How do properties of elements change within period?

Answer 1

As you move from left to right across a row (or period) in the Periodic Table, the following things change: -- atomic size goes down -- electronegativity goes up -- electron affinity goes up See the Web Links and Related Questions links to the left of this answer for more details about why the trends occur and also some important exceptions to these trends.

Answer 2

As atomic number increases, the number of electrons also increases except for Period 1 because it ends with a number of valence electrons with higher energy , (This pattern means that the elements within a group always have the same number of valence electrons having the result of having similar properties.)

Answer 3

They change because the atomic number and mass differ from each other element.

Going across the periodic table to the right, the atoms get smaller because another proton is added each time so the effective nuclear charge experienced by the electrons is greater and the electrons are pulled closer to the nucleus. Electronegativity increases as you progress across a period because smaller atoms are usually more likely to gain an electron. Ionization energy increases across a period because the atoms are smaller, pulled closer to the nucleus, so it takes more energy to break an electron away.

Answer 4

Yes, the properties of the elements within a period vary from element to element.

For example, the metallic character decreases and the non-metallic character increases from left to right within a period.

Answer 5

The properties remain almost the same except the radius of the atom increases as there is an extra energy level.

Answer 6

Because the "properties" [that we're interested in, mostly chemical] are a function of the outer-most electrons of an atom.

Answer 7

As we move across the period the atomic siza decreases and Ionization energy, electron affinity and electronegativity increases.