Chlorine (Cl) is much more electronegative than silicon (Si). This means that chlorine exerts a much stronger "pull" on the electrons in a perchloric acid molecule than silicon does in a silicic acid molecule. The stronger pull makes it easier for a hydrogen ion (H+) to break away. The greater the degree of dissociation the stronger the acid.
Perchloric acid dissociates completely in water, thus marking it as a strong acid. Silicic acid only dissociates partially, thus marking as a weak acid.
Silicic acid
H2SiO3
SiO2 is a covalent network compound known as Silicon dioxide.
Most acids are compounds of nonmetals. But some also contain metalloids such as silicon (in silicic acid H2SiO3). A few contain metals such as chromium (chromic acid, H2CrO4) and maganese (permanganic acid, HMnO4)
(1) Both boron and silicon are typical non-metals, having high m.pt. b.pt nearly same densities (B=2.35gml-1 S=2.34 g//ml). low atomic volumes and bad conductor of current. However both are used as semiconductors. (2) Both of them do not form cation and form only covalent compounds. (3) Both exists in amorphous and crystalline state and exhibit allotropy. (4) Both possess closer electronegativity values (B=2.0; Si=1.8). (5) Both form numerous volatile hydrides which spontaneously catch fire on exposure to air and are easily hydrolysed. (6) The chlorides of both are liquid, fume in most air and readily hydrolysed by water. BCl3 + 3H2O → B(OH)3 + 3HCl SiCl4 + H2O → Si(OH)4 + 4HCl (7) Both form weak acids like H3BO3 and H2SiO3. (8) Both form binary compounds with several metals to give borides and silicide. These borides and silicide react with H3PO4 to give mixture of boranes and silanes. 3Mg+2B → Mg3B2; Mg3B2 + H3PO4 → Mixture of boranes (Magnesium boride) 2Mg + Si → Mg2Si ; Mg2Si + H3PO4 → Mixture of silanes (magnesium silicide) (9) The carbides of both Boron and silicon (B4C and SiC) are very hard and used as abrasive. (10) Oxides of both are acidic and can be reduced by limited amount of Mg In excess of Mg boride and silicide are formed. B2O3 + 3Mg → 3MgO + 2B ; SiO2 + 2Mg → 2MgO + Si (11) Both the metals and their oxides are readily soluble in alkalies. 2B + 6NaOH → 2Na3BO3 + 3H2 (borate) Si + 2NaOH + H2O → Na2SiO3 + 2H2 (silicate) B2O3 + 6NaOH → 2Na3BO3 + 3H2O SiO2 + 2NaOH → Na2SiO3 + H2O Both borates and silicates have tetrahedral structural units and respectively. Boro silicates are known in which boron replaces silicon in the three dimensional lattice. Boron can however form planar BO3 units. (12) Acids of both these elements form volatile esters on heating with alcohol in presence of conc. H2SO4. B(OH)3 + 3ROH → B(OR)3 + 3H2O Si(OH)4 + 4ROH → Si(OR)4 + 4H2O
Silicic acid
The chemical formula of silicon dioxide is SiO2.
H2SiO3
There is no such compound. The compound closest to H4SiO3 you mentioned, is H2SiO3, metasilicic acid.
SiO2 is a covalent network compound known as Silicon dioxide.
Adding one hydrogen to silicate will give you [HSiO3]-1. In order to get an aqueous form of hydrogen silicate, two hydrogens must be added, giving H2SiO3.
Most acids are compounds of nonmetals. But some also contain metalloids such as silicon (in silicic acid H2SiO3). A few contain metals such as chromium (chromic acid, H2CrO4) and maganese (permanganic acid, HMnO4)
(1) Both boron and silicon are typical non-metals, having high m.pt. b.pt nearly same densities (B=2.35gml-1 S=2.34 g//ml). low atomic volumes and bad conductor of current. However both are used as semiconductors. (2) Both of them do not form cation and form only covalent compounds. (3) Both exists in amorphous and crystalline state and exhibit allotropy. (4) Both possess closer electronegativity values (B=2.0; Si=1.8). (5) Both form numerous volatile hydrides which spontaneously catch fire on exposure to air and are easily hydrolysed. (6) The chlorides of both are liquid, fume in most air and readily hydrolysed by water. BCl3 + 3H2O → B(OH)3 + 3HCl SiCl4 + H2O → Si(OH)4 + 4HCl (7) Both form weak acids like H3BO3 and H2SiO3. (8) Both form binary compounds with several metals to give borides and silicide. These borides and silicide react with H3PO4 to give mixture of boranes and silanes. 3Mg+2B → Mg3B2; Mg3B2 + H3PO4 → Mixture of boranes (Magnesium boride) 2Mg + Si → Mg2Si ; Mg2Si + H3PO4 → Mixture of silanes (magnesium silicide) (9) The carbides of both Boron and silicon (B4C and SiC) are very hard and used as abrasive. (10) Oxides of both are acidic and can be reduced by limited amount of Mg In excess of Mg boride and silicide are formed. B2O3 + 3Mg → 3MgO + 2B ; SiO2 + 2Mg → 2MgO + Si (11) Both the metals and their oxides are readily soluble in alkalies. 2B + 6NaOH → 2Na3BO3 + 3H2 (borate) Si + 2NaOH + H2O → Na2SiO3 + 2H2 (silicate) B2O3 + 6NaOH → 2Na3BO3 + 3H2O SiO2 + 2NaOH → Na2SiO3 + H2O Both borates and silicates have tetrahedral structural units and respectively. Boro silicates are known in which boron replaces silicon in the three dimensional lattice. Boron can however form planar BO3 units. (12) Acids of both these elements form volatile esters on heating with alcohol in presence of conc. H2SO4. B(OH)3 + 3ROH → B(OR)3 + 3H2O Si(OH)4 + 4ROH → Si(OR)4 + 4H2O
Due to its small size and similar charge/mass ratio, boron differs from other group 13 members, but it resembles closely with silicon, the second element of group 14 to exhibit diagonal relationship. Some important similarities between boron and silicon are given below, (1) Both boron and silicon are typical non-metals, having high m.pt. b.pt nearly same densities (B=2.35gml-1 S=2.34 g//ml). low atomic volumes and bad conductor of current. However both are used as semiconductors. (2) Both of them do not form cation and form only covalent compounds. (3) Both exists in amorphous and crystalline state and exhibit allotropy. (4) Both possess closer electronegativity values (B=2.0; Si=1.8). (5) Both form numerous volatile hydrides which spontaneously catch fire on exposure to air and are easily hydrolysed. (6) The chlorides of both are liquid, fume in most air and readily hydrolysed by water. BCl3 + 3H2O → B(OH)3 + 3HCl SiCl4 + H2O → Si(OH)4 + 4HCl (7) Both form weak acids like H3BO3 and H2SiO3. (8) Both form binary compounds with several metals to give borides and silicide. These borides and silicide react with H3PO4 to give mixture of boranes and silanes. 3Mg+2B → Mg3B2; Mg3B2 + H3PO4 → Mixture of boranes (Magnesium boride) 2Mg + Si → Mg2Si ; Mg2Si + H3PO4 → Mixture of silanes (magnesium silicide) (9) The carbides of both Boron and silicon (B4C and SiC) are very hard and used as abrasive. (10) Oxides of both are acidic and can be reduced by limited amount of Mg In excess of Mg boride and silicide are formed. B2O3 + 3Mg → 3MgO + 2B ; SiO2 + 2Mg → 2MgO + Si (11) Both the metals and their oxides are readily soluble in alkalies. 2B + 6NaOH → 2Na3BO3 + 3H2 (borate) Si + 2NaOH + H2O → Na2SiO3 + 2H2 (silicate) B2O3 + 6NaOH → 2Na3BO3 + 3H2O SiO2 + 2NaOH → Na2SiO3 + H2O Both borates and silicates have tetrahedral structural units and respectively. Boro silicates are known in which boron replaces silicon in the three dimensional lattice. Boron can however form planar BO3 units. (12) Acids of both these elements form volatile esters on heating with alcohol in presence of conc. H2SO4. B(OH)3 + 3ROH → B(OR)3 + 3H2O Si(OH)4 + 4ROH → Si(OR)4 + 4H2O
::S=Si=S:: = are double bonds : are single lone pairs