Inorganic Chemistry (F-block elements) PDF

# Inorganic Chemistry ## P-block elements - The elements whose last electrons are in the P-subshell are known as P-block elements. - Elements of group 13 to group 18 are known as P-block elements. - The general electronic configuration of P-block elements is: $n^2n^1-6$. ## Group 15 - Elements o...

# Inorganic Chemistry ## P-block elements - The elements whose last electrons are in the P-subshell are known as P-block elements. - Elements of group 13 to group 18 are known as P-block elements. - The general electronic configuration of P-block elements is: $n^2n^1-6$. ## Group 15 - Elements of group 15 are known as the nitrogen family. - The general electronic configuration of group 15 is: $ns^2np^3$. - The common oxidation states of elements of groups 15 are +5, -3. ### Density - Since we know that density depends upon *atomic mass*, as we move down the group, atomic mass increases due to which density will also increase. | Group 15 | Density | | ----------- | ----------- | | N | increases (less) | | P | $d = \frac{mass}{volume}$ | | As | | | Sb | | | Bi | | ## Atomic size and atomic radius - As we move down the group atomic no. as well as no. of electrons increases due to which no. of shell also increases. So, on moving down the group, atomic size increases. Since, we know that radius depends upon size as we move down the group. | Group 15 | At Size | ATradius | | ----------- | ----------- | ----------- | | Al | ↑ incre | | | P | Z=15 | | | As | | | | Sb | | | | Bi | | | ## Ionization Energy - The amount of energy required to remove an electron from any gaseuous atom is known as Ionisation Energy. - Ionisation energy is inversely proportional to the atomic size. I.E increases due to Ionisation energy will decreases. | Group 15 | I.E | At size | | ----------- | ----------- | ----------- | | Al | | ↑ | | P | | | | As | | | | Sb | | | | Bi | Decreases | | ## Metallic property - Metallic property is inversely proportional to the ionization energy and on moving down the group, ionization energy decreases. Due to which metallic property will increase. | Group 15 | Metallic property | I.E | | ----------- | ----------- | ----------- | | Al | ↓ | ↑ | | P | ↓ | | | As | ↑ | | | Sb | Increases | | | Bi | | | ## Electronegativity - On moving down the group, electronegativity increases. | Group 15 | electronegativy | | ----------- | ----------- | | Al | ↓ | | P | 2.1ev | | As | 3.6ev | | Sb | 3.1ev | | Bi | | ## Melting and Boiling point - On moving down the group melting & boiling point increases. | Group 15 | B.P & M.P | | ----------- | ----------- | | N | Increases | | P | | | As | | | Sb | | | Bi | | ## Anomalous behavior of nitrogen - Nitrogen is different from all other elements in its group due to following reasons: - It is found in gaseous state. - It's density is least. - It's atomic size & atomic radius is small. - It's Ionisation energy & electronegativity is maximum - It's metallic property, b.p & M.P is minimum. ## Chemical properties of Group 15 - When elements of group 15 reacts with hydrogen, then hydride of type $EH_3$ is formed. | Element | Reaction with hydrogen | | -------- | ------------------------- | | N | $N_2 + 3H_2 → 2NH_3$ (Ammonia) | | P | $P_4 + 6H_2 → 4PH_3$ (Phosphine) | | As | $2As + 3H_2 → 2AsH_3$ (Arsenic hydride) | | Sb | $2Sb + 3H_2 → 2SbH_3$ (Antimony hydride) | | Bi | $2Bi + 3H_2 → 2BiH_3$ (Bismuth hydride) | - Why $NH_3$ forms hydrogen bond whereas $PH_3$ not? - In $NH_3$, higher, electronegative element *nitrogen* is present whereas in $PH_3$, no any higher electronegative element is present due to which $NH_3$ forms hydrogen bond whereas $PH_3$ not. - Why boiling point of $NH_3$ is greater than $PH_3$? - In $NH_3$ hydrogen bond is present due to which it's boiling point is greater that $PH_3$. ## Reaction with oxygen - When element of group 15 reacts with oxygen then trioxide ($E_2O_3$) and penta oxide ($E_2O_5$) is formed. | Element | Reaction with oxygen | | -------- | ------------------------- | | N | $4N + 3O_2 → 2N_2O_3$ (Trioxide) | | | $2N + 5O_2 → 2N_2O_5$ (Pentaoxide) | | P | $2P + 3O_2 → 2P_2O_3$ | | | $2P + 5O_2 → 2P_2O_5$ | | As | $2As + 3O_2 → 2As_2O_3$ | | | $2As + 5O_2 → 2As_2O_5$ | | Sb | $2Sb + 3O_2 → 2Sb_2O_3$ | | | $2Sb + 5O_2 → 2Sb_2O_5$ | | Bi | $4Bi + 3O_2 → 2Bi_2O_3$ | | | $4Bi + 5O_2 → 2Bi_2O_5$ | - When elements of group 15 reacts with halogen then trihalide and penta halide ($EX_F$) is formed. | Element | Reaction with halogen | | -------- | ------------------------- | | N | $2N+ 3X_2 → 2EX_3$ (Trihalide) | | | $2N + 5X_2 → 2EX_5$ (Pentahalide) | | P | $P_4 + 6Cl_2 → 4PCl_3$ (Phosphorous trichloride) | | | $P_4 + 10Cl_2 → 4PCl_5$ (Phosphorous pentachloride) | | As | $2As + 3Br_2 → 2AsBr_3$ (Arsenic tribromide) | | | $2As + 2Br_2 → 2AsBr_5$ (Arsenic pentabromide) | | Sb | $2Sb + 3I_2 → 2SbI_3$ (Antimony triiodide) | | | $2Sb + 5I_2 → 2SbI_5$ (Antimony pentaiodide) | | Bi | $2Bi + 3Cl_2 → 2BiCl_3$ (Bismuth trichloride) | | | $2Bi + 5Cl_2 → 2BiCl_5$ (Bismuth pentachloride) | ## Reaction with Metal - When elements of group 15 reacts with metal then a binary compound is formed in which the oxidation no. of elements of group 15 is -3. | Element | Reaction with Metal | | -------- | ------------------------- | | N | $3Ca + N_2 → Ca_3N_2$ | | | $3Mg + N_2 → Mg_3N_2$ | | | $2Al + N_2 → 2AlN$ | | P | $3Ca + 2P → Ca_3P_2$ | | | $3Mg + 2As → Mg_3As_2$ | ## Nitrogen or Dinitrogen ### Preparation - **Ammonium chloride:** when ammonium chloride reacts with sodium nitrate then nitrogen is formed. $HCl + NaNO_3 → N_2 + 2H_2O + NaCl$ - **Ammonium dichromate:** when ammonium dichromate is heated then nitrogen is formed. $(NH_4)_2Cr_2O_7 → N_2 + 4H_2O + Cr_2O_3$ - **Heating sodium or barium oxide:** when sodium or barium oxide is heated then Nitrogen is formed. $2Na + N_2 → 2Na_3N$ $3Ba + N_2 → Ba_3N_2$ ### Properties of $N_2$ - It is a colorless, odorless, and tasteless gas. - It is non-toxic. - Its melting and boiling point is low. - It is less soluble in water. ### Reaction with hydrogen - When nitrogen reacts with hydrogen then ammonia is formed. $N_2 + 3H_2 → 2NH_3$ ### Reaction with oxygen - When nitrogen reacts with oxygen then nitrogen monoxide is formed. $N_2 + O_2 → 2NO$ ### Reaction with Metal - When metal reacts with nitrogen then metal nitride is formed $6Li + N_2 → 2Li_3N$ $6Na + N_2 → 2Na_3N$ $6K + N_2 → 2K_3N$ $3Mg + N_2 → Mg_3N_2$ $3Ca + N_2 → Ca_3N_2$ $3Fe + N_2 → Fe_3N_2$ $3Zn + N_2 → Zn_3N_2$ $2Al + N_2 → 2AlN$ ## Ammonia ($NH_3$) ### Preparation - **Urea:** When urea reacts with water then ammonia is formed. $NH_2CONH_2 + 2H_2O → 2NH_3 + H_2O+ CO_2$ - **Ammonium chloride:** When ammonium chloride reacts with calcium hydroxide then ammonia is formed. $2NH_4Cl + Ca(OH)_2 → 2NH_3 + 2H_2O + CaCl_2$ - **Ammonium Sulphate:** When ammonium sulphate reacts with sodium hydroxide then ammonia is formed. $(NH_4)_2SO_4 + 2NaOH → 2NH_3 + 2H_2O + Na_2SO_4$ ### Haber's process - On a large scale, ammonia is prepared by Haber's process. - In this process, nitrogen reacts with hydrogen in the presence of iron catalyst at 700K and 200 atm pressure then ammonia is formed. $N_2 + 3H_2 \rightleftharpoons 2NH_3$ - This is a reversible process, so to obtain more amount of ammonia, high temperature is suitable. ### Properties of $NH_3$ - It is a colorless gas with pungent smell. - Its boiling point is 198.4K. - It is soluble in water. - It is lighter than air. ### Reaction with acid - $NH_3$ is basic in nature, so, it reacts with acid to form salt. $NH_3 + HCl → NH_4Cl$ ### Reaction with water - When $NH_3$ reacts with water to form hydroxide. $NH_3 + H_2O → NH_4OH$ ### Reaction with Metal - $NH_3$ reacts with metal to form nitride $6Li + N_2 → 2Li_3N$ $3Mg + 2N → Mg_3N_2$ $2Al + 2N → 2AlN$ ### Reaction with air - $NH_3$ reacts with air then *NO* is formed. $4NH_3 + 5O_2 → 4NO + 6H_2O$ ## Nitric Acid ($HNO_3$) ### Preparation - $NH_3$ reacts with oxygen in the presence of Pt catalyst at 500K temp & 9 bar pressure and this process is known as Ostwald process. $4NH_3 + 5O_2 \rightleftharpoons 4NO + 6H_2O$ - Nitric oxide combines with oxygen then $NO_2$ is formed. $2NO + O_2 → 2NO_2$ - Nitrogen dioxide reacts with water to form nitric acid $3NO_2 + H_2O → 2HNO_3 + NO$ ### Properties of $HNO_3$ - It is colorless liquid. - Its freezing point is 231.4K and b.p is 355.6K. - Its specific gravity is 1.5. ### Reaction with Base - Nitric acid reacts with base to form salt. $HNO_3 + NaOH → NaNO_3 + H_2O$ ### Reaction with Carbon - $HNO_3$ reacts with carbon to form *carbon dioxide*. $C + 4HNO_3 → CO_2 + 2H_2O + 4NO_2$ ### Reaction with Sulphur - $HNO_3$ react with sulphur to form *sulphuric acid*. $S_8 + 48HNO_3 → 8H_2SO_4 + 48NO_2 + 16H_2O$ ### Reaction with Phosphorous - $HNO_3$ reacts with phosphorous to form *phosphoric acid*. $P_4 + 20HNO_3 → 4H_3PO_4 + 20NO_2 + 4H_2O$ ### Reaction with Iodine - Nitric acid reacts with iodine to form *iodic acid*. $I_2 + 10HNO_3 → 2HIO_3 + 10NO_2 + H_2O$ ### Reaction with Zinc - Zinc reacts with dilute nitric acid to form their nitrate and water. $4Zn + 10HNO_3 (dilute) → 4Zn(NO_3)_2 + 5H_2O + N_2O$ ### Reaction with Copper - Copper reacts with dilute nitric acid to form their nitrate and water. $3Cu + 8HNO_3 (dil) → 3Cu(NO_3)_2 + 4H_2O + 2NO$ - Copper & Zinc react with coned nitric acid to form their nitrate, $NO_2$ and water $Cu + 4HNO_3(Conc) → Cu(NO_3)_2 + 2NO_2 + 2H_2O$ $Zn + 4HNO_3(Conc) → Zn(NO_3)_2 + 2NO_2 + 2H_2O$ ## Allotropes of Phosphorous - **White phosphorous:** - It is waxy solid. - It is poisonous. - It is insoluble in water but soluble in carbon disulphide ($CS_2$). - It is found in the form of $P_4$. - It is more reactive than red phosphorous - It is more stable. - **Red phosphorous:** - It is obtained by heating of *white phosphorous* at 573K. - It is odorless. - It is non-poisonous. - It is insoluble in water as well as carbon disulphide. - It is less reactive than *white phosphorous*. - **Black Phosphorous:** - When red phospherous is heated under with high pressure then *black phosphorous* is formed. Black phosphorous / \ Red phosp. B- Black phosphorous | White phos. B- Black phos. ## Oxoacid of Phosphorous - $H_3PO_2$ (Hypophosphorous acid) H | H-P-H | OH - $H_3PO_3$ (Phosphorous acid) OH | H-P-OH | OH - $H_3PO_4$ (Phosphoric acid) OH | OH-P-OH | OH - $(HPO_3)_3$ (Cyclometa phosphoric acid) O || OH -P / \ P-OH / \ O P - OH || O ## Phosphine ($PH_3$) ### Preparation - Phosphorous reacts with $NaOH$ and $H_2O$ then $PH_3$ is formed. $P_4 + 3NaOH + H_2O → PH_3 + 3NaH_2PO_2$ ### Properties - It is a colorless gas. - It is highly poisonous. - It is soluble in water. - Its Smell is like rotten fish. ### Reaction with HCl - $PH_3$ reacts with HCl then phosphonium chloride is formed. $PH_3 + HCl → PH_4Cl$ ### Reaction with $H_2O$ - $PH_3$ reacts with $H_2O$ to formed phosphonium hydroxide $PH_3 + H_2O → PH_4OH$ ### Reaction with $HNO_3$ - $PH_3$ reacts with $HNO_3$ then phosphonium nitrate is formed. $PH_3 + HNO_3 → PH_4 NO_3$ ## Phosphorous trichloride ($PCl_3$) ### Preparation - Phosphorous reacts with chlorine then phosphorous trichloride is formed. $P_4 + 6Cl_2 → 4PCl_3$ ### Phosphorous trichloride is formed by this reaction: $P_4 + 8SOCl_2 → 4PCl_3 + 4SO_2 + 2S_2Cl_2$ ### Properties - It is colorless oily liquid. - Its boiling point is 347K. - Its melting point is 161K. - Its density is 1.5 $g/cm^3$. ### Reaction with water - PCl3 reacts with water to form phosphorous acid $PCl_3 + 3H_2O → H_3PO_3 + 3HCl$ ### Reaction with oxygen - PCl3 reacts with oxygen to form POCl3. $2PCl_3 + O_2 → 2POCl_3$ ## Phosphorous Pentachloride ($PCl_5$) - Phosphorous reacts with excess of chlorine then $PCl_5$ is formed. $P_4 + 10Cl_2 → 4PCl_5$ ### Properties - It is yellowish white powder. - It is color less. - It is poisonous. - Its b.p is 166°C. - Its melting point is 160.5°C. ### Reaction with water - $PCl_5$ reacts with $H_2O$ then $H_3PO_4$ is formed. $PCl_5 + 4H_2O → H_3PO_4 + 5HCl$ ### Reaction with $SO_2$ - $PCl_5$ react with SO2 to form thionyl chloride. $PCl_5 + SO_2 → SOCl_2 + POCl_3$ ### Action of heat - When $PCl_5$ is heated, then *PCl3 is formed*. $PCl_5 → PCl_3 + Cl_2$ ## Group 16 - Elements of group 16 are known as oxygen family. - The general electronic configuration of group 16 is $ns^2np^4$ - The common oxidation state of elements of group 16 is +6, -2 | Group 16 | Elements | | ----------- | ----------- | | O | Oxygen | | S | Sulphur | | Se | Selenium | | Te | Tellurium | | Po | Polonium | ## Physical properties of Group 16 ### Physical state | Group 16 | Physical state | | ----------- | ----------- | | O | Gas | | S | Solid | | Se | Solid | | Te | Solid | | Po | Solid | ### Density | Group 16 | Density | | ----------- | ----------- | | O | ↑ | | S | | | Se | | | Te | | | Po | | ### Atomic size & Atomic radius | Group 16 | At Size & Radius | | ----------- | ----------- | | O | ↑ | | S | | | Se | | | Te | | | Po | | ### Ionization energy | Group 16 | I.E | At Size | | ----------- | ----------- | ----------- | | O | ↑ | ↓ | | S | | | | Se | | | | Te | | | | Po | | | ### Metallic character | Group 16 | Metallic character | I.E | | ----------- | ----------- | ----------- | | O | ↓ | ↑ | | S | | | | Se | | | | Te | | | | Po | | | ### Electronegativity | Group 16 | Electronegativy | | ----------- | ----------- | | O | ↓ | | S | 2.5ev | | Se | 2.4ev | | Te | 2.1ev | | Po | | ### Melting Point and Boiling Point | Group 16 | Melting point | Boiling point | | ----------- | ----------- | ----------- | | O | 55K | ↑ | | S | 393K | | | Se | 490K | | | Te | 725K | ↓ | | Po | 520K | | ## Chemical properties of Group 16 ### Reaction with hydrogen - Hydrogen reacts with elements of group 16 then hydride of type H2E is formed. - $H_2 + O_2 → 2H_2O$ (Water) - $8H_2 + S_8 → 8H_2S$ (Hydrogen Sulphide) - $H_2 + Se → H_2Se$ (Selenium hydride) - $H_2 + Te → H_2Te$ (Tellurium hydride) - $H_2 + Po → H_2Po$ (Polonium hydride) ### Reaction with oxygen - Element of group 16 reacts with oxygen to form oxide of type $EO_2$ and $EO_3$. - $SO_2, SO_3$ - $SeO_2, SeO_3$ - $TeO_2, TeO_3$ ### Why $H_2S$ is less acidic than $H_2Te$? - On moving down the group acidic character increases due to which $H_2S$ is less acidic than $H_2Te$. ### Why $H_2O$ is liquid whereas $H_2S$ is gas? - In $H_2O$ hydrogen bond is present due to which it is liquid whereas in $H_2S$ hydrogen bond is not present due to which it is gas. ### Reaction with halogen - When elements of group 16 reacts with halogen then halides of type. $EX_2$, $EX_4$, $EX_6$, etc. are formed. ## Oxygen or dioxygen ($O_2$) ### Preparation - **Potassium chlorate:** When potassium chlorate is heated then dioxygen is formed. $2KClO_3 → 2KCl + 3O_2$ - **Potassium nitrate:** When potassium nitrate is heated then oxygen is formed. $2KNO_3 → 2KNO_2 + O_2$ ### Properties of dioxygen - It is a colorless, odorless and tasteless gas. - Its melting point is 54.5K and b.p is 90.5K. - It is soluble in water. - It is paramagnetic in nature. ### Reactivity - Dioxygen is a reactive element, so it reacts with all element except inert gas and forms compound. - *Inert gases:* He, Ne, Ar, Kr, Xe & Rn ### Action on litmus paper - Dioxygen is neutral in nature, so there is no effect on litmus. ## Ozone ($O_3$) ### Preparation - When a slow & dry stream of oxygen is passed through silent electric current then *ozone* is formed. $3O_2 → 2O_3$ ### Properties - Solid - Violet - Liquid - Deep blue - Gas - Light blue - It is heavier than air. - It is odorless. ### Ozone acts as oxidizing agent - Because it produces nascent oxygen. $O_3 → O_2 + O$ ### Reaction with NO - NO reacts with ozone then NO2 is formed. $2NO + O_2 → 2NO_2$ ### Reaction with Zns - Zns reacts with ozone then Znso4 is formed $Zns + 2O_3 → ZnSO_4 + O_2$ ## Rhombic Sulphur or α-Sulphur - It is yellow in color. - Its m.p is 385.8K. - Its specific gravity is 2.06. - It is insoluble in water & soluble in CS2. - It is colorless ## Monoclinic Sulphur (β-Sulphur) - It is colorless. - Its m.p is 393K. - Its specific gravity is 1.98. - It is soluble in CS2. - Both α and β sulphur have S8 molecules. - Sulphur is paramagnetic in nature. ## Sulphur Dioxide ($SO_2$) - When sulphur is burnt in air then sulphur dioxide is formed. $S + O_2 → SO_2$ - FeS2 reacts with oxygen then SO2 is formed $4FeS_2 + 11O_2 → 2Fe_2O_3 + 8SO_2$ ### Properties - It is a colorless gas with pungent smell. - It is soluble in water. - Its boiling point is 263K. ### Reaction with water - SO2 reacts with water then H2SO3 is formed $SO_2 + H_2O → H_2SO_3$ (Sulphurous acid) ### Reaction with oxygen - SO2 reacts with water then H2SO4 is formed. $2SO_2 + O_2 → 2SO_3$ (Sulphur trioxide) ### Reaction with chlorine - SO2 reacts with chlorine then SO2Cl2 is formed $SO_2 + Cl_2 → SO_2Cl_2$ (Sulphoryl Chloride) ### SO3 acts as reducing agent ### Sulphuric Acid ($H_2SO_4$) - Sulphuric acid is prepared by *contact process*. - In this process, first of all sulfur reacts with oxygen then sulfur dioxide is formed. $S + O_2 → SO_2$ - Then after sulfur dioxide reacts with oxygen in the presence of *V2O5* (Vanadium pentaoxide) then sulfur trioxide is formed. $2SO_2 + O_2 \rightleftharpoons 2SO_3$ - Then after, sulfur trioxide reacts with sulphuric acid then oleum is formed. $SO_3 + H_2SO_4 → H_2S_2O_7$ ### Properties of $H_2SO_4$ - It is colorless oily liquid. - Its freezing point is 283K. - Its boiling point is 611K. - Its specific gravity is 1.83. ### Reaction with Copper - Copper reacts with $H_2SO_4$ to form copper sulphate. $Cu + H_2SO_4 → CuSO_4 + H_2$ ### Reaction with Zinc - When zinc reacts with $H_2SO_4$, then zinc sulphate is formed. $Zn + H_2SO_4 → ZnSO_4 + H_2$ ## Group 17 - Elements of group 17 are known as halogens. - The common oxidation state of elements of group 17 is +7, -1 - The general electronic configuration of group 17 is $ns^2np^5$ | Group 17 | Elements | | ----------- | ----------- | | F | Fluorine | | Cl | Chlorine | | Br | Bromine | | I | Iodine | | At | Astatine | ### Physical state | Group 17 | Physical state | | ----------- | ----------- | | F | Gas | | Cl | Liquid | | Br | Liquid | | I | Solid | | At | Solid | ### Density | Group 17 | Density | | ----------- | ----------- | | F | ↑ | | Cl | | | Br | | | I | | ### Atomic size & atomic radius | Group 17 | Atomic size | atomic radius | | ----------- | ----------- | ----------- | | F | ↑ | ↑ | | Cl | | | | Br | | | | I | | | ### Ionization energy | Group 17 | I.E | At size | | ----------- | ----------- | ----------- | | F | ↓ | ↑ | | Cl | | | | Br | | | | I | | | ### Metallic character | Group 17 | Metallic character | I.E | | ----------- | ----------- | ----------- | | F | ↓ | ↑ | | Cl | | | | Br | | | | I | | | ### Electronegativity | Group 17 | Electronegativity | | ----------- | ----------- | | F | ↓ | | Cl | 3.0ev | | Br | 2.8ev | | I | 2.5ev | ### Chemical properties - When metal of group 17 reacts with hydrogen then metal halide is formed. $H_2 + X_2 → 2HX$ (Hydrogen halide) $H_2 + F_2 → 2HF$ (Hydrogen Fluoride) $H_2 + Br_2 → 2HBr$ (Hydrogen Bromide) $H_2 + Cl → 2HCl$ (Hydrogen Chloride) $H_2 + I → 2HI$ (Hydrogen Iodide) ### Why HI is stronger acid than HF? - On moving down the group acidic character increases due to which HI is stronger acid than HF. ## Reactioh with phosphorous - Element of group 17 reacts with phosphorous to form tribolide and pentahalide. $P_4 + 6F_2 → 4PF_3$ $P_4 + 10F_2 → 4PF_5$ $P_4 + 6Cl_2 → 4PCl_3$ $P_4 + 10Cl_2 → 4PCl_5$ $P_4 + 6Br_2 → 4PBr_3$ $P_4 + 10Br_2 → 4PBr_5$ $P_4 + 6I_2→ 4PI_3$ $P_4 + 10I_2 → 4PI_5$ ### Reaction with $H_2O$ - Element of group 17 react with water to form hydrogen halide $2H_2O + 2X_2 → 4HX + O_2$ $2H_2O + 2F_2 → 4HF + O_2$ $2H_2O + 2Cl_2 → 4HCl + O_2$ $2H_2O + 2Br_2 → 4HBr + O_2$ $2H_2O + 2I_2 → 4HI + O_2$ ### Reaction with Metal - Element of group 17 reacts with metal to form metal halide. $2Li^+ + 2F^-_2 → 2LiF$ (Lithium fluoride) $2Na^+ + Cl_2 → 2NaCl$ (Sodium Chloride) $Mg^{+2} + Br_2^{-1} → MgBr_2$ (Magnesium Bromide) $2Al^{3+} + 3I_2^{-1} → 2AlI_3$ (Aluminum Iodide) ### Interhalogen compound - When two halogens of different atomic size combines with each other then interhalogen compound is formed. $XY_n$ - **Large:** - $TF_3$, $ICl_3$, $IBr_3$, $BrCl_3$, $BrF_3$, $ClF_3$ - **Small:** - $TF_5$, $ICl_5$, $IBr_5$, $BrCl_5$, $BrF_5$, $ClF_5$ ## Group 18 (Zero group) - Elements of group 18 are known as insert gas or noble gas. - Generally, electronic configuration of elements of group 18 is $ns^2np^6$. - The common oxidation state of group 18 elements is zero. ### Elements of group 18 - Helium, Neon, Argon, Krypton, Xenon, Radon ## Physical properties of group 18 | Group 18 | Physical State | | ----------- | ----------- | | He | Gas | | Ne | Gas | | Ar | Gas | | Kr | Gas | | Xe | Gas | | Rn | Gas | ###