As you move from left to right across the Periodic Table, the number of protons in the nucleus of each successive atom increases by one. Correspondingly, the number of electrons also increases by one. However, if the elements in question are on the same energy level, the added ''pull" of the protons serves to pull the orbiting electrons closer to the nucleus, thus causing the radius of the atom to become smalller as you move from left to right. As you move down the Periodic Table, atoms get larger. As you move down the table, you continue to add protons and electrons. However, you also add energy levels and, in so doing, the orbiting (and available) electrons get further from the nucleus and the pull of the protons. It is the distance between protons and available electrons that allows the radius of the atoms to get larger. It also explains why reactivity increases as you go down the table. The pull of protons on the available electrons of small atoms is much greater than the pull of protons on the available electrons of large atoms, so the large atoms release their electrons much more readily.
because the atom has one more proton and electron than the one before it.
Electronegativity increases across (left to right) the periodic table and decreases on going down.
Going down a group...electronegativity decreases Going across...electronegativity increases
False,reactivity of elements generally decreases from left to right.As free electrons become less,reactivity decreases.So the given statement is false.
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
Atomic size generally increases as you go down a group
Electronegativity increases across (left to right) the periodic table and decreases on going down.
Atomic size decreases across a period
the number of available electron spaces in the outer electron shell.
Atomic size decreases across the rows of the periodic table
Atomic radius usually decreases from left to right across a period of the periodic table.
it decreases
Across a period the metallic character decreases
Electropositivity decreases along a period. The metallic character also decreases.
A good example of periodicity would be the size of an atom which decreases across the Periodic Table but increases down the column
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
it increases then decreases
Going down a group...electronegativity decreases Going across...electronegativity increases