Why does atomic radius decrease as coulombic attraction increases?
Chlorine has 17 protons and magnesium has 12 protons. Therefore, since chlorine’s nucleus has a greater positive charge, the outer electrons will experience more of that positive charge (increase effective nuclear charge) which causes the chlorine atom to have a smaller atomic radius.
How does atomic radius affect force of attraction?
In the periodic table, the atomic radius of elements tends to decrease as you move across a row from left to right. The number of protons increases left to right, leading to a greater attractive force in the nucleus.
What is the relationship between affinity and atomic radius?
Electron affinity increases from left to right within a period. This is caused by the decrease in atomic radius. Electron affinity decreases from top to bottom within a group. This is caused by the increase in atomic radius.
What is atomic radius Why does atomic radius decrease across a period?
Atomic radius decreases across a period because valence electrons are being added to the same energy level at the same time the nucleus is increasing in protons. The increase in nuclear charge attracts the electrons more strongly, pulling them closer to the nucleus.
What does atomic radius depend on?
The value of atomic radii depends on the type of chemical bond in which the atoms are involved (metallic, ionic, or covalent bond). … When the neighbouring atoms are not alike, as in sodium chloride, part of the observed distance between atoms is assigned to one kind of atom and the rest to the other kind.
What factors influence atomic radius?
Explanation of the general trends
|factor||principle||effect on radius|
|nuclear charge||attractive force acting on electrons by protons in nucleus||decreases the atomic radius|
|shielding||repulsive force acting on outermost shell electrons by inner electrons||increases the atomic radius|
What is the relation between atomic radius and screening effect?
Explanation: Shielding is when electrons in the inner electron shells of an atom can shield the outer electrons from the pull of the nucleus. The nucleus can pull the outer electrons in tighter when the attraction is strong and less tight when the attraction is weakened. … This means the atomic radius will be larger.
How would you describe the coulombic attraction between the nucleus of the atom and the two electrons in the 4s sublevel?
How would you describe the Coulombic attraction between the nucleus of the atom and the two electrons in the 4s sublevel? The attractive force is equal for both electrons. … The attractive force between the valence electrons and the nucleus decreases.
How does Coulomb’s law explain periodic trends?
According to Coulomb’s Law, the attraction is stronger as the charge on the nucleus (Z) increases, and as the electron gets closer to the nucleus. • The charge of the nucleus increases as Z increases, but the electrons do not always “feel” all of the charge due to shielding by the inner electrons (Figure 8.11).
Does coulombic attraction decrease down a group?
The bigger the size of the atom, the electrons, especially the valence electrons are further away from the nucleus. The nucleus is not able to pull the electrons, that are in orbitals further away from the nucleus, towards itself and the coulombic attraction decreases.