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Unit #3: Atomic Structure Exam Review: 1) The atomic number of an element is determined by the number of _________Protons_________ in the nucleus of an atom. 2) The philosopher, ______Democritus_______, believed that all matter consisted of extremely small particles that could not be divided. He called these particles ____Atoms____, which means “uncut” or “indivisible.” 3) ______Ernest Rutherford______ provided evidence for the existence of a nucleus. 4) Complete the following table: Energy Levels: Maximum Number of Electrons: 1 2 3 4 2 8 18 32 5) Complete the following table: Region of Location: Charge: the Atom: Center of Nucleus Positive the Atom Electron Around the Negative Cloud Nucleus 6) Complete the following table: Subatomic Location: Particle: Proton Neutron Electron Nucleus Nucleus Electron Cloud Mass: Volume: Density Large Small Large Small Large Small Charge: Mass: Positive Neutral Negative 1 amu 1 amu 0 amu 7) Complete the following table: Subshell: Maximum Number of Electrons: Number of Orbitals: s p d f 2 6 10 14 1 3 5 7 8) Give the electron configuration, orbital notation, and atomic structure for the following elements: a) Magnesium 1s22s22p63s2 1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ ) ) ) 2e- 8e- 2e- 12 p+ 12 n b) Chlorine 1s22s22p63s23p5 1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ 3p↑↓ ↑↓ ↑_ 17 p+ 18 n ) ) ) 2e- 8e- 7e- c) Potassium 1s22s22p63s23p64s1 1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ 3p↑↓ ↑↓ ↑↓ 4s↑_ 19 p+ 20 n ) ) ) ) 2e- 8e- 8e- 1e- d) Rubidium 1s22s22p63s23p64s23d104p65s2 1s↑↓ 2s↑↓ 2p↑↓ ↑↓ ↑↓ 3s↑↓ 3p↑↓ ↑↓ ↑↓ 4s↑↓ 3d↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 4p↑↓ ↑↓ ↑↓ 5s↑↓ 37 p+ 48 n ) ) ) ) ) 2e- 8e- 18e- 8e- 1e- 9) Identify how many protons, neutrons, and electrons a neutral atom of Fluorine contains. 9 Protons, 10 Neutrons, 9 Electrons 10) Identify how many protons, neutrons, and electrons a neutral atom of Bismuth contains. 83 Protons, 126 Neutrons, 83 Electrons 11) Identify how many protons, neutrons, and electrons a neutral atom of Cesium contains. 55 Protons, 78 Neutrons, 55 Electrons 12) Identify the element symbol for the following elements: a) Aluminum Al c) Potassium K b) Sodium Na d) Manganese Mn 13) ______Neils Bohr______ believed that electrons move around the nucleus like planets orbiting the Sun. 14) In a few sentences describe Ernest Rutherford’s famous gold-foil experiment. Rutherford aimed a beam of alpha particles (Helium nuclei) at a sheet of gold-foil surrounded by a fluorescent screen. Most of the particles passed through, a few deflected. Rutherford concluded that atoms were made up of mostly empty space because most particles passed through. The particles that came close to the nucleus were deflected due to a central, positive charge. 15) _________J.J. Thomson_________ provided evidence for the existence of electrons. 16) ________Eugen Goldstein_______ provided evidence for the existence of protons. 17) ________James Chadwick_______ provided evidence for the existence of neutrons. 18) Identify the atomic number and mass number for Mercury. Atomic Number = 80 Mass Number = 201 19) Identify the atomic number and mass number for Zinc. Atomic Number = 30 Mass Number = 65 20) Identify the atomic number and mass number for Uranium. Atomic Number = 92 Mass Number = 238 21) Using the periodic table, what is the average atomic mass for Calcium? 40.08 amu 22) Using the periodic table, what is the average atomic mass for Silver? 107.87 amu 23) Using the periodic table, what is the average atomic mass for Carbon? 12.011 amu 24) How do you determine the number of protons in an atom? Number of Protons = Atomic Number 25) How do you determine the number of electrons in an atom? Number of Electrons = Number of Protons 26) What is the equation that is used to calculate the number of neutrons in an atom? Number of Neutrons = Mass Number – Atomic Number 27) An atom has 16 protons, 16 neutrons, and 16 electrons. What is the element’s atomic number and mass number? Atomic Number = 16 Mass Number = 32 28) Complete the following table: Element Element Number of Number of Number of Name: Symbol: Protons: Neutrons: Electrons: Lithium Li 3 4 3 Silicon Si 14 14 14 Mercury Hg 80 121 80 Nickel Ni 28 31 28 Bromine Br 35 45 35 Calcium Ca 20 20 20 Argon Ar 18 22 18 Magnesium Mg 12 12 12 29) If the atom is neutral, then the number of protons is equal to the number of ________Electrons_________. 30) _______Mass Number_______ refers to the sum of protons and neutrons in the nucleus of an atom. 31) An element’s ______Average Atomic Mass_________ is an average mass of the different isotopes of an element. 32) _______Isotopes________ are atoms of the same element with different numbers of neutrons. 33) ______Atomic Number_____ refers to the number of protons in the nucleus of an atom. 34) Define the following terms: a) Aufbau Principle: Electrons must enter orbitals of lowest energy first; Chart of Electron Filling. b) Hund’s Rule: When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins. c) Pauli Exclusion Principle: Atomic orbitals may describe at most two electrons and they must have an opposite spin. d) Average Atomic Mass: Weighted average mass of the atoms in a naturally occurring sample of an element. e) Protons: Positively charged subatomic particle that is found in the nucleus, and has a mass of 1 amu. f) Neutrons: Neutral subatomic particle that is found in the nucleus, and has a mass of 1 amu. g) Electrons: Negatively charged subatomic particle that is found in the electron cloud, and does not have a mass. h) Isotope: Atoms of the same element with a different number of neutrons, therefore they have a different mass. i) Element: Substance that cannot be broken down into simpler substances; Contains only one type of atom. j) Atomic Number: Number of protons in the nucleus of an atom; This number identifies the element. k) Mass Number: Sum of the protons and neutrons in the nucleus of an atom. l) Nucleus: Dense, positively charged region that is located in the center of an atom; Contains protons and neutrons. m) Electron Cloud: Negatively charged region that surrounds the nucleus of an atom; Contains electrons. n) Electron Cloud Model: Visual model of the most likely locations for electrons in an atom. o) Energy Levels: Similar energies that electrons in an atom can have. p) Subshells: Energy level that contains electrons that have the same energy. q) Compound: Substance that is made from two or more simpler substances and can be broken down into those simpler substances.