Topic 1 - Atomic Structure & The Periodic Table Flashcards
(40 cards)
Meaning Relative Atomic Mass (Ar)
The weighted mean mass of an atom of an element, compared to 1/12th of the mass of an atom of carbon-12
Meaning Relative Isotopic Mass
The mass of an atom of an isotope, compared to 1/12th of the mass of carbon-12
Meaning Relative Molecular Mass (Mr)
The mean mass of a molecule, compared to 1/12th the mass of an atom of carbon-12
Name all of the orbitals
s, p, d, f
Describe the s orbital
Has 1 orbital, so can hold 2 electrons
Describe the p orbital
Has 3 orbitals, so can hold 6 electrons (2x3)
Describe the d orbital
Has 5 orbitals, so can hold 10 electrons (5x2)
Describe the f orbital
Has 7 orbitals, so can hold 14 electrons (7x2)
Which shape does an S orbital have
Spherical shape
Which shape does a p orbital have
Dumb-bell shaped
Give the electron configuration of iron (26)
1s2 2s2 2p6 3s2 3p6 4s2 3d6
Give the electron configuration of calcium +2
Give the electron configuration of iron +3
Give the electron configuration of copper (29)
1s2 2s2 2p6 3s2 3p6 4s1 3d10
State the different radiations in order of the electromagnetic spectrum
Radio waves, micro waves, infrared, visible light, ultraviolet, X-rays, gamma rays
When do electrons become excited
When electrons absorb energy (endothermic) as it moves up an energy level
In an atomic emission spectra, why do the lines get closer
Because energy and frequency increases
When do electrons show ultraviolet radiation
When an electron falls to the ground state (n=1)
When do electrons show visible radiation
When an electron falls to the second energy level (n=2)
When do electron show infrared radiation
When electrons fall to the third energy level (n=3)
Meaning ionisation
The minimum amount of energy required to remove 1 mole of electrons from 1 mole of atoms in a gaseous state
What are 3 factors of ionisation
Shielding, nuclear charge, atomic size
How does shielding affect ionisation
The more electron shells between the positive nuclei and the negative electron thats is being removed, the less energy required to ionise because theres a weaker attraction
How does nuclear charge affect ionisation
The more protons in the nucleus, the larger the attraction between the nucleus and the outer electrons. This means more energy is needed for ionisation