Since the force of attraction increases across a period the trends noticed down a group are reversed.
Why does the force of attraction decrease?
Since gravitational force is inversely proportional to the square of the separation distance between the two interacting objects, more separation distance will result in weaker gravitational forces. So as two objects are separated from each other, the force of gravitational attraction between them also decreases.
What increases the attraction of an electron?
Higher electronegativity values mean a higher tendency to attract electrons. Atoms with high E.N. are strong oxidants (gain electrons).
Does force of attraction decrease across a period?
With a larger distance between the negatively-charged electron and the positively-charged nucleus, the force of attraction is relatively weaker. Therefore, electron affinity decreases. Moving from left to right across a period, atoms become smaller as the forces of attraction become stronger.
Does force of attraction increase from left to right?
The net force of attraction between the nucleus and the valence electron in an atom increase as you move across a period from left to right. As you move across a period, the valence electrons in the atom experience a stronger pull toward the nucleus.
How does force affect attraction?
The gravitational force is the only force that is purely attractive. Electricity and magnetism can be repulsive as well. For all three forces, the closer the objects are to each other, the stronger the force of attraction. When the objects are far apart, the force of attraction is weaker.
What is intermolecular force of attraction?
Intermolecular forces are the forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions ). These forces are weak compared to the intramolecular forces, such as the covalent or ionic bonds between atoms in a molecule.
Why does the force of attraction between the nucleus and electrons decrease down a group?
As you go down a group, the nuclear charge decreases because the valence electrons move further away from the nucleus depleating the force of attraction between the nucleus and the electrons.
Why does electrostatic attraction decrease down the group?
Down a group, the number of energy levels (n) increases, and so does the distance between the nucleus and the outermost orbital. The increased distance and the increased shielding weaken the nuclear attraction, and so an atom can’t attract electrons as strongly.
What factors affects electrostatic attraction?
As we’ll discuss in this lesson, he found that the force between charged particles was dependent on only two factors: the distance between the particles and the amount of electric charge that they carried.
Does shielding increase down a group?
Shielding increases DOWN a Group because the nuclear core is farther removed from the valence electrons.
Does Zeff increase or decrease down a group?
The effective nuclear charge, Zeff, increases down a group which draws electrons closer towards the nucleus, decreasing atomic radius.
Does nuclear charge decrease down a group?
The periodic table tendency for effective nuclear charge: … Decrease down a group (although nuclear charge increases down a group, shielding effect more than counters its effect).