Name Desk Date Laboratory Instructor . Pre-lab Questions Molecular Geometries of
ID: 1080466 • Letter: N
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Name Desk Date Laboratory Instructor . Pre-lab Questions Molecular Geometries of Covalent Molecules: Lewis Structures and the VSEPR Model Before beginning this experiment in the laboratory, you should be able to answer the following questions. I. Distinguish among ionic, covalent, and metallic bonding. hich of the following molecules possess polar covalent bonds: H2, N2, HCL, HCN, and co? 3. Which of the molecules in question 2 have molecular dipole moments? What are the favored geometrical arrangements for AB, molecules for which the A atom has 2, 3, 4, s, and 6 pairs of electrons in its valence shell? 4. 5. How many equivalent orbitals are involved in each of the following sets of hybrid orbitals: sp. spsp'd and sp'd 6. Define the term formal charge. 7. Calculate the formal charges of all of the atoms in CO, CO2, and CO,Explanation / Answer
1- A covalent bond is formed between two non-metals that have similar electronegativities.compound which form covalent bond have low melting point and they have definite shape, it is formed between two non metals.
Ionic bonding occurs between atoms that have opposite needs for electrons (metals and nonmetals) and results in a transfer of electrons. Non-metals(-ve ion) are "stronger" than the metal(+ve ion) and can get electrons very easily from the metal. These two opposite ions attract each other and form the ionic bond. Compound which have ionic bonding have high melting and boiling point due to polarization, stronger than covallent bond.
Metallic bonds involve all of the metal atoms in a piece of metal sharing all of their valence electrons with delocalized bonds
2-HCl and HCN posses polar covalent bonds.
3-HCL ,HCN have dipole movements.
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