Ionic
Define Ionic Bonding
A bond between a metal and a nonmetal formed from the electrostatic attraction between oppositely charged ions in a chemical compound. This bond forms when the valence electrons of one atom are transferred permanently to another atom
Define Covalent Bonding
A chemical bond that involves the sharing of electrons to form electron pairs between nonmetal atoms
Define Metallic Bonding
A bond between metal atoms that involves the sharing of free electrons among a structure of positively charged ions. A "sea of electrons"
Name this compound: NaCl
Sodium Chloride
Which of the following is NOT an ionic compound?
NaCl BrCl AlO
BrCl
Which of the following is a covalent compound:
LiP CoCl SiBr
SiBr
Which of the following is NOT a Metallic compound:
CuZn IrPd AgGe
AgGe
What do the prefixes tri, penta, and octa mean?
3, 5, 8
Is Magnesium Oxide an example of an ionic bond? Why?
Yes, because Magnesium is a metal and Oxygen is a nonmetal
Is Aluminum Chloride an example of a covalent bond? Why?
No, Aluminum is a metal
Is Lithium Fluoride an example of a Metallic bond? Why?
No, Fluorine is not a metal
What do the prefixes tetra, hepta, and nona mean?
4, 7, 9
Compare and contrast the properties of ionic compounds with those of covalent compounds.
Ionic compounds often have high melting points, are usually soluble in water, and conduct electricity when they are dissolved or melted.
Covalent compounds have lower melting points, don't often dissolve in water, and almost never conduct electricity.
Compare and contrast the properties of covalent and metallic compounds
Covalent compounds are usually poor conductors and are brittle, while metallic compounds are conductive and malleable/ductile
Compare and contrast the properties of metallic bonds and those of ionic bonds.
Metallic compounds are conductive as the electrons can move freely through the structure, but ionic compounds only conduct electricity when dissolved or molten.
Name this compound: P₄O₃
Tetraphosphorus Trioxide
Why does the transfer of electrons create ions and why are these ions attracted to each other?
When an electron leaves an atom, its negative charge leaves the atom, creating a positive charge. When an electron joins an atom, its negative charge is added to the atom, creating a negative charge. These ions are attracted to each other because opposite charges attract.
Why do atoms in covalent bonds share electrons rather than transfer them?
Neither atom has a strong enough pull to completely remove an electron.
Describe the "sea of electrons" and how it creates the properties of metals.
The "sea of electrons" allows electrons to move freely around a lattice structure of positively charged metal ions. Metals are malleable and ductile because of the resilience and flexibility of the structure. The flowing electrons create conductivity, allowing electric currents to flow easily.
Why is AlCl₃ called aluminum chloride (no tri- prefix) but BCl₃ is called boron trichloride?
Prefixes are only for covalent compounds; aluminum chloride is an ionic compound