أكاديميا - كولنز - معاجم الجيب العلمية - الكيمياء - انكليزي - فرنسي - عربي الحرف ٢_ i

Academia - Collins - Pocket Scientific Dictionaries - Chemistry - English - French - Arabic Letter 2_ I

ion
ion m

Stray. Electric type. When an atom gains or loses an electron, it becomes ionized. Stalactites have a positive charge and stalagmites have a negative charge, such as Na+ and O2. Atoms tend to gain or lose electrons to produce an anion in the form of an inert gas.
Groups of atoms (radicals) can also have a charge, such as:
Sulphate -SO4/2
Nitrogen -NO3
Ammonium hydroxide -OH -NH4

These groups are also viewed as strays.


ion - exchange
échange m d'ions

Exchange of electrolytes. Water can be purified by passing it through a tube over a resin called an ion exchange resin. For seawater, hydrogen ions are replaced by sodium ions and hydroxide ions are replaced by chloride ions.
In other words, water is replaced with sodium chloride. The electrolytes bind to the resin (see opposite page), and an exchange occurs. The result is de-ionized water. This method can be used to facilitate the exchange of ions in the resin.

Impure water
Fluid exchange resin
Long glass tube
Pure water

Resin
-OH + CI → resin --- CI- + OH-
Resin
H+ + Na+ → Resin --- Na+ + H+

Water, such as replacing sodium ions with calcium ions.


ionic bonds
liaisons fpl uniques

Stray links. Chemical bonds that form as a result of forces
The electrostatic attraction between negatively and positively charged ions.
Ionic bonds are found in nonmetal compounds of groups I and VII and metallic elements, such as:

Mg2+ Br2
Na+Cl

As well as in compounds containing radicals such as sulfates
And nitrogenes:

K+NO3- and Cu2+SO4/2-

Ionic compounds have giant structures.


ionic equation
Equation fionique

Anionic equation. The reaction between sodium hydroxide and hydrochloric acid can be described by the molecular equation:

NaOH + HCI → NaCl + H2O
(liquid) (aqueous) (aqueous) (aqueous)

This reaction is an anionic reaction and can be represented by the formula:
Stray:

Na+OH- + H+CI- → Na+Cl- + H2O
(liquid) (aqueous) (aqueous) (aqueous)

Because +Na and -CI appear on both sides of the equation, they do not play any role in the reaction and can be omitted. Thus, the anionic equation becomes:

(liquid) H2O → (aqueous) +H + (aqueous) -OH

The other electrolytes are spectator ions.


ionization
ionization f

Homelessness. When an atom loses or gains electrons, it becomes an ion. The loss or gain of electrons is called “displacement.”


iron
fer m

Iron is the most widely used metallic element in the world. It is mainly found in the form of steel alloys, and in this form it is used in columns, beams, machinery bodies (cars, ovens, refrigerators), containers, boxes, barrels, equipment, tools, and many other things used in our daily lives.

Iron is extracted from metals such as hematite (Fe2O3) and magnetite (Fe3O4) by reduction with carbon monoxide. blast furnace In the blast furnace, carbon monoxide, and the fumes produced in this way are fragile and are made into many different types of steel to strengthen them and give them special properties.

One of the main problems with iron is that it rusts, that is, it oxidizes, producing a soft oxide that easily crumbles.

iron
(strong and useful metal)

>>> humid air) >>>

Iron oxide (Fe2O3)
(weak, worthless oxide)

Iron is a transition metal whose valency can be 2 or 3. It reacts with dilute acids to form iron (II) compounds, such as:

Fe + 2HCl → FeCl2 + H2
(gas) (aqueous) (aqueous) (solid)

But it produces iron (III) compounds when reacted with strong oxidizing agents such as chlorine:

2F (solid) + 3Cl2 (gas) → 2FeCl3 (solid)
Iron has a reversible reaction with steam:

3Fe + 4H2O = Fe3O4 + 4H2
(gas) (solid) (gas) (solid)

Iron (III) compounds can be identified by giving them a red color with potassium thiocyanate solution (KCNS). Iron (II) compounds do not do the same thing with a solution of potassium hexacyanoferrate (III) 6(K3F) (CN), but rather give a blue color. Moreover, when iron (II) solutions react with sodium hydroxide solution, they produce a green, clayey precipitate, while The reaction of iron solutions produces a brown-coloured precipitate
Rust .