Metals are elements belonging to first , second or third group. They have one ,two or three valence electrons (electrons present in the last orbit of an atom). They lose this electrons to gain stability as they are highly unstable and by doing so they react .
NOTICE:
An atom can only lose the electron if an atom of other element is ready to take it.
They tend to conduct them, by allowing them passage.
Metals behave in a rather unique way as far as their electrons are concerned.The electrons in metals are de-localised, which in effect means they are not bound to a particular atom, like a "sea of electrons".This property makes them good conductors of electricity because charged electrons can easily travel from one end of the metal to the other whilst maintaining that charge.
The alkali metal group easily lose their outermost electron. This group consists of lithium, sodium, potassium, rubidium, cesium, and francium.
metal conducts electricity because it allows electrons to move freely as well as it has free electrons, unlike insulators(non-metals) which do not have free electrons. When the electrons are allowed to move freely in a substance, it is a good conductor and allows electric charge to flow.
the number of electrons in the outer shell .. for metals its less than 4 .. for non metals its more than 4 .. for semi its 4
The difference in properties between metal and nonmetal solids (i.e. brittleness, malleability, conduction of both heat and electrical current) is due to availability or absence of free electrons. Contrarily to abundance of free electrons in metals, free electrons are much fewer in nonmetal objects. Electrons that are not bound to atoms are free to roam about, and that is what free electrons do (everywhere) in a piece of metal. These electrons would take impact energy and (practically instantly) distribute it throughout the piece, acting like a bumper in a car. It helps to remember that things are mostly empty space as that is how atoms are. Atomic properties explain also the difference in heat transfer: metals feel cold on a touch because free electrons immediately take energy from a tip of a finger and 'run away with it.' (We feel something is colder when we give out energy, instead of receiving it.) E.Silvermint
Metals loss electrons and nonmetals gain electrons.
Metals give up electrons while non-metals gain electrons
Metals lose electrons in a chemical reaction.
No, it is not true. When metals loose electrons they become cations.
Nonmetals tend to gain electrons during a chemical reaction to achieve a stable electron configuration, while metals tend to lose electrons for the same reason. This transfer of electrons helps both types of elements achieve a full outer energy level, often leading to the formation of ionic compounds.
Metals have fewer protons in their nucleus compared to nonmetals, meaning their electrons are held less tightly by the positively charged nucleus. This results in lower ionization energies for metals, making it easier to remove electrons from them compared to nonmetals. Additionally, metals tend to have more outer electrons which are further away from the nucleus, making them easier to remove.
In their regular (lattice) structure, metals have a sea of free electrons. This allows the electrons to flow through the metal at will and this is what makes metals good conductors of electricity (and heat).Their mobile electrons
Yes, electrons move freely in metals.
Metals typically prefer to lose electrons rather than gain them in chemical reactions, as this allows them to achieve a more stable electron configuration. Metals tend to form positively charged ions by losing electrons to achieve a full outer electron shell.
Nonmetals usually accept electrons to become negative ions (anions), e.g. Cl + e- --> Cl-.
Metals have more free electrons/valence electrons/
Covalent bonds are formed when non-metals share electrons. Ionic bonds are formed when metals and non-metals lose and gain electrons.