What are the periodic trends for electronegativity and atomic radius?

What are the periodic trends for electronegativity and atomic radius?

From top to bottom down a group, electronegativity decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius.

What is the trend of atomic radii in the periodic table?

Periodic Trend The atomic radius of atoms generally decreases from left to right across a period. There are some small exceptions, such as the oxygen radius being slightly greater than the nitrogen radius. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level.

What are the trends for electronegativity and electron affinity?

However, this trend applies only to Group-1 atoms. Electron affinity follows the trend of electronegativity: fluorine (F) has a higher electron affinity than oxygen (O), and so on. The trends noted here are very similar to those in ionization energy and change for similar (though opposing) reasons.

What are the trends for atomic radii ionization energy and electron affinity?

Generally, the atomic radius increases with element size (atomic number). Ionization energy and electron affinity also increase with increasing atomic number, but primarily along the same row (left to right) of elements in the Periodic Table. Truong-Son N.

What is the highest electronegativity value?

The largest electronegativity (3.98) is assigned to fluorine and all other electronegativities measurements are on a relative scale. Since metals have few valence electrons, they tend to increase their stability by losing electrons to become cations.

Is oxygen more electronegative than chlorine?

Oxygen is more electronegative than chlorine because of the following reasons : Oxygen is placed towards the left side of fluorine so has one electron less than fluorine. Chlorine is below fluorine and has a new shell of valence electrons is added to it.

Why do both atomic size and ionic size increase as you move down a group?

Basically, as we move down the periodic table, the size of the nucleus increases, and concomitantly more electrons are present to “shield” the valence electrons from the charge. If there are many electrons, its harder to rope them up via electron charge than when there are less.

Why does ionic size increase down a group?

Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius. Ionic radius is the distance from the nucleus to the outer edge of the electron cloud of an ion.

What group has the highest electron affinity?

Atoms, such as Group 7 elements, whose anions are more stable than neutral atoms have a higher electron affinity. The electron affinities of the noble gases have not been conclusively measured, so they may or may not have slightly negative values. Chlorine has the highest electron affinity while mercury has the lowest.

What element has the highest electron affinity?

Chlorine has the highest electron affinity among the elements. Its high electron affinity can be attributed to its large atomic radius, or size. Because chlorine’s outermost orbital is 3p, its electrons have a large amount of space to share with an incoming electron.

Which best describes ionization energy?

Ionization energy refers to the amount of energy needed to remove an electron from an atom. Ionization energy decreases as we go down a group. Ionization energy increases from left to right across the periodic table.

Which element has higher electronegativity Aluminium or phosphorus?

Answer: phophorus has higher electronegativity than aluminium. Explanation: the 1st reason is that in the periodic table from left to right the electronegativity decreases.