Properties Of Elemements and trends on the Periodic Table Flashcards
What are the main properties to focus?
Atomic radius -how big the atoms are
Ionisation energy-the amount of energy needed to remove electrons
Electronegativity-how much attraction an atom is an element has for a pair of covalently bonded electrons
What is group 7
The halogens
Group 0 is…
The noble gases
What does the radius of an atom dependent on
The number of protons in the nucleus
The number of shells
What is the trend down a group in atomic radius
With each element you have one extra shell o electrons. This means the atoms are getting bigger and bigger with that extra shell, therefore the atomic radius increases down a group
Why does the elements across a period increase
The number of protons increase as do the number of electrons but the electrons are filling into the same shell. The increasing number of protons causes an increasing attraction from the nucleus which pulls the shells closer and closer causing the atomic radius to decrease across a period
What is the ionisation energy
Refers directly to the energy needed to remove electrons.
For some elements ionisation is quite easy and the would have low ionisation energy.
Others it is easy to remove an electron and hence have the higher ionisation energy
Ionisation energy of an element depends on
The atomic radius
The nuclear charge
The number of shells
What is the clear trend down a group referring to ionisation energy
When you go down a group both the atomic radius and amount of shells increase meaning the outer shell electrons are feeling less of the attractive force from the nucleus so it can be lost more easily. This results in the ionisation decreasing down a group
What is the clear trend across a period referring to ionisation
The nuclear charge is increasing and the atomic radius is getting smaller because the outer shell gets pulled closer to the nucleus. This means the outer electrons are feeling a stronger attraction form the nucleus making it harder for them to be lost. Making the ionisation increase across a period
What are the three ways in which the periodic table is arranged
In vertical columns called groups
In horizontal rows called periods
Into 4 blocks
What does the nucleus consist of
Positively charged protons,neutrons with no charge negatively charged electrons
What is the atom mass and what is the mass number
The larger number is the mass number or atomic and the bottom number is the atomic number
How can we just get the mass number
The total amount of protons and neutrons
What gives us the atomic number
Number of protons only
What is an isotope
Atoms of the same element with a different number of neutrons
Give an example of an isotope
The most common had 6 protons 6 elections and 6 neutrons
What is isotopic abundance
The relative amount of each isotope found in a sample of a given element
What is the relative atomic mass
The mean mass of an atom of an element compared to 1/12th of the mass of the carbon-12 isotope
How can we Calculate the relative mass
RAM = sum of (isotopic abundance x mass number )/100
What is the most electronegative element on the period table
FLUORINE
Why is fluorine the most electronegative element
This means that a fluorine atom in a covenant bond will have the strongest attraction for the electrons in that bond
Name some trends and properties in the S-Block
Elements in the s-block are all metals
Ionisation energy decreases down both groups,but group 2 is higher than group of
Atomic radius increases down both groups but group 2 is smaller than group 1
Trends and properties in the d-block
D-block elements are all metals as so with the s-block they have the general properties you associate with metals
