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

Element periyodik tablosu, kimyada elementleri organize eden önemli bir referanstır. Tabloda yukarıdan aşağıya numaralandırılmış yedi satır ve gruplar veya aileler olarak adlandırılan on sekiz sütun vardır. Bu gruplar iki farklı şekilde numaralandırılabilir.Uluslararası Temel ve Uygulamalı Kimya Birliği, IUPAC, tarafından önerilen modern numaralandırma sistemi, grupları 1'den 18'e kadar numaralandırırken, Kimyasal Kuramlar Servisi grupları belirtmek için roma rakamları ve harfleri kullanır. Burada ana grup elementleri A harfi ile, geçiş elementleri ise B harfi ile belirtilmiştir. Periyodik tablodaki elementler, atom numarası artırılarak soldan sağa ve yukarıdan aşağıya sıralanır.Benzer özelliklere sahip olanlar aynı gruba girer. Bazı grupların ortak isimleri vardır. Hidrojen dışındaki grup 1'deki elementler alkali metaller ve grup 2'deki elementler alkali toprak metaller olarak bilinir.Bu metallerin tümü oldukça reaktiftir ve doğada diğer elementlerle birlikte bulunur. On yedinci gruptaki son derece reaktif, metal olmayan elementler halojenler olarak bilinir. Grup 18'in reaktif olmayan, metalik olmayan elementleri, asal veya inert gazlar olarak adlandırılır.Elementler üç geniş sınıfa ayrılabilir:metaller, ametaller ve metaloidler. Metaller, periyodik tablonun soluna ve ortasına doğru gruplanır ve elementlerin büyük çoğunluğunu oluşturur. İyi elektrik ve ısı iletkenleridir.Sıvı olan cıva dışında tümü oda sıcaklığında katıdır. Metaller parlaktır ve dövülerek levha haline getirilebilir ve tel yapılabilirler. Potasyum gibi metaller, diğer elementlerle reaksiyona girdiklerinde, pozitif yüklü iyonlar olan katyonlar oluşturmak için elektron kaybetme eğilimindedir.Ametaller, periyodik tablonun sağ tarafında gruplandırılır ve genellikle zayıf ısı ve elektrik iletkenleridir. Oda sıcaklığında, bazıları katı, bazıları sıvı veya gazdır. Ametaller diğer elementlerle reaksiyona girdiklerinde elektron kazanma ve negatif yüklü iyonlar oluşturma eğilimindedir.Yarı metaller, metal ve ametaller arasındaki ayrım boyunca bulunan elementlerdir. En küçük element sınıfıdırlar ve karışık özellikler gösterirler. Tüm yarı metaller oda sıcaklığında katı halde bulunur.Bazıları, örneğin silikon ve germanyum, yarı iletken görevi görür, yani metallerin aksine, sıcaklık arttıkça elektrik iletmede daha iyi hale gelirler. Oda sıcaklığında, tüm yarı metaller katı olarak bulunur. Periyodik tablodaki elementler ayrıca konumlarına göre genelde üç kategoriye ayrılır:ana grup elementleri, geçiş metalleri ve her satırdaki ilk element için lantanitler ve aktinitler olarak da bilinen iç geçiş metalleri.

periyodik tablo

İlk kimyagerler daha fazla element keşfettikçe, çeşitli elementlerin benzer kimyasal davranışlarına göre gruplandırılabileceğini fark ettiler. Bu gruplardan biri lityum (Li), sodyum (Na) ve Potasyum (K) içerir. Tüm bu elementler parlaktır, ısı ve elektriği iyi iletir ve benzer kimyasal özelliklere sahiptir. İkinci grup, aynı zamanda parlak, iyi ısı ve elektrik iletkenleri olan ve ortak kimyasal özelliklere sahip olan kalsiyum (Ca), stronsiyum (Sr) ve baryumu (Ba) içerir. Bununla birlikte, bu iki grubun spesifik özellikleri birbirinden önemli ölçüde farklıdır. Örneğin, Li, Na ve K, Ca, Sr ve Ba'dan çok daha reaktiftir. Ek olarak, Li, Na ve K, iki atomunun bir oksijen atomuna oranında oksijen ile bileşikler oluştururken, Ca, Sr ve Ba, atomları oksijen atomu ile bire bir bileşikler oluşturur. Flor (F), klor (Cl), brom (Br) ve iyot (I) da birbirine benzer özellikler gösterir, ancak bu özellikler yukarıdaki elementlerden herhangi birinden büyük ölçüde farklıdır.
 
 Rusya'dan Dimitri Mendeleev (1869) ve Almanya'dan Lothar Meyer (1870), o dönemde bilinen elementlerin özellikleri arasında periyodik bir ilişki olduğunu bağımsız olarak fark ettiler. Her ikisi de artan atom kütlesine göre düzenlenmiş elementlerle tablolar oluşturdu. Bununla birlikte, Mendeleev Meyer'den bir adım daha ileri gitti; tablosunu alüminyum ve silikona benzer özelliklere sahip olacak ancak henüz bilinmeyen elementlerin varlığını tahmin etmek için kullandı. Galyum (1875) ve germanyumun (1886) keşifleri Mendeleev'in çalışmaları için önemli bir destek sağladı. Mendeleev ve Meyer'in öncelik konusunda uzun bir anlaşmazlığı olmasına rağmen, Mendeleev'in periyodik tablonun gelişimine katkıları artık daha yaygın olarak kabul edilmektedir.
 
 Yirminci yüzyıla gelindiğinde, periyodik ilişkinin atomik kütlelerden ziyade atom numaralarını içerdiği ortaya çıktı. Bu ilişkinin modern ifadesi, periyodik yasa, şunu belirtir: Elementlerin periyodik fonksiyonları, atom numaralarının bir fonksiyonudur. Modern bir periyodik tablo, elementleri atom numaralarının artan sırasına göre düzenler ve aynı dikey sütunda benzer özelliklere sahip atomları gruplandırır. Her kutu bir elemanı temsil eder ve atom numarasını, sembolünü, ortalama atom kütlesini ve (bazen) adını içerir.
 
 Elementler, periyotlar veya seriler olarak adlandırılan yedi yatay satır ve gruplar olarak adlandırılan 18 dikey sütun halinde düzenlenmiştir. Gruplar her sütunun en üstünde etiketlenir. Tablonun tek bir sayfaya sığması için, toplam 14 sütun olmak üzere iki satırın parçaları genellikle tablonun ana gövdesinin altına yazılır.
 
 Birçok element kimyasal ve fiziksel özelliklerinde önemli ölçüde farklılık gösterirken, bazı elementler davranışlarında benzerdir. Örneğin, birçok element parlak görünür, dövülebilir ve sünektir ve ısı ve elektriği iyi iletir. Diğer elemanlar parlak, dövülebilir veya sünek değildir ve zayıf ısı ve elektrik iletkenleridir. Elementler ortak özelliklere sahip büyük sınıflara ayrılabilir: metaller (parlak, dövülebilir, iyi ısı ve elektrik iletkenleri olan elementler - sarı renkli); ametaller (donuk görünen elementler, zayıf ısı ve elektrik iletkenleri; gölgeli kırmızı); ve metaloidler (ısı ve elektriği orta derecede iyi ileten ve metallerin bazı özelliklerine ve ametallerin bazı özelliklerine sahip elementler - gölgeli mor).
 
 <img alt=""Figure1"" src=""https://www.jovecore.com/CDNSource/lessons/806/806_Image_1_white.png"" style=""width: 700px;"" />
 
 Öğeler ayrıca 1A, 2A ve 3A-8A etiketli sütunlardaki ana grup öğelerine (veya temsili öğelere) sınıflandırılabilir; 3B-2B etiketli sütunlardaki geçiş metalleri; ve tablonun altındaki iki sıradaki iç geçiş metalleri. Tablonun altındaki üst satır öğeleri lantanitlerdir ve alt satır öğeleri aktinitlerdir. Elementler, oluşturdukları bileşiklerin bileşimi gibi daha spesifik özelliklerle daha da alt bölümlere ayrılabilir. Örneğin, grup 1A'daki (ilk sütun) elementler, elementin bir atomundan ve bir hidrojen atomundan oluşan bileşikler oluşturur. Bu elementler (hidrojen hariç) alkali metaller olarak bilinir ve hepsi benzer kimyasal özelliklere sahiptir. Grup 2A'daki elementler (ikinci sütun), elementin bir atomundan ve iki hidrojen atomundan oluşan bileşikler oluşturur: bunlar, bu grubun üyeleri arasında benzer özelliklere sahip alkali toprak metalleri olarak adlandırılır.
 
 Spesifik isimleri olan diğer gruplar azot grubu (grup 5A), kalkojenler (grup 6A), halojenler (grup 7A) ve soy gazlardır (inert gazlar olarak da bilinen grup 8A). Gruplar ayrıca grubun ilk elemanı tarafından da adlandırılabilir: örneğin, kalkojenler oksijen grubu veya oksijen ailesi olarak adlandırılabilir. Hidrojen, hem grup 1A hem de grup 7A elementlerine benzer özelliklere sahip benzersiz, metalik olmayan bir elementtir. Bu nedenle, hidrojen her iki grubun en üstünde veya kendi başına gösterilebilir.
 
 Element 43 (teknetyum), element 61 (prometyum) ve atom numarası 84 (polonyum) ve daha yüksek olan elementlerin çoğu, atomik kütlelerini köşeli parantez içinde verir. Bu gösterim, tamamen kararsız, radyoaktif izotoplardan oluşan elementler için kullanılır (radyoaktivite nükleer kimya bölümünde daha ayrıntılı olarak ele alınmıştır). Bu elementler için ortalama bir atom ağırlığı belirlenemez, çünkü radyoizotopları kaynağa bağlı olarak nispi bollukta önemli ölçüde değişebilir veya doğada bile bulunmayabilir. Köşeli parantez içindeki sayı, bu elementin en kararlı izotopunun yaklaşık atomik kütlesi olan atomik kütle sayısıdır.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/2-5-the-periodic-table"">Openstax, Chemistry 2e, Section 2.5: The Periodic Table.</a>

Periyodik Tablo

İlk kimyagerler daha fazla element keşfettikçe, çeşitli elementlerin benzer kimyasal davranışlarına göre gruplandırılabileceğini fark ettiler. Böyle bir gruplama ...

Education

JoVE Core

Kimya

Atoms and Elements

Atomlar ve Elementler

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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 Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

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

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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

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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

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South Carolina College and Career Ready Science Standards

C-PS1-1

C-PS1-2

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New York State Science Learning Standards

HS. Chemical Reactions

HS-PS1-2.

Georgia Standards of Excellence

SPS1.

Periodic Table Trends

SC1.

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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 ...

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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 ...

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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 ...

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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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