M1 Topic 3 part 1: Periodocity (state of matter at room temp, electonic config, atomic radius) Flashcards
Which elements are gases at room temperature(5)
Hydrogen Nitrogen Oxygen Fluorine All of group 18(noble gases)
What elements are liquids at room temperature (6)
Mercury, gallium, francium, rubidium,Caesium, bromine
What is the order of electron shells according to Bohr model for the first 20 elements
2, 8, 8, 2
What are orbitals
Locations/patterns of where specific electrons are
What are the types of orbitals in order
S
P
D
F
How many electrons are in the S orbital
2 electrons
How many electrons are in the P shell
6 electrons
How many electrons in the d shell
10 electrons
Which direction do groups go in on the periodic table
A group go down the periodic table
Which direction do periods go in
Go along (left to right) the periodic table
What is the number at the front of the orbital symbol
(example the 1 in 1S2)
Which period it’s in, on the periodic table
What is does the letter mean in the orbital symbol
Example the S in 1S2
The shape of the orbital
What does the indices mean in the orbital symbol
Example the 2 in 1S2
Number of electrons
How many groups are there
18
How many periods are there
7
Which groups are all the s orbital found
All s orbitals are found in group 1 and 2, except for helium which is found in group 18
Which groups are all the P shells located
In groups 13 to 18
In which groups are D shells located
In groups 3 to 12
What are the guidelines for filling electrons (3)
The Pauli exclusion principle
The Aufbau principle
Hund’s rule
What does the Pauli exclusion principle state.
Each orbital can contain a maximum of two electrons, with each electron having a different spin
What does Aufbau’s principle state
Electrons will occupy lower energy orbitals first
What does Hund’s rule state
Each orbital sub level must contain an electron before electrons can be paired.
