Referring only to a periodic table, give the ionic charge expected for each of these representative elements: (a) S, (b) K, (c) Br, (d) N, (e) Mg, (f) Ne, (g) C, and (h) Al. Write the Lewis symbols and structures that show how Na2O forms from sodium and oxygen atoms.
The Correct Answer and Explanation is :
Here are the expected ionic charges for each of the representative elements based on their position in the periodic table:
(a) S (Sulfur):
- Sulfur is in Group 16 (also known as Group VIA) of the periodic table. It has 6 valence electrons. Since nonmetals tend to gain electrons to achieve a stable octet configuration, sulfur will gain 2 electrons to form an ion with a charge of -2.
Ionic charge: -2.
(b) K (Potassium):
- Potassium is in Group 1 (Group IA), and it has 1 valence electron. Metals tend to lose electrons to achieve a stable configuration. Potassium will lose 1 electron to form an ion with a charge of +1.
Ionic charge: +1.
(c) Br (Bromine):
- Bromine is in Group 17 (Group VIIA), with 7 valence electrons. As a nonmetal, bromine will gain 1 electron to complete its octet, forming an ion with a charge of -1.
Ionic charge: -1.
(d) N (Nitrogen):
- Nitrogen is in Group 15 (Group VA) and has 5 valence electrons. To achieve a stable octet, nitrogen will gain 3 electrons and form an ion with a charge of -3.
Ionic charge: -3.
(e) Mg (Magnesium):
- Magnesium is in Group 2 (Group IIA), and it has 2 valence electrons. Magnesium will lose 2 electrons to form an ion with a charge of +2.
Ionic charge: +2.
(f) Ne (Neon):
- Neon is in Group 18 (Group VIIIA), and it has 8 valence electrons, making it a noble gas with a stable octet. It does not form an ion because it is already stable.
Ionic charge: 0 (neutral).
(g) C (Carbon):
- Carbon is in Group 14 (Group IVA) and has 4 valence electrons. Carbon can either gain 4 electrons to form an ion with a charge of -4, or it can lose 4 electrons to form an ion with a charge of +4. However, it typically forms covalent bonds, so the charge is usually considered neutral.
Ionic charge: 0 or +4.
(h) Al (Aluminum):
- Aluminum is in Group 13 (Group IIIA) and has 3 valence electrons. Aluminum will lose 3 electrons to form an ion with a charge of +3.
Ionic charge: +3.
Formation of Na2O from Sodium and Oxygen:
Sodium (Na) has 1 valence electron, and Oxygen (O) has 6 valence electrons.
- Each sodium atom loses 1 electron to form Na⁺ ions (each with a +1 charge).
- Oxygen gains 2 electrons to form an O²⁻ ion (with a -2 charge).
Since 2 sodium atoms (each with +1 charge) balance the charge of 1 oxygen atom (with a -2 charge), the formula for the compound formed is Na₂O.
Lewis Structures:
- Sodium: Na → [Na]⁺ (after losing 1 electron).
- Oxygen: O → [O]²⁻ (after gaining 2 electrons).
I’ll generate the Lewis structure showing this process now.
Here is the Lewis structure showing how Na₂O forms from sodium (Na) and oxygen (O) atoms. Two sodium atoms each lose one electron to form Na⁺ ions, and one oxygen atom gains two electrons to form an O²⁻ ion. This results in the formation of the ionic compound Na₂O.
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