How do you find the electron configurations of ions?

Answer 1

There are many types of rules for electron configuration. Look at the aufbau principle and Hund's rules.

• In each orbital there is a maximum of two electrons.
• In a "s" orbital, there are two electrons.
• In a "p" orbital, there are three sub-orbitals, each containing two electrons. (Thus containing 6 electrons)
• In a "d" orbital, there are five sub-orbitals, each containing two electrons. (Thus containing 10 electrons)
• In a "f" orbital, there are seven sub-orbitals, each containing two electrons. (Thus containing 14 electrons)

Look at the aufbau diagram I linked below.

The coefficient represents the orbital. Do not use mathematics to try to solve the configurations.

1s2 2s2 2p6 : Neon's Electron Configuration

The letter following the coefficient describes which type of orbital it is, being s,p,d, or f.

The superscript denotes the number of electrons it contains. If you add 2, 2, and 6, you would get 10, Neon's atomic number.

Answer 2

In order to find the electron configuration, you first write out what the electron configuration would look like for the element without the charge. Then all you need to do is subtract or add electrons to your configuration. If the charge is a negative, like Cl-, you will add the number as electrons. For instance, if the charge is -3, you will add three more electrons to your electron configuration. With the positive charges, it is the opposite; instead of adding electrons you simply remove however many the charge suggests. Like, if you had a charge of +2, you would remove two electrons from the configuration. And so on.

Answer 3

There are many types of rules for electron configuration. Look at the aufbau principle and Hund's rules.

• In each orbital there is a maximum of two electrons.
• In a "s" orbital, there are two electrons.
• In a "p" orbital, there are three sub-orbitals, each containing two electrons. (Thus containing 6 electrons)
• In a "d" orbital, there are five sub-orbitals, each containing two electrons. (Thus containing 10 electrons)
• In a "f" orbital, there are seven sub-orbitals, each containing two electrons. (Thus containing 14 electrons)

Look at the aufbau diagram.

The coefficient represents the orbital. Do not use mathematics to try to solve the configurations.

1s2 2s2 2p6 : Neon's Electron Configuration

The letter following the coefficient describes which type of orbital it is, being s,p,d, or f.

The superscript denotes the number of electrons it contains. If you add 2, 2, and 6, you would get 10, Neon's atomic number.

Answer 4

the number of electrons belonging to an element is the atomic number. The electron configuration is the way they are arranged around the nucleus. For example the inner shell can only hold 2 electrons and from then on, each additional shell can hold 8 electrons. Oxygen has 8 electrons so the electron arrangement would be 2.6 (2 on the inner shell, 6 on the outer shell. Potassium has 19 electrons so the electron arrangement would be 2.8.8.1 (2 on the inner shell, 8 on the next, 8 on the next, 1 on the outer shell) Hope this is helpful!

Answer 5

It depends on the element and its ionic state. If the element's ionic state is +1, +2, +3, etc., remove 1, 2, 3, etc. electrons from the element's normal electron configuration. If the element's ionic state is -1, -2, -3, etc., add 1, 2, 3, etc. electrons from the element's normal electron configuration.

Answer 6

The charge of the ion will tell you how many electrons were gained or lost from the original, neutral atom. The atomic number tells you how many electrons there were originally. And we also know how many electrons fit in each shell. With this information you can work out the electron configuration of an ion.

Answer 7

do u have the table for it?

the one have the

1S

2S 2P

3S 3P 3D

4S 4P 4D 4F

5S 5P 5D 5F

6S 6P 6D 6F

7S 7P 7D 7F

Answer 8

A monatomic ion with a charge of -2 has an electronic configuration of 1s22s22p63s23p6

Answer 9

Ions exist in water solutions of ionic compouds. Cations are positive ions and anions are negative ions.