Since the force of attraction increases across a period the trends noticed down a group are reversed.
What happens to attraction as you go down a group or family?
The trend in atomic radius as you go down a group and why this occurs. Increases as you go down a group because higher energy levels have larger orbitals so the size of atom increases. 10. The most reactive nonmetal.
What happens to force of attraction across a period?
Across the period the Atomic radii decreases
The electron repulsion is balanced by the nuclear charge attractions, and as the nuclear charge gets larger, so the electrons get closer together. The net attractive electrostatic attraction is increased as the nuclear charge increases.
What happens going down a group?
Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius. Ionic radius is the distance from the nucleus to the outer edge of the electron cloud of an ion.
Why does coulombic attraction decrease down a group?
The bigger the size of the atom, the electrons, especially the valence electrons are further away from the nucleus. The nucleus is not able to pull the electrons, that are in orbitals further away from the nucleus, towards itself and the coulombic attraction decreases.
Why do electronegativity decrease down a group?
Going down a group, the electronegativity of atoms decreases. As you move down a group in the periodic table, atoms increase in size, with a greater number of energy levels. The extra energy levels and increased covalent radius keep the bonding electrons further away from the nucleus.
What is the trend in fie as you go down a family?
As you go down a family on the periodic table, ionization energy decreases.
Why does the force of attraction between the nucleus and electrons decrease down a group?
As you go down a group, the nuclear charge decreases because the valence electrons move further away from the nucleus depleating the force of attraction between the nucleus and the electrons.
How and why does the force of attraction between the nucleus and the valence electrons change as you move across a period?
The net force of attraction between the nucleus and the valence electron in an atom increase as you move across a period from left to right. As you move across a period, the valence electrons in the atom experience a stronger pull toward the nucleus. DECREASES.
Why does electronegativity decrease down a group and increase across a period?
So, as you move down a group on the periodic table, the electronegativity of an element decreases because the increased number of energy levels puts the outer electrons very far away from the pull of the nucleus. Electronegativity increases as you move from left to right across a period on the periodic table.
What happens to atomic mass when going down a group?
The relative atomic mass is defined as the weighted average of the isotopic masses, while the mass number of each isotope is simply the number of protons plus the number of neutrons, giving each isotopic mass. … Since this occurs as you go down a group, the atomic mass increases as you go down a group.
Why do ionization energies decrease down a group?
Going down a group, the ionisation energy decreases. This is due to the shielding or screen effect of the outer electrons from the nucleus and so the attraction is weaker and they are more easily removed.
What happens when you go across the periodic table?
Elements in the same period have the same number of electron shells; moving across a period (so progressing from group to group), elements gain electrons and protons and become less metallic. This arrangement reflects the periodic recurrence of similar properties as the atomic number increases.
How does Coulombic attractive force affect ionization energy?
The greater the ionization energy, the more difficult it is to remove an electron. Using the same Coulombic attraction ideas, we can explain the first ionization energy trends on the periodic table. … The greater an atom’s electronegativity, the greater is its ability to attract electrons to itself.
How does coulombic attraction impact the atomic size?
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. The Coulombic attraction of the nucleus of an atom for its electrons is referred to as the electronegativity of the atom.
What variables will affect the force of attraction between charged particles?
Charles Coulomb determined how to figure out the strength of the force between charged particles. As we’ll discuss in this lesson, he found that the force between charged particles was dependent on only two factors: the distance between the particles and the amount of electric charge that they carried.