Question

Can radon form an ion?

Answer 1

Radon,  86Rn

General properties

Pronunciation /ˈreɪdɒn/ ​(RAY-don)

Appearance colorless gas

Mass number 222 (most stable isotope)

Radon 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

Xe

↑

Rn

↓

Og

astatine ← radon → francium

Atomic number (Z) 86

Group group 18 (noble gases)

Period period 6

Block p-block

Element category   noble gas

Electron configuration [Xe] 4f14 5d10 6s2 6p6

Electrons per shell

2, 8, 18, 32, 18, 8

Physical properties

Phase at STP gas

Melting point 202 K ​(−71 °C, ​−96 °F)

Boiling point 211.5 K ​(−61.7 °C, ​−79.1 °F)

Density (at STP) 9.73 g/L

when liquid (at b.p.) 4.4 g/cm3

Critical point 377 K, 6.28 MPa[1]

Heat of fusion 3.247 kJ/mol

Heat of vaporization 18.10 kJ/mol

Molar heat capacity 5R/2 = 20.786 J/(mol·K)

Vapor pressure

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

at T (K) 110 121 134 152 176 211

Atomic properties

Oxidation states 6, 2, 0

Electronegativity Pauling scale: 2.2

Ionization energies  

1st: 1037 kJ/mol

Covalent radius 150 pm

Van der Waals radius 220 pm

Color lines in a spectral range

Spectral lines of radon

Other properties

Crystal structure ​face-centered cubic (fcc)Face-centered cubic crystal structure for radon

Thermal conductivity 3.61×10−3  W/(m·K)

Magnetic ordering non-magnetic

CAS Number 10043-92-2

History

Discovery Ernest Rutherford and Robert B. Owens (1899)

First isolation William Ramsay and Robert Whytlaw-Gray (1910)

Main isotopes of radon

Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct

210Rn syn 2.4 h α 206Po

211Rn syn 14.6 h ε 211At

α 207Po

222Rn trace 3.8235 d α 218Po

224Rn syn 1.8 h β− 224Fr

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Radon is a chemical element with symbol Rn and atomic number 86. It is a radioactive, colorless, odorless, tasteless[2] noble gas. It occurs naturally in minute quantities as an intermediate step in the normal radioactive decay chains through which thorium and uranium slowly decay into lead and various other short-lived radioactive elements; radon itself is the immediate decay product of radium. Its most stable isotope, 222Rn, has a half-life of only 3.8 days, making radon one of the rarest elements since it decays away so quickly. However, since thorium and uranium are two of the most common radioactive elements on Earth, and they have three isotopes with very long half-lives, on the order of several billions of years, radon will be present on Earth long into the future in spite of its short half-life as it is continually being generated. The decay of radon produces many other short-lived nuclides known as radon daughters, ending at stable isotopes of lead.[3]

Unlike all the other intermediate elements in the aforementioned decay chains, radon is, under normal conditions, gaseous and easily inhaled. Radon gas is considered a health hazard. It is often the single largest contributor to an individual's background radiation dose, but due to local differences in geology,[4] the level of the radon-gas hazard differs from location to location. Despite its short lifetime, radon gas from natural sources, such as uranium-containing minerals, can accumulate in buildings, especially, due to its high density, in low areas such as basements and crawl spaces. Radon can also occur in ground water – for example, in some spring waters and hot springs.[5]

so no it can not

Answer 2

Yes it will form ion by fluorine.