group 17
Bromine belongs to the halogen family and is in group 17 (group VIIA) of the periodic table.
The element in Group 1A with a higher atomic number than chlorine but lower than bromine is iodine.
Bromine is in Group 7: The Halogens, below Fluorine and Chlorine but above Iodine and Astatine.
The element in the group of MgO, Br, LiF, and PbO is Br (Bromine).
Bromine is in the halogen family or group in the periodic table.
Bromine is an element on the periodic table. It has an atomic number of 35. It can be found near the right side of the table. Bromine is located in the Halogens group, which is group 7A or 17, and is also in period 4.
Group 17. Also known as the Halogen Family.
Bromine belongs to the halogen family and is in group 17 (group VIIA) of the periodic table.
Hydrogen is in the group 1.Francium is in the group 1 (alkali metals).Fluorine and bromine are in the group 17 (halogens).
The nearest noble gas to bromine is krypton. Bromine is located in Group 17 of the periodic table, while krypton is in Group 18, making it the closest noble gas in terms of atomic number and position. Krypton has an atomic number of 36, whereas bromine has an atomic number of 35.
The element in Group 1A with a higher atomic number than chlorine but lower than bromine is iodine.
No, Selenium has 6 valence electrons while Bromine has 7. You can determine this because on the periodic table, Selenium is in Group VI while Bromine is in group VII.
Bromine is on the 17th column of the periodic table.It has atomic number of 35.
Bromine is in Group 7: The Halogens, below Fluorine and Chlorine but above Iodine and Astatine.
Halogens F (fluorine), Cl (chlorine), Br (bromine), I (iodine), At (astatine)
The element in group one with a higher atomic number than chlorine but lower atomic number than bromine is iodine. Its atomic number is 53, which is greater than chlorine's atomic number of 17 but less than bromine's atomic number of 35.
Bromine is the member of group 7 that exists as two stable isotopes: bromine-79 and bromine-81. These isotopes have slightly different atomic masses due to variations in the number of neutrons.