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5 – 3 Electron Configuration and Periodic Properties
Atomic Radius As you move down a group it increases The outermost e - are being added to higher energy levels (further from the nucleus.
Atomic Radius As you move across a period, it decreases Even though e - are being added, they are added to the same energy level (same distance from the nucleus).
Atomic Radius The charge on the nucleus increases as you move across the period and so it has a “tighter” hold on the e - being added.
Shielding Effect The reduction of the attractive force between a nucleus and its outer electrons due to the blocking effect of inner electrons.
Ionization Energy The amount of energy needed to remove an electron from an atom
Ion An atom that has gained or lost an e - If it has gained an e -, it will be _____. If it has lost an e -, it will be _____.
Ionization Energy As you go down a group, it decreases Shielding effect and electrons are being added to higher energy levels.
Ionization Energy As you move across a period, it increases The charge on the nucleus increases as you move across the period and so it has a “tighter” hold on the e - being added.
Electron Affinity The attraction of an atom for an additional e - Metals tend to have low EA Non-metals tend to have high EA
EA As you move down a group, EA decreases. Shielding Effect and electrons are being added to higher energy levels.
EA It increases as you move across the periodic table. The charge on the nucleus increases as you move across the period and so it has a “tighter” hold on the e - being added.
Electronegativity Tendency for an atom to attract e - to itself when combined with another atom. F is the most EN EN decreases as you move down a group EN increases as you move across a period
Electronegativity Based on the Pauling Scale. Linus Pauling 28 Feb 1901 – 19 Aug 1994
Periodic Table Trends. (1) Atomic Radius As one goes from left to right across a period, the atomic radii decreases. Reason: All the elements in a period.
Periodic Trends. Atomic Radius Defined as half the distance between the nuclei of two atoms Going across the periodic table ◦ But why are they smaller.
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Bell Ringer 1. How many valence electrons does N have? 2. Which of the 3 “classes” on the periodic table displays properties of both metals and nonmetals?
Periodic Table Trends. Atomic Radius As you move down a group, atomic radius increases The number of energy levels increases as you move down a group.
I II III Periodic Trends. Valence Electrons Electrons available to be lost, gained, or shared in the formation of chemical compounds Outer energy.
Bond radius Ionization Energy Electronegativity Electron Affinity*
The Periodic Law says: PERIODIC LAW states that when elements are arranged in order of increasing atomic number, there is a periodic repetition of their.
Factors Affecting Periodicity Periodic Trends: Atomic Radius: the distance from the center of the nucleus to the outermost electron (how big an atom is)
Trends of the Periodic Table. Atomic radius - one half the distance between the nuclei of identical atoms that are bonded together.
Periodic Trends. Types of Periodic Trends How elements differ as you move through the periodic table? Atomic Radius Ionic Radius Ionization Energy Electronegativity.
Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.
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Agenda Block 4 Attendance Make Groups for element assignment Get into your groups Preform your trend Powerpoint Homework-Part C and Part D.
Lesson 21 Periodic Trends Objectives: - The student will predict changes in atomic radius, shielding effect, ionization energy, electron affinity, and.
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Periodicity Periodic Table Trends. Describing the Periodic Table periodic law: the properties of elements repeat every so often period: group (family):
3:00 2:59 2:58 2:57 2:56 2:55 2:54 2:53 2:52 2:51 2:50 2:49 2:48 2:47 2:46 2:45 2:44 2:43 2:42 2:41 2:40 2:39 2:38 2:37 2:36 2:35 2:34 2:33 2:32 2:31 2:30.
Periodic Trends Mrs. Wood Chemistry. Part I – Atomic Size.
Atomic Size u Atomic Radius = half the distance between two nuclei of a diatomic molecule. } Radius.
Drill – 11/19 What is meant by “periodic trend”?.
Periodicity Atomic Radius = half the distance between two nuclei of a diatomic molecule. } Radius.
Graphs on the web. Atomic Radius vs Atomic Number The distance from the centre of the nucleus to the outermost electron. As the number of energy levels.
Periodic Trends. Atomic Size Trends often determined by one half the distance between the nuclei of two atoms of the same element when joined Atomic.
Periodic Properties Chemical and physical properties of the elements change with their position in the periodic table.
Periodic Trends Chemistry 5(C). Learning objectives Use the periodic table to identify and explain trends in – Atomic and ionic radii – Electronegativity.
Periodic Trends Definitions & Trends ELECTRONEGTIVITY Electronegativity is the power of an atom, when in a molecule, to attract electrons to itself.
Ionic Radius Cations are smaller than the atom they originated from because the same number of protons in the nucleus pulls on less electrons Anions are.
Section 5.3 – Electron Configuration and Periodic Properties
Periodic Trends!. Periodic Law When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and.
Periodicity Unit Part 3. Periodic Law When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical.
Periodic Trends Section 4.3. Ionization Energy The amount of energy needed to remove an outer electron from a specific atom or ion.
Periodic Trends, Cont. Shielding Ion Size Ionization Energy Electronegativity Shielding Ion Size Ionization Energy Electronegativity.
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Periodic Trends The physical and chemical properties of the elements are periodic functions of their atomic numbers.
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Periodic Properties Atomic Size - the size of the atom decreases as you move from the left side of the chart to the right side of the chart; the size of.
The arrangement of electrons in an atom helps determine the properties and behavior of that atom.
There are 6 patterns or trends we discuss when looking at the periodic table… 1. Reactivity 2. Atomic radius or size 3. Ionic radius 4. Ionization energy.
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