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Why nuclear charge increases when atomic number increases across a period?
Wiki User
∙ 11y ago
Atomic number is the number of protons in the nucleus. The higher the number the higher the nuclear charge
Wiki User
∙ 11y ago
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When moving left to right across the periodic table the atomic number increases and the atomic radius?
The atomic radius decreases from left to right and increases from top to bottom
What trend in ionization energy occurs going across a period on the periodic table and why?
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
Why does the atomic radius decrease with an increase in atomic numbers within a period?
As the atomic number increases, the number of protons in the nucleus increases or the effective nuclear charge of the nucleus increases. As a result the force exerted by the nucleus on the valence electrons is more or the size of the atom is small.
Why does atomic size increase as you go from left to right across a period?
atomic size decreases as we go from left to right. as we go from left to right, the number of protons in the nucleus increases, so the effective nuclear charge increases. due to this the electrons are attracted more towards the nucleus and hence, the size decreases.
As the number of neutrons in the nucleus of an atom increases the nuclear charge of the atom does what?
Nothing happens to the nuclear charge of the atom as the the number of neutrons increases since neutrons do not carry a charge. Plus the nuclear charge also known as the effective nuclear charge is calculated by subtracting the average number of electrons between the nucleus and the electron in question (the number of nonvalence electrons) from the number of protons in the nucleus of the atom, so as you can see the neutrons have no effect on the nuclear charge.
What is the trend in atomic size across the period from sodium to argon?
across a period, the atomic size decreases as the effective nuclear charge increases.
Nuclear charge increases across a period atoms become?
The atoms become smaller in atomic radius.
Does nuclear charge increases as you move from left to right across the periodic table?
moving from left to right across a period, one electron is added for each element.example: Boron has 3, Carbon has 4.
How does size change in a period and in a group?
Atomic size decreases across a period as the effective nuclear charge increases. Atomic size increases down a group as the energy level (shells) increases.
How does atomic radius vary in group and in period on periodic table?
Down a period the atomic radius increases as the number of shells (or energy levels) increases. Across a period the atomic radius decreases as the effective nuclear charge increases.
What to atomic properties have an increasing trend as you move across the periodic table?
As we move across a period, electronegativity increases. Ionization enthalpy also increases because of increasing nuclear charge.
How do atomic radii change from left to right across a horizontal row of the periodic table and what is the main reason?
Atomic radii decreases on moving from left to right as the effective nuclear charge increases.
What happens when the nuclear charge increases across a period?
The atomic size decreases (with some exceptions) , the ionization energy , electronegativity and electron affinity also increase from left to right.
What happens to first ionization energy within groups and across periods?
it increases. the nuclear charge also increases
What happens to first ionization energy within groups across periods?
it increases. the nuclear charge also increases
When moving left to right across the periodic table the atomic number increases and the atomic radius?
The atomic radius decreases from left to right and increases from top to bottom
In general - what happens to the atomic radius from left to right across a period?
Generally, it decreases.*As you move from left to right across a period the elements' number of protons increases, increasing the effective nuclear charge (the charge felt by the outermost [valence] electrons after taking into account the shielding electrons). As effective nuclear charge increases the attraction between the nucleus and the valence electrons increases, pulling the valence electrons closer to the nucleus, decreasing the atomic radius.*Please understand that this is not a hard and fast rule. There are other factors to take into account when determining atomic radius, this is just a general trend witnessed.
