compare the properties of metals and nonmetals on the basis of the following: a) malleability b) electrical conductivity c) thermal conductivity
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Metals[8]MetalloidsNonmetals[8]Form and structureColour
nearly all are shiny and grey-white
Cu, Cs, Au: shiny and golden[9]
shiny and grey-white[10]
most are colourless or dull red, yellow, green, or intermediate shades[11]
C, P, Se, I: shiny and grey-white
Reflectivity
intermediate to typically high[12][13]
intermediate[14][15]
zero or low (mostly)[16] to intermediate[17]
Form
almost all solid
Rb, Cs, Fr, Ga, Hg: liquid at/near stp[18][19][n 4]
all solid[10]
most are gases[21]
C, P, S, Se, I: solid; Br: liquid
Density
generally high, with some exceptions such as the alkali metals[22]
lower than nearby metals but higher than nearby nonmetals[23]
often low
Deformability (as a solid)
most are ductile and malleable
some are brittle (Cr, Mn, Ga, Ru, W, Os, Bi)[24][n 5]
brittle[27]
brittle, when solid
some (C, P, S, Se) have non-brittle forms[n 6]
Poisson's ratio[n 7]
low to high[n 8]
low to intermediate[n 9]
low to intermediate[n 10]
Crystalline structure at freezing point[47]
most are hexagonal or cubic
Ga, U, Np: orthorhombic; In, Sn, Pa: tetragonal; Sm, Hg, Bi: rhombohedral; Pu: monoclinic
B, As, Sb: rhombohedral
Si, Ge: cubic
Te: hexagonal
H, He, C, N, Se: hexagonal
O, F, Ne, P, Ar, Kr, Xe, Rn: cubic
S, Cl, Br, I: orthorhombic
Packing & coordination number
close-packed crystal structures[48]
high coordination numbers
relatively open crystal structures[49]
medium coordination numbers[50]
open structures[51]
low coordination numbers
Atomic radius
(calculated)[52]
intermediate to very large
112–298 pm, average 187
small to intermediate: B, Si, Ge, As, Sb, Te
87–123 pm, average 115.5 pm
very small to intermediate
31–120 pm, average 76.4 pm
Allotropes[53][n 11]
around half form allotropes
one (Sn) has a metalloid-like allotrope (grey Sn, which forms below 13.2 °C[54])
all or nearly all form allotropes
some (e.g. red B, yellow As) are more nonmetallic in nature
some form allotropes
some (e.g. graphitic C, black P, grey Se) are more metalloidal or metallic in nature
Electron-relatedPeriodic table block
s, p, d, f[55]
p[56]
s, p[56]
Outer s and p electrons
few in number (1–3)
except 0 (Pd); 4 (Sn, Pb, Fl); 5 (Bi); 6 (Po)
medium number (3–7)
high number (4–8)
except 1 (H); 2 (He)
Electron bands: (valence, conduction)
nearly all have substantial band overlap
Bi: has slight band overlap (semimetal)
most have narrow band gap (semiconductors)
As, Sb are semimetals
most have wide band gap (insulators)
C (graphite): a semimetal
P (black), Se, I: semiconductors
Electron behaviour
"free" electrons (facilitating electrical and thermal conductivity)
valence electrons less freely delocalized; considerable covalent bonding present[57]
nearly all are shiny and grey-white
Cu, Cs, Au: shiny and golden[9]
shiny and grey-white[10]
most are colourless or dull red, yellow, green, or intermediate shades[11]
C, P, Se, I: shiny and grey-white
Reflectivity
intermediate to typically high[12][13]
intermediate[14][15]
zero or low (mostly)[16] to intermediate[17]
Form
almost all solid
Rb, Cs, Fr, Ga, Hg: liquid at/near stp[18][19][n 4]
all solid[10]
most are gases[21]
C, P, S, Se, I: solid; Br: liquid
Density
generally high, with some exceptions such as the alkali metals[22]
lower than nearby metals but higher than nearby nonmetals[23]
often low
Deformability (as a solid)
most are ductile and malleable
some are brittle (Cr, Mn, Ga, Ru, W, Os, Bi)[24][n 5]
brittle[27]
brittle, when solid
some (C, P, S, Se) have non-brittle forms[n 6]
Poisson's ratio[n 7]
low to high[n 8]
low to intermediate[n 9]
low to intermediate[n 10]
Crystalline structure at freezing point[47]
most are hexagonal or cubic
Ga, U, Np: orthorhombic; In, Sn, Pa: tetragonal; Sm, Hg, Bi: rhombohedral; Pu: monoclinic
B, As, Sb: rhombohedral
Si, Ge: cubic
Te: hexagonal
H, He, C, N, Se: hexagonal
O, F, Ne, P, Ar, Kr, Xe, Rn: cubic
S, Cl, Br, I: orthorhombic
Packing & coordination number
close-packed crystal structures[48]
high coordination numbers
relatively open crystal structures[49]
medium coordination numbers[50]
open structures[51]
low coordination numbers
Atomic radius
(calculated)[52]
intermediate to very large
112–298 pm, average 187
small to intermediate: B, Si, Ge, As, Sb, Te
87–123 pm, average 115.5 pm
very small to intermediate
31–120 pm, average 76.4 pm
Allotropes[53][n 11]
around half form allotropes
one (Sn) has a metalloid-like allotrope (grey Sn, which forms below 13.2 °C[54])
all or nearly all form allotropes
some (e.g. red B, yellow As) are more nonmetallic in nature
some form allotropes
some (e.g. graphitic C, black P, grey Se) are more metalloidal or metallic in nature
Electron-relatedPeriodic table block
s, p, d, f[55]
p[56]
s, p[56]
Outer s and p electrons
few in number (1–3)
except 0 (Pd); 4 (Sn, Pb, Fl); 5 (Bi); 6 (Po)
medium number (3–7)
high number (4–8)
except 1 (H); 2 (He)
Electron bands: (valence, conduction)
nearly all have substantial band overlap
Bi: has slight band overlap (semimetal)
most have narrow band gap (semiconductors)
As, Sb are semimetals
most have wide band gap (insulators)
C (graphite): a semimetal
P (black), Se, I: semiconductors
Electron behaviour
"free" electrons (facilitating electrical and thermal conductivity)
valence electrons less freely delocalized; considerable covalent bonding present[57]
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Metal is malleable but non metal is not malleable.
Metal free ions for conduct electricity , but non metal not conduct.
metals, heat conductivity is primarily due to free electrons. . But non metal have poor conductivity
Metal free ions for conduct electricity , but non metal not conduct.
metals, heat conductivity is primarily due to free electrons. . But non metal have poor conductivity
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