periodic trends - electronegativity practice\nfor each of the following grouping of elements, circle the…

Brief Explanations:

• For questions 1 - 4 (circle the element with the largest electronegativity):
  • Question 1: Germanium (Ge) is a metalloid and iron (Fe) is a metal. Metalloids have higher electronegativity than metals in general.
  • Question 2: Chlorine (Cl) is a non - metal and rubidium (Rb) is an alkali metal. Non - metals have higher electronegativity than alkali metals.
  • Question 3: Fluorine (F) is the most electronegative element in the periodic table. Astatine (At) is a halogen but less electronegative than F.
  • Question 4: Helium (He) is a noble gas with a full valence shell and does not tend to gain electrons (electronegativity is not typically defined for noble gases in the same way as for other elements, but if we consider the trend, noble gases have very low electron - affinity like behavior compared to other elements in terms of electron - seeking). Radon (Rn) is also a noble gas, but as we go down the noble gas group, the atomic size increases and the effective nuclear charge on the outermost electrons decreases. However, since noble gases' electronegativity is not in the same context as for non - noble gas non - metals, but if we assume a comparison based on the general trend of atomic size (smaller atoms in non - metal groups have higher electronegativity - like behavior in terms of electron - holding capacity), He has a smaller atomic size than Rn.
• For questions 5 - 11 (order in increasing electronegativity):
  • Question 5: Lithium (Li) is an alkali metal, beryllium (Be) is an alkaline earth metal, and hydrogen (H) has an electronegativity value that is relatively higher than Li and Be. In the periodic table, as we move from left to right across a period (Li to Be), electronegativity increases. And H has a higher electronegativity than alkali and alkaline earth metals.
  • Question 6: Indium (In) is a metal, boron (B) is a metalloid, and iodine (I) is a non - metal. Metals have lower electronegativity than metalloids, and metalloids have lower electronegativity than non - metals.
  • Question 7: Strontium (Sr) is an alkaline earth metal, tin (Sn) is a metal (post - transition metal), and gold (Au) is a transition metal. In general, alkaline earth metals have lower electronegativity than post - transition metals, and post - transition metals have lower electronegativity than some transition metals (based on their position in the periodic table and electron - holding capacity).
  • Question 8: Seaborgium (Sg) is a synthetic transition metal (very large atomic size and high atomic number, with electrons in inner f and d orbitals which shield the outer electrons from the nucleus), magnesium (Mg) is an alkaline earth metal, and palladium (Pd) is a transition metal. Alkaline earth metals (Mg) have lower electronegativity than some transition metals (Pd), and Sg (due to its large size and electron - shielding) has lower electronegativity than Pd.
  • Question 9: Sodium (Na) is an alkali metal, krypton (Kr) is a noble gas (electronegativity not in the same context as non - noble gas non - metals, but considering atomic size and electron - holding - like behavior, Na has a very low electronegativity as it readily donates electrons. Kr has a full valence shell. Oxygen (O) is a non - metal.
  • Question 10: Titanium (Ti) is a transition metal, cobalt (Co) is a transition metal (Co has a higher effective nuclear charge in the same period as Ti, so higher electronegativity than Ti). Carbon (C) is a non - metal. Non - metals have higher electronegativity than transition metals.
  • Question 11: Rutherfordium (Rf) is a synthetic transition metal (large atomic size, electrons in inner orbitals shield the outer electrons). Neon (Ne) is a noble gas (full valence shell). Selenium (Se) is a non - metal. Non - metals (Se) have higher electronegativity than transition metals (Rf), and noble gases (Ne) have a different electron - configuration context (but in terms of electron - seeking, Se is more likely to gain electrons than Rf).

Answer:

1. Ge
2. Cl
3. F
4. He
5. Li < Be < H
6. In < B < I
7. Sr < Sn < Au
8. Sg < Mg < Pd
9. Na < Kr < O
10. Ti < Co < C
11. Rf < Ne < Se