Module 2 Chapter 5 Flashcards
What happens as the shell number increases
The more electrons can be contained in the shell
What happens in terms of energy as the shell number increases
As the shell number increases the energy of the shells also increases
Why does the energy of the shells increase as the shell number increases
More energy is required to keep them in the atom as they are further away from the nucleus
What is another name for the shell number or energy level number
Principal quantum number
What can the maximum number of electrons in each shell be calculated by
2N squared (where n is the principal quantum number)
What are the maximum number of electrons in each shell
N = 1, maximum number 2
N = 2, maximum number 8
N = 3, maximum number 18
N = 4, maximum number 32
What do electrons behave like
Electrons have wave particle duality meaning they behave both as a wave and a particle
What are shells made up of
They are made up of atomic orbitals
What can orbitals hold
They are a region around the nucleus that can hold up to 2 electrons with 2 opposite spins.
What is an orbital
It’s visualised as a region in space where there is a high probability of finding an electron.
What is a property of the electrons in the orbitals
They have either up or down spin. When one electron has up spin the other has down spin.
Without observation what state are electrons in
They are in superposition when neither is in up spin or down spin, it is in the spin up and down state.
What are the 4 different orbitals
S-, p-, d-, and f- orbitals
What is an s orbital
Electron orbital in the shape of a sphere.
They can hold two electrons
Each shell from n=1 contains one s orbital
What happens to the s orbital as the principle quantum number increases
the radius of the orbital increases
Draw an s orbital
What is a p orbital
The orbital is in the shape of a dumbell
Each p orbital contains 2 electrons
What are the three types of p orbitals
Px,Pz,Py, where the small letter is the axis that they lie on
What do each of the p orbitals look like
Draw it
What principle quantum number 1 what is the maximum number of electrons and number of each orbitals
2 electrons
1S
What principle quantum number 2 what is the maximum number of electrons and number of each orbitals
8 electrons
1S, 2S, 2P (2Px, 2Py, 2Pz)
What principle quantum number 3 what is the maximum number of electrons and number of each orbitals
18 electrons
1S, 2S, 2P (2Px, 2Pz, 2Py), 3S, 3P (3Px, 3Py, 3Pz), 3D
What principle quantum number 4 what is the maximum number of electrons and number of each orbitals
32 electrons
1S, 2S, 2P (2Px, 2Pz, 2Py), 3S, 3P (3Px, 3Py, 3Pz), 3D, 4S, 4P (4Px, 4Py, 4Pz), 4D, 4F
How many d and f orbitals exist in principle quantum number 4
5 - d
7 - f
What does the average energy in the subshells do as the principle quantum number increases
the average energy in the subshells increases as the principle quantum number increases
What is the exception to this rule
The 4S orbital is lower in energy than 3D orbital
How do we fill orbitals
We fill orbitals in increasing energy
What do you use to represent the spin of an electron
You represent the different spins with up and down arrows
What is Hund’s rule
If there are three electrons in a p subshell, one electron will go into each Px, Py, Pz orbital before doubling up
What is Pauli’s exclusion principle
An orbital can only hold two electrons and they must have opposite spin
What are cations and anions
Cations = positive ions = lost electrons
Anions = negative ions = gained electrons
When forming ions what occurs
the highest energy subshells lose or gain electrons
How does the exception of 3D and 4S apply to this rule
3D is filled last/emptied last
4S is filled first/ emptied first
What happens during a chemical reaction between a metal and a non metal
The non metal gains electrons forming anions and the metal loses electrons forming cations
What is an ionic bond
The strong electrostatic forces of attraction between oppositely charged ions.
What is the arrangement of ionic structures
They are arranged in a giant lattice, and each ion experiences many attractions (as there are ionic bonds in all directions)
Why do ionic compounds have a high melting point
They are held together by many strong ionic bonds. These take lots of energy to break so ionic compounds have very high melting points.
What is the correlation between ion charge and melting point
The greater the ion charge the higher the melting point
What is the solution lily of ionic compounds
Many ionic compounds are soluble in polar solutions. This is because water molecules attract and surround the ions once the lattice is broken.
What does the solubility of an ionic compounds depend on
It depends on the relative strengths of attraction within the giant ionic lattice structure and the attractions between ions and water molecules.
What is the general rule of solubility for ionic compounds
Solubility decreases as ionic charge increases
What is the electrical conductivity of ionic compounds
In the solid state the ions are in fixed positions and are not free to move, they don’t conduct electricity. When liquid or in solution, the charge carrying ions are free to move so conduct electricity.
What is a covalent bond
The strong electrostatic forces of attraction between a shared pair of electrons and the positive nuclei of the bonded non-metallic elements.
What is covalent bonding in terms of 1 bond (orbitals)
The overlap between 2 atomic orbitals where each orbital contains 1 electrons, making a shared pair in the overlap
What is a double covalent bond
The electrostatic forces of attraction between 2 shared pairs of electrons and nuclei of bond atoms
What is a triple covalent bond
The electrostatic forces of attraction between 3 shared pairs of electrons and nuclei of bond atoms.
What is a dative covalent bond
The pair of bonding electrons are donated by one of the bonding atoms. You denote this with an arrowhead from the element that provides it.
