A1 - atomic structure, bonding and shapes and molecules Flashcards
Definition of isotope
Atoms of the same element with different number of neutrons and different masses
Definition of isoelectronic
Atoms with the same number of electrons
Definition of relative atomic mass
The weighted mean mass of an atom of the element compared with 1/12th mass of carbon - 12
Definition of relative isotopic mass
The mass of an isotope compared with 1/12th mass of an atom of carbon 12
How many orbitals are in an s-subshell
1 - holds two electrons
What is the order of electronic configuration
1s2 2s2 2p6 3s2 3p6 4s2 3d10
What is an orbital
A region of space where an orbital usually is
Hunds rule about electron configuration
Electrons prefer to occupy orbitals on their own and only pair up when no empty orbitals have f the same energy are available
What is the Aufbau principle about electron configuration
Electrons are placed into shells starting with the lowest energy level first - each shell must me full before the next shell starts to fill
How many subshells in the first shell
1
How many electrons can an s-orbital hold
2 electrons
How many electrons can a p orbital hold
6
How many electrons can d-orbitals hold
10
What orbitals are in the first sub shell
S
What orbitals are in the second subshell
S and P
What orbitals are in the 3rd subshell
S p d
What is the maximum number of electrons in the first shell
2
What is the maximum number of electron in the 2nd shell
8
What is the maximum number of electrons in the 3rd shell
18
Why are 4s subshells filled before 3d subshells
4s subshells had lower energy than the 3D subshell
Definition of ionic bonds
The electrostatic attraction between oppositely charged ions in all directions
What two factors determine the strength of ionic bonding
Magnitude of charge
Size of ion
Why does a smaller ion have a stronger ionic bond
More compact electrostatic density so stronger attraction between ions
Why does having a larger charge on the ion mean a greater ionic bond
Increased pull from the protons in the neutron has a stronger effect on the electrons drawing them closer and having a stronger attraction between ions