How is the crystal lattice of an ionic compound different from the crystal formation of a metallic compound? Select all that apply.

A. An ionic compound has a rigid crystal structure because of the repulsive forces between the negative ions that are sharing the electrons.

B. A metallic compound forms a crystal structure with overlapping valence atomic orbitals and has delocalized electrons that are free to move around.

C. A metallic compound forms a crystal structure because the transferred electrons have an attractive force on the negative ions in the metal nuclei.

D. An ionic compound has a rigid crystal structure with positive and negative ions fixed in place based on attractive forces.

B. A metallic compound forms a crystal structure with overlapping valence atomic orbitals and has delocalized electrons that are free to move around.

D. An ionic compound has a rigid crystal structure with positive and negative ions fixed in place based on attractive forces.

Explanation:

Ionic crystal lattice forces are the strong electrostatic forces of attraction between oppositely charged ions arranged into a crystal lattice of ionic compounds. The forces are by far stronger than hydrogen and van der waals forces.

Metallic bonds joins atoms of metals and alloys together. The metallic bond is an attraction between the positive nuclei of all the closely packed atoms in the lattice and the electron cloud jointly formed by all the atoms losing their outermost shell electrons.

Explanation:

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.