What is the relationship between distance and attractive force between protons and electrons?

What is the relationship between distance and attraction between protons and electrons?

Describe the mathematical relationship between the distance and the attractive force between protons and electrons? As distance increases, attraction decreases.

What is the relationship between distance and attractive forces when it comes to the protons in the nucleus and the electrons on the outside?

Describe the mathematical relationship between distance and the attractive force between protons and electrons. It is inversely proportional.

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.

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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.

When the distance between the nucleus and the electrons increases the attractive force between them?

As the principle energy level of the electron increases, the distance between the nucleus and electron increases. So, the attractive force decreases as the principal energy level increases.

What factors can change the attractive force between the nucleus of an atom and its 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 would decrease the attraction of an electron?

An increase in atomic size leads to a decrease in electron affinity because the incoming electron is added further away from the nucleus, i.e. on a higher energy level. … When you add more protons to the nucleus, it will attract electrons more.

Why is it important that the electrons and protons are attracted to each other?

Since opposite charges attract each other, the negatively charged electrons are attracted to the positively charged protons. Tell students that this attraction is what holds the atom together. … This attraction is what holds the atom together.

Does calcium or barium have a stronger attractive force?

Barium has more electrons shells than calcium, so the nuclear shielding is stronger, and the outmost electrons are further away from the nucleus. This results in a weaker attractive force between the electron and the nucleus, so a smaller energy is required to remove it.

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When protons and electrons are closer the force of attraction is stronger weaker?

Two protons (or two electrons) will repel each other. And again, the closer together they are, the stronger the repulsion. Now the nucleus of an atom is positively charged, while electrons are negatively charged. As a result, a nucleus will attract electrons.

What effect is caused by inner electrons interfering with the attraction of outer electrons?

electron shielding: As more electrons are added to a nucleus, the outer electrons become shielded from the nucleus by the inner shell electrons. inner core electrons: Electrons that prevent attraction between valence electrons and protons.

Why is distance the dominant factor?

DISTANCE is the dominant factor while comparing elements in the same COLUMN. Although there are more protons in certain elements, the larger distance effects in more. … NUMBER OF PROTONS is the dominant factor while comparing elements in the same ROW. Distance is not a factor while comparing elements in the same row.