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Talja [164]
3 years ago
14

Why are the transition metals able to show different properties like varying color and paramagnetism ?

Chemistry
1 answer:
Naya [18.7K]3 years ago
4 0

Answer:

Colors of transition metal compounds are due to two types of electronic transitions. Due to the presence of unpaired d electrons, transition metals can form paramagnetic compounds. Transition metals are conductors of electricity, possess high density and high melting and boiling points.

Explanation:

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it is formed by covalent bonds. the oxygen atom shares one elctron with each chlorine atom, forming single covalent bonds ( cl — o — cl )

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Which body part MOST LIKELY formed this fossil?<br> blood<br> B<br> bones<br> fur<br> D<br> skin
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Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or
Ahat [919]

Answer :

Oxidation number or oxidation state : It represent the number of electrons lost or gained by the atoms of an element in a compound.

Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

Rules for Oxidation Numbers are :

  • The oxidation number of a free element is always zero.
  • The oxidation number of a monatomic ion equals the charge of the ion.
  • The oxidation number of  Hydrogen (H)  is +1, but it is -1 in when combined with less electronegative elements.
  • The oxidation number of  oxygen (O)  in compounds is usually -2.
  • The oxidation number of a Group 17 element in a binary compound is -1.
  • The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
  • The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

Now we have to determine the oxidation state of the elements in the compound.

(a) H_2SO_4

Let the oxidation state of 'S' be, 'x'

2(+1)+x+4(-2)=0\\\\x=+6

Hence, the oxidation state of 'S' is, (+6)

(b) Ca(OH)_2

Let the oxidation state of 'Ca' be, 'x'

x+2(-2+1)=0\\\\x=+2

Hence, the oxidation state of 'Ca' is, (+2)

(c) BrOH

Let the oxidation state of 'Br' be, 'x'

x+(-2)+1=0\\\\x=+1

Hence, the oxidation state of 'Br' is, (+1)

(d) ClNO_2

Let the oxidation state of 'N' be, 'x'

-1+x+2(-2)=0\\\\x=+5

Hence, the oxidation state of 'N' is, (+5)

(e) TiCl_4

Let the oxidation state of 'Ti' be, 'x'

x+4(-1)=0\\\\x=+4

Hence, the oxidation state of 'Ti' is, (+4)

(f) NaH

Let the oxidation state of 'Na' be, 'x'

x+(-1)=0\\\\x=+1

Hence, the oxidation state of 'Na' is, (+1)

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3 years ago
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