Abundance Of Isotopes Worksheet: Fill & Download for Free

Iridium FactsIridium (Ir) has an atomic number of seventy-seven. It is a yellowish-white member of the platinum metals group, but its salts are very colorful.Interesting Iridium Facts:Iridium's discovery has an origin very similar to that of osmium.Scientists dissolved platinum in aqua regia, only to find a dark residue that resembled graphite.Smithson Tennant discovered the residue to contain osmium and iridium in 1803.He published his work and officially named both elements in 1804.It wasn't until 1842 that a scientist, Robert Hare, was able to obtain a sample of pure iridium.Rudolf Mossbauer won the Nobel Prize for Physics for the discovery of what is known as the Mossbauer Effect, often called one of the greatest physics experiments of the 20th century.In this experiment, Mossbauer discovered iridium's gamma ray absorptions properties and led to the technique of Mossbauer spectroscopy.Iridium is one of the rarest elements in the Earth's crust.It is believed to be available at 0.001 parts per million.Gold, silver, mercury, and platinum are all exonentially more abundant than iridium.Iridium is more prevalent in meteorites, and 0.05 parts per million or higher.The largest meteorite ever to land in North America, the Willamette Meteorite, contains a comparably vast concentration of iridium, at 4.7 parts per million.Like osmium, iridium concentrations are highest in a few known geological structures, most notably impact craters from meteorites.Iridium was responsible for the Alvarez Hypothesis, that a massive object collided with the Earth, causing the extinction of most species 65 million years ago.At the time that the event would have taken place, the geological record shows an unusually high level of iridium in the planet's clay layer.One theory about iridium's low abundance is that its high density and siderophilic properties caused it to sink below the Earth's crust while the planet was still primarily molten.Iridium has two stable isotopes, both of which are found naturally.There are also around thirty-four produced radioactive isotopes of iridium.Due to difficulty in extracting iridium, there are not many industrial applications for the element.Most applications of iridium tend to be alloys, since the metal is highly corrosion-resistant at high temperatures.Demand for iridium quintupled from 2009 to 2010, due to the rise of iridium use in electronics and the growth of high-quality crystals.Source : Free Math worksheets, Free phonics worksheets, Math Games and Online activities and QuizzesI hope you got your answer…

Well this is just the same answer to why we have to study Chemistry! Atomic Structure is a fundamental part of Chemistry. Knowing about the electrons, neutrons, protons can help you understand what’s going on in chemistry! For example, if you know an element has 6 protons, you will of course remember the element is carbon! This is very useful in future studies.Electrons, neutrons and protons are very important. Therefore, we have to learn about atomic structure. If we know how the electrons are arranged, we can make sure we understand the covalent bonds and ionic bonds.They are all related to electrons, electrons and electrons. To learn the structure of an atom, it isn’t too difficult at all. So learning doesn’t harm anything. In contrast, it helps us understand a lot of chemical reactions and how those chemistry takes place.To get started with how to study about the atomic structure, I recommend you read the following answer that i posted on another question on Quora:What is the structure of atoms?Before I continue with this very long very long very long post, let me tell you one good news: To understand the structure of atoms through an animated video, I recommend watching this video. This way, you could make sure you don’t have to read these huge amount of words.But if you prefer READING the structure of atoms, instead of EXPLORING, you may continue reading this answer:In the past, people think that atoms are the smallest unit that is indivisible. From the word itself, the word “atom” comes from “atomos”, a Greek word meaning “indivisible”. John Dalton proposed an atomic theory. Atom is the smallest part of the element having the chemical properties of the element.Atoms are made up of protons, neutrons and electrons. Protons are positively charged, neutron is neutral while electrons are negatively charged. Protons and neutrons are in the middle part, which is the centre of an atom – very tiny, and extremely dense. Protons and neutrons packed tightly together in this centre, called the nucleus. The overall charge for the proton will be positively charged. That’s because protons and neutrons are making up the nucleus, in which protons are positive and neutrons are negative. For electrons, they are found in the empty spaces. Electrons are very light in mass. They move around the nucleus.To sum up, we have:protons (+ve)Neutrons (neutral)electrons (-ve)In order to make sure we know how many neutrons there are in an atom, we may use full atomic symbol. So what are full atomic symbol. Let’s first talk about what the atomic number and mass number are.Section A: ProtonsWhat are protons? Protons define the element number, or atomic symbol. We can find out what atom it is from the proton. For example, if there are 6 protons, it must be a carbon atom. If it has one more proton, it’s no longer a carbon atom. it becomes a nitrogen atom.Section B: NeutronsNeutrons also belong to the nucleus, as mentioned before. Let’s continue…Finding the number of NEUTRONS from full atomic symbolThe atomic number of an atom is actually equal to the number of protons in the atom. The mass number of an atom is equal to the sum of the number of protons and the number of neutrons. You might be asking, what about electrons? In fact, electrons are too light that it doesn’t make too much difference in terms of the mass. Therefore, the mass number of an atom is just the number of protons and the number of neutrons. All of these can be found in the nucleus.We know that the number of electrons is equal to the number of protons, as atoms alone are electrically neutral. They kind of act like a balance.However, we can’t decide the number of neutrons directly. In fact, we may consider the following example - carbon-12. In fact, the top-left-hand corner is where it reads “12”. That represents the mass number, which is the sum of protons and neutrons. The number “six” represents the atomic number, which is basically the number of protons. As mentioned before, the number of electrons are equal to the number of protons as atoms alone are electrically neutral. So how can we deduce the number of neutrons it has in carbon-12 just by looking at this full atomic symbol?The number of protons + the number of neutrons will equal to the mass number. That’s why we can set up a formula: 6+n=12. As a result, we can calculate the number of neutrons, denoted by N, is 6.So, to summarize for carbon-12:In the full atomic symbol, we can see:mass number (12)number of protons (6)And we havenumber of electrons = number of protons = 6number of protons + number of electrons = mass numberi.e. number of neutrons= mass number - number of protons= 12–6= 6isotopes - different amount of NEUTRONS in the same type of atomWhy we have to learn how to find the number of neutrons an atom has - that’s because We actually have different isotopes.So, what are isotopes? Sometimes, the number of neutrons are not the same even though it’s the same element. For example, carbon has different isotopes, like Carbon-12, carbon-13, carbon-14, etc. However, these carbon isotopes must have the same number of protons, which is six, because, if it isn’t six, it will no longer be a carbon isotope. It will be a nitrogen. So for carbon 12, in fact, 12 is the mass number. The number of neutron will therefore be 12 minus 6 which is 6. For carbon-13. The number of neutrons will be 13 minus the number of protons. That is 13 minus 6, which gives us 7.There are actually different examples of the isotopes. For all the isotopes, you will notice the atomic number, the number of protons and the number of electrons won’t change. However, the mass number will change as the number of neutrons changed. The abundance varies significantly.So why do we have to study isotopes? In fact, isotopes have helped scientists and our daily life significantly. Uranium 235 can be used to generate electricity. Cobalt-60 can be used to kill microorganisms and pests in fruits, which benefits the preservation of food. Cobalt-60, iodine-125 and iodine-131 can be used to damage cancer cells with radiation.Section C: ElectronsArrangement of ELECTRONS in atomsSo we already know the arrangement of electrons in atoms. They all follow a rule. In fact, there is a formula to find the maximum number of the electron shells. Well, Danish scientist Niels Bohr suggested the electrons orbits around the nucleus, which are the electron shells. The formula is 2n^2, where n is the shell number. For example, the number of electron in the 1st shell will be 2(1)^2 which is 2. The maximum number of electrons in the 2nd shell will be 2(2)^2 which is 8. The maximum number of electrons in the 3rd shell is 2(3)^2 which is 18. The fourth shell will be 32, and so on.This might seem complicated, so let’s have a look at magnesium. The number of electrons will be equal to the number of protons which is 12. So let’s get 12 electrons. Now, we’re going to assign these electrons to the different electron shells. So for the first electron, it will get into the first shell, so as the 2nd one. However, when the third electron wants to get into the first shell, unfortunately, the first shell is already full. What we have to do is the place the electron to the 2nd shell. Here comes the electrons! We will have to continue the process until the second shell is full – which is 8. When it’s full, we will need to place the remaining 2 electrons into the 3rd shell, which has a capacity of 18 electrons.That is the same case for sodium. But this time, let’s use sodium as an example to tell you how to draw an electron diagram. You first put the atomic symbol in the middle. Then, we draw the electron shells represented by circles. Then, we draw the electrons as either dots or crosses. In this case, we will use dots. We can then place 2 electrons on opposite sides in the first shell. Later on, put the electron pairs on the sides, top and bottom of the second shell, as shown in the figure.You should note that potassium, although its number of electron is 19, the electronic arrangement is 2, 8, 8, 1 instead of 2, 8, 9. That’s the same case with calcium. It has an electron number of 20, but the electronic arrangement is 2, 8, 8, 2 instead of 2, 8, 10! But why? Isn’t the third shell’s maximum electron capacity 18? This is really a good question. The simple answer is that the outermost shell must not be greater than 8. However, this is too complicated to be discussed about. We will not study this in this level of study.So, that’s the structure of the atom. Hope this helps! By the way, looking at such a long passage might be tiring - let’s watch a video, instead! I have made some kind of animations to illustrate all these.I recommend going to YouTube to watch it. Worksheets and Interactive Activities are also provided linked in the description.Hope this answer helps!

What is the structure of atoms?Before I continue with this very long very long very long post, let me tell you one good news: To understand the structure of atoms through an animated video, I recommend watching this video. This way, you could make sure you don’t have to read these huge amount of words.But if you prefer READING the structure of atoms, instead of EXPLORING, you may continue reading this answer:In the past, people think that atoms are the smallest unit that is indivisible. From the word itself, the word “atom” comes from “atomos”, a Greek word meaning “indivisible”. John Dalton proposed an atomic theory. Atom is the smallest part of the element having the chemical properties of the element.Atoms are made up of protons, neutrons and electrons. Protons are positively charged, neutron is neutral while electrons are negatively charged. Protons and neutrons are in the middle part, which is the centre of an atom – very tiny, and extremely dense. Protons and neutrons packed tightly together in this centre, called the nucleus. The overall charge for the proton will be positively charged. That’s because protons and neutrons are making up the nucleus, in which protons are positive and neutrons are negative. For electrons, they are found in the empty spaces. Electrons are very light in mass. They move around the nucleus.To sum up, we have:protons (+ve)Neutrons (neutral)electrons (-ve)In order to make sure we know how many neutrons there are in an atom, we may use full atomic symbol. So what are full atomic symbol. Let’s first talk about what the atomic number and mass number are.Section A: ProtonsWhat are protons? Protons define the element number, or atomic symbol. We can find out what atom it is from the proton. For example, if there are 6 protons, it must be a carbon atom. If it has one more proton, it’s no longer a carbon atom. it becomes a nitrogen atom.Section B: NeutronsNeutrons also belong to the nucleus, as mentioned before. Let’s continue…Finding the number of NEUTRONS from full atomic symbolThe atomic number of an atom is actually equal to the number of protons in the atom. The mass number of an atom is equal to the sum of the number of protons and the number of neutrons. You might be asking, what about electrons? In fact, electrons are too light that it doesn’t make too much difference in terms of the mass. Therefore, the mass number of an atom is just the number of protons and the number of neutrons. All of these can be found in the nucleus.We know that the number of electrons is equal to the number of protons, as atoms alone are electrically neutral. They kind of act like a balance.However, we can’t decide the number of neutrons directly. In fact, we may consider the following example - carbon-12. In fact, the top-left-hand corner is where it reads “12”. That represents the mass number, which is the sum of protons and neutrons. The number “six” represents the atomic number, which is basically the number of protons. As mentioned before, the number of electrons are equal to the number of protons as atoms alone are electrically neutral. So how can we deduce the number of neutrons it has in carbon-12 just by looking at this full atomic symbol?The number of protons + the number of neutrons will equal to the mass number. That’s why we can set up a formula: 6+n=12. As a result, we can calculate the number of neutrons, denoted by N, is 6.So, to summarize for carbon-12:In the full atomic symbol, we can see:mass number (12)number of protons (6)And we havenumber of electrons = number of protons = 6number of protons + number of electrons = mass numberi.e. number of neutrons= mass number - number of protons= 12–6= 6isotopes - different amount of NEUTRONS in the same type of atomWhy we have to learn how to find the number of neutrons an atom has - that’s because We actually have different isotopes.So, what are isotopes? Sometimes, the number of neutrons are not the same even though it’s the same element. For example, carbon has different isotopes, like Carbon-12, carbon-13, carbon-14, etc. However, these carbon isotopes must have the same number of protons, which is six, because, if it isn’t six, it will no longer be a carbon isotope. It will be a nitrogen. So for carbon 12, in fact, 12 is the mass number. The number of neutron will therefore be 12 minus 6 which is 6. For carbon-13. The number of neutrons will be 13 minus the number of protons. That is 13 minus 6, which gives us 7.There are actually different examples of the isotopes. For all the isotopes, you will notice the atomic number, the number of protons and the number of electrons won’t change. However, the mass number will change as the number of neutrons changed. The abundance varies significantly.So why do we have to study isotopes? In fact, isotopes have helped scientists and our daily life significantly. Uranium 235 can be used to generate electricity. Cobalt-60 can be used to kill microorganisms and pests in fruits, which benefits the preservation of food. Cobalt-60, iodine-125 and iodine-131 can be used to damage cancer cells with radiation.Section C: ElectronsArrangement of ELECTRONS in atomsSo we already know the arrangement of electrons in atoms. They all follow a rule. In fact, there is a formula to find the maximum number of the electron shells. Well, Danish scientist Niels Bohr suggested the electrons orbits around the nucleus, which are the electron shells. The formula is 2n^2, where n is the shell number. For example, the number of electron in the 1st shell will be 2(1)^2 which is 2. The maximum number of electrons in the 2nd shell will be 2(2)^2 which is 8. The maximum number of electrons in the 3rd shell is 2(3)^2 which is 18. The fourth shell will be 32, and so on.This might seem complicated, so let’s have a look at magnesium. The number of electrons will be equal to the number of protons which is 12. So let’s get 12 electrons. Now, we’re going to assign these electrons to the different electron shells. So for the first electron, it will get into the first shell, so as the 2nd one. However, when the third electron wants to get into the first shell, unfortunately, the first shell is already full. What we have to do is the place the electron to the 2nd shell. Here comes the electrons! We will have to continue the process until the second shell is full – which is 8. When it’s full, we will need to place the remaining 2 electrons into the 3rd shell, which has a capacity of 18 electrons.That is the same case for sodium. But this time, let’s use sodium as an example to tell you how to draw an electron diagram. You first put the atomic symbol in the middle. Then, we draw the electron shells represented by circles. Then, we draw the electrons as either dots or crosses. In this case, we will use dots. We can then place 2 electrons on opposite sides in the first shell. Later on, put the electron pairs on the sides, top and bottom of the second shell, as shown in the figure.You should note that potassium, although its number of electron is 19, the electronic arrangement is 2, 8, 8, 1 instead of 2, 8, 9. That’s the same case with calcium. It has an electron number of 20, but the electronic arrangement is 2, 8, 8, 2 instead of 2, 8, 10! But why? Isn’t the third shell’s maximum electron capacity 18? This is really a good question. The simple answer is that the outermost shell must not be greater than 8. However, this is too complicated to be discussed about. We will not study this in this level of study.So, that’s the structure of the atom. Hope this helps! By the way, looking at such a long passage might be tiring - let’s watch a video, instead! I have made some kind of animations to illustrate all these.I recommend going to YouTube to watch it. Worksheets and Interactive Activities are also provided linked in the description.Hope this answer helps!