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It decreases as you move from left to right because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
Across the period, the total number of shells remain the same. But, atomic number, i.e., no. of protons and electrons goes on increasing. Protons (positively charged) present in the nucleus exert a nuclear charge towards the electrons (negatively charged) present around the nucleus, and pull the shells toward the nucleus. Hence, when no. of protons increases, nuclear charge also increases and hence it pulls the shells with greater force, and shells get closer to the nucleus. Hence, across the period, atomic size, or the radii go on decreasing.
moving from left to right across a period, one electron is added for each element.example: Boron has 3, Carbon has 4.
For the representative elements (main group elements), atomic radius generally decreases from left to right across a period. Example: B and Fl: Fl has the smaller atomic radius Li and Be: Be has the smaller atomic radius
its called a period.
Atomic number increases from left to right across a period.
It decreases as you move from left to right because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
I hate Chemistry!!!!!!!!!!!!!!!!!The number of protons increases as you go across a period.
The atomic number increases from left to right across a period (row). This is because the atomic number is the number of protons in the nuclei of the atoms of each element. No two elements have the same atomic number. It is the protons that define an element.
The size of an atom refers to its atomic radius. Atomic radius generally increases down a group. This is because the number of energy levels increase down a group with each additional period. Each of the subsequent energy levels are larger than the last, increasing the distance of the electrons from the nucleus, which increases the atomic radius.Atomic radius generally decreases across a period. This is because electrons are being added to the same energy level at the same time that protons are being added to the nucleus. This creates a stronger force of attraction by the nucleus for the electrons, which pulls the electrons closer to the nucleus, decreasing the atomic radius.It is important to note that the periodic trends are not laws. There are exceptions to the general trends in both the representative elements and the transitional elements.
Across the period, the total number of shells remain the same. But, atomic number, i.e., no. of protons and electrons goes on increasing. Protons (positively charged) present in the nucleus exert a nuclear charge towards the electrons (negatively charged) present around the nucleus, and pull the shells toward the nucleus. Hence, when no. of protons increases, nuclear charge also increases and hence it pulls the shells with greater force, and shells get closer to the nucleus. Hence, across the period, atomic size, or the radii go on decreasing.
the atomic radius decreses from left to right in periodic table due to increase in the number of succesive element the electrons of the outermost shell are more attracted towards nucleus and the atomic radius or atomic size decreases.
moving from left to right across a period, one electron is added for each element.example: Boron has 3, Carbon has 4.
A period is a horizontal row in the Periodic Table. So far, there are 7 of them. Each period shows patterns as you go across it(left to right). On of the must-know patterns is that the number of period indicates how many orbitals (or energy levels) the elements in that period have. Other patterns include atomic radius and ionic radius.
For the representative elements (main group elements), atomic radius generally decreases from left to right across a period. Example: B and Fl: Fl has the smaller atomic radius Li and Be: Be has the smaller atomic radius
it increases
its called a period.