Topic 1 - Atomic Structure Flashcards
What are the sub-atomic particles that make up an atom?
Protons, electrons, and neutrons.
What are the charges and masses of all the sub-atomic particles?
Protons: 1+, 1
Electrons: 1-, 1/1836
Neutrons: 0, 1
What is an ion?
An ion is a charged particle.
What is an isotope?
An element with the same number of protons but a different number of neutrons.
What is a free radical?
A species with one or more unpaired electrons. E.g. Cl*
How is a free radical represented?
With a dot.
What are the different types of orbitals?
s, p, d, f
What is an s-orbital?
The first orbital in the periodic table found in groups 1 & 2. It has 1 orbital and can hold 2 electrons.
What is a p-orbital?
The second orbital in the periodic table found in groups 13-18. It has 3 orbitals and can hold 6 electrons.
What is a d-orbital?
The third orbital in the periodic table found in groups 3-12. It has 5 orbitals and can hold 10 electrons.
What is a f-orbital?
The fourth orbital in the periodic table found in the lanthanoids and actinoids. It has 7 orbitals and can hold 14 electrons.
Which two elements are not found in groups 1 & 2 but are included in s-block?
Hydrogen and Helium.
What is the shape and movement of electrons in s-orbitals?
They are spherical and the 2 electrons can move anywhere within the sphere.
What is the shape and movement of electrons in p-orbitals?
Dumbbells. Two electrons can move freely within each p-orbital.
What are the three types of p-orbitals and how are they distinguished?
Px orbitals lie on the x-axis.
Py orbitals like on the y-axis.
Pz orbitals lie diagonally between the x and y-axis.
How is electron configuration written?
The first number is the shell. The second part is the type of orbital. The third part tells you the number of electrons. E.g. 2p4 is in shell 2. It is a p-orbital. And it has 4 electrons.
What is ‘spin pairing’ or ‘spin pair repulsion’?
When two electrons occupy one orbital they spin in opposite directions. This is represented by single headed arrows pointing different directions. (one up, one down).
What are the two rules to remember when adding electrons to orbitals?
- Fill from the lowest energy level up.
- Fill orbitals singularly first and then pair up.
What is the rule to remember when removing electrons from orbitals?
Remove from the highest energy level first.
How is the electronic configuration of chromium and copper different from normal?
The take an electron from the 4s sub-shell and add it to their 3d sub-shell to create a more stable atom.
What is the definition of ionisation energy?
The minimum amount of energy required to remove 1 mole of electrons from 1 mole of atoms in the gaseous state.
How does shielding affect ionisation energy?
The more electron shells between the positive nucleus and negative electron that is being removed the less energy is required. There is a weaker attraction.
How does nuclear charge affect ionisation energy?
The more protons in the nucleus the bigger the attraction between the nucleus and outer electrons. This means more energy is required to remove the electron.
How does atomic size affect ionisation energy?
The bigger the atom, the further away from the nucleus the outer electrons are. The attractive force between the nucleus and the outer electrons reduces so it is easier to remove electrons.