Unit 2: Atoms and the Periodic Table

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1 Unit 2: Atoms and the Periodic Table Name Block Learning Goals A. Use the periodic table to identify the group and the period of an element. Your Prior Understanding of Learning Goals Excellent Good Okay Poor B. Identify an element as a metal, nonmetal, or metalloid. C. Describe the electrical charge and location in an atom for a proton, a neutron, and an electron. D. Given the atomic number and the mass number of an atom, state the number of protons, neutrons, and electrons. E. Give the number of protons, electrons, and neutrons in one or more of the isotopes of an element. F. Calculate the atomic mass of an element using the percent abundance and mass of its naturally occurring isotopes. G. Explain how atomic spectra correlate with the energy levels in atoms H. Draw Bohr models to represent energy levels of atoms. I. Describe the sublevels and orbitals in an atom. J. Draw Lewis dot diagrams based on valence electrons. K. Explain the trends in periodic table properties. Set an appropriate academic goal for yourself and your learning for this unit by responding to the following questions. a. What would you like to achieve academically by studying this unit? I want to. b. How will you know that you have met this academic goal? I will have met my goal when. c. What are two specific strategies/activities you plan on using or doing in order for you to achieve your goal? In order to achieve my academic goal, I will. d. Why is this goal important to you? This goal is important to me because. e. What is the deadline for reaching this goal? I will achieve my goal by. 17

2 The Periodic Table Learning Goal: Use the periodic table to identify the group and the period of an element. By the late 1800s, scientists recognized that certain elements looked alike and behaved much the same way. In 1872, a Russian chemist,, arranged the 60 known elements at the time into a periodic table. Elements were arranged by increasing. Elements were grouped based on similar. On the periodic table elements are arranged according to similar properties in vertical columns called or, elements are also located in horizontal rows known as, the first two groups of elements and the last six groups of the periodic table are known as the elements and are numbered, the elements located in the center of the periodic table are known as the elements and are numbered, another numbering system assigns groups numbers across the entire periodic table, the and are part of Periods 6 and 7, but are located the main periodic table to condense its width. Indicate whether the elements are in the same group (G), period (P), or neither (N). a. Li, C, and O e. Br, Cl, and F b. Al, Si, and Cl f. C, N, and O c. Mg, Ca, and Ba g. C, S, and Br d. Li, Na, and K h. K, Ca, and Br 18

3 The Periodic Table Learning Goal: Use the periodic table to identify the group and the period of an element. Several groups on the periodic table have special names. group 1A (1) - soft, shiny metals - react vigorously with and form white products when they combine with - is NOT an alkali metal, even though it is placed at the top of group 1A - named derived from Arabic word for ashes, al-qali, as these elements are found in alkaline ashes that were used to make. group 2A (2) - soft, shiny metals - in nature, only found in minerals and compounds and not in their elemental form - named because they form alkaline solutions when mixed with water and because they are found in fire-resistant substances which were referred to as earth substances by early alchemists groups 3B-2B (3-12) - metals that exhibit metallic properties such as ductility, malleability, conduction of heat and electricity, and magnetism (iron, cobalt, and nickel) group 7A (17) - - form compounds with most of the elements - named because they tend to form ; halogen means salt-forming in Greek group 18A (18) - - possibly named because they tend to not combine with other elements like how nobility were above interacting with common folk 19

4 Metals, Nonmetals, and Metalloids Learning Goal: Identify an element as a metal, nonmetal, or metalloid. The arrangement of the periodic table distinguishes between metals, nonmetals, and metalloids that are located in distinct areas relative to the line that separates them. Metals Nonmetals Metalloids located to the of the zigzag line on the periodic table, opaque most are at room temperature ductile and malleable conductors of heat and electricity acquires the properties of a liquid metal only at high pressures and normally behaves as a nonmetallic located to the of the zigzag line on the periodic table, may be transparent can be at room temperature and shatter when hammered conductors of heat and electricity located the zigzag line on the periodic table, except which is a metal have both metallic and nonmetallic properties conductors of heat electricity which makes them useful as Identify each of the following elements as a metal (M), a nonmetal (NM), or a metalloid (ML). Cl Fe Al C Zn Mg N Si O Ca Sb Ti Which groups on the periodic table contain metals, nonmetals, and metalloids? 20

5 The Atom Learning Goal: Describe the electrical charge and location in an atom for a proton, a neutron, and an electron. The atom is the of an element that retains the characteristics of that element. The first direct evidence for atoms was in 1827 when, a Scottish botanist, noticed that pollen grains in a drop of water under a microscope were continually moving about. The movement, now known as, results from collisions between visible particles and invisible atoms. The structure of the atom and its particles was determined by the contributions of many scientists. J.J. Thomson Ernest Rutherford conducted the gold foil experiment from which he deduced the following about an atom: - small region in the center of the atom ( ) contains positive protons - negative occupy the region of space around the nucleus - most of an atom is James Chadwick nucleus of atom also contains neutral particles called Subatomic Particle Symbol Relative Charge Location in Atom nucleons proton neutron electron 21

6 Atomic Number and Mass Number Learning Goal: Given the atomic number and the mass number of an atom, state the number of protons, neutrons, and electrons. Atomic number is the number of contained in each atomic nucleus. All of the atoms of the have the same number of protons. This property distinguishes atoms of one element from atoms of all the other elements. Atoms are electrically ; the number of protons the number of electrons in a neutral atom. On the periodic table, the atomic number appears above the element symbol. For any atom, its mass number is the of the number of protons and neutrons in the nucleus. Mass number can vary from one atom to the next for atoms of the same element. Chemists use a unit call when measuring the mass of atoms. - One amu equals one-twelfth the mass of the atom with 6 protons and 6 neutrons. - The mass of the atom is due to the nucleons (protons and neutrons) in the nucleus, each with a mass of. - have a much smaller mass, and usually are ignored in calculating the mass of an atom. Give the number of protons in each of the following neutral atoms. a. an atom of the element with atomic number 15 b. an atom with a mass number of 40 and atomic number 19 c. an atom with 9 neutrons and a mass number of 19 d. a neutral atom that has 18 electrons Determine the number of neutrons in each of the following atoms and the symbol of the element. a. has a mass number of 42 and atomic number 20 b. has a mass number of 10 and 5 protons c. an atom with a mass number of 40 and atomic number 19 d. has a mass number of 9 and an atomic number of 4 e. has a mass number of 22 and 10 protons 22

7 Isotopes Learning Goal: Give the number of protons, electrons, and neutrons in one or more of the isotopes of an element. The atoms of an element are not completely identical. An element has a definite number of protons in each of its atoms, but the number of may vary. Atoms of the same element that contain different numbers of neutrons are. Isotopes have the same even if their physical property of mass differs. Isotopes can be written in two ways. has the mass number in the upper left corner and the atomic number in the lower left corner next to the left of the element symbol. has the name or symbol of the element followed by a hyphen and the mass number of the isotope. Carbon-12 or C-12 Complete the following table of information using nuclide notation. 23

8 Average Atomic Mass Learning Goal: Calculate the atomic mass of an element using the percent abundance and mass of its naturally occurring isotopes. Atomic mass is the total mass of an individual atom. Because the masses of the atoms of an element can be different, the periodic table provides the average atomic mass of an element s atoms. On the periodic table, the average atomic mass appears the element symbol. The average atomic mass is. Most elements consist of several isotopes, which is one reason that the average atomic masses on the periodic table are seldom numbers. The average atomic mass is NOT the same as the of an atom. To calculate average atomic mass of an element 1. the mass of each isotope with the of each isotope for a weighted average 2. together the weighted averages to get the average atomic mass Example: Calculate the average atomic mass of copper if copper-63 is 69.17% abundant and copper-65 is 30.83% abundant. The of an element generally can be determined by looking at the average atomic mass and determining which mass number of its isotopes it is closest to. Identify the most common isotope for the following elements. 24

9 Atomic Energy Levels Learning Goal: Explain how atomic spectra correlate with the energy levels in atoms; draw Bohr models to represent energy levels of atoms. In an atom, each electron has a fixed or specific energy known as its energy level. The energy levels are assigned values called which are positive integers (n = 1, n = 2, etc.). Generally, electrons in the energy levels are closer to the nucleus, while electrons in the energy levels are farther away. The number of distinct energy levels that an atom has is determined by the in which it is located on the periodic table. How many energy levels do the atoms of each of the following elements have? Be Sn U Hg Cl Xe When an atom absorbs energy (from heat or electricity), its electrons are temporarily. As the atom releases its extra energy, the atom emits. The atoms of a particular element can emit only certain frequencies, or, of light; each element produces its own distinctive glow when energized. An shows the pattern of frequencies formed by a given element when viewed through an instrument known as a. 25

10 Atomic Energy Levels Learning Goal: Explain how atomic spectra correlate with the energy levels in atoms; Changes in in atoms are responsible for atomic spectra. When the electrons in an atom occupy the lowest energy levels, they are in their state. As electrons gain energy, they may be raised to a higher energy level; these electrons are in an state. An electron energy in the form of electromagnetic radiation when it from an excited state back to its ground state. This lost energy may produce wavelengths in the, producing colors. Danish scientist developed a conceptual model of an atom to illustrate the energy levels of electrons. This model became known as the model. The model does NOT accurately portray the placement and movement of electrons in an atom as it was only developed to explain why elements have unique atomic spectra. 26

11 Bohr Models Learning Goal: Draw Bohr models to represent energy levels of atoms. The model, also referred to as a Bohr model, represents regions of space around the atomic nucleus where electrons may be located. There are shells that correlate to the seven periods of the periodic table. The maximum number of electrons that can be in each shell is equal to the number of elements in each period. - shell 1 = electrons - shell 2 = electrons - shell 3 = electrons - shell 4 = electrons - shell 5 = electrons - shell 6 = electrons - shell 7 = electrons Draw Bohr models for the following elements. 27

12 Atomic Sublevels and Orbitals Learning Goal: Describe the sublevels and orbitals in an atom. Energy levels of an atom have where electrons are found. There are four different sublevels:. The number of sublevels within an energy level is equal to the energy level s (n = 1, n = 2, etc.). The sublevels have different energy values, and the order of increasing energy is < < <. There is no way to know the exact location of an electron in an atom. Instead, scientists describe the location of an electron in terms of. The is the three-dimensional space in which electrons have the highest probability of being found. The orbital is identified by its and ; for example 2s or 4f. electrons can occupy an orbital. Sublevel s p d f # of Orbitals Maximum # of Electrons Complete the following analogies for understanding placement of electrons in an atom. Atoms Electron Cloud Energy Level Sublevel Orbital Park Hill South Your Location Right Now 28

13 Valence Electrons and Lewis Dot Diagrams Learning Goal: Draw Lewis dot diagrams based on valence electrons. The electrons of the outermost occupied and sublevels in any atom are directly exposed to the external environment and are the first to interact with other atoms. These outermost electrons are known as electrons and are involved in, related to the of an element, determine the of an element. The location of an element on the can be used to determine where an element s valence electrons are located. A Lewis dot diagram, also known as an, is a convenient way to represent the valence electrons of an atom. Electrons are shown as dots placed on the sides, top, or bottom of the symbol for the element valence electrons are placed as single dots valence electrons will have one or more electrons paired 29

14 Valence Electrons and Lewis Dot Diagrams Learning Goal: Draw Lewis dot diagrams based on valence electrons. Chemically stable atoms have full outer shells of valence electrons. Atoms want to be chemically stable. For most atoms, the number of electrons needed for a full count is ( from s sublevel plus from p sublevel). This is known as the rule. There are some exceptions to this rule, specifically and atoms. Indicate the number of valence of electrons found in each of the following elements, and then draw a Lewis dot diagram for that element. hydrogen oxygen iron chlorine argon aluminum carbon magnesium phosphorus 30

15 Periodic Table Trends Learning Goal: Explain the trends in periodic table properties. There are trends or patterns within the periodic table that give way to the chemical properties of an element. The of an atom is determined by the distance of the valence electrons from the nucleus. This property going down each group of elements because the valence electrons are farther from the nucleus as energy levels increase, moving across each period from left to right because there are more positive protons to attract and pull in an atom s negative valence electrons. The energy needed to remove one electron from an atom in the gaseous state is known as. This property going down each group of elements because the attraction of a nucleus for valence electrons decreases as those electrons are farther from the nucleus, moving across each period from left to right because there are more positive protons to attract and pull in an atom s negative valence electrons, is low for and high for, is really high for which indicates a chemically atom. The of an atom is its ability to attract electrons. This property going down each group of elements because there is more distance between the positive nucleus and the outermost energy levels, moving across each period from left to right because there are more positive protons that have a greater attraction for electrons, is low for and high for, is not assigned to the noble gases because they typically do not interact with other atoms. 31

16 Unit 2: Atoms and Periodic Table Reflection Learning Goals A. Use the periodic table to identify the group and the period of an element. Your Level of Mastery of Learning Goals Excellent Good Okay Poor B. Identify an element as a metal, nonmetal, or metalloid. C. Describe the electrical charge and location in an atom for a proton, a neutron, and an electron. D. Given the atomic number and the mass number of an atom, state the number of protons, neutrons, and electrons. E. Give the number of protons, electrons, and neutrons in one or more of the isotopes of an element. F. Calculate the atomic mass of an element using the percent abundance and mass of its naturally occurring isotopes. G. Explain how atomic spectra correlate with the energy levels in atoms H. Draw Bohr models to represent energy levels of atoms. I. Describe the sublevels and orbitals in an atom. J. Draw Lewis dot diagrams based on valence electrons. K. Explain the trends in periodic table properties. On a scale of 1 (low) to 10 (high), how well do you think your performance on this exam demonstrated your understanding of these learning goals? Why did you choose this ranking? What learning objective(s) did you enjoy studying the most from this unit? A B C D E F G H I J What learning objective(s) did you enjoy studying the least from this unit? A B C D E F G H I J Did you meet the goal you set for yourself for this unit? If yes, explain what was successful in helping you reach your goal. If no, describe what you could have done to help you reach your goal. 32

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