C. Why is the forth ionization of Aluminum so much larger than its third ionizat

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C. Why is the forth ionization of Aluminum so much larger than its third ionization? 10. Distinguish between lonic, Covalent and Metallic compounds A. Describe a covalent bond. How is this different than an ionic bond? B. Wh bond? C. What is the typical composition of an D. In comparison to covalent and ionic compounds, how are the electrons treated differently in a metallic compound? at is a perfectly or purely covalent bond? How is this different than a polar covalent ionic bond? And the composition of a covalent bond? 11. Explain the trends in ionization noted in the 50 T He following figure Ne A. Why is the ionization energy of Helium greater than that of the other elements? B. Why is the ionization energy on nitrogen larger than that of oxygen? C. Why are the ionization energies of the halogens to much larger than the other elements on the periodic table? D. Why are the ionization energies of the alkali metals all much smaller than the rest of the elements on the table? Rn 1000 Li Ne 1357 9 11 1 15 17 1 31 33 35 37 51 53 55 81 83 Atomic Number 12. Clearly be able to explain and distinguish between ionic, covalent and metallic com pounds Which of the following are ionic, covalent or metallic?

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C The electronic configuartion of aluminium is 1s22s22p63s23px1. The first three electrons to be removed are the three electrons in the 3p and 3s orbitals.The fourth electron is removed from the 2p level which is much closer to the nucleus, and only screened by the 1s2 (and to some extent the 2s2) electrons.

10)

Ionic molecules have ionic bonds which are formed when transfer of electrons takes place. The donor atom donates one or more electrons to another. This leaves the donating atom electron deficient (+ve charged ion) and the other atom electron rich ( -ve charged ion). Electrostatic forces of attraction are seen as they are oppositely charged and thus ionic bond forms.

Covalent molecules show covalent bonding which occurs when atoms/molecules share pairs of electrons.

Metals show metallic bonding. Giant structures of metal atoms arranged in a regular pattern. The outer shell electrons of metals are delocalised (free to move around) and so a metallic structure is a regular arrangment of +ve charged ions with negative electrons in between, held together by electrostatic forces of interaction.

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