Question: Does more protons mean more attraction?

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The more protons, the greater the attraction for an atom’s electrons. The more electrons, the less the attraction for an atom’s electrons.

Does a greater amount of protons mean a greater attraction between the protons and electrons?

We can explain this by considering the nuclear charge of the atom. 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.

How does the number of protons affect the attractive force?

Coulombic: how does amount of protons influence attraction between protons and electrons? The greater the number of protons, the greater the pull on the electrons, which means greater force.

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Does distance or number of protons affect force of attraction more?

More distance between the charges will result in less force, and more charge will have more force of attraction or repulsion. In the simplest case, every electron in an atom would feel the same amount of “pull” from the nucleus. For example, in Li, all three electrons might “feel” the +3 charge from the nucleus.

Does force of attraction increase with more electrons?

e.g. Li → Ne: The atoms have increased “pulling power” as the nuclear charge is increasing. Electrons are held tighter to the nucleus and there is a greater net electrostatic attraction. This allows another atom to be closer and it has a stronger attraction to electrons from that atom, so electronegativity increases.

How does greater distance affect the attraction of protons to electrons?

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).

Why are protons stronger than electrons?

Originally Answered: Why is a proton bigger than an electron if they have equal charge? Mainly, the proton has ca. 1800 times the mass of the electron. The mass is one property of a particle; the electric charge is another one – the two are really independent of one another.

What is the relationship between distance and attraction?

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.

Which electrons are most strongly attracted to the protons in the nucleus?

increases; moving from left to right across a period, protons are added to the nucleus, which increases its positive charge. For this reason, the negatively charged valence electrons are more strongly attracted to the nucleus, which increases the energy required to remove them.

What is the relationship between the number of protons and coulombic attraction?

The size of the charge also affects the coulombic attraction. When there is a high number of protons, the positive charge increases. The increase in positive charge improves the strength of the nucleus and is able to pull the electrons which are even further away.

Which atom has a stronger attractive force?

In an atom, the most important factors that influence the force, as calculated by Coulomb’s equation, are the nuclear charge and the distance from the nucleus to the electron of interest. The closer an electron is to a nucleus, the stronger the attractive force (i.e. the more negative F becomes).

What element has the strongest attractive force between protons and electrons?

Fluorine has the greatest attraction for electrons in any bond that it forms. The attraction of an atom for shared electrons is called its electronegativity.

What is the relationship between attractive force between the electrons and protons and the energy required to remove an electron?

Ionization energy is correlated with the strength of attraction between the positively-charged nucleus and the negatively-charged valence electrons. The higher the ionization energy, the stronger the attractive force between nucleus and valence electrons, and the more energy is required to remove a valence electron.

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How does force of attraction increase?

The force of this attraction is proportional to the size of charge and inversely proportional to the distance between the charges. As we go down a group the distance between the nucleus and valence electrons increases, while the charges involved stay the same.