Chapter C3- Structure and Bonding Flashcards
What’s it called when a solid turns from a solid into a liquid?
What’s it called when a liquid turns into a solid?
What’s it called when a liquid turns into a gas?
What’s it called when a gas turns into a liquid?
What’s it called when a solid turns into a gas?
What does it mean when part of the line is straight on a cooling curve (concerning the temperature and energy)?
Melting.
Freezing.
Evaporation.
Condensation.
Sublimation.
At this point, eg from a gas to a liquid, the temperature isn’t cooling because all of the energy is being focused on breaking down the particles (taking energy from the surroundings).
What are the four points of an element?
What happens when a solid turns into a liquid?
What happens when a liquids turns into a gas?
What happens when a liquid turns into a solid/a gas turns into a liquid?
What is the overall charge of an atom?
What is the overall charge of the nucleus?
What happens when a metal becomes an ion (concerning its name)?
What happens when a non-metal becomes an ion (concerning its name)?
Melting, freezing, boiling and condensing.
The particles gain energy and so can brake down the bonds.
The particles gain enough energy to brake down bonds.
The particles lose energy to their surroundings as it brakes down the bonds of the particles.
0 (neutral) as the electrons and protons cancel each other out being positive and negative.
+1 (because of the protons being positive).
They keep their name.
They become an -ide (eg oxygen to oxide).
Why don’t noble gases (group 8/0 of the periodic table) form ions?
Why is an atom very reactive?
How will a substance react with another substance?
How does ionic bonding happen?
What happens in ionic bonding concerning the charges of the atoms?
What do compounds always have concerning their charge?
What do atoms with four electrons on its outer shell rarely do?
What does this mean?
Because they outer shells are already full.
Because it’s missing electrons in its outer shell.
If it can gain a full outer shell of electrons.
Ionic bonding happens due to electrostatic attractions between positively and negatively charged ions.
The charges of the atoms cancel each other out.
Compounds always have no charge (and so are neutral).
They rarely gain or lose electrons.
They rarely become an ion.
With what type of substances does ionic bonding occur in?
What do ions form in ionic bonding?
What are the two properties of ionic compounds?
What three other things are the properties of ionic compounds?
What do ions form when closely packed?
What are the chemical bonds between ions like?
What are the positive ions in ionic compounds called?
What are the negative ions called?
Ionic bonding happens between metals and non-metals.
Giant ionic bonding.
High melting and boiling points.
They dissolve in solutions that will conduct electricity. They conduct electricity when molten.
They form a closely packed regular giant lattice.
They are very strong.
Cations (CAT-ions).
Anions.
Describe when and how covalent bonding occurs?
Why do elements bond with one another?
What happens in covalent bonding?
What happens in ionic bonding?
What are the two common types of bonds in bonding?
What is the product known as when covalent bonding occurs between two non-metal atoms?
What is this substance?
What will giant ionic structures do and so be able to do?
Covalent bonding:
- Happens in non-metals only.
- Occurs in simple molecules.
- Forms giant structures.
To gain a full outer shell of electrons.
Covalent bonding is sharing electrons to achieve a complete outer shell between atoms.
Ionic bonding is the transferring of electrons to gain a complete outer shell between atoms.
Single and double bonds.
A molecule.
A molecule is a small group of atoms chemically bonded together (they can be all the same atoms).
They will dissolve on solutions that will conduct electricity.
What are intermolecular forces?
When are these forces stronger and weaker?
What does it mean if a substance has stronger intermolecular forces?
What do simple molecules form?
What are the forces like between these molecules?
What do they also form?
What are the properties of these molecules?
What and how does a monomer become?
What does this mean?
What are these substances made from and what is produced if they bond together?
Forces between molecules.
These are stronger in solids and weaker in gases.
The substance will have higher melting/boiling points.
Smaller molecules.
The forces between the molecule are very weak.
They also form strong bonds.
- The melting and boiling points of these molecules are very low.
- Most are gases at room temperature.
- They don’t conduct electricity.
- They don’t dissolve in water (usually).
A monomer becomes a polymer by breaking the double bond.
It means the sharing of two electrons.
Polymers are made from small molecules that bond together to make one big molecule.
What do different polymers have?
What does each carbon atom in graphite form?
What does each carbon atom in diamond form?
Why is graphite unusually soft?
What is diamond unlike graphite?
What are fullerenes?
What is the structure of fullerenes based on?
What are cylindrical fullerenes called?
What are the useful properties of these substances?
What are metals another example of?
What are electrons called in the “sea” of free moving electrons?
What are these free to move throughout?
What are alloys usually?
What are the properties of metals?
They have different strengths of intermolecular force which gives them different properties so they can be used for different things.
It forms only three covalent bonds.
It forms only four covalent bonds in a very rigid, tetrahedral structure.
Because graphite’s carbon atoms forms only three covalent bonds, it creates layers which are free to slide over each other, which is why graphite is soft.
An extremely hard substance (unlike graphite).
The general name for all these hollow-shaped molecules of carbon.
The hexagonal rings of carbon atoms.
Carbon nanotubes, which can also be produced.
- High tensile strength.
- High electrical conductivity and high thermal conductivity.
Giant structures.
Delocalised electrons.
The giant metallic lattice.
Mixtures of metals.
- They are malleable- they can be hammered into different shapes without cracking.
- High melting points.
- Good conductors of thermal energy and electricity.
How are high melting points of metals explained and so explain them?
How are metals also good conductors of thermal energy and electricity and so explain this?
How is the electrical charge and thermal energy transferred quickly through the metal?
By their giant structures. It takes a lot of energy to separate metal ions from their fixed positions and break down the lattice, melting the metal.
This is because their delocalised electrons can readily flow through the giant metallic lattice.
It is transferred quickly by the free-moving delocalised electrons.
