Name: periodic table patterns and element groups
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 3 min 25 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.2.1

The Periodic Table

元素週期表是在化学中用于组织 元素的重要参考。表中从顶到底有七行或称周期，和十八列称为组或族。这些族可以以两种不同的方式编号。虽然被国际纯化学及应用化学联合会（IUPAC）推荐的现代编号系统，族以1至18命名，化学摘要服务社（Chemical Abstracts Services）则使用罗马数字及字 母指定组的名字。在此，主族元素被指定为字母A 且过渡元素被指定为B。在周期表的元素们以 左至右从上到下依 照原子数依序排列。拥有同样属性的元素会被分在同一族中。其中一些族他们具有共同的名称。第一族中，除了氢原子，被称为硷金属，而第二族称为硷土金属。这些金属都很活泼，当在自然界被发现时，通常和其他元素组合在一起。活性强的非金属元素在第十七族，他们被称为卤素。无反应的非金属元素在第十八族，被称为稀有或惰性气体。元素可以被分类成三大类：金属、非金属、类金属。金属类被分类在週 期表左边及中间，并为绝大多数的元素。他们是电及热的良好导体。在室温下皆为固态，除了汞，其为液态。金属为闪亮的，并且可以 被搥成薄片及拉成金属丝。金属，比如钾，在与其他元素反应时，易于失去电子，形成阳离子，即带正电的离子。非金属元素被分 类在周期表的右侧，通常导热及导电性差。在室温下，有些为固态，而其他为液态或者气态。非金属元素和其他元素反应时，易于得到电子而形成负离子，即带负电的离子。类金属元素是在界定金属及非 金属元素的分界上被找到的。他们是元素中最小的一类，其拥有溷合金 属与非金属的属性。所有的类金属在室温下是固态的。有些类金属元素，比如硅和锗，为半导体，因为他们和金属不同，他们随着温度提升 其导电能力越强。在室温下，所有的类金属为固态。週期表中的元素常常被分为三个种类，依据他们的分布的位置：主族元素，过渡元素，及内过渡元素，也称为镧系元素锕系元素，尤其各行的第一 个元素所命名。

元素周期表

随着早期化学家发现更多的元素，他们意识到可以通过相似的化学行为对各种元素进行分组。一种这样的分组包括锂（Li），钠（Na）和钾（K）。所有这些元素都是有光泽的，导热和导电性好，并且具有相似的化学性质。第二类包括钙（Ca），锶（Sr）和钡（Ba），它们也是有光泽的，良好的热和电导体，并且具有共同的化学性质。然而，这两个分组的具体性质彼此明显不同。例如，锂（Li），钠（Na）和钾（K）的反应性比钙（Ca），锶（Sr）和钡（Ba）高得多。另外，锂（Li），钠（Na）和钾（K）以两个原子与一个氧原子的比率与氧形成化合物，而钙（Ca），锶（Sr）和钡（Ba）形成一个原子与一个氧原子的化合物。氟（F），氯（Cl），溴（Br）和碘（I）也表现出相似的性质，但是这些性质与上述任何元素都大不相同。
 
 俄罗斯的狄米特里·门捷列夫（Dimitri Mendeleev，1869）和德国的洛萨·迈尔（Lothar Meyer，1870）独立地认识到当时已知元素的性质之间存在周期性关系。这两个表均根据原子质量的增加排列了元素。然而，门捷列夫比迈尔走了一步。他用他的表来预测元素的存在，这些元素的性质类似于铝和硅，但尚不为人所知。镓gallium（1875年）和锗germanium（1886年）的发现为门捷列夫的工作提供了重要的支持。尽管门捷列夫和迈尔在优先权上存在长期争论，但门捷列夫对元素周期表发展的贡献现在得到了更广泛的认可。
 
 到20世纪，很明显，周期性关系涉及原子数而不是原子质量。关于这种关系的现代说法是周期定律，它陈述如下：元素的性质是其原子序数的周期函数。现代的元素周期表以原子序号从小到大的顺序排列元素，并将具有相似属性的原子分组在同一垂直列中。每个框代表一个元素，并包含其原子序数，符号，平均原子质量和（有时）名称。
 
 这些元素按七个水平行（称为周期或系列）和18个垂直列（称为组）排列。组被标记在每列的顶部。为了使表格适合单个页面，通常将两行的一部分（共14列）写在表格的主体下方。
 
 许多元素的化学和物理性质差异很大，但某些元素的行为相似。例如，许多元素看起来有光泽，具有延展性和韧性，并能很好地传导热量和电流。其他元素没有光泽、没有可延展性或韧性，并且是热和电的不良导体。这些元素可以分为具有共同特性的大类：金属（光泽，可延展的元素，良好的热和电导体-黄色阴影），金属（具有光泽的元素）。非金属（看起来暗淡，热和电不良的元素-红色阴影）；和准金属（导热性和电性适中的元素，并具有金属的某些特性和非金属的某些特性-阴影为紫色）。
 
 <img alt =“ Figure1” src =“ https://www.jove.com/files/core/CDNSource/lessons/806/806_Image_1_white.png” style =“ width：700px; ” /> 
 
 在标记为1、2和13 18的列中，这些元素也可以分为主要组元素（或代表元素）。标记为3到12的列中的过渡金属；表格底部的两行和内部过渡金属。表格底部的上排元素是镧系元素（lanthanides），下排元素是锕系元素（actinides）。元素可以进一步细分为更具体的属性，例如它们形成的化合物的组成。例如，第1组（第一列）中的元素形成的化合物由该元素的一个原子和一个氢原子组成。这些元素（氢除外）被称为碱金属，并且它们都具有相似的化学性质。第2组（第二列）中的元素形成由该元素的一个原子和两个氢原子组成的化合物：这些被称为碱土金属，在该组成员之间具有相似的性质。
 
 其他具有特定名称的族群是光气原（第15组），硫族元素（第16组），卤素（第17组）和稀有气体（第18组，也称为惰性气体）。这些基团也可以用该组的第一个元素来表示：例如，硫族元素可以称为氧基团或氧族。氢是一种独特的非金属元素，其性质类似于第1组和第17组元素。 因此，氢可能会显示在两个组的顶部或单独显示。
 
 元素43 (锝，technetium)，元素61 (钷，promethium) 以及大多数原子序数为84 (钋，polium) 及更高的元素的原子质量在方括号中给出。 可以对完全由不稳定的放射性同位素组成的元素进行此操作（放射性在核化学章节中有更详细的介绍）。 无法确定这些元素的平均原子量，因为它们的放射性同位素可能会根据来源而相对丰度发生显着变化，甚至可能不存在于自然界中。 方括号中的数字是原子质量数，它是该元素最稳定同位素的近似原子质量。
 
 从 <a href="https://openstax.org/books/chemistry-2e/pages/2-5-the-periodic-table">“> Openstax 化学2e，第2.5节：元素周期表。</a>

随着早期化学家发现的元素越来越多，他们意识到可以根据元素相似的化学性质将其分类。其中一种分类方式……

Education

教育

JoVE Core

化学

Atoms and Elements

原子与元素

KEY TERMS AND CONCEPTS

关键术语与概念

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 in a 2-to-1 atom ratio. The calcium group is less reactive, and its elements form oxygen compounds in a 1-to-1 atom ratio. Fluorine, chlorine, bromine, and iodine also share similar properties, but those properties are very different from the metal groups above.

Dimitri Mendeleev in Russia and Lothar Meyer in Germany both recognized this repeating pattern in the elements in the 1860s and 1870s. They arranged the known elements by increasing atomic mass. Mendeleev went further by predicting elements that had not yet been discovered. He expected elements with properties similar to aluminum and silicon. Later, gallium and germanium were discovered, and they supported his work. Mendeleev and Meyer later disputed who deserved priority, but Mendeleev is now more widely recognized for helping develop the periodic table.

By the twentieth century, scientists saw that the pattern depends on atomic number, not atomic mass. The periodic law says that the properties of the elements change in a repeating way as atomic number increases. A modern periodic table follows this rule. It places elements in order of increasing atomic number and groups elements with similar properties in the same vertical column.

Each box on the periodic table shows one element. It usually includes the atomic number, symbol, average atomic mass, and sometimes the name. The table has seven horizontal rows, called periods, and 18 vertical columns, called groups. The group labels appear at the top. To fit the table on one page, parts of two rows are often shown below the main table. These 14 columns belong to the lanthanides and actinides.

Elements can also be sorted by their physical properties. Metals are shiny, malleable, and ductile, and they conduct heat and electricity well. Nonmetals are usually dull and are poor conductors. Metalloids fall between these two groups. They conduct heat and electricity moderately well and have some properties of metals and some of nonmetals. The table also separates main-group elements in columns 1, 2, and 13 through 18, transition metals in columns 3 through 12, and inner transition metals in the two rows at the bottom.

Some groups have special names based on their chemistry. Group 1 elements, except hydrogen, are alkali metals. They form compounds with one atom of the element and one atom of hydrogen. Group 2 elements are alkaline earth metals, and they form compounds with one atom of the element and two atoms of hydrogen. Other named groups include the pnictogens, chalcogens, halogens, and noble gases. The chalcogens are also called the oxygen family. Hydrogen is unusual because it is a nonmetal with properties similar to both group 1 and group 17. It may appear at the top of either group or by itself.

Some elements have atomic masses shown in square brackets. This includes element 43, technetium, element 61, promethium, and most elements with atomic number 84 and higher, such as polonium. These elements are made entirely of unstable, radioactive isotopes. Because their isotopes can vary in abundance or may not occur naturally, an average atomic weight cannot be given. The bracketed value is the mass number of the most stable isotope, which is an approximate atomic mass.

Periodic Table Patterns and Element Groups

periodic-table-patterns-and-element-groups

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

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.

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

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 the periodic table groups elements by repeating patterns, atomic number, and chemical behavior, including metals, nonmetals, groups, and special names.

Periodic Table Patterns and Element Groups | JoVE K12

chemistry

JoVE Core 化学通过简单明了且通俗易懂的动画视频课程，将普通化学概念带入到现实生活当中。此外，在科学家行动视频中，我们演示了在实验室中进行的经典和原始研究实验。

Physical Science

PS.PSc.1.6

Pennsylvania State Academic Standards

Chemical Reactions

3.2.9-12.C

Structure and Properties of Matter

3.2.9-12.A

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

HS-PS1-2

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Periodic trends of the elements

Structure And Properties Of Matter

Periodic Table

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.a

CH.2.d

PS.2

PS.2.b

PS.4

PS.4.a

PS.4.b

Minnesota Academic Standards in Science

3.1.1 9C.2.1.1.1

9C.3.1.1.1

Arizona Science Standards

HS.P1

HS.P1U1.1

new-jersey-student-learning-standards-for-science

New Jersey Student Learning Standards for Science

Matter and Its Interactions

Alabama Course of Study Science

9-12.PS.3.4.a

Next Generation Science Standards

Florida Department of Education

SC.912.P.8

SC.912.P.8.4

SC.912.P.8.5

Texas Essential Knowledge and Skills

Chemistry and Physics

IPC.7

IPC.7.A

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

C-PS1-1

C-PS1-2

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-2.

Georgia Standards of Excellence

SPS1.

Periodic Table Trends

SC1.

periodic-table-trends-atomic-radii-ionization-and-electronegativity

Periodic Table Trends: Atomic Radii, Ionization, and Electronegativity

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 ...

Elements: Chemical Symbols and Isotopes

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.

PS.Chm.1.1

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 ...

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.

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 ...

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.

Periodic Table Patterns and Element Groups

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