Question

Define :

electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties

Answer 1

Answer:

Electronegetivity

Electronegetivity is the tendency of an atom to draw electron density toward itself.

OR

It is the tendency to attract and keep an electron in the atomic shell (of attracting atom).

• High electronegativity means the atom can pull an electron from another weakly electronegative atom.

Ionization energy;

Ionization energy is the amount of energy required to remove an electron from the valence shell of an isolated atom.

Electron affinity;

Electron affinity is the energy which is released when an isolated gaseous atom receives an extra electron in its outermost shell in order to form a uninegative ion.

Atomic radius

The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding shells of electrons

.

Melting point

Melting point is the temperature at which a solid becomes a liquid at normal atmospheric pressure

Metallic character

Metallic character refers to the level of reactivity of a metal. Metals tend to lose electrons in chemical reactions, as indicated by their low ionization energies.

Trends in periodic table:

This table shows the periodic table trends of six different physical properties of the elements: atomic radius, electron affinity, electronegativity, ionization energy, and metallic/nonmetallic character.

Force of Attraction

Definition: How much the outer electrons (-) are attracted to the nucleus (+)

Increases going up periodic table because there is one fewer energy level of electrons that will separate the outer electrons from the nucleus

Increases going right across periodic table because the nucleus gains protons and the atom has the same number of energy levels as you move across a period

2. Shielding Effect

Definition: How much the outer electrons are repelled by inner electrons (negative repels negative), and also describes how much control the nucleus has on outer electrons

Increases going down periodic table because there is an extra energy level of electrons that will shield the outer electrons from the nucleus

Increases slightly going left on periodic table because the nucleus loses protons and the atom has the same number of energy levels as you move across a period

3. Atomic Radius

Definition: A measure of a neutral atom’s size based on the radius of its volume as a sphere

Increases going down because there are more energy levels of electrons and therefore more shielding

Increases going left because as you move across a period right-to-left, an atom loses a positively charged proton and therefore its electrons become slightly less tight and compact

4. Atomic Radii Trends on the Periodic Table

Definition: Same as atomic radius, but for the size of a charged ion, not a neutral atom

Increases for anions (-) because they gain an electron, which leads to more shielding

Decreases for cations (+) because they lose an electron, which means less shielding

5. First Ionization Energy

Definition: The amount of energyneeded to remove an outer electronfrom an atom and make it into an ion

Increases going right because there are more protons in the nucleuspulling in electrons, so it requires more energy to remove an outer electron

Increases going up because there are fewer energy levels and less shielding, so the outer electrons are more tightly held by the nucleus

6. Metallic Character/Metallic Reactivity

Definition: The tendency of an atom to lose an electron (a key characteristic of metals is they lose electrons to become cations)

Increases going left because metals are on the left side of the periodic table and they have fewer protons in their nucleus that are holding in the atom’s electrons

Increases going down because there is more shielding, so outer electrons are easier to lose

7. Non-Metal Reactivity/Electron Affinity

Definition: The tendency of an atom to gain an electron (a key characteristic of non-metals is they gain electrons to become anions)

Increases going right because non-metals are on the right side of the periodic table and they have more protons in their nucleus that attract outer electrons

Increases going up because there are less electron energy levels and therefore a greater attraction to the nucleus for electrons

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Answer 2

Explanation:

Electronegativity:

• It is a tendency of atoms to attract shared pairs of electrons towards themselves.

Ionization energy:

• It is the amount of energy required to free an electron from the outermost shell of an isolated gaseous atom of any element.

Electron affinity:

• It is an amount of energy liberated when the addition of an electron occurs in a neutral atom to make a negatively charged ion.

Atomic radius:

• In simple words, atomic radius is the radius of an atom.
• In other words, it is the distance between the atom's nucleus and the boundary of electrons of the surrounding shells.

Melting point:

• It is the temperature at which solid matters melt, i.e., the temperature at which solid matters are converted into liquid matters.

Metallic character:

• It is the tendency of atoms to lose electrons and become positive ions.
• It is also the ability of metals to react with other elements.

Periodic trends:

• It arises from the arrangement of the periodic table, which provides chemists with an invaluable tool to quickly predict an element's properties.
• There are six periodic trends, which are as follows:

1. Electronegativity:

• In the periodic table, as one moves from left to right, the electronegativity of elements increases, and from top to bottom of the periodic table, it decreases.

2. Ionization energy:

• It increases as it goes from left to right in the periodic table due to valence shell stability and decreases as it goes from top to bottom due to the electron shielding effect.

3. Electron affinity:

• It increases as it goes from left to right in the periodic table due to a decrease in atomic radius and decreases as it goes from top to bottom due to an increase in atomic radius.

4. Melting point:

• Non-metals possess a low melting point, while metals possess a high melting point.
• Carbon, which is non-metal but still possess the highest melting points among all elements; and the other is boron, which is semi-metal and that also possess a high melting point.

5. Metallic character:

• It decreases from right to left due to the decrease in radius of the atom, which allows the outer electrons to ionize rapidly.
• It increases as it goes from top to bottom due to electron shielding.

6. Atomic radius:

• It decreases from left to right because of an increase in the number of protons in the nucleus, which attracts outer electrons towards the nucleus and results in a smaller radius.
• While it increases from top to bottom because of the electron shielding effect.

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