Exploring Ionic Bonds: Key Concepts and Definitions

This video tutorial explores ionic bonds, explaining how atoms achieve stability by forming these bonds. It uses examples of sodium and chlorine, and beryllium and fluorine, to illustrate electron transfer and the formation of ionic bonds. The video concludes with a summary and encourages viewers to subscribe for more content.

What is the primary goal of atoms in terms of their electron configuration?

• To have an equal number of protons and neutrons

• To have a complete outer shell of electrons

• To have an odd number of electrons

• To have more protons than electrons

Which group of elements naturally has a full outer shell of electrons?

• Transition metals

• Noble gases

• Halogens

• Alkali metals

How many electrons does a sodium atom have in its outermost shell?

• One

• Two

• Eight

• Seven

How many electrons are in the outermost shell of a chlorine atom?

• Two

• One

• Eight

• Seven

Why is it easier for sodium to donate one electron rather than gain seven?

• Because it has more protons

• Because it is a non-metal

• Because it is a metal

• Because it has only one electron in its outer shell

What happens to the charge of sodium when it donates an electron?

• It becomes more positive

• It becomes more negative

• It becomes a noble gas

• It remains neutral

What type of bond is formed due to the electrostatic attraction between oppositely charged ions?

• Covalent bond

• Hydrogen bond

• Ionic bond

• Metallic bond

Which type of bond is stronger than both covalent bonds and dispersion forces?

• Van der Waals forces

• Hydrogen bond

• Ionic bond

• Metallic bond

How many fluorine atoms are needed to bond with one beryllium atom?

• Four

• Two

• One

• Three

Tags

NGSS.MS-PS1-1

What is the chemical formula for beryllium fluoride?

• Be2F3

• BeF2

• Be2F

• BeF

Tags

NGSS.MS-PS1-1