Question

1 outline the trends of the periodic table for ionization energy, atomic radius, and electronegativity on the periodic table above. 2. fill in these elements cs, mg, cu, ge, n, s, f on the periodic table above and use them to answer the following questions. a. which of the above elements is the most electronegative? why? b. which of the above elements has the smallest radius of the metals? why? c. which of the above elements has the highest ionization energy? why? d. which of the above elements is the most metallic (most characteristic of a metal)? why? e which of the above elements has the lowest ionization energy? why? f. which of the above elements has the largest atomic radius? why? g which of the above elements is a metalloid with 4 valence electrons? how do you know it has 4 valence electrons? h. which element is the least electronegative?

Explanation:

Step1: Recall periodic - table trends

Electronegativity increases across a period and decreases down a group. Ionization energy increases across a period and decreases down a group. Atomic radius decreases across a period and increases down a group. Metallic character decreases across a period and increases down a group.

Step2: Identify the most electronegative element

Cs is the most electropositive (least electronegative) among the given elements because it is in the lower - left part of the periodic table. As we move down a group, the electronegativity decreases due to the increase in atomic size and the shielding effect.

Step3: Identify the metal with the smallest radius

Among Mg, Cu, Cs (metals), Mg has the smallest radius. As we move down a group, the atomic radius increases, and as we move across a period from left to right, the atomic radius decreases. Mg is higher up in the periodic table compared to Cu and Cs.

Step4: Identify the element with the highest ionization energy

F has the highest ionization energy. Ionization energy increases across a period and F is on the right - hand side of the periodic table among the given elements. It has a small atomic radius and a high effective nuclear charge, making it difficult to remove an electron.

Step5: Identify the most metallic element

Cs is the most metallic. Metallic character increases down a group, and Cs is the element with the largest atomic size and the lowest ionization energy among the given metals, making it most likely to lose electrons.

Step6: Identify the element with the lowest ionization energy

Cs has the lowest ionization energy. As we move down a group, the outermost electrons are farther from the nucleus, and there is more shielding, so it is easier to remove an electron.

Step7: Identify the element with the largest atomic radius

Cs has the largest atomic radius. Atomic radius increases down a group, and Cs is in the lowest period among the given elements.

Step8: Identify the metalloid with 4 valence electrons

Ge is a metalloid with 4 valence electrons. Its electron configuration shows that it has 4 electrons in its outermost shell (4s²4p²), and it lies along the metal - non - metal boundary in the periodic table.

Answer:

a. Cs. Because it is in the lower - left of the periodic table and electronegativity decreases down a group.
b. Mg. As atomic radius decreases across a period and increases down a group, and Mg is higher up among the metals.
c. F. Due to its high effective nuclear charge and small atomic radius, ionization energy is high.
d. Cs. Since metallic character increases down a group and Cs has the largest atomic size and lowest ionization energy among metals.
e. Cs. As ionization energy decreases down a group and Cs is in the lowest period among given elements.
f. Cs. Atomic radius increases down a group and Cs is in the lowest period.
g. Ge. Its electron configuration (4s²4p²) shows 4 valence electrons and it is a metalloid.
h. Cs. Electronegativity decreases down a group and Cs is in the lower - left part of the periodic table among given elements.