5. Electrons and bonding Flashcards
What are shells?
A group of atomic orbitals with the same principal quantum number N.
What are atomic orbitals?
A region around the nucleus that can hold up to two electrons, with opposite spins.
What are the 4 types of orbitals?
- s
- p
- d
- f
What is the shape of s-orbital?
Spherical
What is the shape of p-orbital?
Dumb-bell shape
How many orbitals make up a s-subshell?
1
How many orbitals make up a p-subshell?
3
How many orbitals make up a d-subshell?
5
How many orbitals make up a f-subshell?
7
How many orbitals are there in the 1st shell?
1
How many orbitals are there in the 2nd shell?
4
How many orbitals are there in the 3rd shell?
9
How many orbitals are there in the 4th shell?
16
How many electrons can fill a s-orbital?
2
How many electrons can fill a p-orbital?
6
How many electrons can fill a d-orbital?
10
How many electrons can fill a f-orbital?
14
How many electrons can fill the 1st shell?
2
How many electrons can fill the 2nd shell?
8
How many electrons can fill the 3rd shell?
18
How many electrons can fill the 4th shell?
32
What orbital is in the 1st shell?
s-orbital
What orbitals are in the 2nd shell?
s- and p-orbital
What orbitals are in the 3rd shell?
s-, p- and d- orbital
What orbitals are in the 4th shell?
s-, p-, d- and f-orbital
Rearrange the orbitals in terms of energy level.
1s > 2s > 2p > 3s > 3p> 4s > 3d > 4p > 4d > 4f
What is ionic bonding?
Electrostatic attraction between positive and negative ions.
What are giant ionic lattices?
A three-dimensional structure of oppositely charged ions that are strongly attracted in all directions, bonded together by strong ionic bonds.
How are ionic compounds’ melting point and boiling point? Why?
Ionic compounds have high melting point and boiling point, because they have strong electrostatic attractions between ions, which requires a lot of energy to overcome.
How are ionic compounds’ solubility?
Ionic compounds dissolve in polar solvents, eg. water. Polar molecules break down the lattice and surround each ion in solution.
How are ionic compounds’ electrical conductivity in solid state? Why?
Ionic compounds can’t conduct electricity in solid state, because ions are fixed and can’t move to carry electric charge.
How are ionic compounds’ electrical conductivity in liquid state? Why?
Ionic compounds can conduct electricity in liquid state, because ions can move freely and carry electric charge.
How are ionic compounds’ electrical conductivity in aqueous state? Why?
Ionic compounds can conduct electricity in aqueous state, because ions can move freely and carry electric charge.
What is covalent bonding?
Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
What is dative covalent bonding?
A shared pair of electrons in which the bonded pair has been provided by one of the bonding atom only.
What is average bond enthalpy?
A measurement of covalent bond strength
What does a larger value of average bond enthalpy suggest?
The larger the value of the average bond enthalpy, the stronger the covalent bond.
How are covalent compounds’ electrical conductivity? Why?
Covalent compounds can’t conduct electricity in any state, because they don’t have mobile electrons.
How are simple covalent compounds’ melting point and boiling point? Why?
Simple covalent compounds have low melting point and boiling point, because they have weak London forces between molecules, which are easy to overcome.
How are giant covalent compounds’ melting point and boiling point? Why?
Giant covalent compounds have high melting point and boiling point, because they have a lot of strong covalent bonds between molecules, which requires a lot of energy to overcome.
