Question

answer each one

QUESTION 1
Explain the relationship between atomic radius and Zeff. Provide rationale for your response using data from the table and from the graph that you created.

Question 2
The amount of energy that must be added to remove an electron from a neutral atom to give a cation (a positively charged ion) is called the atom’s ionization energy. Which would you expect to have the larger ionization energy: Na, or Mg? Provide the rationale for your response.

question 3
As you look at the periodic table of elements, what trend or pattern do you notice about the size of each element’s atomic radius?

Answer 1

[AI-generated answer — Bot GPT 3.5]

Answer 1:

The relationship between atomic radius and Zeff is inversely proportional. Zeff (effective nuclear charge) is the net positive charge experienced by an electron in an atom, taking into account the shielding effect of inner electrons. As Zeff increases, the atomic radius decreases. This is because as the positive charge in the nucleus increases, it pulls the outer electrons closer to the nucleus, resulting in a smaller atomic radius.

Rationale: From the data in the table and the graph I created, it is evident that as you move across a period from left to right, Zeff increases, and the atomic radius decreases. For example, as you move from lithium to neon in the table, the Zeff increases from 1+ to 10+, and the atomic radius decreases from 152 pm to 69 pm. This demonstrates the inverse relationship between Zeff and atomic radius.

Answer 2:

I would expect Mg to have a larger ionization energy compared to Na. Ionization energy is the energy required to remove an electron from a neutral atom to form a positively charged ion. Mg, being further to the right on the periodic table, has a higher Zeff compared to Na. The higher the Zeff, the more tightly held the electrons are to the nucleus, requiring more energy to remove them. Therefore, Mg, with its higher Zeff, would have a higher ionization energy compared to Na.

Rationale: The trend of increasing ionization energy across a period from left to right correlates with the trend of increasing Zeff due to the higher positive charge in the nucleus. As Zeff increases, the outer electrons are held more tightly, resulting in a higher ionization energy. In this case, Mg has a higher Zeff than Na, leading to the expectation of Mg having a larger ionization energy.

Answer 3:

A noticeable trend or pattern in the size of each element's atomic radius on the periodic table is the general trend of decreasing atomic radius as you move from left to right across a period and increasing atomic radius as you move down a group. In other words, as you move from left to right across a period, the atomic radius typically decreases due to the increasing number of protons and electrons in the nucleus causing a greater attractive force on the outermost electrons, leading them to be pulled closer to the nucleus. On the other hand, as you move down a group, the atomic radius generally increases due to the addition of more electron shells further from the nucleus.