- Atomic Mass Simulation This Simulation Shows You An Individual Atom Sitting On A Balance Let S Start By Using The Sim 1 (95.75 KiB) Viewed 20 times
- Atomic Mass Simulation This Simulation Shows You An Individual Atom Sitting On A Balance Let S Start By Using The Sim 2 (245.32 KiB) Viewed 20 times
- Atomic Mass Simulation This Simulation Shows You An Individual Atom Sitting On A Balance Let S Start By Using The Sim 3 (83.2 KiB) Viewed 20 times
✓ Atomic Mass Simulation This simulation shows you an individual atom sitting on a balance. Let's start by using the simulation to observe some patterns. Protons: Neutrons: Electrons: ● Neutrons Isotopes and Atomic Mass - Isotopes 1 My Isotope Hydrogen-1 Stable O Mass Number ● Atomic Mass (amu) H Li Be Symbol Periodic Table B C N Abundance in Nature O He F Ne + + PHET:
1. You can change the element the simulation shows by selecting a symbol from the table on the right. The selected element will be red. CN OF Ne He 2. The rows of the periodic table are called periods. This simulation just shows the first two periods of the periodic table. Hydrogen (H) and helium (He) are in period 1, then the remaining elements are in period 2. 3. First, focus on the mass of the atoms. When you select an atom, it will be sitting on the balance which shows you the mass. My Isotope Hydrogen-1 O Stable O Mass Number Atomic Mass (amu) As you go from left to right in a period, what happens to the mass of the atoms? Hint: Try comparing hydrogen (H) and helium (He) from period 1, then try comparing lithium (Li) and neon (Ne) from period 2. The mass increases as you go from left to right in a period. The mass stays the same as you go from left to right in a period. The mass decreases as you go from left to right in a period. Submit Answer 3/3 submissions remaining
4. This simulation shows atoms as a nucleus surrounded by an electron cloud. The distance from the nucleus to the edge of the electron cloud is the atomic radius. This is a measure of how big the atom is. O O O My Isotope Lithium-7 Stable As you go from left to right in a period, what happens to the atomic radius? Hint: Try comparing hydrogen (H) and helium (He) from period 1, then try comparing lithium (Li) and neon (Ne) from period 2. O Mass Number ● Atomic Mass (amu) The atomic radius increases as you go from left to right in a period. Score: 0/1 The atomic radius stays the same as you go from left to right in a period. The atomic radius decreases as you go from left to right in a period. Submit Answer 3/3 submissions remaining
5. The columns on the periodic table are called groups. There are a total of 18 groups on the periodic table, but the simulation skips groups 3 through 12 since those groups don't have any elements in the first two periods. Hydrogen (H) and lithium (Li) are both in group 1 and helium (He) and neon (Ne) are both in group 18. 6. As you go down along a group, what happens to the mass of the atoms? Hint: Try comparing hydrogen (H) and lithium (Li) in group 1 and helium (He) and neon (Ne) in group 2. O O The mass increases as you move down a group. The mass stays the same as you move down a group. The mass decreases as you move down a group. Submit Answer 3/3 submissions remaining Score: 0/1 7. As you go down along a group, what happens to the atomic radius? Hint: Try comparing hydrogen (H) and lithium (Li) in group 1 and helium (He) and neon (Ne) in group 2. The atomic radius increases as you move down a group. The atomic radius stays the same as you move down a group. The atomic radius decreases as you move down a group.
✓ Periodic Table Here is a periodic table you can use to help answer the questions. Feel free to close this section by clicking the arrow next to the title when you aren't using the periodic table. 1. 1 2 1 H Hydrogen 1.008 Li Lithium 6.94 7 3 Sodium 22.99 3 11 12 Na Mg Magnesium 24.31 19 2 Be Beryllium 9.012 K 4 Potassium Calcium 39.10 40.08 55 87 3 Ca Sc Ti Scandium Titanium 44.96 47.88 Cs Ba Caesium 132.9 Barium 137.3 Fr Ra Francium Radium (223) (226) 20 PERIODIC TABLE OF ELEMENTS 56 88 21 Yttrium 88.91 39 Alkali Metals Alkaline Earth Metals Transition Metals Other Metals 57-71 Lanthanides Metalloids Actinides 4 22 5 40 Hafnium 178.5 V Vanadium 50.94 23 Chromium 52.00 73 41 44 38 45 47 37 48 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Silver 5 Rubidium Strontium 85.47 Zirconium 91.22 Niobium 92.91 Molybdenum Technetium Ruthenium Rhodium 95.96 (98) 101.1 102.9 Palladium 106.4 Cadmium Indium 112.4 114.8 107.9 87.62 Non-metals Halogens Noble Gases Lanthanides Actinides 74 Tantalum Tungsten 180.9 183.9 Manganese Iron 54.94 55.85 72 75 76 Hf Ta W Re Os Ir Rhenium Osmium Iridium 186.2 190.2 192.2 H Hydrogen 1.008 43 59 Cobalt 58.93 1-Atomic Number Atomic Symbol 77 Element Name Avg. Atomic Mass 92 - Lanthanum Cerium Praseodymium Neodymium Promethium Samarium 138.9 140.1 140.9 144.2 (145) 150.4 Nickel 58.69 28 46 Copper Zinc 63.55 65.39 78 13 B Boron 10.81 63 5 Europium Gadolinium Terbium 152.0 157.2 158.9 6 7 8 9 10 11 12 24 25 26 27 29 30 31 32 33 34 36 Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Germanium Arsenic Selenium Bromine Krypton 72.64 74.92 78.96 79.90 83.79 Gallium 69.72 Aluminium Silicon 26.98 28.09 14 C Carbon 12.01 49 13 14 15 Al Si P S Phosphorus Sulfur 30.97 30.97 81 15 50 Tin 118.7 N Nitrogen 14.01 57 58 64 65 66 67 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er 16 51 Bismuth 209.0 99 O 52 Sn Sb Sb Tel Oxygen 16.00 Dysprosium Holmium Erbium 162.5 164.9 167.3 83 8 16 68 Antimony Tellurium lodine 121.8 127.6 126.9 17 F Fluorine 19.00 Thulium 168.9 104 107 111 114 115 116 117 118 Rf Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og Rutherfordium Dubnium Seaborgium Bohrium (265) (268) (271) (270) Hassium (277) Meitnerium Darmstadtium Roentgenium Copernicium Nihonium (276) (281) (280) (285) (284) Flerovium Moscovium Livermorium Tennessine Oganesson (289) (288) (293) (294) (294) 17 80 82 84 79 85 86 Pt Au Hg Tl Pb Bi Po At Rn Gold Polonium Astatine Radon Platinum 195.1 Mercury Thallium Lead 200.5 204.38 197.0 207.2 (209) (210) (222) CI Ar Argon Chlorine 35.45 39.95 18 He Helium 4.003 35 53 Ne Neon Neon 20.18 69 70 Ho Er Tm Yb Lu Xe Xenon 131.3 10 18 Ytterbium Lutetium 173.0 175.0 54 96 98 100 101 102 103 97 89 90 91 95 93 94 Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Actinium Thorium Protactinium Uranium (227) 232.0 231.0 238.0 Neptunium Plutonium (237) (244) Americium Curium (243) (247) Berkelium (247) Californium Einsteinium Fermium (251) (252) (257) Mendelevium Nobelium (258) (259) Lawrencium (262) 71
✓ Atomic Mass Trends Let's use the data table and graph to find some trends in the periodic table! 1. Make sure the vertical axis of the graph is Atomic Mass (amu). This is the average mass of naturally occurring versions of the element. The unit amu is an abbreviation for atomic mass unit, where one proton has a mass of 1 amu. 2. Describe the trend in mass as the atomic number increases. Hint: Pay attention to the shape of the graph. What happens to the atomic mass as the atomic number increases? BI U Score: 0/1 3. Why does it make sense for the atomic number to affect the atomic mass? Does the trend on the graph fit with your explanation for why they are related? Hint: What does the atomic number tell you about the structure of an atom? BIU E E % li
✓ Atomic Radius Trends Let's use the data table and graph to find some trends in the periodic table! 1. Change the vertical axis of the graph to Atomic Radius (pm). The unit pm is short for picometers, where 1pm = 1 × 10-¹2m or one trillionth of a meter. In other words, a picometer is very, very small! 2. Notice that there is not one consistent trend in the atomic radius. Instead, there is a repeating pattern. Another way to describe a repeating pattern in a quantity is to say the quantity is periodic. Lots of properties of elements are periodic, which is where the periodic table got its name! 3. Focus on the elements with the largest radius in each set of points. Atomic Radius vs Atomic Number Atomic Number units) Where on the periodic table do you find those elements? Hint: You can move your mouse over a point to see the values, including the atomic number. ● Atomic Radius : 243 pm
The elements with a large radius are all in group 1 (the column to the left of the periodic table). The elements with a large radius are all in group 18 (the column to the right of the periodic table). The elements with a large radius are all in period 1 (the row at the top of the periodic table). The elements with a large radius are all in period 7 (the row at the bottom of the periodic table). Submit Answer 4/4 submissions remaining Score: 0/1 4. Now focus on the elements with the smallest radius in each set of points. 250 Atomic Radius vs Atomic Number Atomic Number units) Where on the periodic table do you find those elements? The elements with a small radius are all in group 1 (the column to the left of the periodic table). The elements with a small radius are all in group 18 (the column to the right of the periodic table). The elements with a large radius are all in period 1 (the row at the top of the periodic table). The elements with a large radius are all in period 7 (the row at the bottom of the periodic table).
5. Now focus on just one set of points on the graph. You can pick any set of points you would like. Atomic Radius vs Atomic Number 0000 Atomic Number Junits) What do all of the elements in a set of points have in common? They are all in the same group (column) on the periodic table. They are all in the same period (row) on the periodic table. They don't have anything in common. Submit Answer 3/3 submissions remaining Score: 0/1 6. According to the graph, what best describes the trend in atomic radius as you move from left to right along a period? As you go from left to right in a period, the atomic radius increases. As you go from left to right in a period, the atomic radius stays the same. As you go from left to right in a period, the atomic radius decreases.
7. According to the graph, what best describes the trend in atomic radius as you move from top to bottom along a group? Hint: Try finding some points on the graph that represent elements from the same group. As you move from top to bottom of a group, the atomic radius increases. As you move from top to bottom of a group, the atomic radius stays the same. As you move from top to bottom of a group, the atomic radius decreases. Submit Answer 3/3 submissions remaining Score: 0/1 ✓ lonization Energy Trends Let's use the data table and graph to find some trends in the periodic table! 1. Change the vertical axis of the graph to lonization Energy (kJ/mol). This is the amount of energy it takes to turn an atom into an ion by removing an electron, also known as ionizing it. Since the energy to remove just one electron from just one atom is very small, this graph shows how much energy it takes to ionize an entire mole of that element. The unit kJ is short for kilojoules, which is a unit of energy. 2. Like atomic radius, ionization energy is periodic and does not have a single consistent trend. The data for ionization energy is a little messier, so it can be harder to see the sets of points in the graph. Here's how they are grouped: lonization Energy vs Atomic Number
2. Like atomic radius, ionization energy is periodic and does not have a single consistent trend. The data for ionization energy is a little messier, so it can be harder to see the sets of points in the graph. Here's how they are grouped: lonization Energy vs Atomic Number 10000 Atomic Number (unit) 3. Focus on the points with the largest ionization energy in each set of points. O O O O 。 lonization Energy vs Atomic Number Atomic Number (unit) Where on the periodic table do you find those elements? The elements with a large ionization energy are all in group 1 (the column to the left of the periodic table). The elements with a large ionization energy are all in group 18 (the column to the right of the periodic table). The elements with a large ionization energy are all in period 1 (the row at the top of the periodic table). The elements with a large ionization energy are all in period 7 (the row at the bottom of the periodic table).
4. Now focus on the elements with the smallest ionization energy in each set of points. O O O O The Where on the periodic table do you find those elements? The elements with a small ionization energy are all in group 1 (the column to the left of the periodic table). elements with a small ionization energy are all in group 18 (the column to the right of the periodic table). elements with a small ionization energy are all in period 1 (the row at the top of the periodic table). The elements with a small ionization energy are all in period 7 (the row at the bottom of the periodic table). The lonization Energy vs Atomic Number Atomic Number (unit) Score: 0/1 Submit Answer 4/4 submissions remaining 5. Now focus on just one set of points on the graph. You can pick any set of points you would like.
5. Now focus on just one set of points on the graph. You can pick any set of points you would like. Ionization Energy vs Atomic Number 19000 Atomic Number (unit) What do all of the elements in a set of points have in common? They are all in the same group (column) on the periodic table. They are all in the same period (row) on the periodic table. They don't have anything in common. Score: 0/1 Submit Answer 3/3 submissions remaining 6. According to the graph, what best describes the trend in ionization energy as you move from left to right along a period? Hint: It's okay of not all the elements perfectly follow this trend! As you go from left to right in a period, the ionization energy increases. As you go from left to right in a period, the ionization energy stays the same. As you go from left to right in a period, the ionization energy decreases.
7. According to the graph, what best describes the trend in ionization energy as you move from top to bottom along a group? Hint: It's okay of not all the elements perfectly follow this trend! As you move from top to bottom of a group, the ionization energy increases. As you move from top to bottom of a group, the ionization energy stays the same. As you move from top to bottom of a group, the ionization energy decreases. Submit Answer 3/3 submissions remaining Score: 0/1 8. Why does it make sense for the period an element is in to affect the ionization energy? Do the trends on the graph fit with your explanation for why they are related? Hint: lonizing an atom means removing an electron. Think about the structure of atoms, including both the nucleus and the placement of electrons, and how that fits with what makes it harder or easier to remove an electron. BIU EE E E Score: 0/1 li
9. What happens to the ionization energy as the atomic radius increases? Why would changing the atomic radius affect the ionization energy? Hint: Try changing the horizontal axis of the graph to plot ionization energy vs. atomic radius. BIU Score: 0/2 € ✓ Electronegativity Trends % # Let's use the data table and graph to find some trends in the periodic table! 1. Change the vertical axis of the graph to Electronegativity. If you changed the horizontal axis, make sure you change it to either Atomic Number or Element. Electronegativity is a measure of how much an atom tends to attract the electrons that it shares during a covalent bond. This number doesn't have a unit and is measured on a relative scale. The higher an element's electronegativity, the more strongly it attracts electrons when it is in a covalent bond. to Because electronegativity is related to bonding and noble gasses normally don't bond with other atoms, most of the noble gasses don't have an electronegativity. Under certain conditions, krypton and xenon can sometimes bond with other atoms, so they have
Because electronegativity is related to bonding and noble gasses normally don't bond with other atoms, most of the noble gasses don't have an electronegativity. Under certain conditions, krypton and xenon can sometimes bond with other atoms, so they have an electronegativity even though they are noble gasses. 2. Focus on the points with the largest electronegativity in each set of points. Where on the periodic table do you find those elements? The elements with a large electronegativity are mostly in group 1 (the column to the left of the periodic table). The elements with a large electronegativity are mostly in groups 17 and 18 (the columns to the right of the periodic table). The elements with a large electronegativity are mostly in period 1 (the row at the top of the periodic table). O O O O The elements with a large electronegativity are mostly in period 7 (the row at the bottom of the periodic table). Submit Answer 4/4 submissions remaining Score: 0/1 3. Now focus on the elements with the smallest electronegativity in each set of points.
3. Now focus on the elements with the smallest electronegativity in each set of points. Where on the periodic table do you find those elements? The elements with a small electronegativity are mostly in group 1 (the column to the left of the periodic table). The elements with a small electronegativity are mostly in group 18 (the column to the right of the periodic table). The elements with a small electronegativity are mostly in period 1 (the row at the top of the periodic table). The elements with a small electronegativity are mostly in period 7 (the row at the bottom of the periodic table). Submit Answer 4/4 submissions remaining Score: 0/1 4. Now focus on just one set of points on the graph. You can pick any set of points you would like. 0000
4. Now focus on just one set of points on the graph. You can pick any set of points you would like. 10000 What do all of the elements in a set of points have in common? They are all in the same group (column) on the periodic table. They are all in the same period (row) on the periodic table. They don't have anything in common. Submit Answer 3/3 submissions remaining Score: 0/1 5. According to the graph, what best describes the trend in electronegativity as you move from left to right along a period? Hint: It's okay of not all the elements perfectly follow this trend! As you go from left to right in a period, the electronegativity increases. As you go from left to right in a period, the electronegativity decreases. As you go from left to right in a period, the electronegativity stays the same. Submit Answer 3/3 submissions remaining
6. According to the graph, what best describes the trend in electronegatvitity as you move from top to bottom along a group? Hint: It's okay of not all the elements perfectly follow this trend! As you move from top to bottom of a group, the electronegativity increases. As you move from top to bottom of a group, the electronegativity decreases. As you move from top to bottom of a group, the electronegativity stays the same. Submit Answer 3/3 submissions remaining Score: 0/1 7. Why does it make sense for the period an element is in to affect the electronegativity? Do the trends on the graph fit with your explanation for why they are related? Hint: Think about the structure of atoms, including both the nucleus and the placement of electrons, and how that fits with what makes at atom more or less likely to attract electrons. BIU Score: E 3 i
Score: 0/1 8. What happens to the electronegativity as the atomic radius increases? Why would changing the atomic radius affect the electronegativity? Hint: Try changing the horizontal axis of the graph to plot electronegativity vs. atomic radius. BIU E = Score: 0/2 E % = 10