• Elements in the periodic table are arranged in order of increasing atomic number and placed in vertical columns (groups) and horizontal rows (periods)
• The elements across the periods show?repeating patterns?in chemical and physical properties
• This is called?periodicity

All elements are arranged in the order of increasing atomic number from left to right

Atomic radius

• The?atomic radius?is the distance between the nucleus and the outermost electron of an atom
• The atomic radius is measured by taking two atoms of the same element, measuring the distance between their nuclei and then halving this distance
• In?metals?this is also called the?metallic radius?and in?non-metals, the?covalent radius

The atomic radius gives a measure of the size of atoms

Atomic radii of Period 3 elements table

The graph shows a decrease in atomic radii of Period 3 elements across the period

• Across the period, the atomic radii decrease
• This is because the number of protons (the nuclear charge) and the number of?electrons?increases by one every time you go an element to the right
• The elements in a period all have the same number of shells (so the?shielding effect?is the same)
• This means that as you go across the period the nucleus attracts the electrons more?strongly pulling them closer?to the nucleus
• Because of this, the atomic radius (and thus the size of the atoms)?decreases?across the period

The diagram shows that across Period 3, the elements gain extra electrons in the same principal quantum shell

Ionic radius

• The?ionic radius?is the distance between the nucleus and the outermost electron of an ion
• Metals produce positively charged ions (cations) whereas nonmetals produce negatively charged ions (anions)
• The?cations?have lost their valence electrons which causes them to be much?smaller?than their parent atoms
• Because there are less electrons, this also means that there is less?shielding?of the outer electrons
• Going across the period from Na+?to Si4+?the ions get?smaller?due to the?increasing?nuclear charge?attracting the outer electrons in the?second principal quantum shell?nucleus (which has an increasing atomic number)
• The?anions?are larger than their original parent atoms because each atom has gained one or more electrons in their?third principal quantum shell
• This increases the repulsion between electrons, while the?nuclear charge?is still the same, causing the electron cloud to spread out
• Going across P3-?to Cl-?the ionic radii?decreases?as the nuclear charge increases across the period and fewer electrons are gained by the atoms (P gains 3 electrons, S 2 electrons and Cl 1 electron)

Ionic radii of ions of Period 3 elements table

Ions of Period 3 elements with increasing positive charge (metals) and increasing of outer electrons across the period

The diagram shows the electron configuration of the ions of Period 3 elements and their relative sizes

Melting point

Melting points of the elements across Period 3 table

Ions of Period 3 elements with increasing positive charge (metals) and increasing of outer electrons across the period

• A general increase in?melting point?for the Period 3 elements up to silicon is observed
• Silicon?has the highest?melting point
• After the Si element the melting points of the elements?decreases?significantly

Electrical conductivity

• Electrical conductivity?refers to how well a substance can conduct?electricity
• Unlike the melting points, the electrical conductivity of the Period 3 elements shows a clear trend
• Going across the period, the electrical conductivity of the elements?decreases?significantly

Trends in electrical conductivity across Period 3 table