Catalyst 1.What would J.J. Thomson say to Dalton to prove that his plum pudding model is superior? 2.What would Ernest Rutherford say to J.J. Thomson.

Slides:



Advertisements
Similar presentations
Trends of the Periodic Table
Advertisements

Jeopardy Atomic Models Atomic Particles Calculate Particles Isotopes Valence Electrons Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400.
Catalyst 1.Open up the Bohr’s Model educanon video for today’s class. Complete the questions associated with the video. 2.Put your laptop at 45 degrees.
Periodic Trends Models of the Atom Orbitals Electron Configuration Valence Electrons
An atom is made of a nucleus containing protons and neutrons; electrons move around the nucleus. Section 2: Defining the Atom K What I Know W What I Want.
Trends and the Periodic Properties
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.
Catalyst: The Springfield Nuclear Power Plant has discovered a new element called Homerium (Hm). Element Homerium (Hm) is located between sodium (Na) and.
Catalyst 1. Order the following elements from smallest electronegativity to largest ionization energy: Aluminum, Silicon, Phosphorous. 2. Why does Germanium.
Catalyst 9/6/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to electronegativity (EN) or ionization energy (IE) as you.
What are the trends for atomic radii? Why do these trends exist? 4.
December 9th Quick Write: 1.Place Study Guide Packet on your desk to be checked during the Quick Write. 2.Why did the measurement of 25mL of water and.
Atomic Structure Topic 3.
Ancient Greece Democritus: .
Periodic Table Trends. Metallic character Metallic Character Depends on how readily the element gives up their valence e-’s.
WELCOME!! 1. Please be in your seats by the time the bell rings. 2. On your catalyst sheet you should be on October November 4 th.
Catalyst 1. What are the trends for ionization energy? Why do these trends exist? 2. As you go across a period, do elements get better or worse at attracting.
STD 1: Atomic Structure.
Atomic Theory.
The Gold Foil and the Nucleus
Section 5.3 – Electron Configuration and Periodic Properties
Catalyst 9/4/13 On your Catalyst Sheet, please answer the following questions: 1. What happens to ionization energy as you go down a group? 2. Sort from.
Catalyst 1. List an element from the following groups: alkali, alkaline earth metal, transition metal, halogen, and Noble gas. 2. Why do different groups.
Catalyst 1. List an element from the following groups: alkali, alkaline earth metal, transition metal, halogen, and Noble gas. 2. Why do different groups.
After today, you will be able to… Explain the periodic trend for ionic size and electronegativity Compare the size of cations to the size of anions.
WHAT ARE THE PERIODIC TRENDS?. Periodic Trends All information in contained in table S Predictable properties/changes that occur as we move down groups.
Periodic Trends 6.3.
Atoms: Building Blocks of Matter
Periodic Trends Section 6.3
Periodic Trends.
Matter Anything that has mass and takes up space. Anything that has mass and takes up space. All matter can be measured All matter can be measured Mass.
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.
 According to Bohr’s model of the atom, atoms are very similar to solar systems.
Catalyst 1. List an element from the following groups: alkali, alkaline earth metal, transition metal, halogen, and Noble gas. 2. Why do different groups.
Atomic Model History.
A Brief History of the Modern Atomic Model ’s Pgs , Chemistry Matter and Change.
Democritus Dalton (JJ Thompson) Rutherford Bohr Electron Cloud
Periodic Trends. Atomic Radius Defined as half of the distance between two bonding atoms nuclei.
Structure of Atom Atom Smallest particle of an element Atomic Structure – arrangement of smaller particles within an atom.
Catalyst IN YOUR JOURNAL! 1. What are the two subatomic particles found in the nucleus? 2. What is the charge of a proton? An electron? 3. How do you.
November 28th Homework: read pgs Take the two worksheets.
400 B.C. Theorized that if you were to cut something in half, then cut it in half again and again… Eventually you would be left with something.
Catalyst 1. List an element from the following groups: alkali, alkaline earth metal, transition metal, halogen, and Noble gas. 2. Why do different groups.
Chapter 5 Atoms: Building Blocks of Matter. Evidence Direct evidence is when you do something to gather the evidence Examples are Doing an experiment.
Periodic Trends There are several important atomic characteristics that show predictable trends. Atomic radius Ionization energy Electron affinity Electronegativity.
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.
Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group ? Do Now: 1. Take out your periodic tables.
PERIODIC PATTERNS Unit 3 – Periodic Table. What patterns exist on the periodic table? Lesson Essential Question:
Chapter 5 The Periodic Law
Atomic Structure and Theory Scientists What’s the Matter?
Periodic Trends Learning Target: Criteria For Success:
Structure of an Atom Nucleus: Nucleus:Proton.
Atomic Structure Where our ideas of the atom come from and what we know now.
 Bond radius  Ionization Energy  Electronegativity  Electron Affinity*
Atomic Structure Notes. Thomson Model The “pudding” had a positive charge and the “plums” had a negative charge.
Historical Development of an Atom. Democritus B.C Democritus was a Greek philosopher ( B.C.) who is the father of modern atomic thought.
History of Atomic Theory Figuring Out Atoms. Dalton’s Atomic Theory 1.Matter is composed of extremely small particles called atoms. 2.Atoms are indivisible.
PERIODIC TRENDS. Periodic Law When elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals.
(8th) Chapter 4-1 Cornell Notes “Introduction to Atoms”
Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group? Do Now: Answer in your notebook If an atom.
Unit 3 Atomic Structure.
Write the Complete Electron Configuration for:
End Catalyst The periodic table is arranged by what?
Periodic Table Trends SWBAT: predict the atomic radius, ionization energy, electronegativity, nuclear charge, and shielding effect of atoms based on the.
Atomic Radius Ionization Energy Electronegativity
Evolution of the atomic model
Periodic Table Trends.
Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group? Do Now: Answer in your notebook Explain.
Atomic Theory The idea that matter is made up of atoms, the smallest pieces of matter.
Effective Nuclear Charge!!
Presentation transcript:

Catalyst 1.What would J.J. Thomson say to Dalton to prove that his plum pudding model is superior? 2.What would Ernest Rutherford say to J.J. Thomson to prove that his atomic model is superior? 3.What would Niels Bohr say to those other dead white guys to prove that his orbiting model is the superior? End

Review - Important Point #1 The atom is mostly empty space. This is why most of the alpha particles went through The majority of the atom does not have anything in it.

Review - Important Point #2 The atom has very small, but very dense nucleus. Alpha particles that bounced back were coming into contact with nucleus. Alpha particles were deflected back because nucleus is positive.

Lecture 1.9 – Bohr’s Electron Shells

Today’s Learning Targets 1.15 – I can define atomic/ionic radius and explain how it relates to the charge of the nucleus and the electron. Furthermore, I can explain how this trend changes as you move throughout the Periodic Table.

Niels Bohr Refined Rutherford’s model of the atom with his discovery in 1913.

What Bohr Knew Shooting electricity through the hydrogen excited electrons. Color produced only for specific values Problem – If electrons were free to roam, then we should get all sorts of colors

Bohr’s Solution Electrons are not free to roam in the electron cloud, electrons are restricted to orbits or energy levels.

The Modern Model Rutherford ’ s space and nucleus Dalton ’ s atom Bohr ’ s energy levels Thompson ’ s electrons

SUMMARIZE

Magnets! How do they work?

Nuclear Attraction The negatively charged electrons are attracted towards the positively charged nucleus. The negatively charged electrons are attracted towards the positively charged nucleus. The more the electron “feels” the nucleus. The tighter it is held The more the electron “feels” the nucleus. The tighter it is held

What do the arrows represent? How does the thickness of the arrows relate to nuclear attraction? How does the size of the atom relate to the positive and negative charges in an atom?

a As you move from the smallest atom to the largest atom, how does the distance between the valence electrons and the nucleus change? As you move from the smallest atom to the largest atom, how does the attractive force between the valence electrons and the nucleus change? What direction does this go on the periodic table? Why are the atoms getting bigger?

Stop and Jot Order the elements from smallest to largest IE: phosphorus, arsenic, nitrogen.

SUMMARIZE

Master Chef - White Board Races

White Board Relay Race Problems 1.Which has a larger atomic radius: chlorine or silicon? 2.Which has a smaller atomic radius magnesium or calcium? 3.Put the following elements in order from smallest atomic radius to largest: B, F, N, O. 4.Put the following elements in order from smallest atomic radius to largest: N, As, Bi, P. 5.Why does bromine do a worse job of attracting electrons than fluorine?

Atomic Radius Atomic Radius – The distance from the center of the nucleus to the outermost edge of the electron cloud Outer edge of electron cloud Nucleus

Atomic Radius Trends Atomic radius increases as you go down a group on the Periodic Table. Atomic radius decreases as you go across a period on the Periodic Table

Why Atomic Radius Increases Down a Group As you add more electron shells to an element, the element becomes “bulkier”. This means that as you go down a group, more orbits are added, so the radius becomes bigger.

Why Atomic Radius Decreases Across a Period As you move across a period, more protons are added to the nucleus. Also, more electrons are added within the same orbit. This means there is a larger positive and negative charge, which results in a higher attraction and a decrease in the radius.

SUMMARIZE

Master Chef - White Board Races

Whiteboard Questions (T/F) 1.Atomic radius is the distance from the center of the nucleus to the first electron orbit. 2.Atomic radius increases across a period and down a group. 3.Atomic radius decreases down a group because you are adding more electron orbits. 4.Atomic radius decreases across a period because there are less electrons in the same orbit.

Whiteboard Questions (cont) 5. Order the following from largest to smallest atomic radius: Ca, Se, Ni - Answer: Se, Ni, Ca 6. Order the following from largest to smallest atomic radius: O, Po, S - Answer: O, S, Po 7. Order the following from smallest to largest atomic radius: Cs, F, Ga - Answer: F, Ga, Cs

Exit Ticket 1. Define atomic radius 2. Define electronegativity. 3. Order from largest to smallest electronegativity: Ca, Se, Ni 4. Order from smallest to largest atomic radius: O, Po, S

Rate Yourself Based on the exit ticket and your current level of understanding, rate yourself 1 – 4 on LT 1.8 and 1.9

Closing Time 1.9 – Electronegativity and Atomic Radius UNIT 1 EXAM Thursday/Friday (9/19/2014)!