Periodic Table Part 3 Flashcards
What are the three ways to excite electrons?
Heat, light and electricity
What is the maximum amount of electrons an electron shell can accomodate?
2n(2) electrons
How do electrons occupy energy levels?
In order of increasing energy, filling from the innermost shells outwards
How are shells numbered?
In order of increasing distance from the nucleus (1,2,3,4)
Why does every element produce a unique emission spectra?
Every element has a unique number of electrons in their shells
What does energy input cause electrons to do?
Jump to higher energy levels, which are unstable
What is the emission spectra of an element?
The spectrum of frequencies of electromagnetic radiation emitted due to an tom or molecular making a transition from a high energy state to a lower energy state
Why does neon have a greater number of emission spectra lines compared to hydrogen?
Neon contains a greater number of electrons and electron shells, allowing for more possible combinations and emission spectra
What are the two major areas of evidence to support Bohr’s atomic model?
Emission spectra and ionisation energies
What is the first ionisation energy?
The energy required to remove the most loosely held electron from atoms to produce +1 ions
What is ionisation energy?
The energy required to remove the most loosely held electron from atoms to produce +1 ions
What is the relationship between electrons closer to the nucleus?
They have a higher attraction to the nucleus and require greater energy to remove them
What did Erwin Schrodinger do?
In 1926, he took the Bohr model and determined the likelihood of finding an electron in a certain position, known as the quantum mechanical model
What are shells?
Regions of space surrounding the nucleus, numbered in order of increasing energy and distance from the nucleus
What are sub shells?
Smaller regions of space within shells, denoted by the letters s, p, d and f
