Isoelectronic Ions and Their Charges

The video tutorial explains isoelectronic systems, which are different nuclei surrounded by the same number of electrons. It uses the periodic table to identify elements with 10 electrons, starting with neon. The tutorial then explores how other elements like fluorine, oxygen, and nitrogen can form isoelectronic systems by gaining or losing electrons to match neon's electron count. It also covers cations such as sodium and magnesium, which become isoelectronic with neon by losing electrons.

What does the term 'isoelectronic' refer to?

• Same number of electrons

• Same number of neutrons

• Same atomic mass

• Same number of protons

Which element is isoelectronic with neutral neon?

• All of the above

• Nitrogen ion (N3-)

• Oxygen ion (O2-)

• Fluorine ion (F-)

How many electrons does a fluoride ion (F-) have?

• 9

• 10

• 11

• 12

What charge does an oxygen ion need to have to be isoelectronic with neon?

• -3

• 0

• -2

• -1

How many extra electrons does a nitride ion (N3-) have compared to neutral nitrogen?

• 4

• 1

• 2

• 3

What is the charge of a sodium ion that is isoelectronic with neon?

• -1

• +2

• +1

• 0

How many electrons does a magnesium ion (Mg2+) have?

• 14

• 12

• 10

• 8

Which of the following is not isoelectronic with neon?

• N3-

• Na+

• O2-

• F-

What is the total charge of a system with 10 electrons and a fluorine nucleus?

• 0

• -1

• +1

• -2

Which of the following ions has the same number of electrons as a neutral neon atom?

• K+

• Mg2+

• Ca2+

• Cl-