are nonmetals, include the halogens
Group 2A elements typically lose 2 electrons when forming ions.
Silicon will tend to gain electrons in order to achieve a stable outer electron configuration, as it has 4 valence electrons and typically forms covalent bonds with other elements by sharing electrons.
Elements in the oxygen family tend to gain electrons in chemical reactions. This is because these elements, like oxygen, have six valence electrons and typically achieve a stable electron configuration by gaining two electrons to complete an octet.
The elements that have 5 electrons in the dot diagram means that they have 5 valence electrons. These elements are found in group 5A. Elements include, nitrogen, phosphorus, arsenic, antimony, and bismuth.
Most elements have multiple energy levels, typically ranging from 1 to 7. The number of energy levels an element has depends on the number of electrons it contains. Each energy level corresponds to specific electron orbitals where electrons can be found.
From one - e.g. Copper - to eight - e.g. Nickel.
+ include the halogens + are non metals
Group 2A elements tend to GAIN electrons!!
no
Group 2A elements typically lose 2 electrons when forming ions.
Elements with electrons that are not tightly held are more likely to form ionic bonds because they have a tendency to lose or gain electrons to achieve a stable electron configuration. This typically occurs in elements with large differences in electronegativity, leading to the transfer of electrons and the formation of ionic compounds. Bonds between such elements are typically less likely to form covalent bonds.
Elements with the same number of valence electrons typically have similar chemical properties. This is because valence electrons determine an element's reactivity and bonding behavior. Elements in the same group on the periodic table have the same number of valence electrons.
The valence electrons in main group elements are typically found in the s and p orbitals. Group 1 and 2 elements have valence electrons in s orbitals, while groups 13-18 elements have valence electrons in both s and p orbitals.
Group 13 elements tend to lose three valence electrons to achieve a full outer shell configuration. They typically form 3+ ions by losing these three electrons.
The elements that typically give up electrons are the ones which have the lowest ionization energy. The valence electron which holds on loosely will be the one to be given out easily.
Because in nature the elements seek to either give out electrons of take electrons. So the elements that gives out electrons bonds with the elements that takes electrons so that both of them are "happy"
Because as we know first that positive attracts to neutral, so protons and neutrons are attracted together and remain together in the nucleus. So there is no chance protons or neutrons can be given up because of attraction forces. Whereas electrons on the other hand are negatives and repel each other and whiz around the atom. So elements typically give up electrons because electrons want to stay away from each other because of the strong repulsion forces. Hence they are given typically by the elements.