Consider the data in Model 1, describe the relationship between force of attraction and the distance between the subatomic particles. The closer the two subatomic particles are, the stronger the force of attraction is. And vice versa.
What is the relationship between the distance between the particles and the force of attraction?
Inverse relationships are common in nature. In electrostatics, the electrical force between two charged objects is inversely related to the distance of separation between the two objects. Increasing the separation distance between objects decreases the force of attraction or repulsion between the objects.
What is the relationship between distance and attractive forces in an atom?
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 attractive forces and distance from the nucleus?
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).
How does the distance between the atoms affect this attraction?
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 is the relationship between force and distance in an inverse square law?
The inverse square law tells us that the force on an object due to another is inversely proportional to the square of the distance between them.
Why force is inversely proportional to square of distance?
This is because the force acts uniformly in all directions from the point source and conserves the energy over the entire surface surrounding the point object. Therefore, the force reduces as the square of the distance. …
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.
What is force attraction?
a force between two bodies, molecules, particles, or the like, that attracts each to the other. … Gravity is the force of attraction between two bodies that have mass.
What force explains the attraction between a proton and an electron?
The electromagnetic force, also called the Lorentz force, acts between charged particles, like negatively charged electrons and positively charged protons. Opposite charges attract one another, while like charges repel. The greater the charge, the greater the force.
When comparing the attractive force between the outer electrons and the nucleus of elements in the same group what is the dominant factor?
The distance seems to be the dominant factor; otherwise we would see an increase in the attractive force as you move from smaller to larger atoms down a column in the periodic table. 19.
Is attractive force positive or negative?
In general when the force is attractive, the potential energy is negative and as shown above force will be negative. In case of repulsion, with the same argument, the force will be positive.
Between which electron and the nucleus is the force of attraction the weakest?
the outer electron gets further from the nucleus as you go down the group. the attraction between the nucleus and outer electron gets weaker as you go down the group – so the electron is more easily lost.
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.
How does coulombic attraction affect atomic radius?
an inverse correlation. According to Coulomb’s Law, as the atomic number increases within a series of atoms, the nuclear attraction for electrons will also increase, thus pulling the electron(s) closer to the nucleus. … Such a relationship between atomic number and atomic radius is a direct correlation.
What is the connection between shielding and effective nuclear charge?
The shielding effect explains why valence-shell electrons are more easily removed from the atom. The effect also explains atomic size. The more shielding, the further the valence shell can spread out and the bigger atoms will be. The effective nuclear charge is the net positive charge experienced by valence electrons.