Revision on Chapter 5

Revision on Chapter 5

Section 2:

Electron Configuration and the Periodic Table

Multiple Choice

The periodic table is divided into how many blocks?

• 1

• 2

• 3

• 4

Multiple Choice

Which elements are considered "main group" elements?

• Elements in s and d blocks

• Elements in d and p blocks

• Elements in s and p blocks

• Elements in f and d blocks

Multiple Select

Which groups of elements belong to the s-block (Choose 2 answers)

• Alkali metals

• Transition metals

• Alkali earth metals

• Halogens

Multiple Select

Which groups of elements belong to the p-block (Choose 2 answers)

• Alkali metals

• Lanthanides

• Noble gases

• Halogens

Multiple Choice

In the s-block, which group of elements is considered the most reactive?

• Alkali-earth metals

• Alkali metals

• Transition metals

• Lanthanides

The periodic table is divided into 4 blocks

s-block (Groups 1 and 2

p-block (Groups 13 to 18)

d-block (Groups 3 to 12)

f-block (between groups 3 and 4; Lanthanides and Actinides)

The main group elements are elements found in the s and p-blocks.

s-block elements

• Group 1 elements; also known as Alkali metals. They are the most reactive metals and are not found free in nature.

• Group 2 elements; also known as Alkali-earth metals. They are very reactive, but less reactive than the group 1 elements. They are also not found free in nature.

p-block elements

• Contain some metals, metalloids, halogens, noble gases and other non-metals

• The halogens are the most reactive of the non-metals

• The noble gases are unreactive.

Open Ended

Without looking at the periodic table, identify the group, period, and block in which the element that has the electron configuration [Xe]6s² is located.

Open Ended

Without looking at the periodic table, write the electron configuration for the Group 1 element in the third period. (Noble gas is Neon)

Open Ended

Without looking at the periodic table, write the outer electron configuration for the Group 14 element in the fifth period. (Noble gas is Krypton)

Open Ended

Without looking at the periodic table, identify the period, block, and group of an element that has the electron configuration [Ar]3d¹⁰4s²4p³

Open Ended

What name is given to Group 18 elements in the periodic table?

Open Ended

What name is given to Group 17 elements in the periodic table?

Open Ended

What name is given to Groups 3 to 12 elements in the periodic table?

Section 3:

Electron Configuration and Periodic Properties

Open Ended

How can you define "Atomic radius"?

Multiple Choice

Which of these IS WRONG about the atomic radius?

• It increases downwards in every group

• It decreases from left to right across a period

• The smallest atom is Helium

• The measurement is from one end of the atom to another end

Multiple Choice

Which of the following elements has the largest atomic radius: Li, O, C, or F?

• Li

• O

• C

• F

Multiple Choice

Which of the following elements has the smallest atomic radius: Li, O, C, or F?

• Li

• O

• C

• F

Multiple Choice

What happens to the atomic radius when an atom forms a positive ion?

• The atomic radius decreases

• The atomic radius increases

• The atomic radius stays the same

• The atomic radius disappears

Multiple Choice

What happens to the atomic radius when an atom forms a negative ion?

• The atomic radius decreases

• The atomic radius increases

• The atomic radius stays the same

• The atomic radius disappears

Atomic and Ionic radius

• Atomic radius increases from up to down in each group

• Atomic radius decreases from left to right in each period

• When an atom forms a positive ion, its radius decreases

• When an atom forms a negative ion, its radius increases.

Atomic and Ionic radius

• Atomic radius increases from up to down in each group

• Atomic radius decreases from left to right in each period

• When an atom forms a positive ion, its radius decreases

• When an atom forms a negative ion, its radius increases.

Open Ended

What do you understand by the term "Ionization"?

Open Ended

What do you understand by the term "Ionization Energy"?

Multiple Choice

Which of these trends IS WRONG about Ionization energy?

• Ionization energy is the same for elements with similar symbols

• Ionization energy increases from left to right of the periodic table

• Ionization energy decreases from top to bottom of the periodic table

• Element in Period 7, group 1 has the lowest ionization energy.

Multiple Choice

From the image, in which ionization energy does Beryllium (Be) have the biggest increase in value?

• 1st ionization energy

• 2nd ionization energy

• 3rd ionization energy

• 4th ionization energy

Open Ended

Why do you think there is a "great increase" in ionization energy at certain levels for all atoms?

Ionization Energy

• Ionization energy is the energy required to remove one electron from a neutral atom of an element

• Across a period, from left to right, ionization energies of the main-group elements increase.

• Along the group, from top to bottom, the ionization energies of the main group elements decrease.

• The first ionization energy (IE₁) is the energy required to remove one electron from an atom. The second ionization energy (IE₂) is the energy required to remove a subsequent second electron from the same atom. Similarly, the third (IE₃), fourth (IE₄) and fifth (IE₅) ionization energies are energies required to remove subsequent third, fourth and fifth electron from the same atom.

Atomic and Ionic radius

• Atomic radius increases from up to down in each group

• Atomic radius decreases from left to right in each period

• When an atom forms a positive ion, its radius decreases

• When an atom forms a negative ion, its radius increases.