8.3.2 Transition Metals and Nonmetals

Question 1

Transition Metals and Nonmetals

Answer 1

• Understanding the periodic table is imperative to understanding the reactivity of elements.
• Transition Metals are characterized by partially filled d orbitals.
• Rare earth elements are electron rich and they tend to lose electrons in reactions

Question 2

note

Answer 2

• Elements in the same group have similar reactivity.
• Each family reacts characteristically with hydrogen (e.g. HF, H 2 O, NH 3 , CH 4 ).
• When transition metals form cations, the s electrons are lost before the d electrons.
• Transition metals are generally harder and have higher
  melting points than the alkali metals and the alkaline earth metals.
• Like the transition metals, the rare earths are very electron rich and they tend to lose electrons in reactions.
• The s orbital fills before the f orbital; but when rare earths form cations, the s electrons are again the first to be lost.
• The noble gases are relatively unreactive, but become more reactive as you move down the group on the periodic table.

Question 3

Which of the following is the correct electron configuration for titanium(II) cation?

Answer 3

[Ar] 3d2

Question 4

The rare earth or inner transition metals often have two s electrons and one d electron as well as a variable number of electrons in the f energy sublevel. As a result of this curious behavior, the rare earth elements often form cations with what charge?

Answer 4

3+

Question 5

Which noble gas forms a compound with what other element?

Answer 5

Xenon with fluorine

Question 6

Using the noble gas configuration, what is the electron configuration for vanadium?

Answer 6

[Ar] 3d34s2

Question 7

Which of the following is the best statement describing a transition metal.

Answer 7

• Any element with a partially filled d orbital.
• Any element in the middle block of the periodic table
• Any element whose 3d orbitals have a higher energy than the 4s orbitals

Question 8

What is the electron configuration of titanium?

Answer 8

1s22s22p63s23p64s23d2

Question 9

How do the transition metals compare to the alkali and alkaline earth metals?

Answer 9

Transition metals are harder and denser.

Question 10

In most of the transition metals, the d orbitals fill up after the s orbitals of the next higher principal quantum number. Why does this occur?

Answer 10

Because the s orbitals have a lower energy

Question 11

Transition metals form a variety of different charged cations. What is the most common charge on the cation formed by the transition metals?

Answer 11

2+

Question 12

Metals are generally involved in the formation of which of the following?

Answer 12

Cations