Transition Metals and Nonmetals (8.3.2)

Question 1

• Understanding the periodic table is imperative to understanding the reactivity of elements.

Answer 1

• Understanding the periodic table is imperative to understanding the reactivity of elements.

Question 2

• Transition Metals are characterized by partially filled d orbitals.

Answer 2

• Transition Metals are characterized by partially filled d orbitals.

Question 3

• Rare earth elements are electron rich and they tend to lose electrons in reactions.

Answer 3

• Rare earth elements are electron rich and they tend to lose electrons in reactions.

Question 4

Elements in the same group have similar reactivity.

Each family reacts characteristically with hydrogen (e.g.
HF, H2O, NH3, CH4).

Answer 4

Elements in the same group have similar reactivity.

Each family reacts characteristically with hydrogen (e.g.
HF, H2O, NH3, CH4).

Question 5

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.

Answer 5

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.

Question 6

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.

Answer 6

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.

Question 7

The noble gases are relatively unreactive, but become
more reactive as you move down the group on the
periodic table.

Answer 7

The noble gases are relatively unreactive, but become
more reactive as you move down the group on the
periodic table.

Question 8

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 8

3+ (C)

Since the d electrons and the s electrons are loosely bound, 3+ cations often form.

Question 9

What is the electron configuration of titanium?

Answer 9

1s22s22p63s23p64s23d2 (B)

This electron configuration can also be written as [Ar] 4s2 3d2.

Question 10

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

Answer 10

All of the above (D)

A transition metal is any element with a partially filled d orbital and whose 3d orbitals have a higher energy than the 4s orbitals. Transition metals are located in the middle block of the periodic table.

Question 11

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

Answer 11

[Ar] 3d2 (B)

This electron configuration correctly shows an ion that has lost the two 4s electrons. It is the electron configuration for the titanium(II) cation, Ti2+.

Question 12

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

Answer 12

[Ar] 3d34s2 (D)

Since vanadium has an atomic number of 23 and argon has an atomic number of 18, the electron configuration should be written with [Ar] representing the core electrons, plus five more electrons. Vanadium is in the fourth row, so n = 4. It is a transition element, so the 3d electrons are at a higher energy than the 4s electrons. Thus the configuration is written as [Ar] 3d34s2

Question 13

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

Answer 13

Transition metals are harder and denser. (B)

The transition metals have metallic characteristics: they conduct electricity and they can be drawn into wires or hammered into sheets. However, they are much harder, denser, and have a higher melting point than the alkali metals.

Question 14

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

Answer 14

Cations (B)

Metals tend to lose electrons and become positive ions or cations. Alkali metals lose one electron. Alkaline earth metals lose two electrons. Transition metals generally lose two electrons although some transition metal cations carry charges of 1+ or 3+. The inner transition metals (rare earth elements) trend to lose three electrons.

Question 15

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

Answer 15

2+ (B)

Most transition metals form cations with a 2+ charge. This is because they easily lose the two outer s electrons.

Question 16

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 16

Because the s orbitals have a lower energy (A)

The electrons in the orbitals of the d energy sublevel experience a higher degree of shielding than the electrons in the orbital of the next higher s energy sublevel.

Question 17

Which noble gas forms a compound with what other element?

Answer 17

Xenon with fluorine (D)

Since xenon is such a large atom, its electrons are the most loosely bound. Fluorine is the most electronegative element, so it is the most likely to form compounds.