Bonding Flashcards
What are the two main classes of bonding?
Covalent - only Non-Metals
Ionic - Non-Metals and Metals
What happens to the electrons in Ionic Bonding?
Electrons are gained or lost to form a full outer shell, giving it an isoelectronic configuration of a noble gas.
Isoelectronic means?
The same number of electrons
What groups form which ionic charges?
Groups 1,2 and 3 form Positive ions of +1,+2 and +3
Groups 5,6 and 7 form Negative ions of -3,-2 and -1
Recite the ionic compounds and elements charges from the table.
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What is Ionic Bonding?
The strong electrostatic force of attraction between two oppositely charged electrons
Why do ionic compounds have a high melting and boiling point?
The strong electrostatic forces of attraction between oppositely charged ions must be broken and this requires a lot of energy.
Do Ionic Compound conduct electricity?
No, Ions are not free to move. However, able to conduct electricity when in aqueous or molten state as ions are now free to move.
What is Covalent Bonding?
The strong electrostatic attraction between the positively charged nuclei of both atoms and the shared pair of electrons.
What are the two different structures in covalent bonding?
Simple molecular structure
Giant structure
Why do most Covalently bonded molecules have a low boiling and melting points?
That is because when the simple molecular structure is heated only the weak intermolecular forces of attraction are broken. As they are weak, it does not take much energy to overcome them. NO COVALENT BONDS ARE BROKEN.
Why do giant covalent structures have high melting and boiling points?
Covalent bonds must be broken. Covalent bonds are strong. Therefore, a lot of energy must be supplied to break them. Do not USUALLY conduct electricity as they have no charged particle able to move.
Name three Allotropes of Carbon.
Diamond
C^60 Fullerene
Graphite
Coal
Why do Diamond and Graphite have a higher boiling point the C^60 Fullerene?
That is because graphite and diamond have a giant covalent structure meaning that you have to break the covalent bonds when melting, however, C^60 Fullerene has a simple molecular structure meaning that you only have to break intermolecular forces when melting. Breaking Covalent bonds take significantly more energy than to break weak intermolecular forces.
Why is diamond harder to break than graphite and not conduct electricity like graphite?
Diamond is hard because to break it apart you have to break the covalent bonds. Graphite is soft because you only need to break the weak intermolecular forces between the layers. Diamond does not conduct electricity because has no charged particles that are free. Graphite conducts electricity because carbon only has 3 bonds so it has one electrons left over which is free to move.
