Respuesta :
Answers :
Solution of each part is given below.
Explanation:
a) [tex]S_8[/tex] non polar covalent ( because each sulphur atom shares electron and the net dipole moment is zero.)
b) RbCl ionic ( Rb have good tendency to donate electron and chlorine is too electro negative therefore they make strong ionic bond.)
c) [tex]PF_3[/tex] polar covalent ( because of triagonal pyramidal geometry and strong electronegativity of F atom it is polar and covalency is due to the share of electron with each F atom.)
d) [tex]SCl_2[/tex] polar covalent ( because of tetrahedral geometry and sharing of electrons between S and Cl.)
e) [tex]F_2[/tex] non polar covalent ( because of linear geometry they are non polar and bond between them is formed due to sharing electrons.)
f) [tex]SF_3[/tex] polar covalent ( because of T- shape geometry they are non polar and due to sharing of electrons they are polar covalent.)
Hence, this is the required solution.
The nature or type of bonds formed by molecules and compounds are greatly influenced by the chemical properties of the element.
Data;
- S8
- RbCl
- PF3
- SCl2
- F2
- SF2
Bonds in the Compounds
The chemical properties of an element often affects how it bonds with other elements to form a compound. In this case, we have several compounds given.
S8: This is a non-polar covalent molecule.
RbCl: This is an ionic compound because it consists of very strong electropositive and electronegative elements.
PF3: This is a polar covalent compound due to the nature of phosphorous.
SCl2: This is a polar covalent compound
F2: This is a non-polar covalent compound
Sf3: This is a polar covalent compound
Learn more on types of bonds here;
https://brainly.com/question/9817093
