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Why does atomic size increase from left to right across a period?
atomic size decreases across a period
How does Atomic Radius behave along the Periodic Table?
Atomic radius increases down a group due to increase in number of shells. Its value decreases along a period due to increase in nuclear charge.
What does atomic radius do across a period?
Atomic radius tends to decrease across a period from left to right. This is because as you move across a period, the number of protons in the nucleus increases, leading to an increase in the effective nuclear charge felt by the outermost electrons, which pulls them closer to the nucleus.
Moving across a period on the periodic table from left to right?
Moving across a period from left to right, the atomic number of the elements increases. This results in an increase in the number of protons and electrons, leading to a greater nuclear charge. As a result, the size of the atoms decreases while the electronegativity and ionization energy increase.
Why electron affinity value decreases from top to bottom?
It decreases as you go down a group because the atomic radius increases, and the energy shells increase, so the attraction is less. also, the number of electrons going down a period also increase, so there is more repulsion, and its harder to add electrons.
An increase in the atomic number the atomic radius moving from left to right across a period.?
decreases
Why does atomic size increase from left to right across a period?
atomic size decreases across a period
Does atomic radius increase in a period?
decreases because of increased nuclear charge
How does Atomic Radius behave along the Periodic Table?
Atomic radius increases down a group due to increase in number of shells. Its value decreases along a period due to increase in nuclear charge.
Why do the atomic size decreases in periods rather than to be increased due to proton repulsion that leads to nucleus to expansion?
As we move across the period, there is an increase in the atomic number i.e., there is an increase in the number of protons inside the nucleus. This means, there is more nuclear force. This nuclear force pulls the electron orbits as close as it can. thus, the radius of the atom decreases. Hence the atomic size decreases.
Why do atom size decreases in periods instead of increasing due to protonic repulsion?
As we move across the period, there is an increase in the atomic number i.e., there is an increase in the number of protons inside the nucleus. This means, there is more nuclear force. This nuclear force pulls the electron orbits as close as it can. thus, the radius of the atom decreases. Hence the atomic size decreases.
What is the trend found in Period 3 on the Periodic Table as the elements increase in atomic number?
1-Atomic size = decreases 2-Ioniztion energy = increases 3-Electronegativity = increases (except Argon) 4-Metallic character = decreases 5-Melting point = first increases then decreases
What accompanies an increase in atomic number within a specific period?
An increase in atomic number within a specific period corresponds to an increase in the number of protons in the nucleus of the atom. This leads to a higher positive charge, causing the outer electrons to be more strongly attracted to the nucleus. As a result, the atomic size tends to decrease across a period as atomic number increases.
How are the size of the elements effected on the periodic table?
Atomic size increase down the group and decreases across the period.
What does atomic radius do across a period?
Atomic radius tends to decrease across a period from left to right. This is because as you move across a period, the number of protons in the nucleus increases, leading to an increase in the effective nuclear charge felt by the outermost electrons, which pulls them closer to the nucleus.
Atomic size generally as you go down a group?
Atomic size generally increases as you go down a group
What is the relationship of ionic radius and atomic number?
As you move across a period from left to right, the atomic number increases and the ionic radius decreases. This is because the increase in positive charge in the nucleus attracts the electrons more strongly, pulling them closer to the nucleus, leading to a decrease in ionic radius.
