Chapter 5 - Electrons and Bonding Flashcards
How does group number relate to electronic structure?
The group number tells you how many electrons in the outermost shell.
What is a shell?
Shells are energy levels, the energy levels increase as the shell number increases. The shell number may also be referred to as principal quantum number.
What is an orbital?
A region around the nucleus that can hold up to two electrons with opposite spins.
It shows us a 95% probability of where an electron will exist.
How many electrons can shell 1 hold?
2 electrons
How many electrons can shell 2 hold?
8 electrons
How many electrons can shell 3 hold?
18 electrons
How many electrons can shell 4 hold?
32 electrons
What shape is an s-orbital?
A spherical shape
What shape is a p-orbital?
A dumb-bell shape
What is an electron?
A cloud of negative charge, which has the shape of the orbital occupied by the electron.
Which orbitals are in shell 1?
1 s-orbital
Which orbitals are in shell 2?
1 s-orbital and 3 p-orbitals
Which orbitals are in shell 3?
1 s-orbital, 3 p-orbitals and 5 d-orbitals.
Which orbitals are in shell 4?
1 s-orbital, 3 p-orbitals, 5 d-orbitals and 7 f-orbitals
What is a sub-shell?
All of the orbitals of the same type in the same shell.
e.g. s sub-shell and p sub-shells
How many electrons can an s sub-shell hold?
2 electrons
How many electrons can a p sub-shell hold?
6 electrons
How many electrons can a d sub-shell hold?
10 electrons
How many electrons can a f sub-shell hold?
14 electrons
Order the sub-shells in terms of energy levels, starting from lowest.
s, p, d and f going up the shells.
With the exception of the 3d sub-shell which has a higher energy than 4s.
Which sub-shells are in shell 1?
1s
Which sub-shells are in shell 2?
2s, 2p
Which sub-shells are in shell 3?
3s, 3p, 3d
Which sub-shells are in shell 4?
4s, 4p, 4d, 4f
What is the short notation for electronic structure?
The closest prior noble gas in square brackets and the remaining electronic configuration.
How are orbitals drawn?
A square with two arrows in it pointing opposite directions to represent the opposite spins
How are orbitals filled for ions?
Draw out the electronic structure of the atom.
For a negative ion, add the extra electrons.
For a positive ion, remove the electrons, if 4s is full remove the electrons from there before removing from 3d.
What is the electronic structure of Chromium (Cr)?
1s2 2s2 2p6 3s2 3p6 4s1 3d5
As it is more stable due to both 4s and 3d being half-full.
What is the electronic structure of Copper (Cu)?
1s2 2s2 2p6 3s2 3p6 4s1 3d10
As is makes a full 3d sub-shell and a half-full 4s sub-shell.
What is ionic bonding?
Electrostatic attraction between positive and negative ions
What are some common cations?
Metal ions and ammonium ions
What are some common anions?
Non-metal ions and polyatomic ions
What is a covalent bond?
Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
What two molecules is a covalent bond between?
Metal and non-metal
Describe a single covalent bond.
A single shared pair of electrons from both the bonding atoms
Describe multiple covalent bonding.
Multiple pairs of shared electrons from both the bonding atoms
Describe a dative covalent bond.
A covalent bond where bond the electrons come from one of the bonding atoms only.
What is average bond enthalpy?
Measurement of covalent bond strength.
What is the structure of a giant ionic lattice?
Ions attraction oppositely charged ions in different directions
Positive metal and negative non-metal ions all attracted to each other
What are the properties of a giant ionic lattice?
High melting and boiling points - due to strong electrostatic forces between ions so high energy is required to overcome the forces of attraction
Mostly water soluble, unless compound has too high charges then it doesn’t dissolve in the water
Conductive in molten and aqueous state but not solid - charge needs to be able to move freely in order to conduct electricity
