Why don’t metals break when pounded into sheets or drawn into wires?
the electrons in metals are shared so that the bond between them is too strong to be broken by pounding.
the electrons in metals allow the cations to slide past and thereby reduce the repulsive force between them.
the electrons in metals are either given up or taken up while bonding, creating a bond too strong to be broken by pounding.
they form molecules in which each atom is bonded to many other atoms, forming a sturdy structure which doesn’t break on pounding.
they form molecules which have a very high boiling and melting point, which makes them resistant to breaking.

The electrons in metals allow the cations to slide past and thereby reduce the repulsive force between them.

Explanation:

In metals, positively charged metal ions and electrons are arranged in  lattice. There is a strong electrostatic force of attraction between the metal cation and a sea of delocalized electrons. As there is free sharing of electrons among a network of metal ions metals don't break when pounded into sheets or drawn into wires.

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g