Periodic Table Flashcards
Periodicity
The variation of properties of elements in a regular pattern both down the groups and across the periods.
Electrical & Thermal Conductivities Trend
Decreases across the period
Increase down the group
Melting & Boiling Point Trend
Hint: 5 points of both non metals and metals combined individually and in groups
Depends on the strength of the forces which exists between the atoms which make up the elements.
• The m.p of metallic elements increase from left-right//decreases from right-left.
• The m.p of non-metallic elements increase from right-left//decreases from left-right.
• Within a group, the m.p & b.p of metallic elements decrease down the group.
• Within a group, the m.p & b.p of non-metallic elements increase down the group.
Atomic Radius
Hint: Definition & Trend
Half the distance between the nuclei of identical neighboring atoms in the solid form of an element.
• Decreases across the period, increases down the group
Ionic Radius Trend
• Decreases across the period till group 3, peaks at group 4, then decreases again.
It increases down the group.
Ionization Energy Trend & Affecting Factors
• It increases across a period & decreases down the group.
Affected by;
1. Size of positive nuclear charge
2. The screening effect of inner electrons
3. The distance of the outermost electron from the nucleus.
What increases the electron attracting power of the atom.?
Atomic radius and nuclear charge
Electronegativity
Hint: Trend & the most electronegative//electropositive element
Trend of nuclear charge & atomic radius
• It increases across a period, decreases down the group.
• As we move across the period, the nuclear charge increases & the atomic radius decreases.
The most electronegative element (the least electropositive element) is Fluorine
The least electronegative (the most electropositive element) is Caesium
Electron Affinity
Energy released when a gaseous atom gains an electron to form a gaseous negative ion.
• It increases across the period.
• With decrease of atomic radii, E.A increases across the period.
• With increase of atomic radii, E.A decreases down the group.
Group 1 elements
Hint: 6 examples
Number of valence electron
Ionization Ability
Reducing Property Trend
Reducing property
Electronegativity
Electricity Conductivity
Reaction in water
Reaction of oxides in water
Effect of heating their trioxonitrate(V) salts
•Lithium, Sodium, Potassium, Rubidium, Caesium & Francium.
• They are univalent (having 1 valence electron).
• By donating electrons, they ionize readily to form positive ions & electrovalent compounds.
• The reducing property decreases down the group; the oxidizing property increases down the group.
• They are good reducing agents(they easily donate electrons)
• They are very electropositive and are good conductors of electricity
• Reacts with cold water vigorously to liberate hydrogen & form alkalis
• Their oxides dissolve in water to form very strong alkalis
• On heating their trioxonitrate(V)salts decompose to give O2 and dioxonitrate(III) salts.
Group 2 elements
Hint: 6 examples
Number of valence electron
Reducing Property
Ionization Ability
Calcium with water
Magnesium with steam
Effects On Calcium & Magnesium in both above reactions respectively
Reaction of oxides in water
Effect of heating their trioxonitrate(V) salts
Effect of heating their trioxocarbonate(V) salts
Beryllium, Magnesium, Calcium, Strontium, Barium, Radium.
They are divalent (2 valence electrons)
They are reducing in nature
They form electrovalent compounds
Calcium reacts very slowly with cold water
Magnesium reacts with steam only
Calcium & Magnesium both liberate H2 but Ca forms a hydroxide, Mg forms an oxide
-MgO is insoluble in water; CaO dissolves sparingly to form Ca(OH)2 in water.
On heating, their trioxonitrate(V) salts decompose to give the oxides, oxygen and brown gas; Nitrogen(IV)oxide
On heating, their trioxocarbonate(IV) salt decompose to give oxides and CO2
Group 3 elements
Hint: 5 examples
Number of valence electron and Reducing property
Ionization Ability of Al
Nature of the hydroxide and oxide of Al
Decomposition of trioxonitrate(V) salt of Al
Existence of trioxocarbonate(IV) salt of Al
Semimetal Boron & Metals Aluminium, Gallium, Indium, Thallium
They are trivalent and are reducing in nature
Al forms electrovalent compounds and also reacts with steam above 600°C to liberate H2
Both hydroxide and oxide of Al are amphoteric(forming complex and normal salts with acids & alkalis)
Aluminium trioxonitrate(V) salt decomposes to give the oxide, O2 and Nitrogen (IV) oxide
Aluminium trioxocarbonate(IV)salt does not exist
Group 4 elements
Hint: 5 examples
Number of valence electron
Ionization Ability
Metal Change Trend
Electronegativity Trend
Oxidation States
Stability trend of +2 & +4 compounds
Type of compounds formed by C & Si with H2
Hydrides of carbon
Reaction of Carbon in water
Reaction of Si & Sn with steam
Carbon, Silicon, Germanium, Tin, Lead
They are tetravalent; they tend to form covalent compounds
The elements change from non-metallic to metallic down the group
The electronegativity decreases down the group
Exhibits 2 oxidation states; +2 & +4
The stability of +2 compounds increases down and that of +4 compounds decreases down the group
Carbon & Silicon form covalent compounds with H2
The hydrides of carbon are known as Hydrocarbons
Carbon does not react with water in any form
Si & Sn react with steam at red hot to form +4 state oxides and hydrogen.
Group 5 elements
Hint: 5 examples
The kind of block elements they are and the arrangement of their valence electrons in its shell
Common valencies of Nitrogen & Phosphorus
Reduction Ability
Oxide formation
Hydride formation
Nitrogen, Phosphorus, Arsenic, Antimony, Bismuth
They are p-block elements(possess s2p3 in their valence shell)
Both Nitrogen & Phosphorus are non metals of two common valencies 3 & 5
They are both electron acceptors
They both form several acidic oxides
They are both capable of forming similar hydrides
Group 6 elements
Hint: 5 examples
The kind of block elements they are & the arrangement of their valence electrons in their shell
Whether or not Oxygen and Sulphur are non-metals
Reducing Property
Combination of Oxygen and Sulphur with Hydrogen
Solubility of Oxygen in water
Solubility of Sulphur in water
Oxygen, Sulphur, Selenium, Tellurium, Polonium
They are p-block elements(possess s2p4 in their valence shell)
Both Oxygen and Sulphur are non-metals & electron acceptors and are oxidizing in nature as they combine directly with H2 to yield H2O & H2S respectively
Oxygen is slightly soluble in water
Sulphur is insoluble in water
