Explain the trends in physical properties(point wise)
A.atomic radius (point wise)
B.Ionic radius (point wise)
C.Ionization Enthalpy (point wise)
D.Electron Gain Enthalpy (point wise)
E.Electronegative (point wise)
Explain the trends in physical properties(point wise)
A.atomic radius (point wise)
B.Ionic radius (point wise)
C.Ionization Enthalpy (point wise)
D.Electron Gain Enthalpy (point wise)
E.Electronegative (point wise)
1.Atomic size gradually decreases from left to right across a period of elements. This is because, within a period or family of elements, all electrons are added to the same shell.
2) Ionic radius increases from left to right.An ionic radius is defined as the radiusof an atom's ion (ex. the radius of Na+). Ionic radii decrease across periods because effective nuclear charge increases. That is, the net positive charge experienced by an electron in the atom increases as a result of the number of protons in the nucleus increasing.
3)As one progresses down a group or across the period on the periodic table, the ionization energy will likely decrease since the valence electrons are farther away from the nucleus and experience greater shielding. They experience a weaker attraction to the positive charge of the nucleus
4) As you move across a period, the size of the atom gets smaller, however, the nuclear charge of the nucleus increases (due to addition of protons as we move across a period). Hence, the nucleus easily attracts the outer electron (the one we are trying to GAIN). Thus as you move across a period, the Electron Gain Enthalpy becomes more and more negative (you can interpret it as - It requires less and less energy).
It’s vice versa when you move down the group as in that case the Atomic Size increases by a significant amount and there is larger screening effect.
5)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.
2) Ionic radius increases from left to right.An ionic radius is defined as the radiusof an atom's ion (ex. the radius of Na+). Ionic radii decrease across periods because effective nuclear charge increases. That is, the net positive charge experienced by an electron in the atom increases as a result of the number of protons in the nucleus increasing.
3)As one progresses down a group or across the period on the periodic table, the ionization energy will likely decrease since the valence electrons are farther away from the nucleus and experience greater shielding. They experience a weaker attraction to the positive charge of the nucleus
4)
As you move across a period, the size of the atom gets smaller, however, the nuclear charge of the nucleus increases (due to addition of protons as we move across a period). Hence, the nucleus easily attracts the outer electron (the one we are trying to GAIN). Thus as you move across a period, the Electron Gain Enthalpy becomes more and more negative (you can interpret it as - It requires less and less energy).
It’s vice versa when you move down the group as in that case the Atomic Size increases by a significant amount and there is larger screening effect.
5)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.
