how many outer shell electrons are there in group 1?
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The atoms of all group 1 elements have similar chemical properties and reactions because they all have one electron in their outer shell.
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The group number is 7 which indicates that halogen atoms contain seven electrons in the outer shell (energy level). In order to achieve stability and have the same structure as the nearest noble gas, these atoms gain a single electron (rather than losing seven electrons which would take much more energy).
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Students should realize that each atom in a group has the same number of electrons in its outermost energy level. For instance, hydrogen, lithium, sodium, and potassium all have 1 electron on their outer energy level. Let students know that these electrons in the outermost energy level are called valence electrons.
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The outermost shell in an atom cannot have more than eight electrons even if it has a capacity to take up more electrons. This is also called the octet rule. Protons and neutrons have nearly same mass(one unit). Electrons have negligible mass.
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Oxygen is #8 in the periodical table. First electron shell can hold 2 electrons; second, 8. Therefore, out of 8 electrons, 2 go to the first shell and 6 to the second; valence electrons are the ones on the outermost shell (there are some exceptions, but they are much further down the table).
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Group 2A elements are the alkaline earth metals and all have two electrons in the outermost energy level because their electron configuration ends in s2. Group 5A elements all have five electrons in the outermost energy level because their electron configuration ends in s2p3.
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Hydrogen ( Hstart text, H, end text), lithium ( Listart text, L, i, end text), and sodium ( Nastart text, N, a, end text), as group 1 elements, have just one electron in their outermost shells. They are unstable as single atoms, but can become stable by losing or sharing their one valence electron.
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Hydrogen (H), lithium (Li), and sodium (Na), as group 1 elements, have just one electron in their outermost shells. They are unstable as single atoms, but can become stable by losing or sharing their one valence electron.
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For groups 1-2 and 13-18, the valency is directly related to group number. So, elements in group one, the alkali metals, have one valence electron, those in group two have two valence, those in group thirteen have three electrons, and so on.
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They are lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). (Like the other elements in Group 1, hydrogen (H) has one electron in its outermost shell, but it is not classed as an alkali metal since it is not a metal but a gas at room temperature.)
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Each H atom (group 1) has 1 valence electron, and the O atom (group 16) has 6 valence electrons, for a total of 8 valence electrons.
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The hydrogen atom has one electron in the outer shell in a stable state. To find out how much outer shell electrons (Valent electrons) an element has look at what group the element is in by looking at what column(group) it is in.
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Elements in group 1 and group 2 are metals. Atoms of group 1 elements have one electron in their outer shell, and atoms of group 2 elements have two electrons in their outer shell. Some elements in groups 6 and 7, and all in group 0 (also known as group 8) are non-metals.
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Why are the Group 1 Elements so Reactive ? The first three elements in Group 1 are Lithium, Sodium and Potassium and the three pictures below show the arrangement of electrons in their atoms. They have all got one electron in the outside shell even though they all have a different number of electrons in total.
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The s subshell has 1 orbital that can hold up to 2 electrons, the p subshell has 3 orbitals that can hold up to 6 electrons, the d subshell has 5 orbitals that hold up to 10 electrons, and the f subshell has 7 orbitals with 14 electrons.
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Lithium, Li Lithium is in Group 1. It has one electron in its outer shell. When this electron is lost, a lithium ion, Li +, is formed.
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Physical properties Whereas all other group 8 elements have two electrons in the outermost shell, in ruthenium, the outermost shell has only one electron (the final electron is in a lower shell). This anomaly is observed in the neighboring metals niobium (41), molybdenum (42), and rhodium (45).