Atomic Structure And Electrons (Completed) Flashcards
Define isotopes
Atoms of the same element (so with the same number of protons) with a different number of neutrons
What is the mass number
The number of protons + neutrons in the nucleus
What is the atomic number
The number of protons in the nucleus
Explain how the chemical properties of isotopes differ or are similar
Isotopes have the same chemical properties and react in the same way because they have the same number of electrons - this is what the reactivity mostly depends on
Define relative isotopic mass
The mass of an atom of an isotope in comparison with 1/12th of the mass of an atom of carbon 12
How can you see the relative isotopic mass of an isotope
The relative isotopic mass is the same as the isotopes mass number
Define relative atomic mass
The weighted mean mass of an atom of an element in comparison to 1/12th of the mass of an atom of carbon 12
Give 2 things the weighted mean mass of an element takes into place
The percentage Abundance of each isotope
The relative mass of each isotope
Give 2 things a mass spectra usually tells us
The number of peaks represents the number of isotopes
The height of the peaks tells us the abundance of the isotope
What is the X acis on a mass spectra usually
m/z
What does m/z represent
Mass to charge ratio
What is the max number of electrons in the first shell
2
What is the maximum number of electrons in the second shell
8
What is the maximum number of electrons in the third shell
18
What is the maximum number of electrons in the fourth shell
32
Give the 4 different types of orbital
S orbital
P orbital
D orbital
F orbital
Define orbital
A region within an atom that can hold up to 2 electrons with opposite spins
What is the shape of an s orbital
Spherical
How many electrons can occupy s orbitals in each shell
In each shell, a maximum of 2 electrons they can occupy s orbitals
What is the shape of a p orbital
The shape of a dumbbell, and there are usually 3 of them which are arranged at right angles to each other
How many electrons maximum can occupy a p orbital in each shell
None can occupy a p orbital in the first shell
From shell 2 and up, 6 electrons can occupy a p orbital
How many D orbitals can fit in a subshell
5
How many electrons can occupy the d Orbitals in each shell
In the first and second shells, no electrons can occupy d Orbitals
From the 3rd shell up, 10 electrons can occupy d Orbitals per shell
Draw the table that shows how electrons occupy each shell, sub-shell and orbital
What are sub-shells
Groups of the same types of orbital
What does the Aufbau principle state
Electrons fill orbitals of the lowest energy first
Draw the graph that shows the order each sub shell is filled
Give the order that the sub shells are filled in up to 4p⁶
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶
What is hund’s rule
Each electron has a negative charge and we would expect the electrons in an orbital to repel one another
Within a sub shell, each orbital has the same energy. Each of the orbitals in a sub-shell has to be filled singly and with parallel spins (same direction) before any electrons can pair up