In the periodic table, periods refer to the horizontal rows. Each period corresponds to the number of electron shells an atom of an element in that period has.
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This refers to the size of an atom. As you move across a period from left to right, atomic radius generally decreases due to increased nuclear charge pulling electrons closer.
This is the energy required to remove an electron from a gaseous atom or ion. It generally increases across a period because increasing nuclear charge makes it harder for electrons to escape.
This measures how strongly atoms attract bonding electrons. It also generally increases across a period because atoms with more protons can attract electrons more strongly.