Podcast
Questions and Answers
Why is a cation smaller than its parent atom?
Why is a cation smaller than its parent atom?
- It has more electrons than the parent atom.
- It has a larger atomic radius.
- It has fewer electrons than the parent atom. (correct)
- It has more protons than the parent atom.
Which ion has a larger ionic radius compared to its parent atom?
Which ion has a larger ionic radius compared to its parent atom?
- Na+ (Sodium ion)
- Li+ (Lithium ion)
- Cl- (Chloride ion)
- F- (Fluoride ion) (correct)
What leads to the increase in the size of an anion compared to its parent atom?
What leads to the increase in the size of an anion compared to its parent atom?
- Addition of electrons leading to increased repulsion (correct)
- Decrease in atomic number
- Decrease in the number of neutrons
- Decrease in the number of protons
What is the term used for atoms and ions containing the same number of electrons?
What is the term used for atoms and ions containing the same number of electrons?
Why does the ionic radius of a cation differ from its parent atom?
Why does the ionic radius of a cation differ from its parent atom?
In general, how do ionic radii compare to atomic radii?
In general, how do ionic radii compare to atomic radii?
Which type of oxide is formed by elements on the extreme right of a period?
Which type of oxide is formed by elements on the extreme right of a period?
What do amphoteric oxides exhibit when reacting with bases?
What do amphoteric oxides exhibit when reacting with bases?
Which element mentioned in the text forms a neutral oxide?
Which element mentioned in the text forms a neutral oxide?
What is the oxidation state of aluminum (Al) as stated in the text?
What is the oxidation state of aluminum (Al) as stated in the text?
Which property generally decreases from left to right in a period?
Which property generally decreases from left to right in a period?
What type of properties are a manifestation of the electronic configuration of elements?
What type of properties are a manifestation of the electronic configuration of elements?
Which group of elements is known for adding one or two electrons to attain a stable noble gas configuration?
Which group of elements is known for adding one or two electrons to attain a stable noble gas configuration?
Why are the noble gases extremely unreactive?
Why are the noble gases extremely unreactive?
Which group of non-metals has highly negative electron gain enthalpies?
Which group of non-metals has highly negative electron gain enthalpies?
What are the elements of Group 3 to 12 in the Periodic Table referred to as?
What are the elements of Group 3 to 12 in the Periodic Table referred to as?
Which elements are included in the p-Block Elements?
Which elements are included in the p-Block Elements?
Why are the compounds of lithium and beryllium different from other s-block elements?
Why are the compounds of lithium and beryllium different from other s-block elements?
What trend is observed in atomic radii as one moves across each period from left to right?
What trend is observed in atomic radii as one moves across each period from left to right?
Which element has the highest electronegativity value on the Pauling scale in Period II?
Which element has the highest electronegativity value on the Pauling scale in Period II?
In the OF2 molecule, which element shares one electron with oxygen?
In the OF2 molecule, which element shares one electron with oxygen?
What is the oxidation state of oxygen in the Na2O compound?
What is the oxidation state of oxygen in the Na2O compound?
Which atom in Group I has the lowest electronegativity value on the Pauling scale?
Which atom in Group I has the lowest electronegativity value on the Pauling scale?
What is the oxidation state of fluorine in the OF2 molecule?
What is the oxidation state of fluorine in the OF2 molecule?
What factor outweighs the shielding effect across a period in the trend of ionization enthalpy?
What factor outweighs the shielding effect across a period in the trend of ionization enthalpy?
Why does it require less energy to remove the outermost electron down a group?
Why does it require less energy to remove the outermost electron down a group?
What makes it easier to remove the fourth 2p-electron from oxygen than one of the three 2p-electrons from nitrogen?
What makes it easier to remove the fourth 2p-electron from oxygen than one of the three 2p-electrons from nitrogen?
Which element in the third period has the highest first ionization enthalpy?
Which element in the third period has the highest first ionization enthalpy?
Why does the ionization enthalpy increase across a period?
Why does the ionization enthalpy increase across a period?
What trend in the ionization enthalpy values of Na, Mg, and Si can be observed in the third period elements?
What trend in the ionization enthalpy values of Na, Mg, and Si can be observed in the third period elements?
