Topic 2 - Electron Configuration Flashcards
What are the exceptions for the Schrodinger model
Chromium and Copper
Within each shell…
there are subshells
each subshell is made up of…
orbitals
How many electrons can orbitals hold?
2
What are orbitals
Locations of electrons in the Schrodinger model
For Abbreviated Configuration what are the rules?
The Nobel gas must be in [ ]
Has to be in shell order, not energy levels.
3 Critical Elements
Magnesium - 100-500
Uranium - 5-50
Phosphorus - 50-100
Critical Elements are
elements that are heavily relied on for industry and society in areas such as renewable energy, electronics, food supply and medicine. Many exist in only very small quantities on earth. The use is not sustainable.
Conflict element (around war)
- gold, tin, tungsten and tantalum
S Group
Group 1 and 2
D Group
Transition metals, 3-12, and last column of the ones at the bottom
F Group
The ones at the bottom except for last column
P Group
Groups 13-18
S has…
1 Orbital
2 Electrons
P has…
3 Orbitals
6 Electrons
D has…
5 Orbitals
10 Electrons
F has…
7 Orbitals
14 Electrons
Elements in the same ____ have similar properties
Group
Why is calcium more reactive than zinc
Zinc has more protons so it has a stronger pull. Electrons are closer to the nucleus and are less likely to be lost or donated
Why does fluorine have a higher ionization energy than iodine
It’s harder to get electrons off fluorine because it has a higher electronegativity. The shielding effect caused Iodine to have a lower electronegativity, the pushing makes it harder for iodine to grab electrons
what is ionization energy
the amount of energy required to remove an electron
the larger th ionization energy, the more difficult it is to remove an electron
top - bottom = decrease
left - right = increases
What is electronegativity
an atom’s desire to grab another atom’s electrons
top - bottom = decreases
left - right = increases
What is the atomic radius?
the total distance from an atom’s nucleus to the outermost orbital of the electron
top - bottom = increases
left to right = decreases
Shielding Effect
electrons in inner energy levels tend to push electrons in outer energy levels away from the nucleus.
What causes the difference in atomic radius
less protons = less attraction to the electron = larger
extra shell = larger
Do non-metals have larger ionization energies?
Yes
What is electronegativity
an atom’s desire’ to grab another atom’s electrons
top - bottom = decreases
left - right = increases
Core/nuclear Charge
Is the pulling power of the nucleus
top - bottom = constant (as you go down the outer electrons are held less tightly
left - right = increases
subshell electron configuration
1,2,3,4 shell order
Phosphorus
- essential for life (DNA)
- used in fertilizers
what determines the chemical properties of an element
number of electrons
