Understanding the Atom for Middle School

Transcription

1 Understanding the Atom for Middle School

2 Table of Contents 1. Accessing Prior Knowledge Activity 2. The Atomic Model Worksheet and Key 3. The Atomic Model of Matter Graphic Organizer and key 4. Atomic Model of Matter Worksheet and key 5. Atom Notes 6. Complete Model of Atom Graphic Organizer and Key 7. Vocabulary Review and Key 8. Periodic Table 9. Understanding the Atom Finding Numbers of Protons, Neutrons, Electrons and Key 10. Drawing Bohr Models of Atoms 1 20 and Key 11. I Have You Have game reviewing concepts of atoms 12. Rules for Counting Atoms 13. Counting Atoms Worksheet and Key 14. Counting Atoms Review and Key 15. spdf Energy Levels Diagram and Periodic Table for Orbital Arrangement 16. Electron Arrangement Practice and Key 17. Electron Arrangement Worksheet and Key 18. Formula Weights

3 Name What You Already Know About the About the Structure of the Atom 1. Take out a piece of lined paper. 2. Number 1 to Write down one fact you know about the atom. 4. Turn paper over. 5. You have 1 minute to circulate the classroom asking as many classmates as possible what they wrote down. You must remember this. You may not write anything down. 6. After one minute back to your desk. 7. Write down as many responses from memory as you can. 8. How many responses can you recall My Fact Post Unit Reflection What I learned about the atom

4 Name Block The Atomic Model of Matter More than thousand years ago, A Greek philosopher named led a group of scientists now known as atomists. These early Greeks thought that the atom was the possible piece of matter that could be obtained. They guessed that the atom was a small, particle, and that all the atoms were made of the same material. They also thought that different atoms were different shapes and sizes, that the atoms were infinite in number, always and capable of joining together. In 1803, proposed an atomic theory. The theory stated that all elements were made of atoms and that the atoms were and indestructible particles. Dalton s theory also said that atoms of the same element were the same, while atoms of different elements were. The theory also said that were made by joining the atoms of two or more elements together. In 1897, J.J. Thomson discovered a particle even smaller than the atom. He named it the, but today we call it the. As a result of his discovery, Thomson proposed a new atomic. According to Thomson s model, the atom was like a plum it was mostly a thick, positively charged material, with negative electrons scattered about it like in a pudding. In 908, Ernest Rutherford took an extremely thin sheet of and bombarded it with electrons. Much to his surprise, most of the electrons went right through the foil, and the occasional was seriously deflected. To him, this seemed as likely as a baseball going

5 through a brick wall. He theorized that the gold foil must be mostly empty, or else the electrons would bounce off most of the time. He figured that the atom was made up of a small, dense, positively charged center, called the. Rutherford s theory has the electrons scattered around the atom s edge. In1913, Neil Bohr narrowed down the actual location of the electrons. Bohr s model was similar to Rutherford s in that it had a made up of positively charged material. Bohr went on to propose that the negative particles ( ) orbited the nucleus much like the planets the sun. Today the atomic model is very similar to Bohr s model. The modern atomic model, the Wave model, does not have exact orbits like Bohr did. Instead the modern model has a scatter region surrounding the where an will probably, but not certainly, be found.

6 The Atomic Model of Matter Key More than 2000 thousand years ago, A Greek philosopher nameddemocritus led a group of scientists now known as atomists. These early Greeks thought that the atom was the smallest possible piece of matter that could be obtained. They guessed that the atom was a small, hard particle, and that all the atoms were made of the same material. They also thought that different atoms were different shapes and sizes, that the atoms were infinite in number, always movingand capable of joining together. In 1803,Dalton proposed an atomic theory. The theory stated that all elements were made of atoms and that the atoms were indivisible and indestructible particles. Dalton s theory also said that atoms of the same element were the same, while atoms of different elements were different. The theory also said that compounds were made by joining the atoms of two or more elements together. In 1897, J.J. Thomson discovered a particle even smaller than the atom. He named it the corpuscle, but today we call it the electron As a result of his discovery, Thomson proposed a new atomic model. According to Thomson s model, the atom was like a plum pudding it was mostly a thick, positively charged material, with negative electrons scattered about it like plumsin a pudding. In 908, Ernest Rutherford took an extremely thin sheet of gold foil and bombarded it with electrons. Much to his surprise, most of the electrons went right through the foil, and the occasional bullet or electron was seriously deflected. To him, this seemed as likely as a baseball going through a brick wall. He theorized that the gold foil must be mostly empty space or else the electrons would bounce off most of the time. He figured that the atom was made up of a small, dense, positively charged center,

7 called the nucleus. Rutherford s theory has the electrons scattered around the atom s edge. In1913, Neil Bohr narrowed down the actual location of the electrons. Bohr s model was similar to Rutherford s in that it had a nucleus made up of positively charged material. Bohr went on to propose that the negative particles (electrons) orbited the nucleus much like the planets orbit the sun. Today the atomic model is very similar to Bohr s model. The modern atomic model, the Wave model, does not have exact orbits like Bohr did. Instead the modern model has a scatter region surrounding the nucleus where an electron will probably, but not certainly, be found

8 Name The Atomic Model of Matter On the graphic organizer provided summarize and illustrate the features of the atom for each model, and state the problem with each model. Democritus Model 2000 yrs ago Dalton Model Thomson Model Rutherford Model Bohr Model Wave Model - Modern

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10 Name Block The Atomic Model of Matter Match the statement to the different atomic model. Write the letter for the atomic model in front of the statement. A - Democritus B - Dalton C - Rutherford D - Thomson E - Bohr F - Modern Wave Model 1. Atoms are indivisible. 2. An atom is the smallest piece of matter. 3. In an atom, electrons are located in energy levels that are a certain distance from the nucleus. 4. Atoms are small, hard particles. 5. An atom has a small, positively charged nucleus surrounded by a large region in which scientists can predict where an electron is likely to be found. 6. In an atom, electrons move in definite orbits around the nucleus. 7. Atoms of the same element are exactly alike. 8. An atom is made of positively charged pudding-like material through which negatively charged particles are scattered. 9. An atom is mostly empty space with a dense, positively charged nucleus in the center. 10. An atom contains negatively charged particles called corpuscles.

11 The Atomic Model of Matter Key 1. A 2. A 3. E 4. A 5. F 6. E 7. B 8. D 9. C 10. D

12 The Atom What is an element? What is a compound? What is an atom? What are subatomic particles? What is a proton? -pure substance where all atoms are the same -cannot be broken down -can be a molecule -made up of two or more kinds of atoms [molecule] -atoms can be separated if enough energy is supplied -the smallest unit of matter consisting of protons, neutrons, electrons -particles that are smaller than an atom and make up the atom. They include protons, neutrons, and electrons -subatomic particle with a positive electric charge that are found within the nucleus at the center of the atom. The relative mass of the proton is 1 amu. What is a neutron? -subatomic particle with a zero electric charge that are found within the nucleus at the center of an atom. The relative mass of the neutron is 1 amu.

13 What is an electron? What is the atomic number? What is the atomic mass number? How do you calculate the number of electrons? -subatomic particles with a negative charge that are found orbiting around the nucleus of an atom. The relative mass of the electron is 1/1840 amu therefore the mass of an electron is considered to be neglible. -the number of protons in the nucleus of an atom Atomic # = # of protons -is the total number of protons and neutrons in the nucleus of an atom. Mass # = # of neutrons + # of protons -In a neutral atom the atomic number is also equal to the number of electrons. Atomic # = # of protons = # of electrons.

14 What is the atomic mass? -The quantity of matter that makes up an atom. The total mass of the protons, neutrons and electrons that make up an atom. It is the average mass of an element s naturally occurring isotopes, taking into account the percentage of occurrence on Earth of each isotope. What is an isotope? -There can be more than one version [isotope] of a particular element. Each version [isotope] has the same number of protons and electrons therefore the same atomic #, but each version has a different # of neutrons therefore a different mass #.

15 The Complete Model of the Atom Name Block Dalton s Atomic Theory

16 The Complete Model of the Atom Key Dalton s Atomic Theory 1. All matter is made up of atoms. 2. All elements that are the same have the same mass. Different elements have different masses. 3. Atoms of different elements bond to form compounds. 4. Matter cannot be created or destroyed. Orbits or energy levels 1 st orbit holds 2 electrons 2 nd orbit holds 8 electrons 3 rd orbit holds 8 electrons Electrons have - charge Outer orbit Holds valence electrons which are involved in chemical bonding Atom has no charge The Atomic Number = Number of Protons Number of Protons = Number of Electrons Atomic Mass = Number of Protons + Number of Neutrons Nucleus Positively charged center Contains Protons and Neutrons Protons + charge Neurons no charge

17 Vocabulary Review Name Block : the smallest particle of an element that has all the properties of that element. The atom has charge. The 3 main subatomic particles that make up the atom are the, and. : small, dense positively charged center of an atom. and are found in the nucleus. : positively charged particles in the nucleus. : neutral particles in the nucleus. : negatively charged particles orbiting the nucleus. The atomic mass of a neutron and a proton is. The atomic mass of an electron is. Number of = number of electrons Atomic mass subtract atomic number = number of. Label the following. 13 Al aluminum 26.98

18 Vocabulary Review Key atom: the smallest particle of an element that has all the properties of that element. The atom has nocharge. The 3 main subatomic particles that make up the atom are the proton, neutron and electron. nucleus: small, dense positively charged center of an atom. protons and neutrons are found in the nucleus. protons: positively charged particles in the nucleus. neutrons: neutral particles in the nucleus. electrons: negatively charged particles orbiting the nucleus. The atomic mass of a neutron and a proton is 1 amu. The atomic mass of an electron is 0 amu. Number of protons = number of electrons Atomic mass subtract atomic number = number of neutrons. Label the following. Atomic Number 13 Al aluminum Chemical Symbol Element Name Atomic Mass

19 Atomic Number 13 Al aluminum Chemical Symbol Element Name Atomic Mass

20 Understanding the Atom Particle Location Charge Mass Proton Neutron Electron Finding Atomic Number Recall Atomic Number = Number of Protons Element Symbol Atomic Number Number of Protons Hydrogen 1 Beryllium 4 Carbon 6 Cobalt 27 Krypton 36 Finding Atomic Mass Recall Mass Number = Number of Protons + Number of Neutrons Element Symbol Mass Number of Number of Number Protons Neutrons Hydrogen 1 0 Chromium Beryllium 4 5 Carbon 12 6 Gold Cobalt Barium Iron 56 26

21 Key Particle Location Charge Mass Proton nucleus + 1 amu Neutron nucleus - 1 amu Electron orbits No charge 0 amu Finding Atomic Number Recall Atomic Number = Number of Protons Element Symbol Atomic Number Number of Protons Hydrogen H 1 1 Beryllium Be 4 4 Carbon C 6 6 Cobalt Co Krypton Kr Finding Atomic Mass Recall Mass Number = Number of Protons + Number of Neutrons Element Symbol Mass Number of Number of Number Protons Neutrons Hydrogen H Chromium Cr Beryllium Be Carbon C Gold Au Cobalt Co Barium Ba Iron Fe

22 Finding the Number of Electrons Recall Atomic Number = Number of Protons = Number of Electrons Element Symbol Atomic Number Number of Protons Number of Electrons Number of Neutrons Mass Number Oxygen 8 16 Sodium Carbon 6 12 Phosphorus Potassium Iron Copper Chlorine Boron Aluminum Maximum Number of Electrons in First Three Orbits The orbit closest to the nucleus must be full before electrons can be place on the next orbit. 1 st Orbit 2 nd Orbit 3 rd Orbit Maximum Number of Electron Look at your periodic table. Notice in period 1 there are only two elements and that the 1 st orbit only holds 2 electrons. In period 2 and 3 there are eight elements and notice that the 2 nd and 3 rd orbit holds 8 electrons. In the 4 th level the placement of electrons becomes more complex.

23 Finding the Number of Electrons Key Recall Atomic Number = Number of Protons = Number of Electrons Element Symbol Atomic Number Number of Protons Number of Electrons Number of Neutrons Mass Number Oxygen O Sodium Na Carbon C Phosphorus P Potassium K Iron Fe Copper Cu Chlorine Cl Boron B Aluminum Al Maximum Number of Electrons in First Three Orbits The orbit closest to the nucleus must be full before electrons can be place on the next orbit. 1 st Orbit 2 nd Orbit 3 rd Orbit Maximum Number of Electron Look at your periodic table. Notice in period 1 there are only two elements and that orbit one only holds 2 electrons. In period 2 and 3 there are eight elements and notice that the 2 nd and 3 rd orbit holds 8 electrons. In the 4 th level the placement of electrons becomes more complex. We will work first with elements 1 to 20.

24 Drawing Bohr Models 1. Write down element name and symbol. 2. Draw circle to represent nucleus. 3. Atomic number = number of protons. 4. Record protons in nucleus as P 5. Round the atomic mass and subtract atomic number. This is the number of neutrons. Record in nucleus as N 6. The number of protons = the number of electrons. 7. Fill 1 st orbit with 2 electrons. 8. Remaining electrons to 2 nd orbit. Fill only to Remaining electrons to 3 rd orbit. Fill only to 8. Example Sodium Na 11 P 12 N

25 Name Block Drawing Bohr Model of Atoms 1 to 20 Write the name of the element and calculate the number of protons and neutrons and draw the electrons on the orbits,

26 Further Practice Element Atomic Number Mass Number Protons Electron Neutrons 1 st orbit 2 nd orbit 3 rd orbit Sodium Aluminum Sulfur Chlorine Magnesium Phosphorus

27 Key Element Symbol Protons Neutrons 1st 2nd 3rd 4th Hydrogen H Helium He Lithium Li Beryllium Be Boron B Carbon C Nitrogen N Oxygen O Fluorine F Neon Ne Sodium Na Magnesium Mg Aluminum Al Silicon Si Phosphorus P Sulfur S Chlorine Cl Argon Ar Potassium K Calcium Ca Further Practice Element Atomic Number Mass Number Protons Electron Neutrons 1 st orbit 2 nd orbit 3 rd orbit Sodium Aluminum Sulfur Chlorine Magnesium Phosphorus

28 Understanding the Atom Review Name Block Completion - Fill in the missing word Element Composition The smallest part of an element with the properties of that element is called the. There are three parts that make up an atom. Given the charge, identify the particle: [+], [-], [0]. The center of the atom is called the. It contains the and the protons. The circle around the center in paths called. The charge on the nucleus of an atom is always. Two subatomic particles must always have the same numbers. The must always equal the. Any substance with only one kind of atom, and it cannot be further broken down, is called:. Any substance that consists of two or more atoms [same or different] is called a. Any substance that consists of two or more different types of atoms is called a. Draw Bohr models of fluorine and sodium. P N P N

29 Complete the Chart Element Symbol Atomic Number Mass Number # of Protons # of Neutrons # of Electrons Helium Mg Ca Silver 26 6 Fl Gold

30 Choose the Best Description for the Vocabulary Term and Place the Letter in front of the Term. 1. atom 2. electron 3. nucleus 4. proton 5. neutrons 6. shell 7. atomic number 8. atomic mass 9. no charge 10. Bohr diagram A. A positively-charged particle in the center of an atom. B. The atom s charge. C. Flattened picture of the electrons in an atom. D. The neutral particles in the center of an atom. E. The empty space between the electrons and the nucleus. F. The combination of atoms to form a compound. G. Bohr s explanation of electron orbits around the nucleus. H. The number of protons in the nucleus. I. Negatively-charged particle discovered by J. J. Thomson. J. Total number of protons and neutrons in the nucleus. K. Positively charged particles that orbit in shells around the nucleus. L. The center of an atom. M. The smallest piece of an element. N. Moving up to a higher electron shell

31 Understanding the Atom Review Key Element Composition The smallest part of an element with the properties of that element is called the atom There are three parts that make up an atom. Given the charge, identify the particle: [+] proton, [-] electron [0] neutron. The center of the atom is called the nucleus. It contains the netrons and the protons. The electrons circle around the center in paths called orbits. Shells, energy levels. The charge on the nucleus of an atom is always positive. Two subatomic particles must always have the same numbers. The protons must always equal the electrons. Any substance with only one kind of atom, and it cannot be further broken down, is called: element. Any substance that consists of two or more atoms [same or different] is called a molecule. Any substance that consists of two or more different types of atoms is called a compound.

32 Sodium Na 11 P 12 N Complete the Chart Fluorine F 9 P 10 N

33 Element Symbol Atomic Number Mass Number # of Protons # of Neutrons # of Electrons Helium He Magnesium Mg Zinc Zn Bromine Br Aluminum Al Uranium U Sodium Na Calcium Ca Silver Ag Iron Fe Carbon C Fluorine Fl Mercury Hg Nitrogen N Gold Au M 6. G 2. I 7. H 3. L 8 J 4. A 9. B 5. D 10. C

34 I Have You Have Cut out the cards and distribute one to each student. The student with the first card begins. They pose the question and the student with the card with answer stands and answers. They then pose the question at the bottom of their card. This game is designed to be used by students using their Periodic Tables. I have the first card. Who has the element with 20 protons I have calcium. Who has matter made up of only one type of atom? I have Element. Who has the positive electric charge within the atom nucleus? I have proton. Who has chart listing all the known elements? I have the Periodic Table. Who has the element with 26 electrons? I have iron. Who has the element with 2 neutrons and 2 protons?

35 I have helium. Who has the element used in thermometers? I have mercury. Who has the negative electric charge which orbits the nucleus? I have electron. Who has the element with atomic number 6? I have carbon. Who has the smallest piece of matter? I have the atom. Who has the element with 55 protons? I have cesium. Who has the second element in the Noble gas family? I have neon. Who has the total number of protons + the total number of neutrons? I have the atomic mass. Who has the neutral electric charge found in the nucleus? I have neutrons. Who has the most abundant element in Earth s crust?

36 I have oxygen. Who has the element with symbol Na? I have sodium. Who has the element used for fancy serving sets and tarnishes? I have silver. Who has the abbreviation for the element name I have a chemical symbol. Who has the element with 19 protons? I have potassium. Who has the lightest element? I have hydrogen. Who has the electric charge on the entire atom? I have no charge. Who has the term by which elements are listed on the Periodic Table? I have the atomic number Who has the element with chemical symbol K? I have potassium. Who has the element with symbol Au?

37 I have gold. Who has the element with 5 protons and 6 neutrons? I have boron. Who has the element which is the most abundant gas in air? I have nitrogen. Who has the unit for measurement for subatomic particles? I have atomic mass units or amu. Who has the element with the atomic number 53? I have iodine. Who has the term for the most numerous elements on the periodic table? I have metals. And I have the last card!

38 3(Ca 3 P 2 ) Coefficient Indicates the number of molecules and multiplies all atoms in the formula that follow Subscript Indicates the number of atoms of that symbol Ca 3 P 2 Na(OH) 3(Ca 3 P 2 ) Au 3 (PO 4 ) Ca 3 (PO 3 ) 2 Add the subscripts. Answer = 5 atoms We never write 1 as a subscript. 1 sodium + 1 oxygen + 1 hydrogen = 3 atoms Add the subscripts and multiply by the coefficient. 5 atoms x 3 = 15 atoms Some atoms are grouped in a bracket. Just add them up. 3 gold+ 1 phosphorus + 4 oxygen = 8 atoms A subscript to the right of a bracket multiplies all the atoms within the bracket to the left. 3 calcium + 2 phosphorus + 6 oxygen = 11 atoms

39 Board Practice NaHCO 3 C 2 H 4 O 2 (NH 4 ) 3 PO 4 3H 3 PO 4 (NH 4 ) 2 (CrO 4 ) 4CaCO 3

40 Board Practice NaHCO 3 1 sodium + 1 hydrogen + 1 carbon + 3 oxygen = 6 atoms C 2 H 4 O 2 2 carbon + 4 hydrogen + 2 oxygen = 8 atoms (NH 4 ) 3 PO 4 3 nitrogen + 12 hydrogen + 1 phosphorus + 4 oxygen = 24 atoms 3H 3 PO 4 9 hydrogen + 3 phosphorus + 12 oxygen = 24 atoms (NH 4 ) 2 (CrO 4 ) 2 nitrogen + 8 hydrogen + 1 chromium + 4 oxygen = 15 atoms 4CaCO 3 4 calcium + 4 carbon + 12 oxygen = 20 atoms

41 Counting Atoms Name Block 1. H NaF 3. Rb(NO 2 ) 4. H(OH) 5. Sc 2 O 3 6. TiBr (V 2 O 5 ) 8. H 2 (SO 4 ) 9. 3[Li(OH)] 10. 2[H 3 (PO 4 )] 11. Na 3 (PO 3 ) 12. Ca 3 (PO 4 ) Ti(ClO 3 ) Sc(MnO 4 ) Fe 2 (Cr 2 O 7 ) [Al(OH) 3 ] 17. 4[H(NO 3 )] 18. 3(C 6 H 11 O 6 ) 19. 2[Al(MnO 4 ) 3 ] 20. Pb(CrO 4 ) [Ti(HCO 3 ) 4 ] 22. (NH 4 )(OH) 23. 2[Mg 3 (AsO 4 ) 2 ] 24. 3[Au 2 (SO 3 )] 25. Co(CN) [(NH 4 ) 2 (Cr )] 27. Sr(ClO 3 ) Pb(CrO 4 ) KI 30. Pb(NO 3 ) 2

42 Counting Atoms Key 1. H hydrogen, 1 oxygen = 3 2. NaF- 1 sodium, 1 fluorine = 2 3. Rb(NO 2 ) - 1 rubidium, 1 nitrogen, 2 oxygen = 4 4. H(OH)-1 hydrogen, 1 oxygen, 1 hydrogen = 3 5. Sc 2 O 3-2 scandium, 3 oxygen = 5 6. TiBr 4-1 titanium, 4 bromine = (V 2 O 5 ) vanadium, 15 oxygen = H 2 (SO 4 ) 2 hydrogen, 1 sulfur, 4 oxygen = [Li(OH)] 3 lithium, 3 oxygen, 3 hydrogen = [H 3 (PO 4 )] 6 hydrogen, 2 phosphorus, 8 oxygen = Na 3 (PO 3 ) 3 sodium, 1 phosphorus, 3 oxygen = Ca 3 (PO 4 ) 2-3 calcium, 2 phosphorus, 8 oxygen = Ti(ClO 3 ) 3 1 titanium, 4 chlorine, 12 oxygen = Sc(MnO 4 ) 3 1 scandium, 3 manganese, 12 oxygen = Fe 2 (Cr 2 O 7 ) 3 2 iron, 6 chromium, 21 oxygen = [Al(OH) 3 ] 2 aluminum, 6 oxygen, 6 hydrogen = [H(NO 3 )] 4 hydrogen, 4 nitrogen, 12 oxygen = (C 6 H 11 O 6 ) - 18 carbon, 33 hydrogen, 18 oxygen = [Al(MnO 4 ) 3 ] 2 aluminum, 6 manganese, 24 oxygen = Pb(CrO 4 ) 4 1 lead, 4 chromium, 16 oxygen = [Ti(HCO 3 ) 4 ] - 3 titanium, 12 hydrogen, 12 carbon, 36 oxygen = (NH 4 )(OH) - 1 nitrogen, 4 hydrogen, 1 oxygen, 1 hydrogen = [Mg 3 (AsO 4 ) 2 ] - 6 manganese, 4 arsenic, 16 oxygen = [Au 2 (SO 3 )] 6 gold, 3 sulfur, 9 oxygen = Co(CN) 3 1 cobalt, 3 carbon, 3 nitrogen = [(NH 4 ) 2 (Cr 2 o 7 )] 4 nitrogen, 16 hydrogen, 4 chromium, 14 oxygen = Sr(ClO 3 ) 2 1 strontium, 2 chlorine, 8 oxygen = Pb(CrO 4 ) 2 1 lead, 2 chromium, 8 oxygen = KI 1 potassium, 1 iodine = Pb(NO 3 ) 2 1 lead, 2 nitrogen, 6 oxygen = 9 1.

43 Counting Atoms Name Block 1. NaBr = atoms 2. MgO = atoms 3. K(MnO 4 ) = atoms 4. Ni(SO 4 ) = atoms 5. Zn(HSO 4 ) 2 = atoms 6. Na 2 (SO 4 ) = atoms 7. (NH 4 )(HCO 3 ) = atoms 8. Ca 3 (PO 4 ) 2 = atoms 9. 2[Li 3 (PO 4 )] = atoms 10. 3[Sc(MnO 4 ) 3 ] = atoms

44 Counting Atoms KEY Name Block 1. NaBr 1 sodium 1 bromine = 2 atoms 2. MgO 1 magnesium 1 oxygen = 2 atoms 3. K(MnO 4 ) 1 potassium, 1 manganese 4 oxygen = 6 atoms 4. Ni(SO 4 ) 1 nickel, 1 sulfur 4 oxygen = 6 atoms 5. Zn(HSO 4 ) 2 1 zinc, 2 hydrogen, 2 sulfur, 8 oxygen = 13 atoms 6. Na 2 (SO 4 ) 2 sodium, 1 sulfur, 4 oxygen = 7 atoms 7. (NH 4 )(HCO 3 ) 1 nitrogen, 5 hydrogen, 1 carbon, 3 oxygen = 10 atoms 8. Ca 3 (PO 4 ) 2 3 calcium, 2 phosphorus, 8 oxygen = 13 atoms 9. 2[Li 3 (PO 4 )] 6 lithium, 2 phosphorus, 8 oxygen = 16 atoms 10. 3[Sc(MnO 4 ) 3 ] 3 scandium, 9 manganese, 36 oxygen = 48 atoms

45 Energy Level Diagram for Quantum Levels, Orbitals, and Related Periods 7p 6d 5f n = 7 7s 6p 5d 4f n = 6 6s 5p 4d n = 5 5s 4p 3d n = 4 4s Energy 3p n = 3 3s 2p n = 2 2s n = 1 1s

46 s orbital block The s, p, d, f orbital blocks of the Periodic Table p orbital block d orbital block f orbital block

47 Board Practice Energy levels for the atoms have sublevels. Sublevels must be completely filled period by period. Look at the energy level diagram for the pattern. The sublevels are represented by letters, spdf Refer to the energy level diagram. Each circle represents 2 electrons. When recording the number of electrons in a sublevel, write the sublevel and follow it with the number of electrons superscripted. For example: Hydrogen Atomic Number 1 1s 1 Magnesium Atomic Number 12 1s 2 2s 2 2p 6 3s 2 Add the superscripts Note it equals 12, the same as the atomic number. Silver Atomic Number 47 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 9

48 Now You Try Element 1 st orbit 2 nd orbit 3 rd orbit 4 th orbit 5 th orbit Sulfur (16) Gallium (31) Strontium (38) Tin (50)

49 Board Practice Element 1 st orbit 2 nd orbit 3 rd orbit 4 th orbit 5 th orbit Sulfur (16) Gallium (31) Strontium (38) Tin (50) 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 5s 2 4d 10 5p 2

50 Complete the Following Table. Show the spdf Electron Arrangement. Name Name Symbol Atomic Number hydrogen helium lithium nitrogen fluorine silicon potassium calcium zinc cobalt krypton zirconium silver Mass Number Protons Neutron 1st 2nd 3rd 4th 5th

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52 1. Determine the name for each element from the chemical symbols 2. Write down the number of atoms for each element. 3. Write down the atomic mass for each element. Round it to the units place. 4. Calculate the total weight of the atoms for each element. Number of atoms x atomic mass 5. Calculate the total weight of the compound by totaling the weight of each individual atom. 6. Don t forget your units.

53 Formula Weights Sodium chloride NaCl Element # of atoms Atomic weight Total weight of atoms Formula Weight Zinc nitride Zn 3 N 2 Element # of atoms Atomic weight Total weight of atoms Formula Weight Barium Nitrate Ba(NO 3 ) 2 Element # of atoms Atomic weight Total weight of atoms Formula Weight

54 Formula Weights Sodium chloride NaCl Element # of atoms Atomic weight Total weight of atoms sodium chlorine Formula Weight 58 amu Zinc nitride Zn 3 N 2 Element # of atoms Atomic weight Total weight of atoms zinc nitrogen Formula Weight 223 amu Barium Nitrate Ba(NO 3 ) 2 Element # of atoms Atomic weight Total weight of atoms barium nitrogen oxygen Formula Weight 261 amu

55 Name Block Calculating Formula Weights Hydrogen sulphate H 2 SO 4 Element # of atoms Atomic weight Total weight of atoms Formula Weight Sodium bicarbonate NaHCO 3 Element # of atoms Atomic weight Total weight of atoms Formula Weight Lead IV arsenate Pb 3 (AsO 4 ) 4 Element # of atoms Atomic weight Total weight of atoms Formula Weight

56 Iron II nitrate Fe(NO 3 ) 2 Element # of atoms Atomic weight Total weight of atoms Formula Weight Aluminum sulphate Al 2 (SO4) 3 Element # of atoms Atomic weight Total weight of atoms Formula Weight Chromium sulphate Cr(SO 4 ) 3 Element # of atoms Atomic weight Total weight of atoms Formula Weight

57 Lead III chromate 2{Fe 2 (CrO4) 3 Element # of atoms Atomic weight Total weight of atoms Formula Weight Scandium bicarbonate Sc(HCO 3 ) 3 Element # of atoms Atomic weight Total weight of atoms Formula Weight Iridium dichromate Ir2(CrO7)3 Element # of atoms Atomic weight Total weight of atoms Formula Weight

58 Calculating Formula Weights KEY Hydrogen sulphate H 2 SO 4 Element # of atoms Atomic weight Total weight of atoms hydrogen sulfur oxygen Formula Weight 98 amu Sodium bicarbonate NaHCO 3 Element # of atoms Atomic weight Total weight of atoms sodium hydrogen carbon oxygen Formula Weight 84 amu Lead IV arsenate Pb 3 (AsO 4 ) 4 Element # of atoms Atomic weight Total weight of atoms lead arsenic oxygen Formula Weight 1177 amu

59 Iron II nitrate Fe(NO 3 ) 2 Element # of atoms Atomic weight Total weight of atoms iron nitrogen oxygen Formula Weight 180 amu Aluminum sulphate Al 2 (SO4) 3 Element # of atoms Atomic weight Total weight of atoms aluminum sulfur oxygen Formula Weight 342 amu Chromium sulphate Cr(SO 4 ) 3 Element # of atoms Atomic weight Total weight of atoms chromium sulfur oxygen Formula Weight 392 amu

60 Lead III chromate 2{Fe 2 (CrO4) 3 Element # of atoms Atomic weight Total weight of atoms lead chromium oxygen Formula Weight 920 amu Scandium bicarbonate Sc(HCO 3 ) 3 Element # of atoms Atomic weight Total weight of atoms scandium hydrogen carbon oxygen Formula Weight 228 amu Iridium dichromate Ir2(CrO7)3 Element # of atoms Atomic weight Total weight of atoms iridium chromium oxygen Formula Weight 876 amu

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