What is the nuclear charge of an atom with a mass of 23 and an atomic number of 11?

What is the nuclear charge of an atom with a mass of 23 and an atomic number of 11?

What is the nuclear charge of an atom with a mass of 23 and an atomic number of 11? How do you figure this out? Would the answer be (1) 11+ since the atomic number is 11 and atomic #=protons which are positive?? Each of the 11 protons in the nucleus has a charge of (+1).

What is always equal in an atom?

Atoms do not always contain the same number of electrons and protons, although this state is common. When an atom has an equal number of electrons and protons, it has an equal number of negative electric charges (the electrons) and positive electric charges (the protons).

What atom has the greatest nuclear charge?

The charge Z of the nucleus of a fluorine atom is 9, but the valence electrons are screened appreciably by the core electrons (four electrons from the 1s and 2s orbitals) and partially by the 7 electrons in the 2p orbitals. So the sodium cation has the greatest effective nuclear charge.

Where can I find Zeff of Na?

For determining effective nuclear charge on sodium(Na), we apply Slater’s rules for calculating sigma and Zeff. These rules are given below: a) Each of the remaining electrons in the nth shell makes a contribution of 0.35 to the value of sigma. b) Each of the electrons in(n – 1) th shell makes a contribution of 0.85.

How do you calculate nuclear charge?

The equation for calculating nuclear charge is Zeff = Z – S, where Zeff is the effective nuclear charge, Z is the number of protons, and S is the number of inner electrons.

What is meant by nuclear charge?

The nuclear charge is the total charge in the nucleus for all the protons. The nuclear charge is the total charge in the nucleus for all the protons. It has the same value as the number of atoms. Going through the periodic table, the nuclear charge increases.

Does Z effective increase down a group?

The effective nuclear charge, Zeff, increases down a group which draws electrons closer towards the nucleus, decreasing atomic radius.

Why does z effective decrease down a group?

Effective Nuclear Charge should decrease down the group due to shielding from shells beneath.