Paper Plate Model of Carbon

Slides:

Advertisements

Similar presentations

Trends of the Periodic Table

Advertisements

Periodic Trends. Atomic Radius Atomic Radius (size) is the distance between the nucleus and the outer electrons in an atom.

Q u a n t u m N u m b e r s M r B o h r w a n t s t o k n o w.

 There are general trends in the properties of atoms and their ions with increasing atomic number.  These trends can be explained using the periodic.

Quiz Grades Rewrite your answer to question 1 on the back of your quiz. If it is correct, I will add up to 20% to your quiz grade (maximum score: 100%).

Atomic Structure. Key 11 Na Sodium Atomic Number Element symbol Element name Average atomic mass*

Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group ? DO Now: 1. Write down the electron configuration.

1 Chapter 3 Electronic Structure and Periodic Law 3.3 The Shell Model and Chemical Properties Copyright © 2005 by Pearson Education, Inc. Publishing as.

1 Chapter 3 Atoms and Elements 3.8 Periodic Trends Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.

The Quantum Mechanical Picture of the Atom

1 Chapter 3 Electronic Structure and Periodic Law 3.6 Property Trends within the Periodic Table Copyright © 2005 by Pearson Education, Inc. Publishing.

The Periodic Table & Electron Energy Levels

Drill – 11/19 What is meant by “periodic trend”?.

Are all atoms the same size? NaMgAlSiPSCl. So then... NaMgAlSiPSCl.

Periodic Trends. Electron attraction Electrons are attracted to protons –and repelled by electrons The closer an e - is to the nucleus, the more pull.

Why do the atoms of elements get smaller when moving from left to right within a row (period) across the periodic table?

Number your paper Write down the correct letter or letter combination that goes with the element. Make sure your upper and lower case letters are.

1 Chapter 4 Atoms and Elements 4.6 Electron Energy Levels · Be · · Mg · · Ca · · Sr · · Ba · Copyright © 2008 by Pearson Education, Inc. Publishing as.

Atomic Structure. Rules Of Atomic Structure 1.The Number of electrons = number of protons 2.Atomic Number = the number of protons/electrons 3.Atomic Mass.

18 Bohr Models Lesson 3.1 Extension. Element Name: _______________________ Chemical Symbol: _______Atomic Number: _______ Diagram the Bohr atom which.

Protons - positive charge Neutrons - no charge Nucleus - Electrons negative charge 1st energy level holds a maximum of 2 electrons (e 1-

The Current Atomic Model

Periodic Table Alkali Metals Group 1A Alkaline Metals Group 2A Transition Metals Group B Metalloids (7) Purple elements Halogens Group 7A Noble Gases Group.

Atoms Smallest part of all matter Made of smaller particles Dalton Rutherford Thompson Chadwick Bohr.

Unit 6: Chemical Compounds How does the interaction of valance electrons form chemical compounds?

Daily Science Oct 16 Write the shorthand electron configurations for the following:  Cu  I  F  Hg.

Atoms Is made Up of 2 Parts: The Nucleus: 1. Protons 2. Neutrons The Rings: 1. Electrons.

Trends of the Periodic Table. Background Electrons can jump between shells (Bohr’s model supported by line spectra) The electrons can be pushed so far.

Lewis Electron Dot Diagrams. Valence Electrons Electrons found in the outermost energy level of an atom Usually involved in chemical changes Lewis Electron.

Chapter 3 Atoms and Elements 3.7 Electron Energy Levels 1.

Oxidation Number the combining ability of an atom (how many electrons it needs to gain or lose to be stable)

Atomic Number Proton Electron ELEMENTAtomic #Atomic MassProtonsNeutronsElectrons N K Ag Na O Ne Al

Atomic Structure Test Review 166 point total. 1.The atomic number is the number of protons. 2. The mass number is the number of protons and neutrons.

Review The elements of the Periodic Table are arranged by: Periods – the number of energy levels. Groups – the number of valence electrons. Blocks – the.

Periodic Trends.

Periodic Trends We will explain observed trends in  Atomic (and Ionic) Radius  Ionization Eenergy  Electronegativity size lose e – attract e – nuclear.

Periodic Trends What pattern do you see? -Number of fingers shown increases from left to right.

Periodic Properties of the Elements Chapter 7. Effective Nuclear Charge Orbitals of the same energy are said to be degenerate. Effective nuclear charge.

PERIODIC PATTERNS Unit 3 – Periodic Table. What patterns exist on the periodic table? Lesson Essential Question:

Order of filling orbitals

Bohr Diagrams or Shell Models

Radii of the Elements. The atomic radius is defined as half the distance between two adjacent atoms in a solid crystal. In a period, the atomic radius.

What are the names of these elements? C O Na Li Fe Mg Pb Ca F Xe Ti K Ba B Si P Cl Be.

Periodic Properties of the Elements © 2009, Prentice-Hall, Inc. Chapter 7 Periodic Properties of the Elements.

Charge effect The more electrons are on the same ring and the more protons are in the nucleus the smaller the atomic radius Opposite charges attract!!!

Hydrogen and Helium Hydrogen does not share the same properties as the elements of group 1. Helium has the electron configuration of group 2 elements however.

Interpreting the Periodic Table H He LiBeBCNOFNe NaMg KCa AlSiPSClAr

Periodic Trends Pages 28 and 29 of your Workbook.

Periodic Trends. Li Na Li K Ne Ar In the periodic table, vertical columns are called groups or families…

Periodic Trends Modified from Mrs. Coyle Chemistry.

Using the Main Group Elements of the Periodic Table to Draw Bohr-Rutherford Diagrams He

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.

Electronegativity What is it? Electronegativity is the power of an atom to attract electron density Remember the definition … … look for where you get.

and Electronegativity

Electrons and Lewis Dot Structures

Write the orbital notation and electron configuration for the following atoms Be B N F Mg.

Chapter 3 Atoms and Elements

Write the Complete Electron Configuration for:

MS. SAMAYOA BIRMINGHAM COMMUNITY CHARTER HIGH SCHOOL CHEMISTRY

Periodic Trends.

Ionization Energy Atomic Radius Electron Affinity Electronegativity

Energy Na 11P 11e.

Daily Science 9/26 Write the shorthand electron configurations for the following: Ag I.

Lewis Dot Structures & Covalent Bonding

Periodic Table Trends.

How do you get charges on an element?

All substances are made from atoms.

Period three TRENDS.

Periodic Trends Chemistry I.

Presentation transcript:

Paper Plate Model of Carbon Atomic Radius Blue = electrons Red = protons Black = neutrons Our scale is: 2 pm : 1 mm If the actual atomic radius of carbon is 77 pm, how big should the radius be on this paper plate model? 77 / 2 = 38.5 cm in this model

Atomic Radii (all in picometers) Element Radius (pm) H 37 He 31 Li 152 Be 111 B 80 C 77 N 74 O 73 F 72 Ne 71 Element Radius (pm) Na 186 Mg 160 Al 143 Si 113 P 110 S 103 Cl 100 Ar 98 K 227 Ca 197 Again, these are all in picometers!!! Remember to scale your model appropriately

The “Shielding Effect” Are electrons attracted to or repelled from each other? Repelled Electrons in shells closer to the nucleus reduce the attraction between the protons and the valence (outer shell) electrons Carbon

First Ionization Energy