Chem: Unit 3: Atomic Concepts - castle learning
A magnesium atom that loses two electrons becomes a 1. positive ion with a smaller radius 2. negative ion with a smaller radius 3. positive ion with a larger radius 4. negative ion with a larger radius
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according to the wave-mechanical model of the atom, electrons are located in 1. orbitals 2. circular paths 3. a small, dense nucleus 4. a hard, invisible sphere
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compared to the energy of an electron in the second shell of an atom of sulfur, the energy of an electron in the 1. first shell is lower 2. first shell is the same 3. third shell is lower 4. third shell is the same
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in all atoms of bismuth, the number of electrons must equal the 1. number of protons 2. number of neutrons 3. sum of the number of neutrons and protons 4. difference between the number of neutrons and protons
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the unstable nucleus spontaneously releases a positron. this is an example of 1. radioactive decay 2. nuclear fusion 3. chemical decomposition 4. thermal conductivity
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the weighted average of the atomic masses of the naturally occurring isotopes of an element is the 1. atomic mass of the element 2. atomic number of the element 3. mass number of each isotope 4. formula mass of each isotope
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what is the net charge of an ion that has 11 protons, 10 electrons, and 12 neutrons 1. 1+ 2. 2+ 3. 1- 4. 2-
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which electron configuration represents the electrons in an atom of sodium in the ground state at STP 1. 2-8-1 2. 2-7-2 3. 2-8-6 4. 2-7-7
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which nuclear emission has the least penetrating power and the greatest ionizing ability 1. alpha particle 2. beta particle 3. gamma ray 4. positron
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which nuclear emission is listed with its notation 1. gamma radiation 00y 2. proton 42He 3. neutron 0-1B 4. alpha particle 11H
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which radioisotope is used to determine the age of once-living organisms 1. carbon-14 2. cobalt-60 3. iodine-131 4. uranium-238
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which radioisotope requires long-term storages as the method of disposal, to protect living things from the radiation exposure over time 1. Pu-239 2. Fr-220 3. Fe-53 4. P-32
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which statement describes the earliest model of the atom 1. an atom is an indivisible hard sphere 2. an atom has a small, dense nucleus 3. electrons are negative particles in an atom 4. electrons in an atom have wave-like properties
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which statement describes the location of protons and neutrons in an atom of helium 1. protons and neutrons are in the nucleus 2. protons and neutrons are outside the nucleus 3. protons are outside the nucleus, and the neutrons are in the nucleus 4.protons are in the nucleus, and neutrons are outside the nucleus
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In the ground state, the valence electrons of a krypton atom are found in 1. the first shell 2. the outermost shell 3. both the nucleus and the first shell 4. both the first shell and the outermost shell
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all matter is made up of 1. cells 2. atoms 3. molecules 4. compounds
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an orbital is a region in an atom where there is a high probability of finding 1. an alpha particle 2. an electron 3. a neutron 4. a positron
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atoms are neutral because the number of 1. protons equals the number of neutrons 2. protons equals the number of electrons 3. neutrons is greater than the number of protons 4. neutrons is greater than the number of electrons
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compared to the energy released per mole of reactant during chemical reactions, the energy released per mole of reactant during nuclear reactions is 1. much less 2. much greater 3. slightly less 4. slightly greater
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if two atoms are isotopes of the same element, the atoms must have 1. the same number of protons and the same number of neutrons 2. the same number of protons and a different number of neutrons 3. a different number of protons and the same number of neutrons 4. a different number of protons and a different number of neutrons
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in which process does a heavy nucleus split into two lighter nuclei 1. titration 2. fission 3. electrolysis 4. neutralization
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the energy released by a nuclear fusion reaction is produced when 1. energy is converted to mass 2. mass is converted to energy 3. heat is converted to temperature 4. temperature is converted to heat
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the part of an atom that has an overall positive charge is called 1. an electron 2. the nucleus 3. the first shell 4. the valence shell
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the results of the gold foil experiment led to the conclusion that an atom is 1. mostly empty space and has a small, negatively charged nucleus 2. mostly empty and has a small, positively charged nucleus 3. a hard sphere and has a large, negatively charged nucleus 4. a hard sphere and has a large, positively charged nucleus
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the stability of an isotope is related to its ration of 1. neutrons to positrons 2. neutrons to protons 3. electrons to positrons 4. electrons to protons
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what is the approximate mass of an atom that contains 26 protons, 26 electrons and 19 neutrons 1. 26 u 2. 45 u 3. 52 u 4. 71 u
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which electron configuration represents the electrons in an atom of sulfur in an excited state 1. 2-8-6 2. 2-7-7 3. 2-8-7 4. 2-7-8
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which electron configuration represents the electrons of an atom in an excited state 1. 2-2 2. 2-2-1 3. 2-8 4. 2-8-1
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which particle has the least mass 1. alpha particle 2. beta particle 3. neutron 4. proton
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which subatomic particles each have a mass of approximately 1 u 1. proton and electron 2. proton and neutron 3. neutron and electron 4. neutron and positron
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which value changes when a Cu atom becomes a Cu2+ ion 1. mass number 2. oxidation number 3. number of protons 4. number of neutrons
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based on table s, an atom of which element has the strongest attraction for electrons in a chemical bond 1. chlorine 2. nitrogen 3. oxygen 4. selenium
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dating once-living organisms is an example of a beneficial use of 1. redox reactions 2. organic isomers 3. radioactive isotopes 4. neutralization reactions
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given a list of atomic model descriptions: A: electron shells outside a central nucleus B: hard, indivisible sphere C: mostly empty space Which list of atomic model descriptions represents the order of historical development from the earliest to most recent 1. A, B, C 2. A, C, B 3. B, C, A 4. B, A, C
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in which type of nuclear reaction do nuclei combine to form a nucleus with a greater mass 1. alpha decay 2. beta decay 3. fusion 4. fission
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the ratio of the mass of U-238 to the mass of Pb-206 can be used to 1. diagnose thyroid disorders 2. diagnose kidney function 3. date geological formations 4. date once-living things
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what is the total number of neutrons in an atom of K-42 1. 19 2.20 3. 23 4. 42
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which electron configuration represents the electrons of an atom is an excited state 1. 2-5 2. 2-8-5 3. 2-5-1 4. 2-6
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which notations represents atoms that have the same number of protons but a different number of neutrons 1. H-3 and He-3 2. S-32 and S-32 3. Cl-35 and Cl-37 4. Ga-70 and Ge-73
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which particle remains undeflected when passing through this electric field 1. proton 2. electron 3. neutron 4. positron
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which particles are found in the nucleus of an argon atom 1. protons and electrons 2. positrons and neutrons 3. protons and neutrons 4. positrons and electrons
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which phrase describes a risk associated with producing energy in a nuclear power plant 1. depletion of atmospheric hydrogen (H2) 2. depletion of atmospheric carbon dioxide (CO2) 3. production of wastes needed long-term storage 4. production of wastes that cool surrounding water supplies
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which phrase describes a risk of using the radioisotope Co-60 in treating cancer 1. production of acid rain 2. production of greenhouse gases 3. increased biological exposure 4. increased ozone depletion
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which process converts mass into energy 1. distillation of ethanol 2. filtration of a mixture 3. fusion of hydrogen atoms 4. ionization of cesium atoms
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which statement describes the charge and location of an electron in an atom 1. an electron has a positive charge and is located outside the nucleus 2. an electron has a positive charge and is located in the nucleus 3. an electron has a negative charge and is located outside the nucleus 4. an electron has a negative charge and is located in the nucleus
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according to the wave-mechanical model, an orbital is defined as the most probable location of 1. a proton 2. a neutron 3. a positron 4. an electron
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an ion that consists of 7 protons, 9 neutrons, and 10 electrons has a net charge of 1. 2- 2. 2+ 3. 3+ 4. 3-
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each line in the spectra represents the energy 1. absorbed as an atom loses an electron 2. absorbed as an atom gains an electron 3. released as an electron moves from a lower energy state to a higher energy state 4. released as an electron moves from a higher energy state to a lower energy state
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in the ground state, an atom of which element has seven valence electrons 1. sodium 2. phosphorus 3. nitrogen 4. fluorine
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in which reaction is an atom of one element converted into an atom of another element 1. combustion 2. fermentation 3. oxidation-reduction 4. transmutation
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in which type of nuclear reaction do two light nuclei combine to produce a heavier nucleus 1. positron emission 2. gamma emission 3. fission 4. fusion
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in which type of reaction can an atom of one element be converted to an atom of another element 1. addition 2. reduction 3. substitution 4. transmutation
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magnesium and calcium have similar chemical properties because their atoms in the ground state have 1. equal numbers of protons and electrons 2. equal numbers of protons and neutrons 3. two electrons in the first shell 4. two electrons in the outermost shell
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the discovery of the electron as a subatomic particle was a result of 1. collision theory 2. kinetic molecular theory 3. the gold-foil experiment 4. experiments with cathode ray tubes
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the mass of an electron is 1. equal to the mass of a proton 2. equal to the mass of a neutron 3. greater than the mass of a proton 4. less than the mass of a neutron
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the three nuclides, U-233, U-235, and U-238, are isotopes of uranium because they have the same number of protons per atom and 1. the same number of electrons per atom 2. the same number of neutrons per atom 3. a different number of electrons per atom 4. a different number of neutrons per atom
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the use of uranium-238 to determine the age of a geological formation is a beneficial use of 1. nuclear fusion 2. nuclear fission 3. radioactive isomers 4. radioactive isotopes
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using equal masses of reactants, which statement describes the relative amounts of energy released during a chemical reaction and a nuclear reaction 1. the chemical and nuclear reactions release equal amounts of energy 2. the nuclear reaction releases half the amount of energy of the chemical reaction 3. the chemical reaction releases more energy than the nuclear reaction 4. the nuclear reaction releases more energy than the chemical reaction
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what evidence indicates that the nuclei of strontium-90 atoms are unstable 1. strontium-90 electrons are in the excited state 2. strontium-90 electrons are in the ground state 3. strontium-90 atoms spontaneously absorb beta particles 4. strontium-90 atoms spontaneously emit beta particles
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which electron configuration represents a potassium atom in an excited state 1. 2-7-6 2. 2-8-5 3. 2-8-8-1 4. 2-8-7-2
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which electron configuration represents an atom of chlorine in an excited state 1. 2-8-7-2 2. 2-8-7 3. 2-8-8 4. 2-7-8
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which electron shell in an atom of calcium in the ground state has an electron with greatest amount of energy 1. 1 2. 2 3. 3 4. 4
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which electrons configuration represents the electrons in an atom of calcium in an excited state 1. 2-8-8 2. 2-8-8-2 3. 2-7-8-1 4. 2-7-8-3
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which ion in the ground state has the same electron configuration as an atom of neon in the ground state 1. Ca2+ 2. Cl- 3. Li+ 4. O2-
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which statement explains why a xenon atom is electrically neutral 1. the atom has fewer neutrons than electrons 2. the atom has more protons than electrons 3. the atom has the same number of neutrons and electrons 4. the atom has the same number of protons and electrons
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which symbol represents a particle that has a mass approximately equal to the mass of a neutron 1. a 2. B+ 3. B- 4. p
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