Bonding Flashcards
Ionic bonding properties
- takes place between non metal and metal
- atoms are held in place by very strong ionic bonds
- they require a lot of energy to break
- they have a high boiling and melting point
Ionic bonding definition
It is the transfer of electrons from a metal to a non metal and has a strong electrostatic force of attraction between the atoms
What is a simple covalent molecule
It is two non-metal particles joined by covalent bonding
What does simple covalent bonding occur between?
Nonmetals which gain electrons in their outer shell meaning that the electrons are shared between them
What type of bonds do simple covalent structures have?
- intermolecular forces between the molecules
And covalent bonds between the molecules
Why are simple covalent bonds weaker than giant covalent structures
Covalent bonds found between the atoms in giant covalent structures are stronger than the weak intermolecular forces found between the molecules in simple covalent structures
Why are ionic compounds so strong
Many strong ionic bonds hold the atoms together, meaning a high a,punt of energy is needed to break them
Where are the covalent bonds in a simple covalent molecule
Between the atoms
What is the difference between simple covalent and giant covalent bonds
Simple covalent bonds - weak intermolecular forces between molecules
Giant covalent structures - many strong covalent bonds between everything
Properties of giant covalent bonds
Many bonds, very strong and hard to break apart and require high amounts of energy to do so
What are electrostatic bonds
Forces between atoms (can be ionic, metallic, covalent etc)
What is metallic bonding
Metallic bonding is the strong electrostatic forces of attraction between the sea of delocalised electrons and positively charged metal metal ions
What is a delocalised electron?
Delocalised electrons are electrons that are free to move and are separated from their shell
When does metallic bonding take place?
It takes place with only one type of metal
When does metallic bonding take place?
It takes place with only one type of metal
Explain the process of metallic bonding
- During metallic bonding, the metal loses its outer electrons,
- there is no other substance there to gain the lost electron meaning that the lost electron sits outside the atom.
- However there is a force of attraction between the lost electron (which is negatively charged) and the newly created ion (which now has a positive charge).
Sodium is another Group 1 metal.
Sodium reacts in a similar way to potassium.
Explain why.
Use ideas about atomic structure in your answer.
Both have one extra electron in their outer shell, meaning they react the same way trying to loose it
Mendeleev did not predict the existence of argon, neon, krypton or xenon.
The electron arrangement of argon is 2,8,8.
What does this tell you about the reactivity of argon?
Explain your answer.
It is a stable element, and is unreactive as its outer shell is full
Why do large covalent structures not conduct electricity
There are no delocalised / free electrons to carry electrical charge
Explain why metals are malleable yet do not break
Metals are arranged in layers of metal ions which are able to easily slide over each-other, making them malleable, yet the strong metallic bonds holds the atoms together
Lithium can conduct electricity in the solid and liquid state.
Explain why metals can conduct electricity.
the DELOCALISED ELECTRONS are able to carry electrical charge and transfer it between the electrons
Methane (CH4) has a low melting point.
Explain why methane has a low melting point.
Use ideas about structure and bonding in your answer.
There are weak intermolecular forces between the molecules, meaning low amounts of energy is needed to break them
All halogens have similar chemical reactions.
Explain why in terms of electronic structure.
They all have 7 electrons in their outer shell, meaning they react the same way to try gain the last electron
Why do covalent bonds not conduct electricity
No delocalised electrons to carry electrical charge
Element C burns in oxygen to make white clouds of its oxide. Describe how you could r the oxide to find out if the element is metal
-. Dissolve it in water
-> add universal indicator
-> indicator would tune blue
Diamond can be described as having a giant lattice structure.
Why is diamond described as a giant lattice structure?
- many strong covalent bonds in all directions between all particles
- arranged in repeating patterns
