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Will electron lattice electron interaction lower the energy of electrons?
latice energy decreases as you move down a group. This is mostly due to the fact that, as you move down a group in the periodic table the atomic radius increases. It follows that since the square of the distance is inversely proportional to force of the attraction between charges (Coulomb's Law), latice energy will decrease as atomic radius increases.
Which compound should have the largest lattice energy?
The compound that should have the largest lattice energy is the one with the highest charge and smallest ionic radius.
What periodic trends are inversely proportional to effective nuclear charge?
Atomic radius and ionization energy are inversely proportional to effective nuclear charge. As the effective nuclear charge increases, the attraction between the nucleus and the electrons increases, causing the atomic radius to decrease. In contrast, the ionization energy increases because it becomes harder to remove an electron from the atom due to the stronger attraction.
What is the correlation of ionization energies to atomic radii for the elements?
There is an inverse relationship between ionization energy and atomic radius: as atomic radius increases, ionization energy decreases. This is because as the distance between the nucleus and valence electrons increases, the attraction between them weakens, making it easier to remove an electron.
Why does the melting point of group 2 oxides decrease down the group?
Group Two elements form oxide consisting of ionic bonds. With that in mind, as you go down group two, the ionic radius increases due to an addtion of a electron shell, so therefore, melting point of group2 oxide decreases down group because the distance between the O2- and Group two ion are further apart. The increase of bond length results in less energy needed to break the ionic bonds, resulting in decrease of energy.
How does lattice energy change with a change in the size of an ion?
Because the electrostatic force of attraction between opposite charges increases as the distance between the charges decreases, smaller ions produce stronger inter ionic attractions and greater lattice energies. When attraction between ions increases and the charge of the ion increases , the lattice energy increases. Down the groups in periods the lattice energy decreases
What are factors affecting lattice energy?
Ionic Charge and Ionic Radius - the smaller the radius the greater the lattice energy
What factors affect lattice energy?
Ionic Charge and Ionic Radius - the smaller the radius the greater the lattice energy
What are the factors affecting lattice energy?
ionic charge and ionic radius; the smaller the ionic radius the greater the lattice energy
Will electron lattice electron interaction lower the energy of electrons?
latice energy decreases as you move down a group. This is mostly due to the fact that, as you move down a group in the periodic table the atomic radius increases. It follows that since the square of the distance is inversely proportional to force of the attraction between charges (Coulomb's Law), latice energy will decrease as atomic radius increases.
Which compound should have the largest lattice energy?
The compound that should have the largest lattice energy is the one with the highest charge and smallest ionic radius.
Lattice energy is effected by all the following factors except what charge of ion size of ion or number of electrons shared in the chemical bond?
Number of electrons shared in the chemical bond. Lattice energy is affected by the charge of the ions and the size of the ions, as these factors determine the strength of the electrostatic interactions within the lattice structure. The number of electrons shared in the chemical bond is not directly related to lattice energy, as lattice energy is primarily influenced by the arrangement of ions in the crystal lattice.
How does the atomic radius change from top to bottom in a group 1 and 2 in the periodic table?
Going down and to the left on the periodic table, atomic radius increases. Therefore, the smallest atomic radius is that of Helium (He), and the largest is that of Francium (Fr). Coincidentally, these are also the most and least reactive elements.
What happens to the energy of the electrons in the orbits as the radius of each orbit increases?
What happens to the energy of the electrons in the orbits of each orbit increases
How does atomic radius vary in group and in period on periodic table?
Down a period the atomic radius increases as the number of shells (or energy levels) increases. Across a period the atomic radius decreases as the effective nuclear charge increases.
What happens to atomic radius as you move from bottom to top of the periodic table?
atomic radius decreases from bottom to top of the periodic table.
What happendS to atomic radius as u go down the periodic taBLE?
the atomic radius increases down the periodic table as the number of shell (or energy level) increases.
