Complete the following chart: (assume the overall charge on all atoms = 0...except the last one. #of Protons. #of Neutrons. He 4

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1 Name: Period: Complete the following chart: (assume the overall charge on all atoms = 0....except the last one Element Symbol Atomic Number #of Protons #of Neutrons Hydrogen 1 Mass Numbra- (amu) #of Electrons He 4 Na 12 Potassium Rb 86 Carbon 6 Xenon At Copper 64 Ne Lithium Ion Li' 3

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3 Name:. Period: For the following atoms/ions determine the number of protons, neutrons, electrons, mass number, and nuclear charge. ATOM or ION? PROTONS NEUTRONS ELECTRONS MASS NUMBER Cu*2 206pb 208pb Zn*2 Mg S-2 you know this.. /

4 OP ION? NEUTRONS glectrons MASS NUMBER NUaEAR CHAR&E He Au U a ' Question: W lich of the at >ove atoms are isotopes of one another? Exp ain how you know this.

5 Name: Period: Calculate the atomic mass of each of the following isotopes. SHOW ALL WORK. Element Mass Percent Abundance 1) copper-63 copper amu amu 69.17% 30.83% 2) uraniuin-235 xiranium amu amu 0.72% 99.28% 3) hydrogen-1 hydrogen amu amu % 0.015% 4) element Q-8 element Q-9 element Q amu 9.0 amu 10.0 amu 10.0% 20.0% 70.0%

6 1) Element X exists in three isotopic forms. The isotopic mixture consists of 10.0% ^ X, 20.0% "x, and 70.0% ^^X. What is the average atomic mass of this element? 2) Element Y exists in three isotopic forms. The Isotopic mixture consists of 15.0% ^^X, 65.0% ^^X, and 20.0% ^^X. That is the average atomic mass of this element? 3) A mystery element occurs in nature as two isotopes. Isotope A has a mass of amu and its abundance is 19.9%; Isotope B has a mass of amu and its abundance is 80.1%. From this data, calculate the atomic mass of the element and show all work. Lastly, identify the element. 4) A mystery element occurs in nature as two isotopes. Isotope A has a mass of amu and its abundance is 69.17%; Isotope B has a mass of amu and its abundance is 30.83%. From this data, calculate the atomic mass of the element and show all work. Lastly, identify the element.

7 Draw Lewis Dot Diagrams for the following: Charge # Valence e # unpaired valence e" # of bonds Charge # Valence e" # unpaired valence e # of bonds N L r Charge # Valence e' # unpaired valence e' # of bonds Charge # Valence e' # unpaired valence e' # of bonds C He Charge # Valence e # unpaired valence e" # of bonds 0 Charge # Valence e' # unpaired valence e' # of bonds B Charge # Valence e" # unpaired valence e" # of bonds s Charge # Valence e" # unpaired valence e" # of bonds Kr Charge # Valence e" Charge # Valence e # unpaired valence e # of bonds # unpaired valence e' # of bonds

8 Construct Bohr diagrams for the following: Na electron configuration F electron configuration O electron configuration Li^ electron configuration C\~ electron configuration Ne electron configuration

9 Bohr and Lewis Dot Diagrams Name Element Electron Configuration # Valence e" # Kernel e' Bohr Dic^ram Lewis Ctot Boron Valence e" = P = n = Kernel e = e = Argon Valence e = P = n = Kernel e" = e Nttrogett Valence e" = P = n = e = Kernel e = Lead Valence e = P = n = Kernel e' = e =

10 Electron Configuration Wori<sheet For the questions 1-10, assume all atoms are neutral. Use the electron configurations to determine the identity of the element and whether it is in the ground or excited state. Electron Configuration Identity round/excited Give an electron configuration for the following: 11, Sulfur in its ground state. 12. Helium in an excited state. 13. Give the ground state electron configuration for calcium. 14. Give the correct electron configuration for the Ca*^ ion. 15. How many valence electrons are there in atom of bromine? ^ 16. How many valence electrons are there in a cr ion? 17. How many kernel electrons are there in a phosphorus atom? 18. How many valence electrons are there in a neon atom? 19. How many principal energy levels are there in a iron atom? _

11 20.When atoms of an element are emitting a certain wavelength (or color) of light, it means that a) the atoms have gained energy and electrons have jumped to an excited state. b) the atoms have gained energy and electrons have fallen back to the ground state. c) the atoms have lost energy and electrons have fallen back to the ground state. d) the atoms have lost energy and electrons have jumped to an excited state. Use the emissions spectra results below to answer questions 14 and 15: Gas A Gas B Gas C Gas D Unknown Gas 21. According to these experimental spectra results, the unknown gas is a mixture of which gases? 22. Each line on the visible light spectrum for the gases above represents a) electrons jumping to the same excited state or energy level. b) electrons falling back down to their ground state from the same energy level. c) electrons jumping to multiple excited states or energy levels. d) electrons falling back down to their ground state from multiple energy levels. 23. HOW do the energy and the most probable location of an electron in the third shell of an atom compare to the energy and the most probable location of an electron in the first shell of the same atom? a) In the third shell, an electron has more energy and is closer to the nucleus. b) In the third shell, an electron has more energy and is farther from the nucleus. c) In the third shell, an electron has less energy and is cbser to the nucleus. d) In the third shell, an electron has less energy and is farther from the nucleus.

12 24. An atom of oxygen is in an excited state. When an electron in this atom moves from the third shell to the second shell, energy is a) emitted by the nucleus b) absorbed by the nucleus c) emitted by the electron d) absorbed by the electron 25. Which electron configuration could represent a strontium atom in an excited state? a) b) c) d) magine an emission spectrum produced by a container of hydrogen gas. Changing the amount of hydrogen in the container will change the colors of the lines in the spectrum. a) True b) False 27.1n the previous question, changing the gas in the container from hydrogen to helium will change the colors of the lines occurring in the spectrum. a) True b) False 28. An absorption spectrum appears as a continuous spectrum interrupted by a series of dark lines. a) True b) False 29. Emission spectra are characterized by narrow bright lines of different colors. a) True b) False 22

13 Name: Unit 2: Atomic Structure Review Pacl(et Dalton's Model: 1.1 can describe John Dalton's contribution to our understanding of the atom. What it looked like: Thomson's Experiment: 2.1 can describe SS Thomson's contribution to our understanding of the atom. Thomson's Model: What it looked like: Rutherford's Experiment: 3. i can describe Ernest Rutherford's contribution to our understanding of the atom. Rutherford's Model: What it looked like: Bohr's Model: 4.1 can describe Niels Bohr's contribution to our understanding of the atom. What k>oked Wke: What does the modern model of the atom look like? 5.1 can describe our understanding of the atom. Where, in an atom, are electrons likely to be found according to the modern model?

14 From oldest to newest, list the models that we have used to describe an atom. 6.1 can state the chronological order of atomic models. Particle #1 Particle #2 Particle #3 Name 7.1 can state the three subatomic particles, their location in an atom, their charges, and their masses (in amu). Charge Mass Location in Atom 8.1 can exdiain whv atoms are electrically neutral. Atoms are electrically neutral because the number of equa\o the nymber of Definitions: mass number is 9.1 can define mass number and atomic number. atomic number 10. Given the mass number, t can determine the number of protons, neutron, and electrons in an atom can use the Periodic Table to determine the atomic number of an element. In an atom of ^^^Po, how many protons are present? 84 In an atom of ^^^Po, how many electrons are present? 84 In an atom of ^^^Po, how many neutrons are present? 84 How many protons are in an atom of selenium? How many protons are in an atom of silicon? 12.1 can define isotooe. Definition: isotope

15 13.1 can represent an atom in any of the four methods of isotopic notation. Write the four different methods of isotopic notation for an atom of bromine that has 45 neutrons. Method 1 Method 2 Method 3 Method 4 / 14.1 can calculate average atomic mass given the masses of the naturally occurring isotopes and the percent abundances. Element Q has two isotopes. If 77% of the element has an isotopic mass of 83.7 amu and 23% of the element has an isotopic mass of 89.3 amu, what is the average atomic mass of the element? Definitions: ion and anion can define ion, cation, cation anion How many protons are in l^pl-? Given the mass number and the charge, 1 can determine the number of protons, neutrons, and electrons in an ion. How many neutrons are in 1%1"? 9 How many electrons are in 1^1'? 9

16 Definitions: principal energy JeveJ orbital ground state 17.1 can define Drincioai energy level, orbital, ground state, excited state^ electron configuration, and bright line spectrum. excited state electron configuration bright line spectrum 18.1 can state the relationship between distance from the nucleus and energy of an electron. As the distance between the nucleus and the electron increases, the energy of the electron A brightlme spectrum is created when 19.1 can exdiain. in terms of subatomic particles and energy states, how a bright line spectrum is created. mmmoi j 1 f [ } j 1 ^ o j i 1 1 III 1 1 i 20. lean identify the elements shown in a bright line spectrum. " - " 1 1 I I i 7i0 mn 360 nm Which element{s) is/are present in the mixture?

17 electrons can define valence Definition: valence electron 22. i can locate and interpret an element's electron configuration on the Periodic Table. How many vatence etectrons does an atom of rubnjfum have m the ground state? How many principal energy levels contain electrons in an atom of iodine in the ground state? Which electron configuration represents an atom of potassium in the excited state? 23.1 can identify an electron configuration that shows an atom in the excited state. A) B) C) D) can draw Lewis electron dot diagrams for a given element. Draw the Lewis electron dot diagram for the following atoms: Li Be B C N 0 F Ne Definition: octet of valence electrons 25. i can define and state the importance of "octet of valence electrons." The importance of having a complete"octet of valence electrons" is

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19 Unit! 1. What information is necessary to determine the atomic mass of the element chlorine? (1) the atomic mass and the relative abundance of each naturally occurring and artificially produced isotope of chlorine (2) the relative abundance of each naturally occurring isotope of chlorine, only (3) the atomic mass and the relative abundance of each naturally occurring isotope of chlorine (4) die atomic mass of each artificially produced isotope of chlorine, only 2. An orbital is defined as a region of the most probable location of (1) an electron (3) a proton (2) a neutron (4) a nucleus 3. Which quantity can vary among atoms of the same element? (1) mass number (2) numbers of electrons (3) number of protons (4) atomic number 4. Which statement describes how an atom in the ground state becomes excited? (1) The atom absorbs energy, and one or more electrons move to a higher electron shell. (2) The atom absorbs energy, and one or more electrons move to a lower electron shell. (3) The atom releases energy, and one or more electrons move to a lower electron shell. (4) The atom releases energy, and one or more electrons move to a higher electron shell. 5. Compared to the energy and charge of the electrons in the first shell of a Be atom, the electrons in the second shell of this atom have (1) more energy and the same charge (2) less energy and a different charge (3) less energy and the same charge (4) more energy and a different charge 6. A neutron has a charge of (1) +1 (2) +2 (3) 0 (4) -1 Atomic Structure 7. Which particles have approximately the same mass? (1) a neutron and an alpha particle (2) an electron and an alpha particle (3) a neutron and a proton (4) an electron and a proton 8. What is the overall charge of an ion that has 12 protons, 10 elections, and 14 neutrons? (1) 2~ (2) 2+ (3) 4^ (4) A sample of matter must be copper if (1) each atom in the sample has 29 protons (2) the sample melts at 1768 K (3) atoms in the sample react v^th oxygen (4) the sample can conduct electricity 10. A bromine atom in an excited state could have an electron configuration of (1) (3) (2) (4) An atom in die ground state has two electrons in its first shell and six electrons in its second shell. What is the total number of protons in the nucleus of this atom? (1)5 (2)2 (3)7 (4)8 12. Wliat is the mass number of a oarbon atom that contains six protons, eight neutrons, and six electrons? (1) 14 (2) 6 (3) 8 (4) The atomic mass of titanium is atomic mass units. This atomic mass represents the (1) total mass of all the protons and neutrons in an atom of Ti (2) weighted average mass of all die naturally occurring isotopes of Ti (3) weighted average mass of the most abundant isotope of Ti (4) total mass of all the protons, neutrons, and electrons in an atom of Ti 14. What is the total number of valence electrons in an atom of germanium in the ground state? (1) 8 (2) 2 (3) 14 (4) 4 Pagel

20 15. What can be determined if only die atomic number of an atom is known? (1) the total number of neutrons in the atom, only (2) the total number of protons in the atom, only (3) the total nimiber of protons and the total number of electrons in the atom (4) die total number of protons and the total number of neutrons in the atom 16. Which two particles have opposite charges? (1) a proton and a neutron (2) a proton and a positron (3) an electron and a neutron (4) an electron and a proton 17. Which statement describes the relative energy of the electrons in the shells of a calcium atom? (1) An electron in the first shell has more energy than an electron in the second shell. (2) An electron in the tliird shell has more energy than an electron in the second shell. (3) An electron in the first shell has the same amount of energy as an electron in the second shell. (4) An electron in the third shell has less energy than an electron in the second shell. 18. During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms (1) aie lost by the atoms (2) return to lower energy states within the atoms (3) are gained by the atoms (4) move to higher energy states within the atoms 19. An atom of any element must contain (1) an equal number of protons and neutrons (2) an equal number of protons and electrons (3) more electrons than neutrons (4) more electrons than protons 20. Each diagram below represents the nucleus of a different atom. D E Q R Which diagrams represent nuclei of the same element? (1) i?, and E (3) D and E, only (2) D, E, and Q (4) Q and i?, only 21. Which atom in the ground state has an outermost election with the most energy? (1) Na (2) Cs (3) Li (4) K 22. What must occur when an electron in an atom returns from a higher energy state to a lower energy state? (1) A random amount of energy is released. (2) A specific amount of energy is released. (3) The atom undergoes transmutation. (4) The atom spontaneously decays. 23. An electron in a sodium atom moves from the third shell to the fourth shell. This change is a result of the atom (1) absorbing energy (3) gaining an electron (2) losing an electron (4) releasing energy 24. The isotopes K-37 and K-42 have tiie same (1) mass number for dieir atoms (2) decay mode (3) total number of neutrons in their atoms (4) bright-line spectrum 25. What is the charge of the nucleus of an oxygen atom? (1) 0 (2) -2 (3) +8 (4) Which subatomic particle is negatively charged? (1) positron (3) proton (2) neutron (4) election Version 1 Page 2

21 27. The total number of protons, electrons, and neutrons in each of four different atoms are shown in the table below. Atom Subatomic Particles in Four Different Atoms Total Number of Protons Total Number of Electrons Total Number of Neutrons A D X z Which two atoms are isotopes of the same element? (1) ^andd (3)XandD (2) A and Z (4) Xand Z 28. Which atom in the ground state has the same electron configuration as a calcium ion, Ca^^, in the ground state? {l)mg (2)Ar (3)Ne (4) K 29. Which pliiase describes an atom? (1) a positively charged nucleus surrounded by negatively charged protons (2) a positively charged nucleus surrounded by negatively charged electrons (3) a negatively charged nucleus surrounded by positively charged protons (4) a negatively charged nucleus surrounded by positively charged electrons 30. Which subatomic particles are located in the nucleus of a carbon atom? (1) neutrons, only (2) protons, only (3) protons and neutrons (4) protons and electron 31. The greatest composition by mass in an atom of ^^so is due to the total mass of its (1) protons (3) positrons (2) electrons (4) neutrons Pages

22 Base your answers to questions 32 through 34 on the information below. The bright-line spectra for three elements and a mixture of elements are shown below. lithium 1 Bright-Line Spectra cadmium strontium mixture j n I I n Wavelength (nm) 32. Explain, in terms of both electrons and energy, how the bright-line spectrum of an element is produced. 33. Identify all the elements in the mixture. 34. State the total number of valence electrons in a cadmium atom in the ground state. Base your answers to questions 35 and 36 on the information below 36. Write the electron configuration of this atom in the ground state. An atom in an excited state has an electron configuration of Explain, in terms of subatomic particles, why this excited atom is electrically neutral. Version 1 Page 4

23 37. Copper has two naturally occurring isotopes. Information about the two isotopes is shown in the table below. Isotope Naturally Occurring isotopes of Copper Atomic Mass (atomic mass units, u) Percent Natural Abundance (%) Cu Cu In the space in your answer booklet, show a numerical setup for calculating the atomic mass of copper. 38. Explain, in terms of protons and neutrons, why U-235 and U-238 are different isotopes of uranium. Base your answers to questions 39 and 40 on the information below The element boron, a trace element in Earth's crust, is found in foods produced from plants. Boron has only two naturdly occurring stable isotopes, boron-10 and boron State, in terms of subatomic particles, one difference between the nucleus of a caibon-11 atom and die nucleus of a boron-11 atom. 40. Write an isotopic notation of die heavier isotope of the element boron. Your response must include tlie atomic number, the mass number, and the symbol of this isotope.

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