Name: halogens: trends and reactions
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 1 s
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Physical Science

Matter and its Interactions

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Halogens

الهالوجينات هي مجموعة من خمسة عناصر غير معدنية الفلور والكلور والبروم واليود والأستاتين تنتمي إلى المجموعة 17. توجد الهالوجينات الأولية كجزيئات ثنائية الذرة. في درجة حرارة الغرفة،الفلور والكلور غازات،البروم سائل،واليود مادة صلبة.لا يعرف الكثير عن خصائص العنصر الخامس،أستاتين،والذي هو مادة صلبة نادرة وعالية النشاط الإشعاعي. الخصائص الفيزيائية للهالوجينات،مثل لون العنصر،تختلف بالانتقال إلى أسفل المجموعة. يزيد نصف القطر الذري مع زيادة العدد الذري،ونقطة الانصهار والغليان تظهر اتجاها تصاعديا من الفلور إلى اليود.في المقابل،فإن الخصائص الدورية مثل السالبية الكهربية،التفاعلية وتقارب الإلكترون،فإنها تقل بأسفل المجموعة. تكوينات الهالوجينات الإلكترونية تشير إلى أن لديهم سبعة إلكترونات تكافؤ وينقصهم إلكترون واحد للوصول إلى أقرب تكوين للغازات النبيلة. لذلك،تظهر الهالوجينات سالبية كهربية عالية،مع ميل قوي للحصول على إلكترون إضافي واحد،لإكمال الثمانيات الخاصة بهم،مما يجعلها عالية التفاعل وعوامل مؤكسدة قوية،مقارنة بالمجموعات الأخرى.الفلور هو أقوى عامل مؤكسد بين الهالوجينات واليود أقلها. تظهر الهالوجينات أيضًا تقاربات إلكترونية سالبة للغاية،وهي التغيير في الطاقة عندما يكون الإلكترون مكتسب من ذرة محايدة. يتم التعبير عنها بالكيلو جول لكل مول،وتشير القيمة السالبة إلى الطبيعة الطاردة للحرارة للتفاعل.تتفاعل الهالوجينات مع معظم المعادن لإنتاج هاليدات معدنية. على سبيل المثال،يتفاعل الكلور والصوديوم لإنتاج كلوريد الصوديوم،وهو مركب أيوني. تتفاعل الهالوجينات مع الهيدروجين لتكوين مركبات تساهمية قطبية،تسمى هاليدات الهيدروجين،والتي تذوب في الماء غالبًا لتشكيل الأحماض المائية.تتفاعل الهالوجينات أيضًا مع الماء. تفاعل الفلور مع الماء طارد للحرارة بدرجة عالية،منتجاًفلوريد الهيدروجين حمض قوي والأكسجين. ومع ذلك،يتفاعل الكلور بشكل أبطأ،منتجاًحمض الهيدروكلوريك وحمض هيبوكلوروس عامل مؤكسد قوي.بالإضافة إلى ذلك،يمكن أن تتفاعل الهالوجينات مع بعضها البعض،منتجة مركبات ثنائية تساهمية تسمى مركبات انترهالوجين. على سبيل المثال،يتفاعل البروم مع الفلور لتشكيل ثلاثي فلوريد البروم.

الهالوجينات

عناصر المجموعة 17، المعروفة باسم الهالوجينات، هي عناصر لا معدنية. وفي درجة حرارة الغرفة، يكون الفلورين والكلور من الغازات، والبروم سائل، واليود صلب. أستاتين هو عنصر إشعاعي بشكل شديد وهو غير مستقر، لذلك حالياً، كثير من خواصه مجهولة ويعزى السبب إلى عمره النصفي القصير. تينينسين هو عنصر اصطناعي من المتوقع أيضاً أن يكون في هذه المجموعة.  لا توجد الهالوجينات كذرات مفردة ولكنها موجودة كجزيئات ثنائية الذرة. يزداد نصف القطر الذري من الفلورين إلى اليود. إن التوزيع الإلكتروني لغلاف التكافؤ للهالوجينات هو ns2np5، وهي تميل إلى قبول الإلكترون لتحقيق تكوين الغاز النبيل. ترد في الجدول 1  الخصائص المختلفة للهالوجينات. الجدول 1 : خصائص الهالوجينات. <table style="margin-left: auto; margin-right: auto;"><tbody style="border: 1px solid black;"><tr><td style="color: black; border: 1px solid black; text-align: center;">العنصر </td><td style="color: black; border: 1px solid black; text-align: center;">التوزيع الإلكتروني </td><td style="color: black; border: 1px solid black; text-align: center;">نصف القطر الذري (pm) </td><td style="color: black; border: 1px solid black; text-align: center;">IE1 (كيلوجول/مول) </td><td style="color: black; border: 1px solid black; text-align: center;">EA (كيلوجول/مول) </td><td style="color: black; border: 1px solid black; text-align: center;">الكثافة عند 25 درجة مئوية </td><td style="color: black; border: 1px solid black; text-align: center;">نقطة الانصهار (درجة مئوية) </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">و </td><td style="color: black; border: 1px solid black; text-align: center;">[HE] 2s22p5 </td><td style="color: black; border: 1px solid black; text-align: center;">71 </td><td style="color: black; border: 1px solid black; text-align: center;">1680 </td><td style="color: black; border: 1px solid black; text-align: center;">328 </td><td style="color: black; border: 1px solid black; text-align: center;">1.70 جم/لتر </td><td style="color: black; border: 1px solid black; text-align: center;">-219 </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">CL </td><td style="color: black; border: 1px solid black; text-align: center;">[NE] 3s23p5 </td><td style="color: black; border: 1px solid black; text-align: center;">99 </td><td style="color: black; border: 1px solid black; text-align: center;">1250 </td><td style="color: black; border: 1px solid black; text-align: center;">-348 </td><td style="color: black; border: 1px solid black; text-align: center;">3.12 جم/لتر </td><td style="color: black; border: 1px solid black; text-align: center;">-101 </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">br </td><td style="color: black; border: 1px solid black; text-align: center;">[ar] 4s24p5 </td><td style="color: black; border: 1px solid black; text-align: center;">114 </td><td style="color: black; border: 1px solid black; text-align: center;">1140 </td><td style="color: black; border: 1px solid black; text-align: center;">-324 </td><td style="color: black; border: 1px solid black; text-align: center;">3.19 غ/سم3 </td><td style="color: black; border: 1px solid black; text-align: center;">-7 </td></tr><tr><td style="color: black; border: 1px solid black; text-align: center;">أنا </td><td style="color: black; border: 1px solid black; text-align: center;">[KR] 5s25p5 </td><td style="color: black; border: 1px solid black; text-align: center;">133 </td><td style="color: black; border: 1px solid black; text-align: center;">1010 </td><td style="color: black; border: 1px solid black; text-align: center;">-295 </td><td style="color: black; border: 1px solid black; text-align: center;">3.96 جم/سم3 </td><td style="color: black; border: 1px solid black; text-align: center;">114 </td></tr></tbody></table>
 
 إنجذاب الإلكترون للهالوجينات يجعل لها قيم سالبة كبيرة؛ وبالتالي، فإن الهالوجينات هي عوامل مؤكسدة قوية. الفلور هو أقوى عامل مؤكسد في المجموعة مع أكثر تقارب إلكتروني سلبي. تتفاعل الهالوجينات مع المعادن للحصول على الإلكترون وإنتاج هاليد معدني مطابق. على سبيل المثال، يتفاعل الكلور مع الحديد ليعطي كلوريد الحديد ومع الصوديوم ليعطي كلوريد الصوديوم. تتفاعل الهالوجينات مع الهيدروجين لتكوين هاليدات الهيدروجين ، والتي تذوب في الماء لتنتج أحماض الهيدروهاليك. حمض الهيدروفلوريك هو أضعف هالوسيد. يتفاعل الفلور بقوة مع الماء. يكون التفاعل شديد الحرارة وينتج الأكسجين. يكون تفاعل الكلور أقل شدة مع الماء. حمض الهيبوكلوروس الناتج في هذا التفاعل هو عامل مؤكسد قوي. تتفاعل الهالوجينات مع بعضها البعض لتكوين مركبات بين الهالوجين ، وكثير منها عبارة عن مركبات ثنائية. الصيغة الجزيئية العامة للمركبات الهالوجينية هي ABn ، حيث A هو الهالوجين ذو العدد الذري الأعلى وهو رقم فردي. أمثلة قليلة على مركبات الهالوجين هي ICl و IBr و BrF و BrCl و ClF. تتفاعل الهالوجينات مع الكربون لتكوين مركبات ذات أهمية تجارية.  على سبيل المثال ، يتفاعل الإيثيلين مع الفلور ليعطي بيرفلورو إيثيلين. هذا النص مقتبس من <a href="https://openstax.org/books/chemistry-2e/pages/6-5-periodic-variations-in-element-properties">Openstax, Chemistry 2e, Section 6.5: Periodic Variations in Element Properties.</a>

عناصر المجموعة 17 ، المعروفة باسم الهالوجينات ، هي لاقلامية. في درجة حرارة الغرفة ، الفلور والكلور غازات ، والبروم سائل ، واليود صلب. ...

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Periodic Properties of the Elements

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halogens: trends and reactions

Halogens are Group 17 nonmetals that show clear trends in structure and reactivity. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid. Astatine is highly unstable and radioactive, so most of its properties are still unknown because it has a very short half-life. Tennessine is a synthetic element that is also predicted to belong to this group.

These elements do not usually exist as single atoms. Instead, they form diatomic molecules, which means each molecule has two atoms. Their atomic radius increases from fluorine to iodine, and their outer-shell electron pattern is ns2 np5. This electron arrangement helps explain why halogens tend to gain one electron and reach a noble gas configuration.

The table of halogen properties shows important changes across the group. Fluorine has the smallest atomic radius, while iodine has the largest. First ionization energy decreases from fluorine to iodine, and electron affinity stays strongly negative for the group. Because of this, halogens are powerful oxidizing agents, and fluorine is the strongest oxidizing agent in the group.

Halogens react with metals to form metal halides. For example, chlorine reacts with iron to make iron chloride, and it reacts with sodium to make sodium chloride. They also react with hydrogen to form hydrogen halides. When these dissolve in water, they produce hydrohalic acids, and hydrofluoric acid is the weakest haloacid.

Halogens also react with water, but not in the same way. Fluorine reacts very vigorously, and the reaction is highly exothermic, which means it releases a large amount of heat. It also produces oxygen. Chlorine reacts less vigorously with water, and the hypochlorous acid formed is a strong oxidizing agent.

Halogens can react with one another to form interhalogen compounds, which are often binary compounds. Their general formula is ABn, where A is the halogen with the higher atomic number and n is an odd number. Examples include ICl, IBr, BrF, BrCl, and ClF. Halogens also react with carbon to form useful compounds, such as perfluoroethylene from the reaction of ethylene with fluorine.

Halogens: Trends and Reactions

periodic classification of the elements

How Valence Electrons Shape the Periodic Table

The periodic table organizes elements by increasing atomic number, and it also shows why elements in the same group behave alike. As the electron configurations are placed into the table, a repeating pattern appears in the outer shells of atoms. These outer electrons are called valence electrons, and they play the biggest role in chemical reactions. They are the highest-energy electrons in an atom, so they are easier to lose or share than core electrons. Valence electrons also help determine...

ionization energy

Ionization Energy Trends in the Periodic Table

Ionization energy is the energy needed to remove an electron from a gaseous atom or ion in its ground state. The first ionization energy, or IE1, removes the most loosely bound electron and forms a 1+ cation. The second ionization energy, IE2, removes the next electron, and each later ionization energy removes another electron from the atom or ion. Ionization always requires energy, so these processes are endothermic. That means ionization energy values are always positive. In general, larger...

atomic radii and effective nuclear charge

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Periodic Trends in Atomic Size

Periodic trends in atomic size help explain why atoms get larger or smaller across the periodic table. Elements in the same group show similar chemical behavior because they have the same number and arrangement of valence electrons. Across a period, each new element adds one proton to the nucleus and one electron to the valence shell. Down a group, the number of valence electrons stays the same, but the principal quantum number increases by one. Atomic radius is not easy to define with perfect...

ionic radii

How Ionic Charge Changes Ion Size

Ionic radius describes the size of an ion. It changes when an atom gains or loses electrons. Cations are positive ions with fewer electrons than the parent atom, and they are smaller than the atoms they come from. Aluminum shows this pattern clearly. A neutral aluminum atom has a covalent radius of 118 pm, while Al3+ has an ionic radius of 68 pm. When electrons are removed from the outer valence shell, the remaining core electrons feel a stronger effective nuclear charge, or Zeff. That pull...

electron affinity

Electron Affinity Trends on the Periodic Table

Electron affinity is the energy change that happens when a gaseous atom gains an electron and becomes a negative ion, or anion. For many elements, this process releases energy, so the electron affinity value is negative. For some elements, energy must be added instead, so the value is positive. Electron affinity also applies when more than one electron is added. The second electron affinity is the energy change for adding an electron to an anion to make a 2− ion. Later electron affinities...

alkali metals

Alkali Metals: Reactivity Trends

Alkali metals are Group 1 elements with one valence electron. They are soft, shiny metallic solids that are malleable, ductile, and good conductors of heat and electricity. Their melting points are unusually low for metals and drop as you move down the group. Density generally increases down the group, except for potassium. The trend in atomic size helps explain their behavior. Moving from lithium to cesium, each element has a higher principal quantum number, so the outer electron is farther...

halogens

Halogens are Group 17 nonmetals that show clear trends in structure and reactivity. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid. Astatine is highly unstable and radioactive, so most of its properties are still unknown because it has a very short half-life. Tennessine is a synthetic element that is also predicted to belong to this group. These elements do not usually exist as single atoms. Instead, they form diatomic molecules, which means...

noble gases

Noble Gases: Sources, Uses, and Reactions

Noble gases are the group 18 elements helium, neon, argon, krypton, xenon, and radon. They were called “noble” because they were once thought to be nonreactive. That idea changed in 1962, when Dr. Neil Bartlett at the University of British Columbia showed that this assumption was not fully correct. These gases occur in very small amounts in the atmosphere. Some natural gas contains 1–2% helium by mass. Helium is separated from natural gas by removing the condensable components, which leaves...

key terms and concepts

Explore halogen trends, from physical states and electron configuration to oxidizing strength, metal halides, hydrohalic acids, and interhalogen compounds.

Halogens: Trends and Reactions | JoVE K12

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Electron Configuration and Chemical Properties

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 ...

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Colloids

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Construct an explanation to classify matter as a pure substance or mixture; homogeneous or heterogeneous; element or compound; solution, colloid or suspension.

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Phase Transitions

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Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize ...

Vapor Pressure

When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally ...

Clausius-Clapeyron Equation

The equilibrium between a liquid and its vapor depends on the temperature of the system; a rise in temperature causes a corresponding rise in the vapor ...

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy ...

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Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and ...

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. ...

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Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

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Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Carry out investigations to compare physical and chemical properties of matter.

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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 ...

The Bohr Model

Following the work of Ernest Rutherford and his colleagues in the early twentieth century, the picture of atoms consisting of tiny dense nuclei surrounded ...

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a ...

The de Broglie Wavelength

In the macroscopic world, objects that are large enough to be seen by the naked eye follow the rules of classical physics. A billiard ball moving on a ...

The Uncertainty Principle

Werner Heisenberg considered the limits of how accurately one can measure properties of an electron or other microscopic particles. He determined that ...

Use models to interpret the data presented in Bohr diagrams and electron dot diagrams for neutral atoms of elements 1 through 18.

PS.PSc.1.4

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use models to compare representations of atoms, ions, and isotopes.

PS.PSc.1.5

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 ...

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 ...

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 ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name &ldquo;noble&rdquo; because they were ...

Use the Periodic Table as a model to predict the relative properties (metallic/nonmetallic character, ionic charge, and reactivity) and arrangement of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

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 ...

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 ...

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 ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Construct an explanation to classify the type of chemical bond that occurs (covalent, ionic, or metallic) in a given substance.

PS.PSc.2.1

Nomenclature of Alkanes

In the late 19th-century, the number of new chemical compounds discovered increased tremendously. Hence, the necessity arose to develop a naming system ...

Use models to apply International Union of Pure and Applied Chemistry (IUPAC) conventions to name and write formulas for simple compounds.

PS.PSc.2.2

Understand types, properties, and structure of matter.

Halogens: Trends and Reactions

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