Properties of Matter - Periodicity Flashcards
What does reactivity with water mean?
The ability for an element to react with water
What are the trends with reactivity of water? Why is it like this?
Only groups 1 and groups 2 elements react with water, and the rest don’t.
What does metallic character mean?
Metallic character refers to the reactivity of a metal and is determined by whether or not it can give electrons away easily
What are the trends with metallic character?
Metallic character decreases left to right across a period (higher ionisation energy), it also increases from the top of the group to the bottom (lower ionisation energy = easier to remove)
What is electron affinity?
Electron affinity is the energy that is released when an electron is added to a neutral atom on a gaseous state
What are the trends with electron affinity?
Electron affinity increases from left to right across a period.
Electron affinity decreases from the top of the group to the bottom
What is electronegativity?
Electronegativity is the quantitative measure of the ability of an atom to attract electrons towards itself
What are the trends in electronegativity? Why is it like this?
Electronegativity increases left to right across a period because there is greater electrostatic attraction within the nucleus. The electrostatic attraction means that there is a stronger pull from the positively charged nucleus towards the electrons. Also, it would be easier to gain electrons than lose them once it hits a certain point.
Electronegativity decreases down a group because there are more shells which make the valence electrons further away from the nucleus. This means that there is greater nuclear shielding and less electrostatic attraction
What is first ionisation energy?
First ionisation energy refers to the amount of energy required to remove a valence electron from an atom in a gaseous state
What are the trends in first ionisation energy? Why is it like this?
The first ionisation energy increases from left to right across a period because the electrons are more attracted to the nucleus and the electron shells are being filled to max capacity
When going down a group, the first ionisation energy decreases. This is because there are more shells which make the valence electrons further away from the nucleus, because there is more nuclear shielding (shells between the valence electrons), there is less electrostatic attraction, and thus less ionisation energy
What is atomic radius?
The atomic radius refers to the distance between the centre of the nucleus and the outermost electron
What are the trends in atomic radii? Why is it like this?
Across a period, the atomic radius decreases as the effective nuclear charge and electrostatic interactions between the nucleus and electrons increase, causing them to be drawn in
Down a group, atomic radius increases as electrons are added to shells progressively
Therefore the alkali metals have the largest radius, whereas the noble gasses have the smallest radius
What are the trends in states of matter at room temperature? ( i think)
There are two liquids : Hg and Br (‘Hug the Bear’)
The noble gases, Nitrogen, Oxygen, Fluorine, Chlorine and Hydrogen are gases
The rest are solids
What area of the periodic table is the most reactive?
Bottom left, also top left, excluding noble gases
What is the name of group 1
Alkali metals
