Some elements like iron, cobalt, and holmium make very good ...

[JGIBBSON]

Some elements like iron, cobalt, and holmium make very good natural magnets. Which of the following statements best describes why?
  a.Selection rules for multi-electron atoms tend to maximize electron spin and orbital angular momentum.
  b.Atoms in the crystalline structure of the solid metal tend to antialign their spin and orbital angular momentum.
  c.Large numbers of paired electron spins are essential to good magnets.
  d.The filled s shells with high n and paired electrons create larger atomic radii and therefore the electrons can contribute more to the magnetic field.

Question 2

The anomalous Zeeman effect is different from the normal Zeeman effect because
 

 

a.to observe the normal Zeeman effect, the atom must be in a magnetic field, while the anomalous Zeeman effect depends on the external electric field.
  b.the split of energy levels from the anomalous Zeeman effect depends on the Lande g factor and the split from the normal Zeeman effect depends on the gyromagnetic ratio.
  c.the split of energy levels from the anomalous Zeeman effect depends on the intrinsic spin quantum number and the split from the normal Zeeman effect depends on the magnetic quantum number.
  d.the total angular momentum vector only precesses in the anomalous Zeeman effect.

  e. only the normal Zeeman effect depends on the angular momentum L.
 

[rachel]

Answer to Question 1

a.
Hund's rules state for atoms with less than filled subshells, the spin and orbital angular momentum should be maximized (in that order). This means that the magnetic dipoles of the atoms in solid iron, cobalt, and holmium can align and add to form large total magnetic moments. The key to these atoms is the large number of unpaired spins.

Answer to Question 2

c,
he anomalous Zeeman effect depends on the intrinsic spin of the electron, while the normal Zeeman effect is primarily based on the magnetic moment of the angular momentum of the electron

[JGIBBSON]

TY

[rachel]

You're welcome