Use electron configurations to explain why copper is paramagnetic while its 1+ i

ID: 498206 • Letter: U

Question

Use electron configurations to explain why copper is paramagnetic while its 1+ ion is not.

Match the words in the left column to the appropriate blanks in the sentences on the right

These are the choices:

one unpaired electron

several unpaired electrons

only paired electrons

This is the question

The copper cation (Cu+) contains( ) in the( ) orbitals and is diamagnetic.

Copper (Cu) contains( ) in the( ) orbital and is paramagnetic.

These are the choices:

one unpaired electron

several unpaired electrons

only paired electrons

This is the question

The copper cation (Cu+) contains( ) in the( ) orbitals and is diamagnetic.

Copper (Cu) contains( ) in the( ) orbital and is paramagnetic.

Electronic configuration of copper(Cu) = [Ar] 3d10 4s1

Electronic configuration of copper(Cu+1) = [Ar] 3d10

Copper has odd number of electrons - 29, i. e. it has one unpaired electron, which causes paramagnetic properties.

Copper ion Cu+ has even number of electrons - 28, i. e. it has no unpaired electron, which causes diamagnetic (= no magnetic) properties.

The copper cation (Cu+) contains( no unpaired electron) in the( 3d) orbitals and is diamagnetic.

copper (Cu) contains( single unpaired electron ) in the( 4s) orbital and is paramagnetic.

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