Understanding Electronic Configurations of Atoms and Ions

The video tutorial explains the relationship between an element's position in the periodic table and its electronic structure. It covers the basics of atoms and ions, focusing on electron configuration and how electrons fill shells from the innermost to the outermost. The tutorial discusses the stability of full outer shells, the formation of ions, and how metals and non-metals differ in their approach to achieving noble gas configurations. Key examples include sodium, neon, chlorine, lithium, beryllium, and aluminum.

What determines the number of electrons in a neutral atom?

• The atomic mass

• The atomic number

• The number of neutrons

• The number of electron shells

How is the electron configuration of neon represented?

• 1.8.1

• 2.8

• 2.8.1

• 2.7

What happens to the electron configuration as you move down a group in the periodic table?

• A new electron shell is added

• The number of occupied shells decreases

• The atomic number decreases

• The number of outer electrons increases

Why are noble gases considered stable?

• They can easily gain electrons

• They have the most protons

• They have a full outer shell of electrons

• They have the highest atomic numbers

How do non-metal atoms achieve a full outer shell?

• By increasing atomic mass

• By sharing protons

• By gaining electrons

• By losing electrons

What type of ion does aluminum form to achieve stability?

• Neutral atom by sharing electrons

• Positive ion by losing electrons

• Negative ion by losing protons

• Negative ion by gaining electrons

Which group of elements tends to lose electrons to form positive ions?

• Transition metals

• Noble gases

• Groups 1, 2, and 3

• Groups 5, 6, and 7