Davies Exam Flashcards
The two leftmost columns make up the …
This is called the … because elements in it have all their valence electrons in s orbitals.
Note, Helium is also an s block element because it has the electron configuration __
The two leftmost columns make up the s block.
This is called the s block because elements in it have all their valence electrons in s orbitals.
Note, Helium is also an s block element because it has the electron configuration 1s2.
The six rightmost columns make up the ___
This is called the p block because elements in the p block have a partially filled p sub-shells
The six rightmost columns make up the p block.
This is called the p block because elements in the p block have a partially filled p sub-shell.
The d block lies …
Elements in the d block have a …
Elements in the d block are often called ____
The d block lies between the s and p blocks.
Elements in the d block have a partially filled d sub-shell.
Elements in the d block are often called transition metals.
Atomic radius ___ along a period.
This is because …
As you add protons, you also add ___. But these are all being added to the same shell, so this does not affect the …
So each electron ____
Atomic radius decreases along a period.
This is because the number of protons in the nucleus increases across the period.
As you add protons, you also add electrons. But these are all being added to the same shell, so this does not affect the radius.
So each electron feels a stronger attraction to the nucleus and is held closer.
In Period 3, sulfur has a smaller atomic radius than phosphorus
Sulfur has one more electron but still only fills up the same shell (3p) as phosphorus, so the radius is not affected.
But sulfur has one more proton than phosphorus - this does affect …
___ has a greater nuclear charge because of …
This pulls …
This means the …
In Period 3, sulfur has a smaller atomic radius than phosphorus.
Sulfur has one more electron but still only fills up the same shell (3p) as phosphorus, so the radius is not affected.
But sulfur has one more proton than phosphorus - this does affect the radius.
Sulfur has a greater nuclear charge because of having more protons.
This pulls the electrons closer.
This means the atomic radius is smaller.
Ionisation energy ___ along a period.
This is because the …
The attraction increases because the …
Ionisation energy increases along a period.
This is because the electrostatic attraction of each electron to the nucleus increases.
The attraction increases because the proton number increases.
In Period 3, chlorine has a greater nuclear charge than sulfur because …
So the electrostatic charge between electrons and the nucleus in chlorine will be ___
So the … is greater
In Period 3, chlorine has a greater nuclear charge than sulfur because it has a greater proton number.
So the electrostatic charge between electrons and the nucleus in chlorine will be greater.
So the ionisation energy is greater.
… decreases down a group.
This is because the …
The electrostatic attraction of …
Ionisation energy decreases down a group.
This is because the outer electron is further from the nucleus down the group.
The electrostatic attraction of the outer electron to the nucleus decreases down the group.
In Group 2, magnesium is below beryllium.
Magnesium fills up an extra electron shell than beryllium.
This means an electron is further from the nucleus in magnesium and so …
So the … of magnesium is lower than beryllium.
In Group 2, magnesium is below beryllium.
Magnesium fills up an extra electron shell than beryllium.
This means an electron is further from the nucleus in magnesium and so the electrostatic attraction is less.
So the ionisation energy of magnesium is lower than beryllium.
Across a period:
1 The ... increases 2 So the ... increases 3 ... between electrons and nucleus 4 Requires more energy to ...
Across a period:
1 The proton number increases 2 So the nuclear charge increases 3 Greater electrostatic attraction between electrons and nucleus 4 Requires more energy to remove an electron
The periodic atomic radii trend is that the atomic radius will …
The periodic atomic radii trend is that the atomic radius will decrease across a period.
Structure on mpt
For metals:
The greater the … the greater the melting point.
For covalent compounds:
Molecular solids have ___ melting points.
Giant covalent structures have relatively ___ melting points.
Structure on mpt
For metals:
The greater the number of valence electrons, the greater the melting point.
For covalent compounds:
Molecular solids have low melting points.
Giant covalent structures have relatively high melting points.
As you move along a period, you go from metals to giant covalent structures, to molecular solids.
The melting pints …
We will look at Period 3 to showcase this trend.
As you move along a period, you go from metals to giant covalent structures, to molecular solids.
Using our knowledge of melting points of different structures from the previous slide:
The melting points increase, peak sharply, and then decrease.
We will look at Period 3 to showcase this trend.
Na, Mg Al all have ___ structures.
… increase from Na to Al.
This is because each …
The … are greater, so …
Na, Mg Al all have metallic structures.
Melting point and boiling point increase from Na to Al.
This is because each element donates one more electron to the sea of free electrons.
The electrostatic attractions are greater, so the melting point rises.
Silicon has the highest ___
This is because …
To melt silicon, you must … and this …
Silicon has the highest melting point.
This is because it has a giant covalent structure.
To melt silicon, you must break strong covalent bonds, which requires a lot of energy.
