Chemistry, asked by nemichandverma317, 6 months ago

How to denote 5 chlorine atoms

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Answered by mohammadgull137
0

Answer:

Chlorine is a chemical element with the symbol Cl and atomic number 17. The second-lightest of the halogens, it appears between fluorine and bromine in the periodic table and its properties are mostly intermediate between them. Chlorine is a yellow-green gas at room temperature. It is an extremely reactive element and a strong oxidising agent: among the elements, it has the highest electron affinity and the third-highest electronegativity on the Pauling scale, behind only oxygen and fluorine.

Chlorine, 17Cl

A glass container filled with chlorine gas

Chlorine

Pronunciation

/ˈklɔːriːn, -aɪn/ (KLOH-reen, -⁠ryn)

Appearance

pale yellow-green gas

Standard atomic weight Ar, std(Cl)

[35.446, 35.457] conventional: 35.45

Chlorine in the periodic table

Hydrogen

Helium

Lithium

Beryllium

Boron

Carbon

Nitrogen

Oxygen

Fluorine

Neon

Sodium

Magnesium

Aluminium

Silicon

Phosphorus

Sulfur

Chlorine

Argon

Potassium

Calcium

Scandium

Titanium

Vanadium

Chromium

Manganese

Iron

Cobalt

Nickel

Copper

Zinc

Gallium

Germanium

Arsenic

Selenium

Bromine

Krypton

Rubidium

Strontium

Yttrium

Zirconium

Niobium

Molybdenum

Technetium

Ruthenium

Rhodium

Palladium

Silver

Cadmium

Indium

Tin

Antimony

Tellurium

Iodine

Xenon

Caesium

Barium

Lanthanum

Cerium

Praseodymium

Neodymium

Promethium

Samarium

Europium

Gadolinium

Terbium

Dysprosium

Holmium

Erbium

Thulium

Ytterbium

Lutetium

Hafnium

Tantalum

Tungsten

Rhenium

Osmium

Iridium

Platinum

Gold

Mercury (element)

Thallium

Lead

Bismuth

Polonium

Astatine

Radon

Francium

Radium

Actinium

Thorium

Protactinium

Uranium

Neptunium

Plutonium

Americium

Curium

Berkelium

Californium

Einsteinium

Fermium

Mendelevium

Nobelium

Lawrencium

Rutherfordium

Dubnium

Seaborgium

Bohrium

Hassium

Meitnerium

Darmstadtium

Roentgenium

Copernicium

Nihonium

Flerovium

Moscovium

Livermorium

Tennessine

Oganesson

F

Cl

Br

sulfur ← chlorine → argon

Atomic number (Z)

17

Group

group 17 (halogens)

Period

period 3

Block

p-block

Element category

Reactive nonmetal

Electron configuration

[Ne] 3s2 3p5

Electrons per shell

2, 8, 7

Physical properties

Phase at STP

gas

Melting point

(Cl2) 171.6 K (−101.5 °C, −150.7 °F)

Boiling point

(Cl2) 239.11 K (−34.04 °C, −29.27 °F)

Density (at STP)

3.2 g/L

when liquid (at b.p.)

1.5625 g/cm3[1]

Critical point

416.9 K, 7.991 MPa

Heat of fusion

(Cl2) 6.406 kJ/mol

Heat of vaporisation

(Cl2) 20.41 kJ/mol

Molar heat capacity

(Cl2)

33.949 J/(mol·K)

Vapour pressure

P (Pa) 1 10 100 1 k 10 k 100 k

at T (K) 128 139 153 170 197 239

Atomic properties

Oxidation states

−1, +1, +2, +3, +4, +5, +6, +7 (a strongly acidic oxide)

Electronegativity

Pauling scale: 3.16

Ionisation energies

1st: 1251.2 kJ/mol

2nd: 2298 kJ/mol

3rd: 3822 kJ/mol

(more)

Covalent radius

102±4 pm

Van der Waals radius

175 pm

Color lines in a spectral r

The most common compound of chlorine, sodium chloride (common salt), has been known since ancient times. Around 1630, chlorine gas was first synthesised in a chemical reaction, but not recognised as a fundamentally important substance. Carl Wilhelm Scheele wrote a description of chlorine gas in 1774, supposing it to be an oxide of a new element. In 1809, chemists suggested that the gas might be a pure element, and this was confirmed by Sir Humphry Davy in 1810, who named it from Ancient Greek: χλωρός, romanized: khlôros, lit. 'pale green' based on its colour.

Because of its great reactivity, all chlorine in the Earth's crust is in the form of ionic chloride compounds, which includes table salt. It is the second-most abundant halogen (after fluorine) and twenty-first most abundant chemical element in Earth's crust. These crustal deposits are nevertheless dwarfed by the huge reserves of chloride in seawater.

Elemental chlorine is commercially produced from brine by electrolysis, predominantly in the chlor-alkali process. The high oxidising potential of elemental chlorine led to the development of commercial bleaches and disinfectants, and a reagent for many processes in the chemical industry. Chlorine is used in the manufacture of a wide range of consumer products, about two-thirds of them organic chemicals such as polyvinyl chloride (PVC), many intermediates for the production of plastics, and other end products which do not contain the element. As a common disinfectant, elemental chlorine and chlorine-generating compounds are used more directly in swimming pools to keep them sanitary. Elemental chlorine at high concentration is extremely dangerous, and poisonous to most living organisms. As a chemical warfare agent, chlorine was first used in World War I as a poison gas weapon.

In the form of chloride ions, chlorine is necessary to all known species of life. Other types of chlorine compounds are rare in living organisms, and artificially produced chlorinated organics range from inert to toxic. In the upper atmosphere, chlorine-containing organic molecules such as chlorofluorocarbons have been implicated in ozone depletion. Small quantities of elemental chlorine are generated by oxidation of chloride to hypochlorite in neutrophils as part of an immune system response against bacteria.

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