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What happens to the electropositive character of elements moving from left to right in a periodic table?
  • a)
    Increase
  • b)
    Decreases
  • c)
    First increases then decreases
  • d)
    First decreases then increases
Correct answer is option 'B'. Can you explain this answer?
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What happens to the electropositive character of elements moving from...
Electropositive character of an element is its ability to lose electrons and form positive ions. Now, as on moving from left to right in a period of periodic table, the nuclear charge increases due to the gradual increase in number of protons, so the valence electrons are pulled more strongly by the nucleus. Thus, it becomes more and more difficult for the atoms to lose electrons causing a decrease in the electropositive character of elements moving from left to right in a periodic table.
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What happens to the electropositive character of elements moving from...
Electropositivity refers to the tendency of an element to lose electrons and form positive ions. As we move from left to right across a period in the periodic table, the electropositive character of elements generally decreases. This can be explained by the following factors:

1. Atomic Radius:
- The atomic radius decreases as we move from left to right across a period. This is because the number of protons in the nucleus increases, resulting in a greater attraction between the nucleus and the valence electrons.
- A smaller atomic radius means that the outermost electrons are closer to the nucleus, making it more difficult for the element to lose electrons and become positively charged.

2. Effective Nuclear Charge:
- The effective nuclear charge is the positive charge experienced by the outermost electrons.
- As we move from left to right across a period, the effective nuclear charge increases. This is because the number of protons in the nucleus increases while the number of inner shell electrons remains relatively constant.
- The increased effective nuclear charge pulls the outermost electrons closer to the nucleus, making it harder for the element to lose electrons and become positively charged.

3. Electron Shielding:
- Electron shielding refers to the repulsion between electrons in different energy levels. Inner shell electrons shield the outermost electrons from the full effect of the positive charge in the nucleus.
- As we move from left to right across a period, the number of inner shell electrons remains constant while the effective nuclear charge increases.
- The lack of additional shielding from inner shell electrons further increases the attraction between the nucleus and the outermost electrons, reducing the electropositive character of the element.

Overall, the combination of a smaller atomic radius, increased effective nuclear charge, and decreased electron shielding leads to a decrease in electropositivity as we move from left to right across a period in the periodic table. Therefore, the correct answer is option 'B' - decreases.
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Read the given passage and answer the questions:Metallic Character: The ability of an atom to donate electrons and form positive ions (cation) is known as electro-positivity or metallic character. Down the group, metallic character increases due to increase in atomic size and across the period, from left to right electropositivity decreases due to decrease in atomic size. Non-Metallic Character: The ability of an atom to accept electrons to form a negative ion (anion) is called non-metallic character or electronegativity. The elements having high electro-negativity have a higher tendency to gain electrons and form anion. Down the group, electronegativity decreases due to increase in atomic size and across the period, from left to right electro -negativity increases due to decrease in atomic size.Hydrogen is placed along with Alkali metals in the modern periodic table though it shows nonmetallic character

Read the given passage and answer the questions:Metallic Character: The ability of an atom to donate electrons and form positive ions (cation) is known as electro-positivity or metallic character. Down the group, metallic character increases due to increase in atomic size and across the period, from left to right electropositivity decreases due to decrease in atomic size. Non-Metallic Character: The ability of an atom to accept electrons to form a negative ion (anion) is called non-metallic character or electronegativity. The elements having high electro-negativity have a higher tendency to gain electrons and form anion. Down the group, electronegativity decreases due to increase in atomic size and across the period, from left to right electro -negativity increases due to decrease in atomic size.Identify the reason for the gradual change in electronegativity in halogens down the group.

Read the given passage and answer the questions:Metallic Character: The ability of an atom to donate electrons and form positive ions (cation) is known as electro-positivity or metallic character. Down the group, metallic character increases due to increase in atomic size and across the period, from left to right electropositivity decreases due to decrease in atomic size.Non-Metallic Character: The ability of an atom to accept electrons to form a negative ion (anion) is called non-metallic character or electronegativity. The elements having high electro-negativity have a higher tendency to gain electrons and form anion. Down the group, electronegativity decreases due to increase in atomic size and across the period, from left to right electro -negativity increases due to decrease in atomic size.Which of the following reasons correctly justifies that “Fluorine (72pm) has a smaller atomic radius than Lithium (152pm)”?

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What happens to the electropositive character of elements moving from left to right in a periodic table?a)Increaseb)Decreasesc)First increases then decreasesd)First decreases then increasesCorrect answer is option 'B'. Can you explain this answer?
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