weak
Valence electrons are further away from the nucleus and experience less attraction to the positively charged protons in the nucleus compared to core electrons. This makes valence electrons easier to remove from an atom. Core electrons are located closer to the nucleus and are more strongly attracted to the nucleus, requiring more energy to remove them from the atom.
•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. •It is also referred to as the screening effect or atomic shielding. •Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. Also, it has trends in the Periodic Table
The arrangement of electrons in atoms determines their chemical properties. Specifically, the number of electrons in an atom's outermost energy level (valence electrons) and how easily those electrons can be gained, lost, or shared with other atoms dictate the chemical behavior of an element.
Metals can be thought of as a lattice of metal ions surrounded by electrons. Again the force of attraction is electrostatic. These electrons are delocalised and metals get their conductiity from thir movement under an applied electric field. Positive metal ions in chemical compounds are surrounded by negativelly charged anions. The force between the oppositely charged ions is electrostatic.
The two main types of bonds formed between atoms are ionic bonds and covalent bonds. An ionic bond is formed when one atom accepts or donates one or more of its valence electrons to another atom. A covalent bond is formed when atoms share valence electrons. The atoms do not always share the electrons equally, so a polar covalent bond may be the result. When electrons are shared by two metallic atoms a metallic bond may be formed. In a covalent bond, electrons are shared between two atoms. The electrons that participate in metallic bonds may be shared between any of the metal atoms in the region.
The force of attraction by group 1 metals for their valence electrons is weak. This is because group 1 metals have a single valence electron that is loosely held and easily lost to form positive ions.
The force of attraction between the atom's nucleus and its valence electrons are the least. Hence valence electrons are lost easily.
Valence electrons are further away from the nucleus and experience less attraction to the positively charged protons in the nucleus compared to core electrons. This makes valence electrons easier to remove from an atom. Core electrons are located closer to the nucleus and are more strongly attracted to the nucleus, requiring more energy to remove them from the atom.
It is called shielding or screening effect. Inner electrons shield the valence electrons from the positive charge of the nucleus, reducing the attractive force between them.
Cations are formed by the loss of electrons, anions are formed by the gain of electrons. The force of attraction between cations and anions results in ionic bond.
The alkali metals tend to lose valence electrons because they have one electron in their outermost energy level, which makes them unstable. By losing this electron and achieving a full outer shell, they become more stable like the noble gases. This stability is the driving force behind their tendency to lose valence electrons.
electrostatic force
•The shielding effect describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. •It is also referred to as the screening effect or atomic shielding. •Shielding electrons are the electrons in the energy levels between the nucleus and the valence electrons. They are called "shielding" electrons because they "shield" the valence electrons from the force of attraction exerted by the positive charge in the nucleus. Also, it has trends in the Periodic Table
The force you are referring to is magnetism. Certain metals, such as iron, nickel, and cobalt, are attracted to magnets, while others, like aluminum and copper, are not. This attraction or repulsion is due to the arrangement of electrons within the material.
they have few valence electrons and aren't close to having eight valence electrons
The force that pulls electrons and protons together is electromagnetic force. This force is responsible for the attraction between opposite charges (electrons are negatively charged and protons are positively charged), which keeps the electrons orbiting the nucleus of an atom.
The outer shell is the valence electrons and they are very loosely bound to the nucleus - less force by the nucleus on the valence electrons, so valence shell's electrons are exchanged first in any reaction.