How does distance between the nucleus and the electrons affect the attraction between them?
Down a group, the number of energy levels (n) increase and the distance is greater between the nucleus and highest-energy electron. The increased distance weakens the nuclear attraction to the outer-most electron, and is easier to remove (requires less energy).
What happens to the attractive force between the nucleus and the electrons?
The attractive force of the nucleus on its electrons is known as the effective nuclear charge ( Zeff ), and decreases as you get further from the nucleus. The nucleus is positive and the electrons are negative, which obviously means they attract. … As you move further from the nucleus, S increases, and so Zeff decreases.
What would cause the attractive force between the nucleus and outer electrons to be increased?
Why? increases; because the number of charges on the nucleus increases, that attracts the bonding pair of electrons more strongly.
What is the relationship between distance and attractive force?
Increasing the separation distance between objects decreases the force of attraction or repulsion between the objects. And decreasing the separation distance between objects increases the force of attraction or repulsion between the objects.
What happens to the distance between the nucleus and the outermost electrons going left to right across a period?
(a) What happens to the distance between the nucleus and outermost electrons going ACROSS a period? (refer to above section on atomic radius!) The distance decreases as the increasing nuclear charge pulls the electrons closer. … The nuclear charge increases.
How does increasing the magnitude of the charge of the particles affect the attractive force between them?
The magnitude of the force is directly related to the magnitude of charge on the particles (higher charge yields stronger force) and indirectly related to the distance between the particles (large distance yields weaker force).
When protons and electrons are closer together the force of attraction is?
That is, a proton and an electron will attract each other. The closer they are together, the stronger this attraction will be. Two protons (or two electrons) will repel each other. And again, the closer together they are, the stronger the repulsion.
What force causes attraction in the nucleus?
Inside the nucleus, the attractive strong nuclear force between protons outweighs the repulsive electromagnetic force and keeps the nucleus stable. Outside the nucleus, the electromagnetic force is stronger and protons repel each other.
How would the force change if the distance between the nucleus and the valence electron increases?
Ans: As you go down a column, the valence electrons are on levels that are further away from the nucleus. According to Coulomb’s law, the further the distance, the less force holding the electrons, so they are easier to lose.
What 2 factors affect the attractive force between the nucleus and valence electrons?
1) Nuclear charge: The greater the nuclear charge (more positive), the stronger the force of attraction. 2) Distance from the nucleus: The further away the electrons, the greater the number of filled electron shells shielding it from the nucleus, and therefore the weaker force of attraction.
What is the relationship between attractive force between the electrons and protons and the energy required to remove an electron?
The more protons in the nucleus, the stronger the attraction of the nucleus to electrons. This stronger attraction makes it more difficult to remove electrons. Within a group, the ionization energy decreases as the size of the atom gets larger.