Study Set Content:
exhibit a negative charge and are found around the nucleus of the atom in electron orbitals
electrons
defined as the volume of space in which the electron can be found within 95% probability
orbitals
four different types of orbitals
s, p , d f
shape of s orbital
spherical shape
shape of p orbital
dumbbell shape
shape of d orbital
clover shape
shape of f orbital
double-dumbbell shape
d block
transition metals
f block
lanthanides and actinide series
s block
alkali metals and helium
p block
main group elements
The number of electrons in an atom is equal to the atomic number. Each added electron will enter the orbitals in the order of increasing energy. An orbital cannot take more than 2 electron
Aufbau principle
As the (n+l) value increases, the energy of the electron increases.
N+l rule
Every orbital in a sub-shell is singly occupied with one electron before any one orbital is doubly occupied.
Hund's Rule of maximum multiplicity
represent the orbitals
Letters
say which energy level the orbitals are found in
Big Numbers
say how many electrons live in each orbital that are available
Superscripts
- tells us the number of atoms of each element in a compound. It contains the symbols of the atoms of the elements present in the compound as well as how many there are for each element in the form of subscripts.
Chemical formula
a representation of a molecule that uses chemical symbols to indicate the types of atoms followed by subscripts.
Molecular Formula
- a compound gives the information as its molecular formula but also shows how the atoms are connected in the molecule.
Structural Formula
