Atoms increase in size as you go down a column and are larger going from right to left across a row.
because while going from left to right in a period electrons enter in the same orbit and hence the attraction between the nucleus increasees
Going across a period, the ionic radius decreases for metals forming cations, as they lose their outer electron orbit. for non-metal atoms, the ionic radius increases as the effective nuclear charge is decreased due to having more electrons than protons.
As with all atomic radii, ionic radii increases going down a group.
For +ve ions of the same element, ionic radii decreases with increasing positive charge
For -ve ions of the same element, ionic radii increases with increasing negative charge
The ionic radius increases down the group.Because of increase in number of shell.
Ionic radius decreases across a period due to increase in nuclear charge.
Atomic radius decreases through a period. Atomic radius increases down a group. Helium has the least atomic radius.
Ionic size is the size of the atom after it loses its outermost electron (after the first Ionization Energy)
the trend is that it increases in size goeing right to left and as you go down.
the atomic size is increasing from left to right
The ionic radius increases down the group.Because of increase in number of shell.
Ionic radius decreases across a period due to increase in nuclear charge.
Atomic radius decreases through a period. Atomic radius increases down a group. Helium has the least atomic radius.
Bigger as you go down the chart; smaller as you go from left to right.
The ionic radius increase in a column going down.
The ionic radius depends on the electrical charge of the ion.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
Because the trend is the same. Atomic radius decreases from left to right across a period.
across a period, the atomic size decreases as the effective nuclear charge increases.
Magnesium isn't smaller than chlorine, it's larger. The atomic radius for magnesium is 145 pm and the atomic radius for chlorine is 79 pm. Both magnesium and chlorine are in the third period of the periodic table. The trend for atomic radius is that the elements generally get smaller as you move from left to right across the table in the same period.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
if you mean metals ..... for the same valence the radius decreases across a period and increases down a family
Atomic radius
It is a trend in itself, it isn't caused by a trend.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
what is the reason for ionization energy across a period
Because the trend is the same. Atomic radius decreases from left to right across a period.
Because the trend is the same. Atomic radius decreases from left to right across a period.
The atomic radius decreases along a period. It is because of increasing effective nuclear charge along a period.
Electronegativity increases across a period (left to right).
across a period, the atomic size decreases as the effective nuclear charge increases.
Magnesium isn't smaller than chlorine, it's larger. The atomic radius for magnesium is 145 pm and the atomic radius for chlorine is 79 pm. Both magnesium and chlorine are in the third period of the periodic table. The trend for atomic radius is that the elements generally get smaller as you move from left to right across the table in the same period.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.