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Question 2: Atomic size of an atom is one of the most important parameter that affect various physical and chemical properties like ionization potential, electron a...

Question

Question 2: Atomic size of an atom is one of the most important parameter that affect various physical and chemical properties like ionization potential, electron affinity, metallic character etc . Discuss various factors that affect the atomic size of an element in a period and in a group. [Words limit 300, Maximum marks 30]

Question 2: Atomic size of an atom is one of the most important parameter that affect various physical and chemical properties like ionization potential, electron affinity, metallic character etc . Discuss various factors that affect the atomic size of an element in a period and in a group. [Words limit 300, Maximum marks 30]



Answers

Atomic size seems to play an important role in explaining some of the differences between the first element in a group and the subsequent group elements. Explain.

Here for the solution. First element for groups 1823 has non metallic character were asked. All other elements in these groups are metals. This is due to a smaller size of first elements in groups wanted to created. It's H, B and B have large polarizing effect when compared with the remaining elements in the same group. This is also due to small size for group 48 to 6 A. The main difference between first Element and remaining element is formation of my bones. First element can form strong by bond because in a small atoms, P orbital's can overlap with each other more effectively than in larger atoms. Four groups 782 small size of F F two has less bone disassociation, dissociation energy than CL two. Also, F has low electron affinity than CL due to. It's a small size, so this is a complete explanation for the solution. Please go through this. Thank you

So as you go down the periodic table, the atomic size or radius of the items increases. And the reason is that each successive row of the periodic table means the addition of energy level. So like lithium has a certain number of energy level. It's too specifically, so it's relatively small and sodium has electrons in an energy level higher, further from the nucleus and can expand further in space and then potassium has an additional energy level of electrons further from the nucleus and so on, and then going from right to left. The radius increases. So basically you go diagonal down to get bigger atoms. And the reason is that within a period you have the same number of energy levels. So lithium beryllium boron and so on. Have the same number of energy levels. Electrons are relatively the same distance apart from the nucleus. Um but as you go from left to right, the nuclear charge increases and pulls effective nuclear charge. And it pulls the outer electrons closer. So the items on the right side are more compact

Hey, one general terms. How does each of the following atomic properties influence the metallic character of the main group? Elements in a period, Um, a ionization energy be atomic radius. See the number of outer electrons and d effective nuclear charge. So I have given you a picture of the periodic table on your board, and I've also put the periodic trends of each of those 8 30 questions. So in the top right corner, we have the highest ionization energy, the most number of outer electrons, also known as valence electrons and the highest F effective nuclear charge. And then in the bottom left corner, we have the largest atomic radius. It's worth mentioning that, um, the left side of the periodic table up until about. Here is where we have our medals on our periodic table and then on the right side in the corner is where we have our non metals located. So that should give you a hint that ionization energy having a high ionization energy number of outer electrons and effective nuclear charge is inversely related to metallic properties. But we should talk about each of them specifically, let's begin with effective nuclear charge though, because I think that's the most important out of all of these. So effective nuclear charge is a measure of how strong the attraction is between the outer valence electrons and the protons that are located in your atoms nucleus. So if you remember the structure of an atom in our nucleus, we have these positively charged protons and then in our orbital surrounding the nucleus is where we have our electrons of effective nuclear charge is a measure of how strong these electrons are attracted to our inner protons. Remember, opposite charges attract. So if we have the highest effective nuclear charge here, meaning they are most closely bonded, um, to our inside, that means that we're less likely to give up those valence electrons which decreases our metallic character. Remember, metals can easily trade electrons amongst each other. That's one of the principles of conductivity. Um, and then ionization energy again is a measure of how easily we can give up electron, so that is directly telling us how metallic our substance is. All of these answer choice is kind of all feeding together because, you know, if we have a high number of outer electrons, that means we have more negative charge in our outside nucleus, which means we also have more positive charge. Uhm, in our nucleus, which again all of these kind of go hand in hand they are directly related to our metallic character.

Hello said today In general terms, how does following the Tommy properties influenced the metallic character of the period? So I have put the periodic table up on your board and I also shown the periodic trends that each of the four follow so ionization energy, the number of outer electrons and the effect of nuclear charge our highest in the upper right corner. And then we have our largest atomic radius in the bottom left corner. Now what is a metal? A metal is something that can easily give up its valence electrons to other surrounding Adams. This is a property of conductivity. So if you also are familiar with the periodic table, you'll know that metals are concentrated on this side of the table. They're organized on this side of the table, on the left, going up too, about there and then non metals are in the top right corner, where I'm outlining right now, So that should give you a clue as to how each of these properties of atoms affect our metallic property. So the higher the ionization energy, the greater the number of outer electrons, the higher the effective nuclear charge, the less metallic our substance is and the larger the atomic radius, the more metallic our substance is on. We can talk about each of these specifically in a little bit more detail, but they all go hand in hand. All of these properties kind of affect one another. I think the most important one is effective nuclear charge, which again goes hand in hand with the number of outer electrons. Effective nuclear charge. It is a measure of how strongly our valence electrons on the outermost shell of our Adam are attracted to the protons that are in the nucleus of our Adam. So if you're familiar with the structure of an atom, that would mean how strongly are these Valence electrons? Right here, Um, attracted to the positively charged protons. And here remember, opposite signs attract. Now, if they are more attracted to each other, meaning they have a higher, um, effective nuclear charge. That means that they're less likely to give up an electron, which means that they're less metallic. I hope that helps


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