Core UNIT 3: Atomic Theory & The Periodic Table. Section 1: Atom Basics Section 2: Isotopes Section 3: Periodic Table Trends
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1 Core UNIT 3: Atomic Theory & The Periodic Table Section 1: Atom Basics Section 2: Isotopes Section 3: Periodic Table Trends
2 Core UNIT 3 Synapsis In our second unit we will take a in depth look at atoms. We will start in parts 1 and 2 with some basic things that you may already know, and a few other basic things you may not know. Then we will explore how atoms of the same element can be different because of how many neutrons they have. In part 3 we will look at the periodic table and it s trend.
3 Section 1: Atom Basics This part of the Unit is covered on pages in your textbook
4 Section 1: Atom Basics / Objectives After this lesson I can define an atom & its three parts. Identify an element when give a number of protons and a Periodic Table recall the charge, mass, symbol and location of all three sub atomic particles. give an analogy for the size of the nucleus compared to the rest of the atom. recall that the strong nuclear force and the neutrons are what overcome the repulsive force between the protons and holds the nucleus together in stable atoms.
5 Protons Atoms are the fundamental building block of matter and we learned previously that matter is basically everything. All atoms are 1 of 118 elements. An element is the type or identity of an atom and is determined by the number of protons the atom has. The number of protons an atom has is also called it s atomic number. Examples: 1 proton = hydrogen 8 protons = oxygen 26 protons = iron. 92 protons = uranium Protons are Located in the Nucleus (the center of the atom) Positively charged have a mass of 1 a.m.u (atomic mass unit). go by the symbol p + or H +
6 Neutrons & Electrons 98% of hydrogen atoms contain just 1 proton. Atoms of all the other elements and a small percentage of Hydrogen atoms have neutrons as well. Neutrons are Located in the nucleus Have a mass of 1 a.m.u. Do not have a charge Use the symbol n Finally there are the electrons. Electrons don t change what element an atom is, and don t really matter for nuclear change. They are the real role players during chemical change because they are shared or exchanged when atoms bond with each other. Electrons are Located outside the nucleus Have a mass so small (.0002 a.m.u.) we often say their mass is negligible Have a negative charge Use the symbol e -
7 Very Simple Model of the Atom Image Credit: encyclopedia Britannica
8 Another Very Simple Model of the Atom Image Credit: googlesites.com
9 The Nucleus You can think of the nucleus as being this tightly packed ball of protons and neutrons. Unlike the models we are going to use to describe the electrons later in the unit, this is actually very close to reality. heavier atoms with higher numbers of protons and neutrons are actually shaped more like footballs but you get the point. Students often wonder how positively charged protons could be tightly packed together given that positive charges repel one another. There are two explanations why: The neutrons help to spread the charge out The strong nuclear force binds the protons together The other major things you need to know about the Nucleus can be difficult to imagine because there is nothing in the big world that really compares to the reality of an atom and it s nucleus. The nucleus is roughly 100,000 times smaller than the atom as a whole contains all of the atoms mass. In other words, the nucleus is all of the mass and none of the volume.
10 Model of the Nucleus Image Credit: :mscl.msu.edu
11 Analogies for the Nucleus Compare to the Rest of the Atom If the atom were the size of ford field the nucleus would be the size of a marble If the atom were the size of a church the nucleus would be just barely visible. About the size of a spec of dust suspend in air If the atom were the size of new York city the nucleus would be about the size of an orange
12 The Nucleus & The Electron Cloud So what takes up all the space within an atom then? The answer is nothing. Atoms are almost completely empty space (about 99.99%) The electrons occupy the vast region outside of the nucleus that we call the electron cloud. They are very tiny though and do not come close to taking up all that space. They don t fill up the electron cloud, it s simply where they can be found
13 Video Time!!! Crash Course Chemistry #1 Video: The Nucleus TedED Video: Just How Small is an Atom?
14 Section 1 Additional Resources & Links Science Post Video: Basic Parts of the Atom prontons, neutrons, electrons, nucleus Fuse School Video: What is an Atom
15 Section 2: Isotopes This part of the Unit is covered on pages in your textbook
16 After this lesson I can define isotopes. Section 2: Isotopes / Objectives determine the number of protons & neutrons in isotopes write isotope names and symbols (mass numbers) determine the number of electrons in an ion. distinguish mass numbers, atomic mass, and average atomic mass. calculate the average atomic mass of an element when give the percent abundance, atomic mass, and the mass numbers of it s naturally occurring isotopes (when given the Table of Isotopic Masses and Natural Abundances )
17 Video Time!!! Veratsium Video: What are Atoms and Isotopes?
18 Isotopes Earlier it was noted that the number of protons in an atom s nucleus determines what element that atom is, but atoms can have a different number of neutrons and still be the same element. An isotope is the type or version of an element and is determined by the number of neutrons. Isotopes are different atoms of the same element. Isotopes have a mass number which indicates the total number of protons & neutrons. If the isotope is given by name, the mass number is written after the dash. If the isotope is given by symbol, the mass number is written as a superscript to the left of the symbol. Isotope examples: Carbon-12 = (6 protons, 6 neutrons) = 12 C Carbon-13 = (6 protons, 7 neutrons) = 13 C Carbon-14 = (6 protons, 8 neutrons) = 14 C Sometimes the number of protons is written below the mass number. This is redundant because the number of protons is given by the element name or symbol but there are examples in a few slides.
19 Additional Examples of Isotopes Nitrogen-14 = (7 proton, 7 neutrons) = 14 N Nitrogen-15 = (7 protons,8 neutrons) 15 N Oxygen-15 = (8 protons, 7 neutrons) = 15 O Oxygen-16 = (8 protons, 8 neutrons) = 16 O Oxygen-17 = (8 protons, 9 neutrons) = 17 O Krypton 71 = (36 protons, 35 neutrons) = 71 Kr Krypton 74 = (36 protons, 38 neutrons) = 74 Kr Krypton 76 = (36 protons, 40 neutrons) = 76 Kr Note that Nitrogen-15 & Oxygen-15 have the same mass number but are different isotopes and different elements.
20 Isotope Image #1 Image Credit: :kaffee.50webs.com/science/activities/chem/activity.isotopes.table.htm
21 Isotope Image #2 Image Credit:
22 Isotope Image with Atomic Number Included Image Credit: astronomy.swin.edu.au
23 Isotope Image #4 Image Credit: highschoolpedia.com
24 Practice Problems: Decoding Isotopes Directions: Write the number of protons & neutrons for each isotope below 1) 25 Al 2) 33 P 3) Silver ) Uranium ) 181 Au 6) 30 S 7) 122 Xe 8) Beryllium -9 9) 4 He 10) Nickel ) 56 Fe 12) 38 Ar 13) 73 As 14) Tellurium - 134
25 Practice Problems: Writing Isotopes Directions: Write the isotope symbol and name for the given atom 1) 15 protons, 16 neutrons 2) 27 protons, 32 neutrons 3) 79 protons, 100 neutrons 4) 79 protons, 102 neutrons 5) 31 protons, 36 neutrons 6) 8 protons, 8 neutrons 7) 100 protons, 165 neutrons 8) 78 protons, 99 neutrons 9) 34 protons, 42 neutrons
26 Ions Atoms usually have the same number of electrons as they do protons and are thus neutral overall. Atoms that have more or less electrons than they do protons are called ions. When an atom is an ion it has a charge written as a superscript on the right side of the element s symbol. Examples: Aluminum atom with 10 electrons: Al 3+ Iron atom with 23 electrons: Fe 3+ Chlorine atom with 18 electrons: Cl - Oxygen atom with 10 electrons: O 2- Sodium atom with 10 electrons Na +
27 Example and Explanation of Isotope or Atom Symbols
28 Practice Problems: Ions Directions: Write down the element symbol & charge 1) 15 protons, 18 electrons 2) 2 protons, 0 electrons 3) 20 protons, 18 electrons 4) 23 protons, 18 electrons 5) 28 protons, 26 electrons 6) 35 protons, 36 electrons 7) 7 protons, 10 electrons
29 Practice Problems: Ions Directions: Determine the number of protons, neutrons, & electrons in each ion 1) 45 As 3-2) 29 Si 3) 139 I - 4) 71 Se 2-5) 33 S 2-6) 57 Fe 3+ 7) 35 Cl - 8) 17 O 2-9) 36 Ar
30 Percent Abundance Some isotopes of a given element are more common the others. For example 98.9% of all carbon atoms on planet earth are Carbon-12, only 1% are Carbon-13, & less than.1% are Carbon-14. The percentage of an isotope for a given element as it naturally occurs on earth is called it s natural abundance or percent abundance. Most elements have at least 2 isotopes that occur naturally, some have just 1, other have 5 or more. 10 is the highest (Tin if your curious) You can see all the naturally occurring isotopes for all the elements in a table called Table of Isotopic Masses and Natural Abundances. The vast majority of isotopes that naturally occur are known as stable isotopes. Basically that means the nucleus is going to exist forever as far as we can tell. Unstable isotopes will break down and most elements have a dozen or more unstable isotopes with very few occurring naturally. These isotopes radioactively decay or undergo fission. Studying these isotopes is a branch of chemistry called nuclear chemistry. Nuclear chemistry will not be covered in Chemistry A or B this year. However, there are a few really cool short videos that talk about nuclear chemistry at the end of this section.
31 Difference between Mass Number & Atomic Mass The mass number of an isotope is it s total number of protons and neutrons. The atomic mass of an isotope is it s true mass that we have determined through repeated experiments with very precise instruments. You d think these numbers would be identical, but they are not. All isotopes have a very slight difference between mass number and atomic mass. The one exception to this is Carbon-12 which has a atomic mass of exactly Understanding why there is a slight difference is not in our learning objectives. You can find the actual atomic mass for isotopes that naturally occur on the same table that lists natural abundances. It s worth noting that the difference between atomic mass and mass number is so slight, that many educators and instructional videos you find on the internet will not even mention it.
32 Average Atomic Mass The Average Atomic Mass of an element, which is the number that appears below atomic number on your periodic table, is the average atomic mass of the natural occurring isotopes of an element. It takes into account each isotopes percent abundance. If an element only has 1 naturally occurring isotope (and many do) than the average atomic mass is just the true atomic mass of it s only naturally occurring isotope. Using the Table of Isotopic Masses and Percent Abundances you should be able to calculate the average atomic mass that appears for each element on the periodic table. There are two examples on the next two slides.
33 Average Atomic Mass Calculation Example: Titanium Naturally Occurring Isotopes of Titanium Isotope Atomic Mass % Abundance 46 Ti % 47 Ti % 48 Ti % 49 Ti % 50 Ti % 46 Ti: = Ti: = Ti: = Ti: = Ti: = ( ) = 47.87
34 Average Atomic Mass Calculation Example: Neon 20 Ne: = Ne: = Ne: = ( ) = 20.18
35 Section 2 Additional Resources & Links Tyler Dewitt s Video: What are Isotopes Tyler Dewitt s Video: Isotope Notation Tyler Dewitt s Video: What s an Ion Tyler Dewitt s Video: Atomic Mass: An Introduction Tyler Dewitt s Video: How to Calculate Atomic Mass: Practice Problems YouChemTutorials Video: Calculating Average Atomic Mass
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