Chapter 5 - Electrons And Bonding Flashcards Preview

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Flashcards in Chapter 5 - Electrons And Bonding Deck (18)
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1
Q

What are shells regard as?

A

Are energy levels. The energy increases a the shell number increases.

2
Q

What are shells made up of?

A

Atomic orbitals which can contain a maximum of 2 electrons with opposite spins

3
Q

What can an electron be referred as?

A

Can be though of as a negative-charge cloud

4
Q

What type of orbitals are there?

A
  • s
  • p
  • d
  • f
5
Q

Describe a s-orbital

A

Electron cloud is in a shape of a sphere. Each shell from n = 1 contains 1 s-orbital. The greater the shell number, the greater the radius of its s-orbital

6
Q

Describe a p-orbital

A

Shape of a dumb-bell. There are three separate p-orbitals at right angles to one another. Each shell from n = 2 contains three p-orbitals. The greater the shell number, the further the p-orbital is from the nucleus.

7
Q

Describe a d-orbital

A

More complex then the rest. Each shell from n = 3 contains five d-orbitals.

8
Q

Describe a f-orbital

A

More complex. Each shell from n = 3 contains seven f-orbitals

9
Q

What are sub-shells?

A

A group of orbitals of the same type within a shell

10
Q

What is the order of the shells and the orbitals in them?

A

1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p

This is how you would write it. But when filling the orbitals the 4s and the 4p is filled before the 3d

11
Q

What is the electron configuration?

A

A short hand representation that shows how electrons occupy sub-shells

12
Q

Define ionic bonding

A

Is the electrostatic attraction between positive and negative ions held together in an ionic compound by the bonds between the cations and anions

Non-metal + metal -> product

13
Q

What are the properties of an ionic bonding?

A
  • high melting point - a lot of energy is needed to required to overcome the electrostatic attraction
  • solubility - soluble in polar solution. However if too high of attraction between the ions it will not be soluble in water.
  • electrical conductivity only in molten as in solid the delocalised electrons are not free to move around in the ionic compound.
14
Q

What is a covalent bond?

A

Are formed when atoms share electrons and the nuclei of the bonded atoms. Only happened with non-metals. Can be a single, trouble, triple bonds

15
Q

A covalent bond is localised. What does that mean?

A

Attraction is acting between a pit of shared electrons and the nuclei if the bonded atoms. Can be called a molecule.

16
Q

What is a lone pair?

A

Paired electrons which are not shared represent as •• in displayed formula.

17
Q

What is a dative covalent bond?

A

Atoms sharing 2 electrons which have both come from the just 1 atom. Those two electrons where originally line ours.

18
Q

What else can a dative covalent bond be called?

A

Coordinate bond