Which of the following properties or characteristics do not apply to metals (two correct answers) : (a) good thermal conductivity, (b) high strength, (c) high electrical resistivity, (d) high stiffness, and (e) ionic bonding?

(c) high electrical resistivity and (e) ionic bonding

Explanation:

The bond between metals it's called metallic bond. The ionic bond occurs between metallic and non-metallic atoms in the periodic table. In the case of metals, we have a bond between metallic atoms. The atom shares all its valence electrons with its neighbors creating a cloud of electrons, this allows the free movement of electrons in the structure that's why they can easily transport heat and electricity. So, metals have a good thermal and electrical conductivity that's is the opposite to high electrical resistivity which is not a characteristic of metals. When an atom shares its valence electrons, we end up with a positive ion in the center with all the electrons around it (cloud of electrons) this structure in the ideal case allows symmetric because the ions are the same. This symmetry creates very packet structures that explained the high density, strength, and stiffness in metals.