The website has the complete lesson note for all the subjects in secondary school but this piece showcases the SS2 Chemistry Lesson Note on Periodic Properties. You can use the website search button to filter out the subject of interest to you.
CLICK HERE to download the complete Document: DOWNLOAD HERE
TOPIC: PERIODIC TABLE
CONTENT:
PERIOD 1 AND 2: PERIODIC PROPERTIES. Some properties of the atom change along a group or across a period on the periodic table. Atomic radius which is measured of the size is one of such properties. The orbiting electrons in an atom are best represented by an electron cloud which has no distinct limit as the size of an action cannot be defined easily.
This is because going down any group on the periodic table the number of valence electrons remains constant while the shells increase in size (radius) despite increase in nuclear charge. The atomic radius of potassium is greater than that of Sodium. The atomic radius of caesium is greater than that of rubidium.
Across a period, electrons are added to orbitals in the same shell, all the valence electrons are therefore at the same energy level. As atomic number increase the positive charge of the nucleus increases giving rise to greater attraction between the positive nucleus and negative electrons. This is turn result in contraction of the electrons cloud resulting in a smaller atom. Atomic radii therefore decrease across a given period on the periodic table.
A negative ion (anion) is bigger than the corresponding non- metal atom because the effective nuclear charge is reduced.
As we move across the second short period, the cationic radii decrease from sodium to aluminium while the anionic radii increase from phosphorous to chlorine.
K + e– → K+
The energy required to do this is called ionization energy or ionization potential.
First ionization energy of an element is the energy needed to remove one mole of electron(s) from one mole of atoms in the gaseous state. It is expressed in kilo- joules per mole of atoms ionized.
First ionization energy increase across the period with noble gases having the highest. As we go down, he the group, the value of first ionization energy decreases.
FIRST IONIZATION ENERGIES OF ALKALI METALS
Element | LI | Na | K | Rb | Cs |
First ionization energy KJMOL-1 | 520 | 500 | 420 | 400 | 380 |
FIRST IONIZATION ENERGIES OF THE ELEMENTS IN THE THIRD PERIOD OF THE PERIODIC TABLE
Element | Na | Mg | Al | Si | P | S | Cl | Ar |
First ionization energy KJMOL-1 | 496 | 737 | 577 | 786 | 1012 | 999 | 1255 | 1521 |
Three factors that affect the ionization potential of an atom
Ionization potential of an atom is affected by.
Moving from left to right across a period, there is a general rise in the first ionization energy. This is due to the fact that the nuclear charge is increasing across the period. This in turn causes a decrease in atomic radius that is a decrease in the distance of the outermost electrons from the nucleus. The screening effect is almost the same across the period. Down a group of the periodic table, ionization energy decreases because the nuclear charge on the outermost electron is reduced. The outermost electron are properly shielded from the effect of nuclear charge
Click on the Downloadable Button to get the FULL NOTE
Veterinary medicine is the branch of medicine that deals with the prevention, diagnosis, and treatment…
Anthropology is the scientific study of human beings and their cultures. It encompasses a wide…
Sociology is the scientific study of human society, culture, and behavior. It examines the social…
Social Work is a profession dedicated to helping individuals, families, and communities to cope with…
Religious studies is an academic discipline that explores the beliefs, practices, and history of various…
Public administration is the field of study and practice that focuses on the organization and…