Examples of main group elements include helium, lithium, boron, carbon, nitrogen, oxygen, fluorine, and neon. Elements that are not main group elements are the transition metals (such as titanium, copper, and gold), the lanthanides (such as lanthanum and erbium), and the actinides (such as actinium and plutonium).

There are two basic types of acids organic and inorganic acids. Inorganic acids are sometimes referred to as mineral acids. As a group, organic acids are generally not as strong as inorganic acids. The main difference between the two is the presence of carbon in the compound; inorganic acids do not contain carbon.

The main group includes the elements (except hydrogen, which is sometimes not included) in groups 1 and 2 (s-block), and groups 13 to 18 (p-block). Main-group elements (with some of the lighter transition metals) are the most abundant elements on earth, in the solar system, and in the universe.

Its oxide was first isolated from rare-earth ores by Cleve in 1878. The element’s name comes from Holmia, the Latin name for the city of Stockholm. Elemental holmium is a relatively soft and malleable silvery-white metal….

Properties of Hydrogen Hydrogen is a nonmetal and is placed above group in the periodic table because it has ns1 electron configuration like the alkali metals. Because hydrogen is a nonmetal and forms H- (hydride anions), it is sometimes placed above the halogens in the periodic table.

Hydrogen as a halogen? Hydrogen, like the halogens, has one electron short of a complete outer shell and can form H- ions like Cl- and therefore forms ionic compounds with reactive metals – NaH similar in structure to NaCl. Hydrogen also exists as a diatomic gas like fluorine and chlorine.

Hydrogen is not an alkali metal itself, but has some similar properties due to its simple one proton (loctated in the nucleus), one electron arrangement. The lone electron exists in a s -orbital around the nucleus. Cesium Orbitals. This one electron is very easily removed during chemical reactions.

s-block elements are the elements found in Group 1 and Group 2 on the periodic table. Hydrogen is a nonmetal grouped with the alkali metals because it has one electron in its valence shell.

S block comprises 14 elements: hydrogen (H), lithium (Li), helium (He), sodium (Na), beryllium (Be), potassium (K), magnesium (Mg), rubidium (Rb), calcium (Ca), cesium (Cs), strontium (Sr), francium (Fr), barium (Ba), and radium (Ra).

Why does the s-block span two groups of elements? Because s orbitals hold two electrons at most. Because the three p orbitals can hold a maximum of six electrons.

The s block has two columns corresponding to one of the s orbitals holding a maximum of two electrons. The p block has six columns corresponding to the three p orbitals with two electrons each. The lettered group number of a main-group element is equal to the number of valence electrons for that element.

P-block elements are unified by the fact that their valence electrons (outermost electrons) are in the p orbital. The p orbital can hold a maximum of six electrons, hence why there are six columns in the p-block. Elements in column 3A, the first column of the p-block, have one valence electron.

The s-block and p-block elements are so called because their valence electrons are in an s orbital or p orbital respectively. They are also called Typical Elements to distinguish them from the transition and inner transition series.

The p-block contains groups 13, 14, 15, 16, 17, and 18, with the exception of Helium.

The p-block elements are found on the right side of the periodic table. They include the boron, carbon, nitrogen, oxygen and flourine families in addition to the noble gases. The noble gases have full p-orbital’s and are nonreactive.

D block elements are the elements which can be found from the third group to the twelfth group of the modern periodic table. The valence electrons of these elements fall under the d orbital. D block elements are also referred to as transition elements or transition metals.

transition metals

D-block elements it includes are Lutetium (Lu), Hafnium (Hf), Tantalum (Ta), Tungsten (W), Rhenium (Re), Osmium (Os), Iridium (Ir), Platinum (Pt), Gold (Au) and Mercury (Hg). Mnemonic for Period 6: L(u)a HafTa Warna Reh Us(Os) Irritating Popat ke saath Aur Hoj(g)a pagal.

The d-block elements are called transition elements because they exhibit transitional behaviour between s-block and p-block elements. Their properties are transitional between highly reactive metallic elements of s-block which are ionic in nature and the elements of p-block which are covalent in nature.

When visible light falls on a transition metal compound or ion, the unpaired electrons present in the lower energe d-orbital get promoted to high energy d-orbitals, called d-d transition, due to the absorption of visible light. Therefore, transmitted light shows some colour complementary to the absorbed colour.

For example, if the electrons in an octahedral metal complex can absorb green light and get promoted from the dyz orbital to the dz2 orbital, the compound will reflect all the colours except green. Hence, the complementary colour of green will be observed as the colour of the compound.

Answer. Answer: Transition metals and their compounds function as catalysts either because of their ability to change oxidation state or, in the case of the metals, to adsorb other substances on to their surface and activate them in the process.

the colour of transition elements is due to the presence of unpaired electrons. cu+ is colourless as its outermost configuration is 3d10 …so there are no unpaired electrons which causes the colour .

Cu+ has completely filled orbital: [Noble gas] 3d10, where as Cu2+ has partially filled orbital : [Noble gas]3d9. Hence Cu+ is colourless but Cu2+ is coloured.

The copper atom is in the +1 oxidation state in which it has a full (totally occupied) set of ‘d’ orbitals. There can be no transitions between the non-degenerate orbitals and so there can be no frequencies of light absorbed due to d-d transitions.

Why? Ans. Cu2+ (3d 9 4s 0) has one unpaired electron in d-subshell which absorbs radiation in visible region resulting in d-d transition and hence Cu2+ salts are coloured. No radiation is absorbed for d- d transition and hence Zn2+ salts are colourless.

Copper has an unpared electron which acts as a F centre and allows electron transition in visible region importing color while Zn+2 is having no unpaired electrons hence colorless.