17 Cl Chlorine 9 F Fluorine Elements in Periodic Table Group 17: Halogen Prepared by: Nurul Huda Mahfuzah binti Yahya (151331) Aimy Batrisyia binti Zolkefli (153409) -From Group 11
1H3Li 11 Na19K37 Rb55 Cs87 Fr 4 Be12 Mg20 Ca38 Sr56 Ba88 Ra 21 Sc39Y57-71 89-103 22 Ti 40 Zr72 Hf104 Rf 23V41 Nb73 Ta105 Db 24 Cr42 Mo74 W106 Sg 25 Mn43 Tc75 Re107 Bh 26 Fe44 Ru76 Os108 Hs 27 Co45 Rh77 Ir109 Mt 28 Ni 46 Pd78 Pt110 Ds 29 Cu47 Ag79 Au111 Rg 30 Zn48 Cd80 Hg112 Cn 5B13 Al 31 Ga49 In81 Ti 6C14 Si 32 Ge50 Sn82 Pb 7N15P33 As51 Sb83Bi 8O16S34 Se52 Te84 Po 9F17 Cl 35 Br53I85 At 2 He10 Ne18 Ar36 Kr54 Xe86 Rn 57 La 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu 89 Ac 90 Th 91 Pa 92U 93 Np 94 Pu 95 Am 96 Cm 97 Bk 98 Cf 99 Es 100 Fm 101 Md 102 No 103 Lr 113 Nh 114 Fl 115 Mc 116 Lv 117 Ts 118 Og 9F 17 Cl 35 Br 53I 85 At 117 Ts Elements in Group 17 are known as Halogen. Halogen include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At), tennessine (Ts) . Halogen have seven valence electrons and they are highly reactive nonmental since they only one more electron to achieve octet electron. Group 17 in the Periodic Table HALOGEN
F Fluoride Cl Chlorine Br Bromine I Iodine At Astatine Ts Tennessine Atomic number: 17 Physical state: Greenish-yellow gas at room temperature. Odor: Pungent and suffocating. Properties: Strong oxidizing agent. Uses: Essential for water purification (as chlorine gas or in the form of hypochlorites), cleaning products, and production of Polyvinyl Chloride (PVC). Atomic number: 9 Physical state: Pale yellow gas at room temperature. Odor: Distinct odor. Properties: Highly reactive, most electronegative element, known for its incredible ability to react with nearly all elements, including noble gases under certain conditions. Uses: Used in dental care (e.g., fluoride toothpaste), in the production of fluoropolymers (e.g., Teflon), and in refrigerants. Overview of Each Elements of Halogen Atomic number: 53 Physical state: Bluish-black solid at room temperature (sublimes into purple vapors). Odor: Distinctive, pungent odor that is somewhat sweet Properties: Less reactive than bromine. Uses: Used in medicine (e.g., as iodide in thyroid medications), for disinfectant, and dietary supplement. Atomic number: 35 Physical state: Reddish-brown liquid at room temperature (only non-metallic liquid at room temperature). Odor: Pungent and irritating. Properties: Less reactive than chlorine but still a strong oxidizing agent. Uses: Used in flame retardants (e.g., in textiles and electronics), pharmaceuticals (e.g., sedatives), and photography (Silver bromide is used in photographic films) Atomic number: 85 Physical state: Radioactive halogen, extremely rare in nature, primarily synthesized in laboratories. Odor: Extremely rare and radioactive, so its odor is not well-documented. Properties: Highly unstable due to its radioactivity, shares similarities with iodine chemically. Uses: Used in nuclear batteries, and radiation therapy (Astatine-211 use in treating cancer). Atomic number: 117 Physical state: Predicted to be a synthetic element, not naturally occurring, expected to be highly radioactive with a short half-life. Odor: Synthetic and highly radioactive, has not been directly observed or documented. Properties: Theoretical predictions suggest it would behave similarly to other halogens due to its position in Group 17. Uses: Development of new materials and technologies, and nuclear physics research.
Boiling & Melting Points INCREASES down the group due to van der Waals forces Definition: Melting point: temperature at which solid begins to change into a liquid Boiling point: temperature at which liquid begins to convert to gas. When the size of molecules increases down the group, the strength of van der Waals forces also increases. High van der Waals forces requires more energy to break the attraction between molecules DECREASES down the group Definition: measurement of the tendency of an atom to attract a bonding pair of electrons Number of electrons increases down the group. So, electrons become distance (far) from the nucleus which resulted in lesser attraction between them. Electronegativity INCREASES down the group Definition: the total distance from the nucleus of an atom to the outermost orbital of its electron As number of protons increases, the atomic radius of the atom increases. Atomic Radius DECREASES down the group Definition: the amount of energy required to remove an electron from an isolated atom or molecule. more distance between outer valence electron and nucleus, less energy required to remove them. Ionization Energy DECREASES down the group Definition: the potential energy change of the atom when an electron is added to a neutral gaseous atom to form anion. If the electron is far from nucleus, the electron affinity is low. Electron Affinity Reactivity DECREASES down the group Noted that all elements in Group 17 have 7 valence electrons which they only needed one additional electron to achieve octet. Down the group, the atomic radius of element increases relative to the distance between outer shell of electrons and the nucleus. Therefore, attraction between nucleus and outermost shell of electrons is reduce and electron affinity decreases. Periodic Trend
BOILING POINT (Celcius) MELTING POINT (Celcius) ELECTRONE GATIVITY IONIZATION ENERGY (kJ/mol) ELECTRON AFFINITY (kJ/mol) -188 -220 4.0 1681 -328.0 -35 -101 3.0 1251 -349.0 58.8 -7.2 2.8 1140 -324.6 184 114 2.5 1008 -295.2 337 302 2.2 890±40 -270.1 610 350-550 N/A 736.9 165.9 9 F Fluorine 17 Cl Chlorine 35 Br Bromine 53 I Iodine 85 At Astatine 117 Ts Tennassine DOWN THE GROUP BOILING & MELTING POINT ELECTRONEGATIVITY ATOMIC RADIUS IONIZATION ENERGY ELECTRON AFFINITY REACTIVITY INCREASES DECREASES INCREASES DECREASES DECREASES DECREASES Table of Periodic Trend SUMMARY FUN FACT : DID YOU KNOW ? Tennessine (Ts) element is previously known as ununseptium which means “one-one-seven-ium” in Latin. In 2010, element 117 was discovered and the International Union of Pure and Applied Chemistry (IUPAC) approved the name in November 2016. Discoverers at the Joint Institute for Nuclear Research in Dubna, Russia; Oak Ridge National Laboratory in Tennessee; Vanderbilt University in Tennessee; and Lawrence Livermore National Laboratory in California suggested names for elements 115 and 117. The elements—tennessine and moscovium—are named in honor of the places where tests related to their creation were conducted. (The Halogens – Reactions With Halogens, 2024)
Question 1 Why does fluorine always have an oxidation state of -1 in its compounds? Solution: Electronegativity increases across a period, and decreases down a group. Therefore, fluorine has the highest electronegativity out of all of the elements. The oxidation state of fluorine is always -1. This is because fluorine has 7 electrons in its outermost valence shell and requires only one more electron to complete its shell. As a result, it gains one electron and acquires an oxidation state of -1. Question 2 What happens to the melting points and boiling points as you go down group 17? Solution: Atomic Size: The atoms become larger as you descend the group because they gain extra electron shells. This increase in size leads to stronger intermolecular forces between the molecules. Intermolecular Forces: These forces are responsible for holding molecules together in a substance. As the intermolecular forces become stronger, more energy is required to break them during melting or boiling. Consequently, the melting and boiling points rise. Trend: Fluorine (at the top of Group 7) is the most volatile, with the lowest melting and boiling points. In contrast, iodine (at the bottom) has the highest melting and boiling points, making it less volatile. Practice Question
53 I Iodine 9 F Fluorine 35 Br Bromine 17 Cl Chlorine Thankyouand havefuninlearning! References QRcode below containthelist of references: