front 1 Limitations of Rutherford's Atomic Model | back 1 -Could not explain chemical properties of elements -Needed a model that better describes behavior of electrons |
front 2 Neils Bohr | back 2 Developed the Bohr Model (Planetary Model) -Incorporated discoveries about how energy of atom changes when light is absorbed or emitted -Proposal:electrons travel in specific orbitals -Electron orbits have a fixed energy -Amount of energy gained or lost is not the same -Quantum: Amount of energy required to move an electron from one energy level to another |
front 3 The Quantum Mechanical Model/Electron Cloud Model | back 3 -Erwin Schrondinger- Came up with equation describing behavior of electron; mathematical solutions led to quantum mechanical model -Determines allowed energies an electron can have and how likely it is to find the electron in various locations |
front 4 Heisenberg's Uncertainty Principle | back 4 Impossible to know the velocity and position of election at the same time |
front 5 Atomic Orbital | back 5 Mathmatical expression describing probability of finding an electron -Three dimensional region around the nucleus -Principal quantum number (n)-energy level -Energy sublevel corresponds to one or more orbitals of different shapes |
front 6 Electron Configuration | back 6 Tells how electrons are arranged in orbitals |
front 7 Noble Gas Configuration | back 7 Shorthand electron configuration -Portion of electron configuration summarized with noble gas (group 18 element) in brackets |
front 8 Aufbau's Principle | back 8 Electrons occupy the orbitals of lowest energy first |
front 9 Pauli's Exclusion Principle | back 9 Atomic orbitals can hold a maximum of two electrons -Electrons must have opposite spins (either up, closewise or down, counterclockwise) |
front 10 Hund's Rule | back 10 Electrons of same spin placed in orbital before pairing |
front 11 Orbital diagrams | back 11 A visual representation of electron arrangement in atoms |
front 12 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p4 | back 12 Se |
front 13 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p5 | back 13 Br |
front 14 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 | back 14 Kr |
front 15 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s1 | back 15 Fr |
front 16 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s24d10 5p6 6s2 4f14 5d8 | back 16 Pt |
front 17 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f10 | back 17 Dy |
front 18 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p4 | back 18 Po |
front 19 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d5 | back 19 Mn |
front 20 The following electron configuration is for a _________________ atom. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p2 | back 20 Sn |
front 21 The electron configuration for sodium is _________. | back 21 1s22s22p63s1 |
front 22 The electron configuration for argon is _____. | back 22 1s22s22p63s23p6 |
front 23 The electron configuration for iron is _____. | back 23 1s22s22p63s23p64s23d6 |
front 24 The electron configuration for cobalt is _____. | back 24 1s22s22p63s23p64s23d7 |
front 25 The electron configuration for Mg+2 is _____. | back 25 1s22s22p6 |
front 26 The electron configuration for P-3 is ____ | back 26 1s22s22p63s23p6 |
front 27 [Kr] 5s2 4d10 5p3 | back 27 Sb |
front 28 The following noble gas configuration is for an atom of _____. [Kr] 5s2 4d10 5p6 | back 28 Xe |
front 29 The following noble gas configuration is for an atom of _____. [Ar] 4s1 | back 29 K |
front 30 The following noble gas configuration is for an atom of _____. [Xe] 6s2 4f9 | back 30 Tb |
front 31 The following noble gas configuration is for an atom of _____. [Xe] 6s2 4f14 5d7 | back 31 Ir |
front 32 The following noble gas configuration is for an atom of _____. [Ne] 3s2 3p1 | back 32 Al |
front 33 The noble gas configuration for radium is _____. | back 33 [Rn]7s2 |
front 34 The noble gas configuration for gold is _____. | back 34 [Xe]6s24f145d9 |
front 35 The noble gas configuration for carbon is _____. | back 35 [He]2s22p2 |
front 36 The noble gas configuration for beryllium is _____. | back 36 [He]2s2 |
front 37 After drawing the orbital diagram for selenium, how many unpaired electrons remain? | back 37 2 |
front 38 After drawing the orbital diagram for carbon, how many unpaired of electrons remain? | back 38 2 |
front 39 After drawing the orbital diagram for fluorine, all of the orbitals are filled with paired electrons. | back 39 False |
front 40 What is wrong with the following configuration? Choose all that apply. 1s22s33s22p63p5 | back 40 violates Pauli's exclusion principle and violates Aufbau's principle |
front 41 Use the following electron configuration to answer the question. 1s2 2s2 2p6 3s2 3p6 4s2 How many shells (energy levels) does this atom have? | back 41 4 |
front 42 s | back 42 sphere, 1 orbital, maximum 2 electrons |
front 43 p | back 43 dumbbell, 3 orbitals, ,maximum 6 electrons |
front 44 d | back 44 double dumbbell, 5 orbitals, maximum 10 electrons |
front 45 f | back 45 complex, 10 orbitals, maximum 14 electrons |
front 46 sublevel 1 | back 46 1s maximum 2 electrons |
front 47 sublevel 2 | back 47 2s, 2p maximum 8 electrons |
front 48 sublevel 3 | back 48 3s, 3p, 3d maximum 18 electrons |
front 49 sublevel 4 | back 49 4s, 4p, 4d, 4f maximum 32 electrons |
front 50 After drawing the orbital diagram for oxygen, _______ electrons remain unpaired. | back 50 2 |
front 51 The electron configuration for potassium is ___________________. ( | back 51 1s22s22p63s23p64s1 |
front 52 [Kr]5s2 is the noble gas configuration for ________. | back 52 Sr |
front 53 Aufbau Principle | back 53 Electrons are added one at a time to the lowest energy levels first |
front 54 Hund's Rule | back 54 Electrons occupy equal-energy orbitals so that a maximum number of unpaired electrons results |
front 55 Pauli Exclusion Principle | back 55 An orbital can hold a maximum of 2 electrons |
front 56 arrows | back 56 electrons |
front 57 lines/boxes | back 57 orbitals |
front 58 The maximum number of electrons that can occupy the 2nd energy level, n=2, is | back 58 8 |
front 59 The following electron configuration shows the distribution of electrons in an atom of ____________. 1s22s22p63s23p64s23d6 | back 59 Fe |
front 60 Which of the following statements are true regarding electron arrangement in atoms? | back 60
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front 61 Is calcium a metal, nonmetal, or metalloid? | back 61 Metal |
front 62 What is the name of the element located in Group 17, Period 3? | back 62 Chlorine |
front 63 What is the symbol of the element that has an atomic mass of 200.59? | back 63 Hg |
front 64 What period and group do you find silver? (Enter it in like this: period number, group number) | back 64 5, 11 |
front 65 How many protons does iron have? | back 65 26 |
front 66 What is the name of the element that has a mass number of 35? | back 66 Chlorine |
front 67 What is the atomic number for gold? | back 67 76 |
front 68 What is the symbol of the element found in Group 15, Period 5? | back 68 Sb |
front 69 What is the mass number of cobalt? | back 69 59 |
front 70 Is sulfur a metal, nonmetal, or metalloid? | back 70 nonmetal |
front 71 How many electrons does a neutral atom of Sr have? | back 71 38 |
front 72 What is the symbol of the element that has an atomic mass of 237.048 amu? | back 72 Np |
front 73 Write the symbol for bohrium. | back 73 Bh |
front 74 What period and group would you find osmium? | back 74 6, 8 |
front 75 What is the symbol of the element found in Group 6, Period 4? | back 75 Cr |
front 76 What is the number of neutrons in Kr? | back 76 48 |
front 77 Which series (s, p, d, or f) is uranium located? | back 77 f |
front 78 What is the name of the group barium is located in? | back 78 Alkaline Earth Metals |
front 79 What is the name of the group iodine is located in? | back 79 Halogens |
front 80 What series (s, p, d, or f) is hassium located? | back 80 d |
front 81 Alkali Metals | back 81 Group 1 excluding Hydrogen s block 1 valence electron |
front 82 Alkaline Earth Metals | back 82 Group 2 s block 2 valence electron |
front 83 Transition Metals | back 83 Groups 3-12 d block n-1 |
front 84 Metalloids | back 84 B, Si, Ge, As, Sb, Te, Po p block 3-6 valence electron |
front 85 Halogens | back 85 Group 17 p block 7 valence electrons |
front 86 Noble Gases | back 86 Group 18 p block 8 valence electrons |
front 87 Diatomic Molecules | back 87 Cannot stand alone in nature, 2 of same atom bonded Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine |
front 88 Inner Transition Elements | back 88 F block n-2 |
front 89 Atomic Radius and Shielding Effect | back 89 Right-Small Bottom-Large |
front 90 Ionization Energy and Electronegativity | back 90 Right-high Bottom-Lower |
front 91 Ionization Energy | back 91 energy to remove e |
front 92 Electronegativity | back 92 ability to attract e |
front 93 Shielding Effect | back 93 inner e shield outer e |
front 94 Which of the following trends increase across a period? | back 94 electronegativity ionization energy |
front 95 Elements in group 1 will typically (gain/lose) 1 electron. | back 95 lose because cations lose electrons |
front 96 Noble gases, with the exception of helium, have _____ electrons in their outermost shell (valence electrons). | back 96 8 |
front 97 The most electronegative atom is ________ | back 97 Fluorine |
front 98 Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements? | back 98 Dmitri Mendeleev |
front 99 Which of the following decreases with increasing atomic number in Group 2? | back 99 ionization energy |
front 100 After drawing the orbital diagram for a sodium atom, how many unpaired electrons are there? | back 100 1 |
front 101 Which group contains the alkaline earth metal family of elements? | back 101 2 |
front 102 Atoms will gain, lose, or share electrons in order to achieve an electron configuration of what type of elements? | back 102 noble gases |
front 103 What charge will halogens more than likely form? | back 103 -1 |
front 104 Transition metals have electron configurations that end in the _________ sublevel. | back 104 d |
front 105 Look at your periodic table. Which atom has the largest atomic radius? | back 105 Radium |
front 106 The element with the following electron configuration, 1s22s22p63s23p64s23d104p1 , has electrons in what highest energy level? | back 106 4 |
front 107 How many periods are on the periodic table? | back 107 7 |
front 108 The Periodic Law states that when elements are arranged in order of increasing _____, their chemical and physical properties show a periodic pattern. | back 108 atomic number |
front 109 The alkali metals belong to group _____. | back 109 1 |
front 110 What is the electron configuration for Oxygen? | back 110 1s2, 2s2, 2p4 |
front 111 Many of the groups on the periodic table have names you should know. The halogen s belong to group _____. | back 111 17 |
front 112 The periodic table we use today reflects the arrangement of elements as done by _____. | back 112 Henry Moseley |
front 113 How many valence electrons does Nitrogen have? | back 113 5 |
front 114 Which of the following elements would most likely gain electrons in order to achieve stability? | back 114 N |
front 115 The following information is true for carbon | back 115 The highest energy level containing electrons in a carbon atom is the 2nd energy level. Carbon has 4 valence electrons. C-12 and C-14 are isotopes of carbon. |
front 116 Of the periodic trends, which of the following decrease within a group from top to bottom? | back 116 Electronegativity Ionization Energy |
front 117 Because these elements have achieved octet (a full valence shell), they do not have an attraction for electrons | back 117 Rn Ne |
front 118 What happens to the shielding effect when you move from left to right on the periodic table? | back 118 there is no change |
front 119 J.J. Thomson | back 119 no data |