An electrochemical cell consists of two different metals submerged in an electrolyte such as an acid or salt solution. Electrons flow from the more reactive metal, creating a voltage. For example, in a zinc-copper cell, zinc releases electrons into the electrolyte more readily than copper, becoming the negative electrode. The electrons flow to the copper electrode.
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
An electrochemical cell consists of two different metals submerged in an electrolyte such as an acid or salt solution. Electrons flow from the more reactive metal, creating a voltage. For example, in a zinc-copper cell, zinc releases electrons into the electrolyte more readily than copper, becoming the negative electrode. The electrons flow to the copper electrode.
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
Water is made up of two hydrogen atoms and one oxygen atom, with a molecular weight of 18 units. Water exists in three states: liquid, gas, and solid ice. It freezes at 0°C and boils at 100°C. There are several types of water including hydrogen peroxide, distilled water, and hard water containing dissolved salts. Water can dissolve many substances like hydroxides, some carbohydrates, and some salts.
The document outlines 10 rules for assigning oxidation numbers to elements in chemical compounds:
1) Cations are written first followed by anions with oxidation numbers of +1 for cations and -1 for anions like H in HCl.
2) Free elements have an oxidation number of 0 like He and N2.
3) The oxidation number of a monatomic ion equals its charge like +1 for Na+ and -3 for N3-.
4) Hydrogen's oxidation number is usually +1 except in metal hydrides where it is -1. Oxygen is usually -2 except in compounds like H2O2. Group 1A elements are +1 and Group 2A elements
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, loss and gain of electrons, Balancing redox reactions, Half reaction method, Types of redox reaction- direct and indirect method, Electrochemical cell, Classification of redox reactions.
Chelation therapy involves intravenous injections of chelating agents like EDTA that bind to heavy metals like mercury and minerals in the blood to remove them from the body. It is most often used to treat heavy metal poisoning but some practitioners claim it can treat heart disease and other disorders by reducing calcium plaque buildup or oxidative stress, though these theories lack scientific proof. Potential side effects range from minor reactions at the injection site to life-threatening drops in blood pressure or calcium levels.
This document discusses the properties and reactivity of metals. It begins by describing the physical properties of metals, such as their hardness, malleability and conductivity. It then discusses the chemical properties of metals, including how they form positive ions and react with oxygen, water and acids. The document introduces metal alloys and explains why they are stronger than pure metals. It also defines the reactivity series and uses it to predict and describe the reactions of different metals. The document discusses the reactions of various metal compounds and how the position of metals in the reactivity series affects their reactivity and the stability of their compounds.
Covalent bonding forms between non-metals through the sharing of electron pairs, which can be represented as single, double, or triple bonds between the atoms. Water (H2O) is an example of a covalent molecule where oxygen shares electron pairs with two hydrogen atoms in a bent geometry.
The document discusses various properties of water including its composition, structure, and ability to dissolve many substances. It explains that water is a compound made of hydrogen and oxygen atoms, and it can act as both an acid and a base by producing H+ and OH- ions. Water has a high capacity for dissolving substances due to its polar nature. The document also covers topics like solvents, solutions, factors affecting solubility, and hardness of water. It provides examples and videos for additional explanation.
Water is made up of two hydrogen atoms and one oxygen atom, with a molecular weight of 18 units. Water exists in three states: liquid, gas, and solid ice. It freezes at 0°C and boils at 100°C. There are several types of water including hydrogen peroxide, distilled water, and hard water containing dissolved salts. Water can dissolve many substances like hydroxides, some carbohydrates, and some salts.
The document outlines 10 rules for assigning oxidation numbers to elements in chemical compounds:
1) Cations are written first followed by anions with oxidation numbers of +1 for cations and -1 for anions like H in HCl.
2) Free elements have an oxidation number of 0 like He and N2.
3) The oxidation number of a monatomic ion equals its charge like +1 for Na+ and -3 for N3-.
4) Hydrogen's oxidation number is usually +1 except in metal hydrides where it is -1. Oxygen is usually -2 except in compounds like H2O2. Group 1A elements are +1 and Group 2A elements
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, loss and gain of electrons, Balancing redox reactions, Half reaction method, Types of redox reaction- direct and indirect method, Electrochemical cell, Classification of redox reactions.
Chelation therapy involves intravenous injections of chelating agents like EDTA that bind to heavy metals like mercury and minerals in the blood to remove them from the body. It is most often used to treat heavy metal poisoning but some practitioners claim it can treat heart disease and other disorders by reducing calcium plaque buildup or oxidative stress, though these theories lack scientific proof. Potential side effects range from minor reactions at the injection site to life-threatening drops in blood pressure or calcium levels.
This document discusses the properties and reactivity of metals. It begins by describing the physical properties of metals, such as their hardness, malleability and conductivity. It then discusses the chemical properties of metals, including how they form positive ions and react with oxygen, water and acids. The document introduces metal alloys and explains why they are stronger than pure metals. It also defines the reactivity series and uses it to predict and describe the reactions of different metals. The document discusses the reactions of various metal compounds and how the position of metals in the reactivity series affects their reactivity and the stability of their compounds.
Covalent bonding forms between non-metals through the sharing of electron pairs, which can be represented as single, double, or triple bonds between the atoms. Water (H2O) is an example of a covalent molecule where oxygen shares electron pairs with two hydrogen atoms in a bent geometry.
The document discusses various properties of water including its composition, structure, and ability to dissolve many substances. It explains that water is a compound made of hydrogen and oxygen atoms, and it can act as both an acid and a base by producing H+ and OH- ions. Water has a high capacity for dissolving substances due to its polar nature. The document also covers topics like solvents, solutions, factors affecting solubility, and hardness of water. It provides examples and videos for additional explanation.
3. Elektrotik Dissosiasiya nədir?
Bildiyimiz kimi bəzi maddələr müsbət və mənfi ionlardan ibarət möhkəm
əlaqəli sistemdir.Belə sistemi ionlar arsındakı güclü cazibə
xarakterli elektrik qüvvələri yaradır.Buna məsəl xörək duzunu
yəni NaCl-ni gətirmək olar.Bu molekul müsbət natrium ionu (Na+) və
mənfi xlor ionundan (Cl-1) ibarət güclü əlaqəli sistemdir.
Ona görə də bu maddələr xarici elektrik sahəsinə gətirildikdə tərkibində sərbəst
yükdaşıyıcılar olmadığı üçün elektrik keçirmir , yəni dielektrikdirlər.
4. Elektrotik Dissosiasiya nədir?
Amma biz belə maddələri suda həll etsək necə olar?
Bu maddələri biz suda həll etdiyimiz zaman , ionlar
arasındakı cazibə qüvvəsi xeyli zəifləyir.
Bu zaman maddənin molekulları müsbət və
mənfi ionlara ayrılır.Bu ionlarda məhluldakı
sərbəst yükdaşıyıcılara çevrilir və məhlul ,keçiriciyə çevrilir.
5. Cavablar:
• Sual : Elektrolit nədir?
• Cavab : Məhlulları (və ya ərintiləri) elektrik cərəyanını
keçirən maddələr elektrolitlər adlanır.
• Sual : Elektrolitik dissosiasiya nədir?
• Cavab : Suda neytral molekulların parçalanması zamanı
müsbət və mənfi ionların yaranma prosesi elektrolitik
dissosiasiya adlanır.
6. İon keçiriciliyi haqqında:
Elektrolitdə elektrik cərəyanı müsbət və mənfi ionların nizamlı hərəkətidir.
Gəlin bunu təcrübi olaraq sübut edək.
2 kömür elektrod cərəyan mənbəyinin qütblərinə birləşdirilir.
Qeyd: Cərəyan mənbəyinin müsbət qütbünə birləşdirilən elektrod anod, mənfi qütbünə
birləşdirilən elektrod isə katod adlanır.
Elektrodlar elektrolitik vannaya, məsələn, xörək duzunun (NaCl) suda məhluluna daxil edilir və
dövrə qapanır. Yaranan elektrik sahəsi vasitəsi ilə müsbət natrium ionları katoda doğru, mənfi
xlor ionları isə anoda doğru istiqamətlənmiş hərəkət edir.
7.
8. Elektroliz haqqında
Katoda çatan müsbət yüklü ionlar neytral atoma çevrilir və katod üzərində
natrium (Na) təbəqəsi əmələ gəlir : Na+ + e-1 Na0
Mənfi yüklü ionlar isə artıq elektronlarını verməklə neytrallaşır, onun səthində
qaz qabarcıqları şəkində xlor (Cl) ayrılır : Cl-1 – e-1Cl2
Deməli ,ion keçiriciliyində maddə daşınması baş verir.
Elektrolitdən cərəyan keçərkən elektrodlar üzərində maddə ayrılması
prosesi elektroliz adlanır.
9.
10. Elektroliz qanunu haqqında
İngilis alim Maykl Faradey elektroliz zamanı elektrodlar üzərində ayrılan maddənin kütləsinin
hansı fiziki kəmiyyətlərdən asılı olduğunu müəyyənləşdirmişdir.
Elektroliz zamanı elektrodlar üzərində ayrılan maddənin kütləsi elektrolitdən keçən elektrik
yükünün miqdarı ilə düz mütənasibdir.
m = k * q və yaxud m = k * I * t
(m – elektrod üzərində ayrılan maddənin kütləsi, q – elektrolitdən keçən elektrik yükünün
miqdarı, k – mütənasiblik əmsalı olub maddənin elektrokimyəvi ekvivalentidir.)
11. Elektrokimyəvi ekvivalent haqqında
Maddənin elektrokimyəvi ekvivalenti ədədi qiymətcə elektrolitdən 1Kl yük
keçərkən elektrod üzərində ayrılan maddənin kütləsinə bərabərdir.
Elektrokimyəvi ekvivalenti müxtəlif maddələr üçün müxtəlif qiymətə malikdir
Elektrokimyəvi ekvivalentin BS-də vahidi:
[k] = [m] /[q] = 1 kq /Kl
