Question

В ряду Na,Mg, Al у атомов металлов: 1)увеличивается раидиус 2) возраставют восстановительные свойства 3)увеличивается число валетных электронов 4)возрстает число электронных слоёв

Answer 1

Ответ 3,эти вещества стоят в одной группе,значит у них одинаковое кол-во слоёв.Восстановительные св-ва уменьшаются.

Answer 2

Trends in the properties of sodium (Na), magnesium (Mg), and aluminum (Al)

The question asks about trends in atomic properties of the metals sodium (Na), magnesium (Mg), and aluminum (Al) in the periodic table.

The atomic radius increases down the group from Na to Mg to Al. This is because the principal quantum number and hence the distance of the outermost electrons from the nucleus increases, as we move from left to right within a period of the periodic table.

The reducing properties increase from Na to Mg to Al. This is due to the decrease in the ionization energy of the outermost electrons as we move down the group. Sodium has the lowest ionization energy and is the strongest reducing agent among the three.

The number of valence electrons increases from Na (1) to Mg (2) to Al (3) as we go down the group. The group number is equal to the number of valence electrons in the outer shell.

The number of electron shells remains the same at 3 for all three elements as they all belong to the third period of the periodic table.