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β 11y agoAll halogens have 7 valence electrons. They gain one electron and achieve noble gas electronic configuration
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β 10y agoThe alkaline earth metals.
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β 10y agohalogens
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β 12y agohalogens
The group attains electron configuration of noble gases by gaining one electron is the halogens. They have seven valence electrons and need one more electron to complete their outer shell, resulting in a full valence shell like the noble gases.
Ions derived from representative elements achieve stability by gaining or losing electrons to achieve a full outer electron shell. For example, Group 1 elements tend to form +1 ions by losing one electron to achieve a noble gas configuration, while Group 17 elements tend to form -1 ions by gaining one electron. This process allows the ions to attain a more stable electron configuration similar to that of a noble gas.
This group has the electron configuration of sulfur. The element sulfur has 16 electrons, and its electron configuration is 1s2 2s2 2p6 3s2 3p4.
Bromine (Br) needs to gain one electron to achieve a stable noble gas electron configuration because it is in Group 17 (halogens) and has 7 valence electrons. By gaining one electron, bromine will have a full outer electron shell like a noble gas.
Elements in Group 2 of the periodic table will have an electron configuration that ends in s2. This group includes elements such as beryllium, magnesium, and calcium. They have two electrons in their outermost s sublevel.
The group attains electron configuration of noble gases by gaining one electron is the halogens. They have seven valence electrons and need one more electron to complete their outer shell, resulting in a full valence shell like the noble gases.
The ion formed when potassium achieves noble-gas electron configuration is K+ (potassium ion). This occurs when potassium loses one electron to have a full outer electron shell, similar to the nearest noble gas, argon.
Ions derived from representative elements achieve stability by gaining or losing electrons to achieve a full outer electron shell. For example, Group 1 elements tend to form +1 ions by losing one electron to achieve a noble gas configuration, while Group 17 elements tend to form -1 ions by gaining one electron. This process allows the ions to attain a more stable electron configuration similar to that of a noble gas.
This group has the electron configuration of sulfur. The element sulfur has 16 electrons, and its electron configuration is 1s2 2s2 2p6 3s2 3p4.
Potassium (K) needs to lose one electron to become stable, as it belongs to group 1 in the periodic table and has one electron in its outer shell. By losing this electron, potassium achieves a full outer shell and attains a stable electron configuration.
The halogens, specifically the group 17 elements, have the most negative electron affinities. This is because they have a strong attraction for gaining an electron to achieve a stable electron configuration with a full outer shell. Fluorine has the highest electron affinity among the halogens.
The group of elements that have a stable electron configuration are the noble gases.
Elements from Group 17, also known as the halogens, are most likely to react with potassium to form ionic compounds. This is because halogens have a high affinity for gaining an electron to achieve a stable electron configuration and potassium has a tendency to lose one electron to achieve stability.
Halogens, such as fluorine, chlorine, and iodine, tend to form negative ions with a -1 charge by gaining one electron to achieve a stable electron configuration.
Group 17 and group 16 in general.
The outer electron configuration for all group 1 elements is ns1, where n represents the energy level of the outermost electron. This means that group 1 elements have one electron in their outermost shell.
Group 7A elements, also known as the halogens, need to gain one electron to achieve a stable electron configuration, typically by gaining an electron to achieve a full outer energy level of eight electrons (octet).