Trends In Periodic Table

1. What is ionization energy?

Energy required to combine two atoms to form a molecule.

Energy required to remove 1 mol of electrons

Energy released when an atom gains electrons.

Energy needed to remove an electron from an isolated gaseous atom or ion.

Energy absorbed by an atom when it gains electrons.

Ionization energy is the energy required to remove one or more electrons from an atom or ion. It is a measure of the tendency of an atom to attract a bonding pair of electrons.

Explanation

Ionization energy is the energy required to remove one or more electrons from an atom or ion. It is a measure of the tendency of an atom to attract a bonding pair of electrons.

2. What is electron affinity?

The force of attraction between protons and neutrons within an atom

The distance between two electrons in an atom

The movement of electrons within an atom

The energy change in the addition of 1 mol of electrons to 1 mol of gaseous atoms/ions

Electron affinity specifically refers to the energy change when adding electrons to gaseous atoms/ions, not the other concepts mentioned.

Explanation

Electron affinity specifically refers to the energy change when adding electrons to gaseous atoms/ions, not the other concepts mentioned.

3. What is paramagnetism?

A term used to describe the property of being attracted to magnets.

A species with paired electrons.

A species with unpaired electrons

A type of radioactive decay.

Paramagnetism occurs in species with unpaired electrons, causing them to be weakly attracted to magnetic fields.

Explanation

Paramagnetism occurs in species with unpaired electrons, causing them to be weakly attracted to magnetic fields.

4. What is diamagnetism?

A type of magnetism found in ferromagnetic materials.

A process by which an object acquires a magnetic moment when exposed to a magnetic field.

A property exhibited by only certain elements on the periodic table.

A species with paired electrons

A species with unpaired electrons.

Diamagnetism is a property of all materials and is characterized by the presence of paired electrons, which results in a weak repulsion from magnetic fields.

Explanation

Diamagnetism is a property of all materials and is characterized by the presence of paired electrons, which results in a weak repulsion from magnetic fields.

5. What is electronegativity (E)?

Measure of an atom's stability in a covalent bond.

Ability of an atom to attract electrons towards itself in a covalent bond

Ability of an atom to repel electrons away from itself in a covalent bond.

The number of electrons an atom can donate in a covalent bond.

Electronegativity is a measure of an atom's ability to attract electrons towards itself in a covalent bond, not repel them. It is also not directly related to the stability of an atom or the number of electrons it can donate in a bond.

Explanation

Electronegativity is a measure of an atom's ability to attract electrons towards itself in a covalent bond, not repel them. It is also not directly related to the stability of an atom or the number of electrons it can donate in a bond.

6. What is the result of E multiplied by F?

6

12

2

4

To find the result of E multiplied by F, we simply multiply the two values (2 * 2) which equals 4. Therefore, the correct answer is 4.

Explanation

To find the result of E multiplied by F, we simply multiply the two values (2 * 2) which equals 4. Therefore, the correct answer is 4.

7. What is the value of E in O?

4.2

3.5

5.1

2.8

The correct value of E in O is 3.5.

Explanation

The correct value of E in O is 3.5.

8. What is the atomic number of Chlorine?

23

3

19

20

The atomic number of Chlorine is 17, which indicates the number of protons found in the nucleus of a Chlorine atom. It is represented by the symbol Cl.

Explanation

The atomic number of Chlorine is 17, which indicates the number of protons found in the nucleus of a Chlorine atom. It is represented by the symbol Cl.

9. What is the trend in size?

It decreases as you move left, it increases as you move down

It increases as you move left, it decreases as you move down

It stays constant as you move left, it increases as you move down

As you move left, it increases
as you move down, it increases

The trend in size involves an increase as you move left and down, which indicates a pattern of growth in both directions.

Explanation

The trend in size involves an increase as you move left and down, which indicates a pattern of growth in both directions.

10. What is the trend in electron affinity?

Increase from left to right across a period

Remains constant across the periodic table

(look at pic)

Decrease from top to bottom within a group

Electron affinity generally increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This is due to the effective nuclear charge and atomic size factors affecting the attraction of electrons.

Explanation

Electron affinity generally increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This is due to the effective nuclear charge and atomic size factors affecting the attraction of electrons.

11. What is the trend in ionization energy?

As you move right on the periodic table, it decreases; as you move up, it increases.

As you move left on the periodic table, it increases; as you move down, it increases.

As you move left on the periodic table, it decreases; as you move up, it increases.

As you move right on the periodic table, it increases; as you move down, it decreases.

As you move left it decreases,
as you move down, it decreases

Ionization energy decreases as you move left on the periodic table due to the increase in atomic radius, making it easier for electrons to be removed. Additionally, ionization energy decreases as you move down a group because the valence electrons are further away from the nucleus, experiencing weaker attractions.

Explanation

Ionization energy decreases as you move left on the periodic table due to the increase in atomic radius, making it easier for electrons to be removed. Additionally, ionization energy decreases as you move down a group because the valence electrons are further away from the nucleus, experiencing weaker attractions.

12. What is the trend in metallic behavior?

Metallic behavior decreases as you move left on the periodic table.

Metallic behavior decreases as you move down a group on the periodic table.

Metallic behavior increases as you move right on the periodic table.

As you move left, it increases
as you move down, it increases

The correct answer is that metallic behavior increases as you move left on the periodic table (from right to left across a period) and as you move down a group. These trends are influenced by factors such as atomic radius, electron shielding, and effective nuclear charge.

Explanation

The correct answer is that metallic behavior increases as you move left on the periodic table (from right to left across a period) and as you move down a group. These trends are influenced by factors such as atomic radius, electron shielding, and effective nuclear charge.

13. What is the trend in ionic size?

As you move right on the periodic table, it decreases. As you move down a group, it stays the same.

As you move right on the periodic table, it increases. As you move down a group, it decreases.

As you move right on the periodic table, it increases. As you move down a group, it increases.

As you move right, it increases
as you move down, it increases

As you move right on the periodic table, it decreases. As you move down a group, it decreases.

In general, ionic size decreases as you move right across the periodic table due to increasing nuclear charge pulling electrons closer. On the other hand, ionic size increases as you move down a group since more electron shells are being added, leading to a larger atomic radius.

Explanation

In general, ionic size decreases as you move right across the periodic table due to increasing nuclear charge pulling electrons closer. On the other hand, ionic size increases as you move down a group since more electron shells are being added, leading to a larger atomic radius.