodic table. In chemical reactions, the nucleus stays unchanged, but electrons may be transferred, lost, or shared. When atoms gain or lose electrons during compound formation, they become ions, which are electrically charged particles. A positive ion is called a cation. A cation has more protons than electrons because it lost electrons. A negative ion is called an anion. An anion has more electrons than protons because it...

the periodic table

Periodic Table Patterns and Element Groups

The periodic table organizes elements by repeating patterns in their properties. Chemists first noticed that some elements behaved alike, so they grouped them by chemical behavior. Lithium, sodium, and potassium are one example. They are shiny and conduct heat and electricity well. Calcium, strontium, and barium form another group with similar physical and chemical properties. Yet these two groups are not the same. The lithium group is much more reactive, and its elements form oxygen compounds...

atomic mass

Average Atomic Mass and Isotopes

Average atomic mass explains why many elements on the periodic table have decimal values. Atoms are extremely small, so scientists use the atomic mass unit, or amu, to measure them. A carbon atom weighs less than 2 × 10−23 g, and the amu is defined from carbon-12. One amu is exactly 1/12 the mass of one carbon-12 atom, which is 1.6605 × 10−24 g. The dalton (Da) and the unified atomic mass unit (u) mean the same thing as the amu. For a single atom, atomic mass is usually close to its mass...

molar mass

Mole, Mass, and Avogadro’s Number

The mole links mass and the number of particles in a substance. It gives chemists a standard way to count atoms and molecules in samples that are far too small to see. It also helps show why substances with the same kinds of atoms can still have very different properties, like water, H2O, and hydrogen peroxide, H2O2. The mole is an amount unit, like a pair or a dozen. One mole contains 6.02214076 × 10^23 discrete entities, such as atoms or molecules. This number is usually rounded to 6.022 ×...

key terms and concepts

Learn how chemical symbols, atomic numbers, and isotope notation identify elements, from mercury and iron to magnesium and hydrogen isotopes.

Reading Element Symbols and Isotope Notation | JoVE K12

chemistry

JoVE Core 화학은 간결하고 이해하기 쉬운 애니메이션을 통해 일반 화학 개념을 설명합니다. 또한, 과학자가 직접 고전실험과 연구실험을 진행하는 실사 영상을 제공합니다.

Physical Science

PS.PSc.1.1

PS.PSc.1.5

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Classification of matter

Atoms

Structure And Properties Of Matter

Quantifying matter

Physical Geology

Minerals

Atoms and elements

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.a

PS.4

PS.4.a

PS.4.b

Texas Essential Knowledge and Skills

High School

Earth Systems Science

112.49.c.7.

112.49.c.7.A.

Arizona Science Standards

HS.P1

HS.P1U1.1

HS+C.P1

HS+C.P1U1.1

CHEM.6

CHEM.6.D

Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.1.a

9-12.C.1.1.b

9-12.PS.3.4

9-12.PS.3.4.d

Next Generation Science Standards

HS-PS1-2

HS-PS1-7

Earth and Space Science

Earth’s Place in the Universe

HS-ESS1-3

Florida Department of Education

SC.912.P.8

SC.912.P.8.4

Chemistry and Physics

IPC.7

IPC.7.A

Georgia Standards of Excellence

SC1.

Isotopes and Atomic Mass

Scientific Laws and Theories

Scientific Laws

In science, a law is defined as a concise, verbal or mathematical, statement that summarizes a vast number of experimental observations. ...

The Scientific Method

Chemistry is an empirical science. Scientists often pose questions to understand the chemistry in everyday life and seek answers to these questions. To ...

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Use models to explain how the scientific understanding of atomic structure has evolved.

Radioactivity and Nuclear Equations

Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for ...

Types of Radioactivity

The most common types of radioactivity are &#945; decay, &#946; decay, &#947; decay, neutron emission, and electron capture.
Alpha (&#945;) decay is the ...

Nuclear Stability

Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10&#8722;15 meters, a nucleus is ...

Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

electron-configuration-of-multielectron-atoms

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

bond-polarity-dipole-moment-and-percent-ionic-character

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Reading Element Symbols and Isotope Notation

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