Answers To Questions On Periodic Trends From Electronegativity Thru Metallic Characteristics

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7, There is a highlighted "stairs" on right side of most Periodic Table. Metals are to the left of the stairs, Non-metals are to the right. Any element that has "stairs" as side of its element block, is a Semi-metal (also called Metalloid).

Answers to Questions on Periodic Trends from Electronegativity thru Metallic Characteristics.

The phrase Shielding effect is not acceptable part of your answer. You will need to explain via Coulombic Force (CF).

1. Higher the EN, the higher the CF of nucleus to valence electrons. For example, high EN elements tend to pull valence electron towards the nucleus thereby either sharing or taking valence electron.

2. EN decreases as you down a Group since the CF is decreases since the valence electron are in higher energy levels causing them to be held less tightly to the nucleus.

3. EN increases as go across since the nuclear charge is increasing causing the nucleus to have a greater pull (CF) to the nucleus.

4a. Top right

4b. Bottom left

5. Rb, Cr, Si, Cl

6. Ionic radii (IR) increase as you go Down a Group

7, There is a highlighted "stairs" on right side of most Periodic Table. Metals are to the left of the stairs, Non-metals are to the right. Any element that has "stairs" as side of its element block, is a Semi-metal (also called Metalloid).

8. Since the nucleus in metal elements tend to have weaker pull on the valence electrons (low CF), it takes little energy to have those valence electron be released from the atom (results in a positively charged ion called cations).

9. Since the nucleus in non-metal elements tend to have greater pull on the valence electrons (higher CF), it takes more energy to have those valence electron be release so tend to stay (sometime it is called sharing) and valence electrons from other atoms could be drawn to the non-metal nucleus (non-metal element could take these electron causing a negatively charged ion called anion).

10. Atomic radii (AR) are also larger than Ionic radii (IR) for metal elements.

11. IR are also larger than AR in non-metals. Since the anion has obtained one more electron, there is more electron-electron repulsion thereby making the valence electron farther away from each other (increasing size from atom to ion).

12. MC increases as you down a Group.

13. MC decreases as you go across a Period. Since the CF increase as you go across Period, it takes more energy to pull an electron from the nucleus while makes it harder to release an electron (definition of metal).

14. Bottom left

15. Q7 indicates that the Metals are to the right of "stairs" on the Periodic Table which corresponds to Down a Group and moving Right to Left on Period to get the highest MC elements that we call Metals. The opposite explanation is true for non-metals.

16. Cl, S, As, Ag, Ba