3.1.3.1 Ionic Bonding Flashcards
What is a chemical bond?
The transfer or share of electrons between atoms to achieve a full outer shell (more stable structure)
Define ionic bonding
The transfer of electrons from a metallic element to a non-metallic elememt, to leave both elements involved with a full outer shell.
What ions do metals form?
Positive ions/ cations as they lose electrons
What ions do non-metals form?
Negative ions/ anions as they gain electrons
Why do ionic compounds have high melting and boiling points?
There are many strong electrostatic forces of attraction, which require lots of energy to overcome.
Describe how an ionic bond is formed
-the outer electron(s) from one atom are transferred to the outer shell of another atom, so that both atoms have a full outer shell.
-the atom that loses electrons forms a positive ion, and the atom that gains electrons forms a negative ion
-electrostatic forces between the oppositely charged ions holds them together in an ionic bond
What are the forces that hold an ionic bond together?
Electrostatic forces of attraction (act in all directions)
Describe the structure of an ionic bond
-arranged in a regular and repeating arrangement called a giant ionic lattice
-it is held together by strong electrostatic forces of attraction
(Ionic bonds)
-These forces act equally and in all directions
Give 2 limitations of the ball and stick model
-the ions are far apart but they are much closer in real life
-it also doesn’t show the forces acting in all directions
Why do ionic compounds have high melting points and boiling points, and are hard?
There are many strong electrostatic forces of attraction between oppositely charged ions that require lots of energy to overcome.
Why are ionic compounds brittle?
The bonds are directional, but if a force is applied, then layers shift. Ions (same charges) line up and repel each other, so bonds between layers break, meaning little energy is required to break bonds.
