BIOCHEM LAB_At-Home 02 Periodic Table and Ionic Bonding_3ed

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Feb 20, 2024

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Integrated General Biology Name Laboratory At Home Instructor BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding Before You Start Part A will require that you use the nucleus cut-out included at the end of this lab or the ones you received in your materials box. You will require a hard copy of these two pages: 1) Subatomic Particles 2) Diagram of Nucleus and Electrons Energy Levels Part B will require that you insert a graph as part of the lab. You can make the graph in MS Excel or Google Sheets, you can draw the graph on graph paper, or you can use another statistics app to create your graph. Whichever method you choose, you will need to insert it as a picture. Part A — Patterns in the Periodic Table Protons are the defining part of the atom—the number of protons determines which element it is. In this activity, use your periodic table to answer questions and look for patterns. 1. Write the chemical symbol next to the correct number of protons. Number of Protons Chemical symbol 1 H 2 He 3 Li 4 Be 5 B 6 C © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 1

Integrated General Biology Name Laboratory At Home Instructor 2. Refer to the Periodic Table to answer the following questions. In terms of how the periodic table is arranged, what pattern do you notice? Atomic number increases as you move to the right and down the columns How many protons does uranium have? 92 Are there any uranium atoms that don’t have this number of protons? No 3. Atoms are electrically neutral—that means that their overall charge must be equal to zero. What is the charge on protons? Positive What is the charge on neutrons? Neutral charge or no charge What is the charge on electrons? Negative In regards to the number of sub-atomic particles, what has to happen in order for an atom to be electrically neutral? Must have an equal number of protons and electrons 4. Determine the number of protons and electrons for the following elements (all in atomic form). Chemical symbol Protons Electrons Na 11 11 Mg 12 12 Cl 17 17 Ar 18 18 Fe 26 26 5. What two subatomic particles determine charge? Electron and Proton 6. What two subatomic particles determine mass? Protons and Neutrons While every atom of carbon has exactly 6 protons, they do not all have the same number of neutrons— there are different types of carbon atoms, called isotopes . There are three naturally occurring isotopes of carbon. If you found a carbon atom, it would have 6 protons, but it may have 6, 7 or 8 neutrons. These isotopes occur in different relative amounts in nature. Generally speaking, the most common isotope is the nearest whole number to the average atomic mass. © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 2

Integrated General Biology Name Laboratory At Home Instructor To examine isotopes, we will look only at the nucleus of these isotopes, without any of the electrons orbiting around the nucleus. Which one is the most common variety of carbon. Is it carbon-12, carbon-13 or carbon-14? If you were able to capture carbon atoms one at a time, and you gathered a whole bunch of them, you would find that you had a lot of carbon-12 atoms, very few carbon-13 atoms, and a super small number of carbon-14 atoms. And if you took the average of all of these atoms, it would be very close to 12. This is why it is the most common isotope of carbon. Generally speaking, the most common isotope is the whole number that is nearest to the average atomic mass. Chemical symbol Protons Average Atomic Mass Nearest Whole Number Most Common Isotope (MCI) Neutrons in MCI H 1 1.008 1 Hydrogen-1 0 He 2 4.0026 4 Helium-4 2 Li 3 6.941 7 Lithium-7 4 Be 4 9.012 9 Beryllium-9 5 B 5 10.811 11 Boron-11 6 C 6 12.011 12 Carbon-12 6 N 7 14.007 14 Nitrogen-14 7 O 8 15.999 16 Oxygen-16 8 F 9 18.998 16 Flourine-19 10 Ne 10 20.1797 `19 Neon-20 10 7. Complete the table. The “Neutrons in MCI” column refers to the number of neutrons in the most common isotope. Other isotopes will have a different number of neutrons. © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 3

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Integrated General Biology Name Laboratory At Home Instructor 8. Refer to the worksheets at the end of this lab. Using the Subatomic Particles sheet, cut out the protons, neutrons and electrons. Choose an “A” group element (from a column like 7A) and make the MCI for an element in that group. Only use an element from rows 2 or 3 (don’t use rows 1, 4 or higher). Insert a picture of your element here. © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 4

Integrated General Biology Name Laboratory At Home Instructor Part B — Solving a Mystery with Geometry Now that you have mastered the number of subatomic particles in each element, it is time to focus on the subatomic particle that determines how an atom behaves chemically: the electron . Get your periodic table out and refer to it as often as necessary. Quickly glance at table 1 , and then read ahead. Table 1: First and Second Ionization Energies for the first 36 elements Atomic Number Element (Symbol) 1 st Ionization Energy J (x10 -19 ) 2 nd Ionization Energy J (x10 -19 ) 1 H 21.8 Does not have a 2 nd electron 2 He 39.4 87.2 3 Li 8.6 121.2 4 Be 14.9 29.2 5 B 13.3 40.3 6 C 18.0 39.1 7 N 23.3 47.4 8 O 21.8 56.3 9 F 27.9 56.0 10 Ne 34.6 65.6 11 Na 8.2 75.8 12 Mg 12.3 24.1 13 Al 9.6 30.2 14 Si 13.1 26.2 15 P 16.8 31.7 16 S 16.6 37.4 17 Cl 20.8 38.2 18 Ar 25.2 44.3 19 K 7.0 50.7 20 Ca 9.8 19.0 21 Sc 10.5 20.5 22 Ti 10.9 21.8 23 V 10.8 23.5 24 Cr 10.8 26.4 25 Mn 11.9 25.1 26 Fe 12.7 25.9 27 Co 12.6 27.3 28 Ni 12.2 29.1 29 Cu 12.4 32.5 30 Zn 15.1 28.8 31 Ga 9.6 32.9 32 Ge 12.7 25.5 33 As 15.7 29.9 34 Se 15.6 34.0 35 Br 18.9 34.9 36 Kr 22.4 39.0 © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 5

Integrated General Biology Name Laboratory At Home Instructor The periodic table can seem very confusing at first. But, being a scientist, you know to look for patterns. You have already found the patterns of increasing proton numbers and average atomic masses. Now we need to find a pattern in electrons, especially the outermost number of electrons (or valence electrons). Patterns often become more obvious when we make a picture—in mathematics, this is called geometry, and a graph is a type of picture. 1. Examine Table 1. This table shows how much force (measured in Joules) is required to remove an electron (or two) from the outermost shell of electrons (the highest energy level). When an atom gains or loses an electron, it is now called an ion. This is the reason it is called ionization, which is the process of forming an ion. Metals generally lose electrons, while nonmetals tend to gain electrons. We will look for patterns that emerge from this data. This is the stuff of science— gathering data and analyzing it! One of the best ways to see patterns is with a graph. You may print the graph paper in this document at the end of this part, or use your own graph paper or a computer program. 2. Make a graph of the first ionization energies (not the second) that shows how the ionization energies vary as the atomic number increases. The x-axis should be labeled “ Atomic number ,” with 1 through 36, since there are 36 elements in the chart. The y-axis should be labeled “Ionization Energies (J x10 -19 ),” with 0 to 130. Upload your graph to the end of this assignment. 3. Write the first ionization energy of 8.6 x 10 -19 in standard decimal form. 0.00000000000000000086 4. Is this a large or small value? Is it positive or negative? Explain. It has a small value and a positive number because its more than zero. 5. Now that you have plotted the data and made a graph, some patterns become visible. Based on the graph answer the following questions. What column has the peaks, with high ionization energies? Column 8A What column has the low points after the peaks? Column 1 © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 6

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Integrated General Biology Name Laboratory At Home Instructor 6. Draw four bold lines down your graph that group the elements into their four periods, or rows, as represented on the periodic table. (For example: Row 1 has only H and He in it—draw the first line on your graph directly on the vertical line with He, atomic number 2.) What patterns emerge? Click or tap here to enter text. 7. When a relatively large amount of energy is required to remove an electron, that atom is considered to have a relatively stable arrangement of electrons, or electron configuration . Complete the table. Row Atomic Numbers Element with the most stable arrangement (highest 1st ionization energy) 1 1 – 2 Helium 2 3 – 10 Neon 3 11 – 18 Argon 4 19 – 36 Krypton 8. Which elements are not stable, with low ionization energies after peaks? Alkali metals 9. Which column do these elements fit into (generally)? Column 1A 10. How many valence electrons do atoms in this column have? 1 valence elecreon 11. Generally speaking, describe what the second ionization energy is like for elements in column 1. Explain why this would be so. (Remember that the second ionization energy means that a second electron is being removed.) The second ionization energy is bigger thanthe fist because it requires more energy to remove an electron from a cation than from a neutral atom. © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 7

Integrated General Biology Name Laboratory At Home Instructor 12. Look at the 2 nd ionization energy, for Be, Mg and Ca and compare them to the 2 nd ionization energy of the element before them. How do these compare? Valence electrons 13. Which column do these elements fit into? 2a 14. How many valence electrons do atoms in this column have? 2 valence electrons 15. Generally speaking, state a rule about elements in the second column that relates their number of electrons in their outermost shell (valence) and how they form an ion. Click or tap here to enter text. 16. Insert a picture of your graph of the first ionization energies here. © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 8

Integrated General Biology Name Laboratory At Home Instructor Title: _________________________________ (Turn this graph sideways) © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 9

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Integrated General Biology Name Laboratory At Home Instructor Part C — Ionic Bonds When a metal bonds with a nonmetal, an ionic bond is formed—this is named an ionic bond because both atoms have now formed into ions. The metal loses a negative electron and becomes positive. The nonmetal gains a negative electron and becomes negative. But what is the size of the charge on the ion? How many of each atom is necessary to form the bonds? Use the cutouts to help you see how this works. These are another form of a geometric solution! 1. The valence electrons play the critical role in an atom’s chemical behavior. Sodium is in column 1, so it has one valence electron. Sodium is a metal —it is malleable and shiny, it conducts electricity well, and it holds its outermost electron loosely (it has a small ionization energy). When sodium loses an electron, it becomes a sodium ion. When sodium loses its outermost electron, it now has the same electron configuration as the noble gas neon—a very stable arrangement indeed. How many positive protons does sodium have? 11 How many negative electrons does a sodium ion have? 10 What is the charge (number and sign) on a sodium ion? +1 What column is sodium in? 1st column 2. Chlorine is a nonmetal —it does not conduct electricity well and it gains electrons when it forms an ion. When chlorine gains an electron, it has the same electron configuration as the noble gas argon—a stable arrangement. How many positive protons does chlorine have? 17 How many negative electrons does a chlorine ion have? 18 What is the charge on a chlorine ion? 1- What column is chlorine in? Column 7a Review the charges on the sodium ion and on the chloride. Notice how they balance each other. Ionic compounds will form in a way so that their overall charge is zero. This may mean that there will be more than one of each atom, but not in this case. Na 1+ and Cl 1- balance to zero. Na 1+ and Cl 1- 1+ and 1- 1 + -1 = 0 © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 10

Integrated General Biology Name Laboratory At Home Instructor 3. Since each chlorine atom is able to accept one electron, explain how sodium chloride is formed. (Notice that the metal is said and written first, and the nonmetal’s ending is changed to “–ide” when it has formed an ion.) Refer to the Lewis dot structures, that show an atom’s valence electrons as the dots, that are provided for you in your explanation. An electron I stransferred from sodium to chlorine. Sodium becomes a positive ion and chlorine becomes a negative ion. Positive and negative ions attract each other and form an ionic bond and the compound sodium chlroine. 4. Magnesium is in column 2. How many valence electrons does it have? 2 For magnesium to have a stable electron configuration (like a noble gas), it has to lose two electrons. What is the ionic charge on a magnesium ion? 2+ How many chlorine atoms would be necessary to accept the 2 electrons from magnesium? 2 atoms Mg 2+ and two Cl 1- Mg 2+ and Cl 1- and Cl 1- 2+ and 1- and 1- 2 + -1 + -1 = 0 Draw the Lewis dot structures that show how this works and upload a picture of your drawing in this space. (Hint: you’ll have to draw a total of three Lewis dot structures this time.) Use arrows to show where the electrons go. 5. What would the formula be for magnesium chloride? mgCl2 (Remember that chemical formulas are written with the number of atoms in the compound as a © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 11

Integrated General Biology Name Laboratory At Home Instructor subscript—except for “1”s, which are simply left blank. For example, “CO 2 ” has one atom of carbon and two atoms of oxygen. But for now, it is fine if you write the “1”s, like “C 1 O 2 ”.) 6. Ionic bonds are formed when a metal bonds with a nonmetal. The nonmetal essentially takes the electron(s) away from the metal. Predict the formula for aluminum bromide. Draw Lewis dot structures, if you like. AlBr3 7. Where are the metals found on the periodic table? Click or tap here to enter text. 8. Where are the nonmetals found on the periodic table? Click or tap here to enter text. 9. Atoms in columns 1A, 2A, or 3A will generally lose their valence electron(s), making the shell underneath its new valence shell, which is complete like its nearest noble gas. Atoms in columns 5A, 6A, or 7A will generally gain electrons in their outermost shell until they have the same arrangement as a noble gas. Column 4A could gain, lose or share electrons, depending on the situation. Column 8A (the Noble Gases) does not commonly bond with other atoms, since it already has a stable arrangement. The transition metals usually have a roman numeral following their symbol which tells you how many valence electrons that atom has—these numerals can be different in different problems since many transition metals are not consistent with their number of valence electrons. Predict the formula for calcium oxide (Ca 2+ and O 2- ). One Ca 2+ and one O 2- = 2 + -2 = 0 Click or tap here to enter text. Predict the formula for aluminum sulfide (Al 3+ and S 2- ). Two Al 3+ and three S 2- = 3 + 3 + -2 + -2 + -2 = 0 Click or tap here to enter text. Predict to formula for iron (III) iodide (Fe 3+ and I 1- ). One Fe 3+ and three I 1- = 3 + -1 + -1 + -1 = 0 Click or tap here to enter text. An interesting pattern can be seen when writing ionic charges before writing the chemical formula. (Remember: charges are written superscript while how many atoms there are is written subscript.) Ionic charges Formula Ca 2+ O 2- Ca 1 O 1 Mg 2+ F 1- Mg 1 F 2 Li 1+ N 3- Li 3 N 1 Al 3+ S 2- Al 2 S 3 © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 12

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Integrated General Biology Name Laboratory At Home Instructor Did you notice the pattern? Once the ionic charges have been determined, you can figure out the formula by dropping the signs and switching the values. But, be careful: be sure to simplify if the numbers have a common factor. Once again, refer to your periodic table to answer the following questions. 10. How many valence electrons do neon, argon and krypton have? Click or tap here to enter text. What column are these elements in? Click or tap here to enter text. What is the ionic charge when an element from this column forms an ion? Click or tap here to enter text. What is the name for the elements in this column? Click or tap here to enter text. 11. How many valence electrons do lithium, sodium and potassium have? Click or tap here to enter text. What column are these elements in? Click or tap here to enter text. What is the ionic charge when a metal from this column forms an ion? Click or tap here to enter text. What is the name for the elements in this column? Click or tap here to enter text. 12. How many valence electrons do beryllium, magnesium and calcium have? Click or tap here to enter text. What column are these elements in? Click or tap here to enter text. What is the ionic charge when an atom from this column forms an ion? Click or tap here to enter text. What is the name for the elements in this column? Click or tap here to enter text. 13. How many valence electrons do fluorine, chlorine and bromine have? Click or tap here to enter text. What column are these elements in? Click or tap here to enter text. What is the ionic charge when an atom from this column forms an ion? Click or tap here to enter text. What is the name for the elements in this column? Click or tap here to enter text. © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 13

Integrated General Biology Name Laboratory At Home Instructor © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 14

Integrated General Biology Name Laboratory At Home Instructor Subatomic Particles Electrons Neutrons Protons – – – – – – – – – – – – – – – – – – – – – – – – – – – – – – + + + + + + + + + + + + + + + + + + + + + + + + © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 15

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Integrated General Biology Name Laboratory At Home Instructor Diagram of Nucleus and Electron Energy Levels Nucleus © 2020 Socratis, LLC. This material may not be reproduced, displayed, modified or distributed without express prior permission. BIOCHEMISTRY At-Home Lab: Periodic Table and Ionic Bonding 16

BIOCHEM LAB_At-Home 02 Periodic Table and Ionic Bonding_3ed

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