Valence Electrons and Ionic Compounds

This video tutorial explains how to write the Lewis structure for strontium fluoride (SrF2). It begins by identifying the element symbols for strontium and fluorine, noting that Sr is a metal and F is a non-metal, forming an ionic compound. The video details the valence electrons of each element, with strontium having two and fluorine seven. It describes the electron transfer process where strontium loses electrons to fluorine, resulting in stable octets for fluorine and a positive charge for strontium. The tutorial concludes by emphasizing the utility of Lewis structures in understanding ionic bonds.

What are the element symbols for strontium and fluorine in the Lewis structure of SrF2?

• Sr and F

• S and F

• St and Fl

• Sr and Fl

What type of compound is SrF2?

• Ionic

• Covalent

• Molecular

• Metallic

How many valence electrons does strontium have?

• 8

• 7

• 2

• 1

How many valence electrons does each fluorine atom have?

• 7

• 8

• 5

• 6

What happens to strontium's electrons in the formation of SrF2?

• They remain with strontium

• They are lost to the environment

• They are transferred to fluorine

• They are shared with fluorine

What charge does strontium have after losing electrons?

• 2-

• 1-

• 2+

• 1+

What charge does each fluorine ion have after gaining an electron?

• 2-

• 1-

• 2+

• 1+

Why are brackets used in the Lewis structure of SrF2?

• To highlight the metal

• To separate the elements

• To show the ionic charges

• To indicate shared electrons

What is the significance of the Lewis structure for SrF2?

• It determines the melting point

• It explains the ionic bond formation

• It shows the molecular shape

• It predicts the color of the compound

What does the crystal structure of SrF2 consist of?

• Individual molecules

• Repeating formula units

• Randomly arranged atoms

• Covalent networks