explain each of the following observations using principles of atomic stucture and/or bonding.
a] potassium has a lower first-ionization engergy than lithium.
b] the ionic radius of N3- is larger than that of O2-.
c] a calcium atom is larger than a zinc atom.
d] boron has a lower first-ionization than beryllium.
a] Both K and Li have relatively low first-ionization energies because they want to get to noble gas configuration. However, Li has more electrons, and therefore, a greater shielding effect. That means that the pull of the electrons by the protons in the nucleus is weaker in Li and it takes less energy to take away outer electrons.
b] Both have the same number of electrons. However, O2- has 8 protons and N3- only has 7. The pull of the electrons by the protons in the nucleus is stronger in O2- because there are more of them, so the ion is pulled tighter and smaller.
c] I'm not positive on this one.
d] Boron has one electron unpaired in the p-subshell and it would like to lose it so it will have all full subshells. Beryllium already has all paired electrons so it takes more energy to pull one away.
Emily. I think you should think this through. Li has fewer electrons than K. since K is much larger than Li, its electron is further from the nucleus; therefore, its ionization potential is lower than that of Li.
b. The nitride ion is larger because there are more electrons in the outer orbit. Since they have the same charge, they repel each other, and the ionic radius increases for the nitride ion over that of oxide ion.
c. hint: look where Ca and Zn are in the periodic table. Remember that the 3d electrons are entering AFTER Ca and leading up to Zn.
d. The answer by Belinda is ok for this one.
Sorry I made a mistake in part a. Li has less electrons so potassium has a higher shielding effect so its proton strength is less and it is easier to remove an electron.
um some of this is WRONG
you might want to double check your information before you put it up next time
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a] Potassium has a lower first-ionization energy than lithium due to its larger atomic size and greater shielding effect. The valence electron in both elements is in the same energy level, but in potassium, it is further away from the nucleus and experiences greater shielding from inner electrons. This reduces the effective nuclear charge experienced by the valence electron, making it easier to remove compared to lithium.
b] The ionic radius of N3- is larger than that of O2- due to the difference in the number of protons in their respective nuclei. Although both ions have the same number of electrons, nitrogen has one less proton than oxygen. As a result, the effective nuclear charge experienced by the outermost electrons in the N3- ion is lower, resulting in weaker attraction and a larger ionic radius compared to O2-.
c] A calcium atom is larger than a zinc atom due to their respective positions in the periodic table. Calcium is an alkaline earth metal located in Group 2, while zinc is a transition metal located in Group 12. When moving across a period, the atomic size generally decreases due to the increased positive charge in the nucleus. Therefore, as you move from left to right in the periodic table, the atomic radius tends to decrease. Since calcium is located to the left of zinc, it has a larger atomic radius.
d] Boron has a lower first-ionization energy than beryllium due to the electron configuration of their respective atoms. Boron has an electron configuration of 1s^2 2s^2 2p^1, with an unpaired electron in the 2p orbital. This unpaired electron experiences electron-electron repulsion, making it easier to remove compared to beryllium, which has a paired electron in the 2s orbital and a more stable electron configuration.
a] The observation that potassium has a lower first-ionization energy than lithium can be explained by considering the principles of atomic structure and periodic trends. The first-ionization energy is the energy required to remove one electron from an atom in its gaseous state. In the case of potassium and lithium, both elements have similar electron configurations (K: [Ar] 4s1, Li: [He] 2s1), with one valence electron. However, the electron in potassium is further away from the nucleus compared to lithium because of the additional electron shell. This greater distance results in weaker electrostatic attraction between the nucleus and the valence electron in potassium, making it easier to remove the electron and lowering the first-ionization energy of potassium compared to lithium.
b] The observation that the ionic radius of N3- is larger than that of O2- can be explained by understanding the principles of atomic structure and the concept of effective nuclear charge. When an atom gains or loses electrons to form an ion, the size of the resulting ion is influenced by the effective nuclear charge experienced by the electrons. The effective nuclear charge is the net positive charge experienced by an electron and is determined by the number of protons in the nucleus and the shielding effect from inner electrons.
In the case of N3- and O2-, both ions have gained two additional electrons, which increases the electron-electron repulsion and results in an expansion of the electron cloud. However, nitrogen has one less proton in its nucleus compared to oxygen. As a result, the effective nuclear charge experienced by the electrons in N3- is lower than that experienced by the electrons in O2-. This decrease in effective nuclear charge weakens the attraction between the nucleus and the electrons, causing the electron cloud to spread out more and increasing the ionic radius of N3- compared to O2-.
c] The observation that a calcium atom is larger than a zinc atom can be explained by considering the principles of atomic structure and the concept of electron configuration. Calcium (Ca) is located in the third period of the periodic table, while zinc (Zn) is located in the fourth period. As we move across a period from left to right, the atomic radius generally decreases due to an increase in effective nuclear charge.
In the case of calcium and zinc, their electron configurations are as follows: Ca: [Ar] 4s2 and Zn: [Kr] 4d10 5s2. Although both elements have the same number of valence electrons in the 4s orbital, the presence of the 3d orbital in zinc creates greater effective nuclear charge and stronger attraction towards the nucleus. As a result, the atomic radius of zinc is smaller than that of calcium.
d] The observation that boron has a lower first-ionization energy than beryllium can be explained by considering the principles of atomic structure and electron configuration. The first-ionization energy is the energy required to remove one electron from an atom in its gaseous state.
In the case of boron and beryllium, both elements have similar electron configurations: B: [He] 2s2 2p1 and Be: [He] 2s2. Boron has an unpaired electron in the 2p orbital, while beryllium has all its electrons paired in the 2s orbital. Breaking the pair of electrons in the 2s orbital of beryllium requires more energy compared to removing the single unpaired electron in the 2p orbital of boron. Therefore, boron has a lower first-ionization energy than beryllium.