Which statement comparing ionic and covalent bonds is correct?

b

Covalent bonds tend to be less polar than ionic bonds.

If 40g of Sodium (Na) completely reacts with 60g of Chlorine (Cl2), what is the mass of the products?

a
40 g
b
60 g
c
100 g
d
160 g

d

160 g

c2h5OH+2o2->2co2+3h2o is this balanced

No, this equation is not balanced.

The balanced equation for this reaction should be:

C2H5OH + 3O2 -> 2CO2 + 3H2O

The correct statement comparing ionic and covalent bonds is:

b
Covalent bonds tend to be less polar than ionic bonds.

To determine the correct statement comparing ionic and covalent bonds, let's analyze each option:

a) "More electrons are transferred from covalent bonds than ionic bonds."
This statement is incorrect. Ionic bonds involve a complete transfer of electrons from one atom to another, while covalent bonds involve the sharing of electrons between atoms.

b) "Covalent bonds tend to be less polar than ionic bonds."
This statement is correct. Covalent bonds occur between atoms that have similar electronegativities and therefore share electrons more equally, resulting in a less polar bond. In contrast, ionic bonds occur between atoms with a large electronegativity difference, leading to a more polar bond.

c) "Elements in Group 1A are more likely to form covalent bonds than ionic bonds with other atoms."
This statement is incorrect. Elements in Group 1A (also known as alkali metals) tend to have low ionization energies, making it easier for them to lose electrons and form positively charged ions through ionic bonding.

d) "The difference between electronegativities is greater in covalent bonds than for atoms in ionic bonds."
This statement is incorrect. Ionic bonds result from a large difference in electronegativities between atoms, while covalent bonds arise from a smaller difference in electronegativities. Therefore, the difference in electronegativities is greater for atoms in ionic bonds.

Based on the analysis, the correct statement is: "Covalent bonds tend to be less polar than ionic bonds." (Option b)