Intro. to Bonding
What is the difference between intra and intermolecular forces?
Intramolecular forces are within the same substance.
Intermolecular forces are between different substances.
Explain the connection between electronegativity and the formation of an ionic bond.
The difference in electronegativity is so great that one atom takes the electrons from the other because it has such a greater attraction to them.
Explain what makes a metallic bond different from an ionic versus a covalent.
•They are different from ionic because they do not lose their valence electrons, instead they share.
•They are different from covalent because they do not result in a compound being formed.
List the number of atoms of each element in the compound
Ca(ClO3)2
Calcium: 1
Chlorine: 2
Oxygen: 6
What is an ion?
Charged atom
What is meant by the statement: "Bonding is a spectrum?"
The type of bond is dependent on the difference in electronegativity.
Use an example of an ionic compound to explain the “rule of zero charge”.
MgCl2 is one atom of magnesium with a 2+charge, and two atoms of chlorine, each with a 1- charge.
Describe the unique properties that result from metallic bonds.
•Malleable (can be made into thin sheets)
•Ductile (can be made into wires)
•Can conduct electrical and thermal energy
Strong absorbers and reflectors of light
Write the chemical formula for the following compound:
a) Magnesium Flouride
MgF2
Define a polyatomic ion.
A positively or negatively charged, covalently bonded group of atoms
Give me a sentence to summarize the connections between chemical bonds, chemical reactions, and compounds.
Explain why it is necessary to include a Roman numeral when naming an ionic compound with a transition metal.
You cannot determine the charge of a transition metal from the periodic table, so the Roman numeral is necessary to indicate the charge of the metal ion.
Explain delocalized electrons.
Electrons not associated with a single atom or bond.
Write the chemical formula for the following compounds:
a) Lead (IV) Sulfate
Pb(SO4)2
Define metallic bond.
An interaction that holds metal atoms together through a shared pool of valence electrons
Explain why most atoms form chemical bonds and why some atoms don't.
They form bonds to be stable with full outer energy levels of electrons.
Nobel gases don't form chemical bonds because they are already stable.
Give an example of a common compound and how the properties of the elements that make it up are different from that of the compound itself.
•NaCl = sodium chloride
•Sodium on its own is extremely explosive when in contact with water.
•Chlorine on its own is extremely poisonous.
•Together they make table salt, which we can eat.
Give an example of an alloy and include its definition.
•Mixture of multiple metals.
14K gold is part gold, part silver and copper (usually)
Bronze- Copper and Tin
Brass- Copper and Zinc
Draw the Lewis structure for the bond that would form between calcium and chlorine. Then write its chemical formula and name.
Image should include Ca with 2+, 2 Cl atoms with a - next to each one with a full outer shell.
Define the octet rule.
The tendency of atoms to prefer to have 8 valence electrons
List 2 properties of covalent versus ionic compounds. (2 for ionic, 2 for covalent)
Ionic:
Crystalline solids
High BP and Melting Point
Can conduct electricity when dissolved in water.
Covalent:
Can be a solid, liquid or gas
Low boiling or melting point
Cannot conduct electricity when dissolved in water
Name the following compounds:
a)Na2CO3
b) Mn(OH)2
a) Sodium Carbonate
b) Manganese (II) Hydroxide
Explain why the “sea of e-” forms in metallic bonds and why this makes them good electrical conductors.
•The “sea of e-” forms because metals like to form lattices, but they are often bigger so their orbitals overlap. They also have lower electronegativities so their attraction for electrons in a bond is lower.
•Because of this, the electrons are delocalized, making them good at creating a flow of e- when conducting electricity.
Write the chemical formula for the following compounds:
a)Gold (II) carbonate
B)Calcium phosphate
a) AuCO3
b) Ca3(PO4)2
Define crystal lattice.
Network of cations and anions that are mutually attracted to one another