Periodic Table Trends When you think of a periodic table‚ you think of elements like oxygen‚ neon‚ lead‚ and iron. You may even think of numbers‚ rows‚ and columns. You may not think about trends that are happening throughout a periodic table. There are many different trends that go on in a periodic table. The trends that I am going to be describing throughout this paper are atomic mass‚ atomic radius‚ first ionization energy‚ and electronegativity. When you study a normal/ordinary periodic
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CSEC CHEMISTRY NOTES ON PERIODIC TRENDS From Chemistry for CSEC by Tania Chung-Harris and Mike Taylor Chemistry for CAPE by Susan Maraj and Arnold Samai Periodic Trends in Group II Elements in Group II The elements in Group II are called alkaline earth metals. Be‚ Mg‚ Ca‚ Sr‚ Ba‚ Ra Beryllium‚ Magnesium‚ Calcium‚ Strontium‚ Barium‚ Radium These elements bond by metallic bonds (intramolecular forces) to form giant metallic structures. The size of the
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PART I ATOMIC RADUIS TREND GOING ACROSS THE PERIODIC TABLE PART II ATOMIC RADUIS TREND GOING DOWN A GROUP 1. Refer to the graph that you created in Part I of this assignment. Describe the general trend or patterns that you observed in the atomic radius as you go across the periodic table. (2 points) It looks like the atomic radius is bigger if the atomic number is small. This may be because of the decrease of the pull that the protons give the electrons the smaller the atomic number.2. In Part
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Chemistry CP O3.03 Periodic Trends Part I: Atomic Radius Trend Going Across the Periodic Table Part 2: Atomic Radius Trend Going Down A Group Part 3: Analysis and Conclusion After completing both graphs‚ answer the questions below in complete sentences. Both the question and your answer should be included in the document (along with the two graphs) that you submit to your instructor. 1) Refer to the graph that you created in Part 1 of this assignment. Describe the general trend or patterns that
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Introduction: The periodic is a table of the elements‚ organized in order of increasing atomic number. Elements that have similar chemical properties and electronic structures appear in vertical columns‚ or also called groups. The Periodic Law states that when elements are placed in order of increasing atomic number‚ their physical and chemical properties display a periodic pattern. The purpose of the lab was to discover how two periodic properties‚ atomic radius‚ and first ionization energy‚ vary
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Periodic trends across the period three oxides Clare Smerdon Access to Higher Education Science 08/04/2015 Julie Day Periodic trends across the period three oxides Objective This experiment is intended to explore the relationship between the physical properties of the oxides of Period 3 elements (sodium to chlorine) and their structures. Argon is obviously omitted because it doesn’t form an oxide. Hypothesis This experiment will be investigating the following
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in second and third IE is experimental evidence for the electron shell structure of atoms • Ionization energy for the removal of the second electron is large because the second electron is removed from a much lower energy (inner) subshell • The trend across a period is rationalized by the increase in effective nuclear charge Electron Affinity • The energy of a process in which an electron is acquired by the atom (the greater the affinity‚ the more negative the value‚ exothermic reaction) •
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look over 6 properties of the elements and determine if they follow a periodic trend or if they do not. A periodic trend increases or decreases across both a period and down a group. A quasi-periodic trend does not follow a periodic trend. The quasi-periodic trend is a trend that increases or decreases down a group. Our guiding question was Which properties of the elements follow a periodic trend? To discover the trends for each property of the elements‚ my group and I graphed each property
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Periodic Table Trends Quiz 1. The most reactive metals are located in the lower left hand corner of the periodic table 2. Which of the following atoms listed below has the largest atomic radius? Ca 3. Compared to the atomic radius of a rubidium atom‚ the atomic radius of a strontium atom is smaller. The smaller radius is primarily the result of the strontium atom having greater effective nuclear charge 4. An element is most likely to have properties similar to those of another
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CHAPTER 5: PERIODIC TABLE Development of the Periodic Table • i) Substance exist: naturally in elemental form Example: Gold‚ Uranium as unstable compound Example: Radioactive compounds as stable compound (majority) How to know whether a substance is a compound OR an element? ii) iii) • • • Grouping system: 1800: 31 elements identified 1865: 63 elements identified Audi Majdan – DMC 101 – KLIUC 1 • Dmitri Mendeleev: i) ii) iii) iv) Develop a system to group
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