Chemistry quiz periodic trends
Using your knowledge of Coulombic attraction and the structure of the atom, explain the trend of ionization energy that you identified in question 7.
As you go down a group, there is less of a Coulombic attraction because of the increase in the amount of energy levels. This decrease of attraction and increase of energy levels causes the radius to be larger as well. Because of this, the ionization energy decreases as you go down because of the loose hold, meaning less energy is need to take away electrons.
What is the trend in electronegativity going across a period?
It increases because the atom is smaller.
In general, what is the trend in ionization as you go across a period?
It increases.
Explain the existence of the trend described in part c in terms of atomic structure and Coulombic attraction.
As you go across a period, there is a stronger attraction which decreases the size of the radius. Because the radius is smaller it is easier for the nucleus to pull in more electrons.
Explain the existence of the trend described in part a in terms of atomic structure and Coulombic attraction.
As you go down a group, the increase in amount of energy levels decreases the Coulombic attraction within the atom. This means that electronegativity would decrease as you go down a group because it would be even harder for the nucleus to pull in electrons that far away.
Using your knowledge of Coulombic attraction and the structure of the atom, explain the trend in ionization energy that you identified in Question 9.
As you go across a period, the Coulombic attraction increases which decreases the radius of the atom. Because of this tight hold, there is more energy needed to ionize an atom.
In general, what is the trend in ionization energy as you go down a group? Support your answer using examples from three groups.
As you go down a group, the ionization energy decreases because there is less of an attraction within it. Because of this weak attraction, it's easier for an electron to be taken out because it's loose.
Atoms with loosely held electrons are usually classified as metals. They will exhibit high conductivity, ductility, and malleability because of their atomic structure. Would you expect metals to have high ionization energies or low ionization energies? Explain your answer in one to two complete sentences.
Because of the loose hold, I would expect metals to have a low ionization energy because it is easier to remove an electron.
What is the trend in electronegativity going down a group?
It decreases because a big atom is too far from the nucleus.
Which takes more energy, removing an electron from an atom where the nucleus has a tight hold on its electrons, or a weak hold on its electron? Explain.
It is harder to remove an electron from an atom with a tight hold because that means that there is a stronger attraction and force within it. If there is a weak hold, it's easier for an electron to be taken out because there it is looser.
Using your knowledge of Coulombic attraction, explain why ionization-removing an electron an atom-takes energy.
The Coulombic attraction makes it hard to take an electron because they are getting pulled together so it makes it difficult to remove an electron from the force.
