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Chapter 13: Problem 2

Give the Lewis representation for each of the following atoms. a) iodine b) calcium c) phosphorus

Short Answer

Expert verified
The Lewis structure for iodine atom consists of seven dots around 'I', representing its 7 valence electrons. For Calcium atom, there are two dots around 'Ca' symbolising its 2 valence electrons. Lastly, for Phosphorus atom, there are five dots around 'P', symbolising its 5 valence electrons.

Step by step solution

01

Understanding atomic structure

An atom consists of a nucleus with protons and neutrons, surrounded by electrons in orbits. The amount of electrons in the outermost orbit, also known as valence electrons, determine an atom's ability to bond with other atoms.
02

Find the number of valence electrons for Iodine (I)

Iodine is in Group 17 of the Periodic Table and therefore has 7 valence electrons. Remember that the group number for main groups in the Periodic Table gives the number of valence electrons.
03

Draw the Lewis structure for Iodine (I)

The Lewis dot structure for iodine is a single atom with seven dots which represent its valence electrons.
04

Find the number of valence electrons for Calcium (Ca)

Calcium is in Group 2 of the Periodic Table and therefore has 2 valence electrons.
05

Draw the Lewis structure for Calcium (Ca)

The Lewis dot structure for calcium is a single atom with two dots representing its two valence electrons.
06

Find the number of valence electrons for Phosphorus (P)

Phosphorus is in Group 15 of the Periodic Table and therefore has 5 valence electrons.
07

Draw the Lewis structure for Phosphorus (P)

The Lewis dot structure for phosphorus is a single atom with five dots representing its five valence electrons.

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Most popular questions from this chapter

For \(\mathrm{H}_{2} \mathrm{CO}\) : a) Is the sum of the bonding electrons and lone pair electrons around the carbon atom consistent with the Lewis model? b) Is the sum of the bonding electrons and lone pair electrons (nonbonding electrons) around the oxygen atom consistent with the Lewis model?

For each of the following neutral atoms give the core charge. a) Li. b) \(\quad \ddot{C l}\) c) He:

Given the shell model of the atom, suggest a possible reason that Lewis proposed a maximum of two electrons for hydrogen and a maximum of eight for carbon, nitrogen, oxygen, and fluorine atoms?

For \(\mathrm{Cl}_{2}\), is the sum of the bonding electrons and the lone pair electrons (also known as nonbonding electrons) around each \(\mathrm{Cl}\) atom consistent with the Lewis model?

Use your checklist to determine whether or not the following is a correct structure for \(\mathrm{CO}_{2}\) $$ \ddot{\mathrm{O}}=\mathrm{C}=\ddot{\mathrm{O}} $$
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