Covalent
What are the types of elements in this bond?
Two nonmetal atoms.
What types of elements make up this bond?
A nonmetal and a metal.
What are the types of elements in this bond?
Two metal atoms.
What suffix do we add to the second element of binary compound names?
-ide
Why don't noble gases form covalent bonds, even though they are nonmetals?
Because noble gases already have a full outer shell of electrons.
What happens to the electrons in this bond?
The electrons are completely transferred, or "stolen".
Why is there a low electronegativity difference in metallic bonds?
Because both of the atoms are metals, and as such are quite similar in composition and electronegativity.
What is the name for NaCl?
Sodium Chloride
What is happening to the electrons in covalent bonding?
The electrons are equally shared.
Explain why there is a high electronegativity difference between the two atoms involved in ionic bonds. (Costa Level 2)
Because metals give a few electrons and thus have a low electronegativity, while nonmetals have many electrons.
What makes metallic compounds useful?
Their high conductivity, luster, malleability, and strong manner make metals highly useful in art, construction, and especially electronics.
Explain why covalent compounds do use prefixes and suffixes when naming them. (Costa Level 2)
Unlike ionic and metallic compounds, there is always a set charge for nonmetal atoms, so the ratio of the two atoms will remain the same when balanced.
Show some reasons why there is a low electronegativity difference in covalent compounds. (Costa Level 2)
There are fewer nonmetals than there are metals on the periodic table, they are similar in nature, and most nonmetals are in the same few groups.
Explain why ionic compounds generally form a crystal lattice structure when in solid form. (Costa Level 3)
Due to the conflicting charges from the cations and the delocalized electrons, the ions arrange themselves in an array pattern to maximize attraction between atoms.
How does the loose sharing of electrons in metallic bonds lead to a high conductivity? (Costa Level 2)
Electrons are able to move more freely because of the loose space between atoms.
Why do you think the cation is typically placed before the anion when naming a compound? (Costa Level 3)
This is because the cation appears on the periodic table before the anion does.
Why do you think covalent compounds tend to be liquid or gaseous at room temperature? Explain. (Costa Level 3)
This is because covalent compounds have low melting points, which in turn is caused by the weak force of attraction that comes from bonding with atoms that have similar electronegativities.
Predict why ionic compounds generally can't conduct as a solid, but can conduct when melted or dissolved. (Costa Level 3)
The ions are very close in ionic bonds due to the high attraction of the cations and anions, so when they are spaced apart after melting or dissolving, there is more room for electrons to flow through the compound.
Infer what may cause the properties such as malleability in metallic compounds. (Costa Level 2)
The bonds in metals aren't as strong, and since they are loose and free, the atoms and electrons move apart rather than break apart when struck.
Hypothesize why suffixes and prefixes aren't used when naming metallic and ionic compounds. (Costa Level 3)
Metals can have many different charges depending on the specific atom, and as such there are multiple combinations to metallic compounds. So it would be misleading to attach ratios to metallic compounds.