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Group 2 (Alkaline Earth Metals)
Beryllium: 1s2 2s2
Magnesium: 1s2 2s2 2p6 3s2
Calcium: 1s2 2s2 2p6 3s2 3p6 4s2
Strontium: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2
Barium: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2 4d10 5p6 6s2
Radium: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4f14 4d10 4p6 5s2 5d10 5p6 6s2 6s2 6p6 7s2
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Compared with Group 2A elements Group 6A elements have?
Group 6A elements have a higher electronegativity and a greater tendency to gain electrons to achieve a stable octet configuration. In contrast, Group 2A elements have a lower electronegativity and typically lose electrons to form cations.
When group 2a elements form ions what happens?
Group 2A elements (alkaline earth metals) tend to lose two electrons to form 2+ ions. This is because they have two valence electrons and tend to achieve a stable electron configuration similar to noble gases by losing those two electrons.
When a group 2A elements form ions they?
When group 2A elements form ions, they lose two electrons to achieve a stable electronic configuration. This results in the formation of 2+ cations.
How many elements are in group 2A?
There are 3 elements in Group 2A of the periodic table: Beryllium, Magnesium, and Calcium.
Which family of elements is characterized by an ns2 np5 valence configuration?
Elements that have configuration of ns2np5 are members of the Halogen group(Group VIIA). They are, Fluorine, Bromine, Iodine and Astatine.
Compared with Group 2A elements Group 6A elements have?
Group 6A elements have a higher electronegativity and a greater tendency to gain electrons to achieve a stable octet configuration. In contrast, Group 2A elements have a lower electronegativity and typically lose electrons to form cations.
Does group 2A gain electrons or lose electrons in order to achieve a noble gas configuration?
Group 2A elements tend to lose 2 electrons to achieve a noble gas configuration, as this will result in a full outer shell and stability.
When group 2a elements form ions what happens?
Group 2A elements (alkaline earth metals) tend to lose two electrons to form 2+ ions. This is because they have two valence electrons and tend to achieve a stable electron configuration similar to noble gases by losing those two electrons.
When a group 2A elements form ions they?
When group 2A elements form ions, they lose two electrons to achieve a stable electronic configuration. This results in the formation of 2+ cations.
How many elements are in group 2A?
There are 3 elements in Group 2A of the periodic table: Beryllium, Magnesium, and Calcium.
Which family of elements is characterized by an ns2 np5 valence configuration?
Elements that have configuration of ns2np5 are members of the Halogen group(Group VIIA). They are, Fluorine, Bromine, Iodine and Astatine.
What does group 6A elements have compared to group 2A?
Group 6A elements have six valence electrons and are nonmetals, while group 2A elements have two valence electrons and are metals. Group 6A elements have a higher electronegativity and form more covalent bonds compared to group 2A elements.
What is similar about the electron shells as you look across a periods?
All the elements in the same group have (usually) the same configuration of the valence electrons. For example, second-group elements (alkaline earth metals) all have ns2 configuration (where n=2-7). All halogens have ns2np5, etc. The similarity of electron configuration results in similarity of chemical properties.
How many electrons will group 2a lose?
Group 2A elements typically lose 2 electrons when forming ions.
Does group 2A elements lose or gain protons or electrons?
Group 2A elements typically lose electrons to form a +2 cation with a full outer electron shell. They do not gain protons or electrons, as their positive charge is due to the loss of electrons.
What is the general valence shell configuration for the elements in group 7A?
The general valence shell configuration for elements in group 7A is ns2np5, where n represents the principal quantum number of the valence shell. This configuration results in these elements having 7 valence electrons in their outermost shell.
How do 1A and 2A differ from the other group A elements?
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